Matter/Naming/Solutions Unit
Table
of
Contents
CHAPTER
2
-‐
MATTER
AND
CHANGE
. ..........................................................................................................................
3
2.1
PROPERTIES
OF
MATTER .
.................................................................................................................................................................
5
2.2
MIXTURES .
...........................................................................................................................................................................................
7
2.1
AND
2.2
HOMEWORK
. .......................................................................................................................................................................
8
2.3
ELEMENTS
AND
COMPOUNDS
. .........................................................................................................................................................
9
2.3
HOMEWORK
. ....................................................................................................................................................................................
1 3
2.4
CHEMICAL
REACTIONS
. ..................................................................................................................................................................
1 4
CHEMICAL
AND
PHYSICAL
CHANGES
WORKSHEET
..........................................................................................................................
1 5
2.4
HOMEWORK
. ....................................................................................................................................................................................
1 6
CHAPTER
2
STUDY
GUIDES
..........................................................................................................................................
1 7
2.1:
PROPERTIES
OF
MATTER
–
STUDY
GUIDE .
........................................................................................................................
1 7
2.2:
MIXTURES
–
STUDY
GUIDE
.......................................................................................................................................................
1 8
2.4:
CHEMICAL
REACTIONS
–
STUDY
GUIDE
.............................................................................................................................
1 9
CHAPTER
2
PRACTICE
QUIZ
. ................................................................................................................................................................
2 0
CHAPTER
9
-‐
CHEMICAL
NAMES
AND
FORMULAS .
................................................................................................
2 2
9.1
NAMING
IONS .
..................................................................................................................................................................................
2 3
9.1
HOMEWORK
. ....................................................................................................................................................................................
2 5
9.2
NAMING
AND
WRITING
FORMULAS
FOR
IONIC
COMPOUNDS
. ................................................................................................
2 6
9.3
NAMING
AND
WRITING
FORMULAS
FOR
MOLECULAR
COMPOUNDS .
....................................................................................
2 9
9.2/9.3
HOMEWORK
(GRADECAM
BOX
ON
NEXT
PAGE) .
....................................................................................................
3 1
CHAPTER
9
STUDY
GUIDES
..........................................................................................................................................
3 3
9.1:
NAMING
IONS
–
STUDY
GUIDE
................................................................................................................................................
3 3
9.2
NAMING
AND
WRITING
FORMULAS
FOR
IONIC
COMPOUNDS
-‐
STUDY
GUIDE
.................................................
3 4
9.3
NAMING
AND
WRITING
FORMULAS
FOR
MOLECULAR
COMPOUNDS
-‐
STUDY
GUIDE .
..................................
3 5
CHAPTER
9
PRACTICE
QUIZ
. ................................................................................................................................................................
3 6
CH.
15
-‐
AQUEOUS
SYSTEMS
CH.
16
-‐
SOLUTIONS
. ...............................................................................
3 7
15.2
HOMOGENEOUS
AQUEOUS
SYSTEMS
(ONLY
PAGES
494-‐495)
. ..........................................................................................
3 8
15.2
HOMEWORK
..................................................................................................................................................................................
4 0
16.1
PROPERTIES
OF
SOLUTIONS
. ......................................................................................................................................................
4 1
16.2
CONCENTRATIONS
OF
SOLUTIONS
............................................................................................................................................
4 2
16.1/16.2
HOMEWORK
(I
WILL
GRADE
#S
12/13
BEFORE
YOU
SCAN
YOUR
HOMEWORK)
. .................................................
4 4
CHAPTERS
15
AND
16
REVIEW .
..........................................................................................................................................................
4 5
CHAPTER
16
STUDY
GUIDES
. .......................................................................................................................................
4 7
16.1:
PROPERTIES
OF
SOLUTIONS
–
STUDY
GUIDE .
...............................................................................................................
4 7
16.2:
CONCENTRATIONS
OF
SOLUTIONS
–
STUDY
GUIDE .
..................................................................................................
4 8
CHAPTER
15/16
PRACTICE
QUIZ .
......................................................................................................................................................
4 9
CHEMICAL
AND
PHYSICAL
CHANGES
LAB
...............................................................................................................
5 0
“FREESI”
–
FREEMAN’S
SCIENTIFIC
INVESTIGATION
. ...........................................................................................
5 3
“MAKING”
IONIC
COMPOUNDS
LAB
. ..........................................................................................................................
5 5
RATE
OF
DISSOLVING
LAB
. ...........................................................................................................................................
5 6
MOLARITY
OF
LEMONADE
LAB
. ..................................................................................................................................
5 8
BEVERAGE
DENSITY
LAB
..............................................................................................................................................
6 1
UNIT
TEST
SETUP
. ...........................................................................................................................................................
6 6
UNIT
REVIEW
MATERIALS .
...........................................................................................................................................
6 7
CHAPTER
2
VOCABULARY
REVIEW
. ....................................................................................................................................................
6 7
CHAPTER
9
VOCABULARY
REVIEW
. ....................................................................................................................................................
6 8
UNIT
REVIEW
–
CHAPTERS
2
AND
9
..................................................................................................................................................
6 9
Chapter
2
-‐
Matter
and
Change
2.1 – Properties of Matter
Objectives
• Identify physical properties and physical changes
• Distinguish intensive properties from extensive properties
• Differentiate among three states of matter
Vocabulary • substance • gas
• mass
• physical property • vapor
• volume • solid • physical change
• extensive property • liquid
• intensive property
2.2 – Mixtures
Objectives
• Classify a sample of matter as a substance or a mixture
• Distinguish between homogeneous and heterogeneous samples of matter
• Describe two ways that components of mixtures can be separated
Vocabulary • phase
• mixture • filtration
• heterogeneous mixture • distillation
• homogeneous mixture
• solution
2.4 – Chemical Reactions
Objectives
• Explain the difference between an element and a compound
• Distinguish between a substance and a mixture
• Identify the chemical symbols of elements, and name elements, given their symbols
Vocabulary • chemical change
• chemical symbol
• element
• compound
2.4 – Chemical Reactions
Objectives
• Describe what happens during a chemical change
• Identify possible clues that a chemical change has taken place
• Apply the law of conservation of mass to chemical reactions
Vocabulary • reactant • precipitate
• chemical property
• chemical reaction • product • law of conservation of mass
2.1
Properties
of
Matter
After reading Lesson 2.1, answer the following questions.
Describing Matter
1. The of an object is a measure of the amount of matter the object contains.
2. How does an extensive property differ from an intensive property?
Extensive (_________________) Properties – the numbers in a measurement are called
____________________ figures (the _______ digit is estimated).
mass = volume = length = cm
g mL
temperature =
pressure = °C
mm Hg
Intensive (_________________) Properties Intensive (qualitative) properties
3. Matter that has a uniform and definite composition is called a .
4. Is the following sentence true or false? All samples of a substance have different physical
properties.
5. A physical property is a quality or condition of a substance that can be
or without changing the substance’s
composition.
6. Circle the letter of the term that is NOT a physical property.
a. hardness b. color c. boiling point d. melting
7. Look at Table 2.1. What is the melting point of bromine?
___________
8. Look at Table 2.1. Circle the letter of the substance that
is a yellow solid and melts at 115°C.
a. sulfur b. chlorine
c. gold d. copper
9. Is the following sentence true or false? Physical
properties can help a chemist identify a
substance.
States of Matter
10. Circle the letter of the term that is NOT a physical state of matter.
a. water b. gas c. liquid d. solid
11. Complete the table about the properties of the three states of matter. Use these terms:
definite, indefinite, easily, and not easily.
Properties of the States of Matter
Property
Solid
Liquid
Gas or Vapor
Shape
indefinite
Volume
definite
indefinite
Can be compressed
not easily
12. Match each arrangement of the particles in matter with a physical state.
Physical State
Arrangement
___ gas a. packed tightly together
___ liquid b. close, but free to flow
___ solid c. spaced relatively far apart
13. Is the following true or false? The words gas and vapor describe the same thing. _____________
14. The term gas is limited to those substances that exist in the gaseous state at ________________.
15. What does vapor describe?
15a. Smoke is a mixture of ________, water vapor and gas particles in a ___________________ (solid
particles are “_______” (suspended) in the vapor).
Physical Changes
16. A physical change alters a given material without changing its chemical __________________.
17. What are some words that describe physical changes?
18. What is true about all physical changes that involve a change of state?
2.2
Mixtures
After reading Lesson 2.2, answer the following questions.
Classifying Mixtures
1. Is the following sentence true or false? Most samples of matter are mixtures. _______________
2. What is a mixture?
3. Is the following sentence true or false? A heterogeneous mixture is one that has a completely uniform
composition.
4. What is another name for a homogeneous mixture?
5. Circle the letter of the term that describes a part of a sample having uniform composition and properties.
a. solution b. mixture c. state d. phase
6. How many phases exist in these types of mixtures?
a. Homogeneous b. Heterogeneous _________________
acetone water
and and
water methylene
chloride
Separating Mixtures
7. In general, what is used to separate mixtures?
8. The process that separates a solid from a liquid in a heterogeneous mixture is called
.
9. What happens during distillation?
2.1
and
2.2
Homework
1-6: Matching – Match the term with the description.
1. another term for qualitative A. 25.3 g
properties B. color
2. another term for quantitative C. extensive
properties D. intensive
3. example of an extensive E. mass
property AB. substance
4. example of an intensive
property
5. matter with uniform and
definite composition
6. the amount of matter an object
contains
7-13. Categorize the following descriptions as that describing a (S)olid, (L)iquid, or (G)as.
__7. definite shape AND definite volume
__8. particles close together, but easily slide past each other
__9. particles tightly packed and not much movement of particles
__10. particles very far apart
__11. takes the entire volume of its container and has no real shape
__12. takes the shape of its container to its definite volume
__13. very compressible
__14. __describes the gaseous state of a substance that is generally a liquid or solid at room temperature.
A. gas B. vapor C. smoke
__15. A gas is a substance that normally exists in the gaseous state at __ temperature.
A. freezing B. boiling C. room
__16. During a(n) __ change, the properties of a material change, but not it’s composition.
A. physical B. chemical C. energy
__17. Smoke is a mixture of solids, water vapor, and gases in a(n) __ (the particles are held in the vapor).
A. gas B. suspension C. container
18-25. Categorize the following physical changes as (R)eversible or (I)rreversible.
__18. boiling __22. dissolving
__19. condensing __23. freezing
__20. crushing __24. grinding
__21. cutting __25. splitting
26-30: Matching: Match the term with the description.
__26. a homogeneous mixture A. distillation
__27. a physical combination of two or more substances B. filtration
__28. part of a mixture with uniform composition and properties C. mixture
__29. process to separate a heterogeneous mixture of a solid and liquid D. phase
__30. process to separate liquids of different boiling points E. solution
2.3
Elements
and
Compounds
Distinguishing Elements and Compounds
How are elements and compounds different?
Substances can be classified as elements or compounds.
• An _________________________ is the simplest form of matter that has a unique set of properties.
– Oxygen and hydrogen are two of the more than __________ known elements.
• A compound is a substance that contains two or more elements _________________________ combined in a
fixed proportion.
Carbon, oxygen, and hydrogen are chemically combined in the compound sucrose.
• In every sample of sucrose, there are ___________________ as many hydrogen particles as oxygen particles.
• The proportion of hydrogen particles in sucrose is ___________________.
There is a key difference between elements and compounds.
• Compounds can be broken down into simpler substances by _________________________ means, but elements
cannot.
Breaking Down Compounds
Physical methods that are used to separate mixtures _________________ be used to break a compound into
simpler substances.
• Boil liquid water and you get _________________________, not the oxygen and hydrogen that water contains.
• _________________________ a sugar cube in water and you still have sucrose, not oxygen, carbon, and
hydrogen.
– This does not mean that sucrose or water cannot be broken down into simpler substances.
– But methods must involve a _________________________________________.
A chemical change is a change that produces matter with a _________________________ composition than the
original matter.
_________________________ is one of the processes used to break down compounds into simpler substances.
• The layer of sugar is heated until it ____________ ______________ into solid carbon and water vapor.
Can the substances that are produced when sugar is broken down when heated also be broken down?
• There is no _________________________ process that will break down carbon into simpler substances because
carbon is an element.
When an electrical current passes through water, it is broken down into __________________ and hydrogen.
Properties of Compounds
In general, the properties of compounds are quite ____________________________ from those of their
component elements.
• Sugar is a sweet-tasting white solid, but carbon is a ____________________________ black solid.
• Hydrogen is a gas that burns in the presence of oxygen—a colorless gas that _____________________ burning.
– The product of this chemical change is __________________, a liquid that can stop materials from burning.
When the elements sodium and chlorine combine ____________________________ to form
sodium chloride, there is a change in composition and a change in properties.
• Sodium is a soft _____________ metal.
• Chlorine is a pale yellow __________________________________ gas.
• Sodium chloride (commonly known as table salt) is a _____________ solid.
Can elements be broken down by chemical changes? Can compounds?
There are _____ chemical processes that can break down an element into simpler substances.
Compounds can be broken down by _______________________ changes.
Distinguishing Substances and Mixtures
Deciding whether a sample of matter is a substance or a _______________________ based solely on appearances
can be difficult.
• After all, ____________________________ mixtures and substances will both appear to contain only one kind
of matter.
Sometimes you can decide by considering whether there is more than one version of the material in question.
• You can buy whole milk, low-fat milk, no-fat milk, light cream, or heavy cream.
– From this information, you can conclude that milk and cream are ____________________________.
– You might infer that these mixtures differ in the amount of __________ they contain.
• Most gas stations offer at least two blends of gasoline.
– The blends have different ________________________ ratings and different costs per gallon.
– So, gasoline must be a mixture.
If the composition of a material is fixed, the material is a ____________________________.
If the composition of a material may ________________, the material is a mixture.
Symbols and Formulas
What do chemists use to represent elements and compounds?
Chemists use chemical symbols to represent ____________________________, and chemical
____________________________ to represent compounds.
Using symbols to represent different kinds of matter is not a new idea.
• For thousands of years, _____________________________ used
symbols, such as the ones below, to represent elements.
• Alchemists and the English chemist John Dalton (1766–1844) both used
____________________________ to represent chemical elements.
The symbols used today for elements are based on a system developed by
Swedish chemist Jöns Jacob Berzelius (1779–1848).
• He based his symbols on the __________________ names of elements.
• Each element is represented by a one- or two-letter chemical symbol.
– First letters of chemical symbols are ____________________________.
– When a _____________________ letter is used, it is lowercase.
If the English name and the Latin name of an element are similar, the symbol will appear to have been
derived from the ____________________________ name.
• Examples include Ca for calcium, N for nitrogen, and S for sulfur.
Symbols and Latin Names for Some Elements
Name Symbol Latin name
Sodium Na natrium
Potassium K kalium
Antimony Sb stibium
Copper Cu cuprum
Gold Au aurum
Silver Ag argentum
Iron Fe ferrum
Lead Pb plumbum
Tin Sn stannum
Chemical symbols provide a ____________________________ way to write the chemical formulas of
compounds.
• The symbols for hydrogen, oxygen, and carbon are H, O, and C.
• The formula for water is __________.
• The formula for ______________________, or table sugar, is C12H22O11.
__________________ in the chemical formulas tell you how many of each type of element are in the
compound.
• The subscript 2 in H2O indicates that there are two parts of _____________________ for each part of
oxygen in water.
• Because a compound has a ________________ composition, the formula for a compound is always the
same.
The Periodic Table
Why is a periodic table useful?
All the known elements are organized in a special table called the periodic table.
• A periodic table is an arrangement of elements in which the elements are separated into groups based
on a set of ____________________________ properties.
The periodic table allows you to easily compare the properties of one element (or a group of elements)
to another element (or group of elements).
Each element is identified by its ____________________________ placed in a square.
• The elements are listed in order from left to right and top to bottom by
____________________________,
a number that is unique to each element.
• The atomic number of the element is shown centered above the symbol.
– Hydrogen (H), the _________________ element, is in the top left corner.
– Helium (He), atomic number 2, is at the top ____________________.
– Lithium, atomic number 3, is at the __________ end of the second row.
Each horizontal row of the periodic table is called a ____________________________.
• There are ___________________ periods in the periodic table.
• The number of elements per period ranges from 2 (hydrogen and helium) in Period 1 to 32 in Period 6.
Within a period, the properties of the elements _______________ as you move across the period.
• This pattern of properties then _____________________ as you move to the next period.
Each vertical column of the periodic table is called a group, or _______________________.
• Elements within a group have _________________________ chemical and physical properties.
• Note that each group is identified by a number and the letter A or B.
– Group _____ contains the elements beryllium (Be), magnesium (Mg), calcium (Ca), strontium
(Sr), barium (Ba), and radium (Ra).
2.3
Homework
1-10. Use the terms on the right to complete the passage
below. Some answers may be used more than once and some
may not be used at all.
A substance is either a(n) __1__ or a(n) __2__. a. chemical
Compounds are made up of __3__(s), which are always b. compound
present in the same __4__ in a given compound. Compounds c. substance
can be broken down into simpler substances by __5__ means. d. symbol
e. element
If the composition of a material is fixed, it is a __6__. If ab. mixture
the composition of a material may vary, it is a __7__. ac. P
ad. K
Each element is represented by a one- or two-letter ae. proportion (part)
__8__. For example, carbon is represented by the symbol bc. C
__9__, while potassium is represented by the symbol __10__.
11-14. Classify each of these statements as always true, A; sometimes true, S; or never true, N.
11. Heating a chemical compound produces elements.
12. Compounds can be broken down into elements by physical means.
13. An element is the simplest form of matter that has a unique set of properties.
14. Compounds are represented by chemical formulas.
15-19. Match each description in Column B to the correct term in Column A.
Column A Column B
15. element a. substance that can be separated into simpler
16. compound substances only by chemical means
17. mixture
18. chemical symbol b. a physical blend of two or more components
19. chemical change c. one or two letters that represent an element
d. simplest form of matter that has a unique set
of properties
e. a change that produces matter with a different
composition than the original matter
2.4
Chemical
Reactions
After reading Lesson 2.4, answer the following questions.
Chemical Changes
1. What is a chemical property?
2. Is the following sentence true or false? Chemical properties are observed only when a substance undergoes a
chemical change.
3. What happens during a chemical reaction?
4. In chemical reactions, the substances present at the start of the reaction are called .
, and the substances produced are called
5. Circle the letter of the term that best completes the sentence. A change in the
composition of matter occurs during a chemical reaction.
a. sometimes b. rarely c. always d. never
6. Which representation of a chemical reaction is correct?
a. products → reactants b. reactants → products
6 C3H7OH(l) + 25 O2(g) → 18 CO2 (g) + 22 H2O(g)
(reactants) (products)
Recognizing Chemical Changes
7. List FIVE possible clues to a chemical change.
8. Is the following statement true or false? If you observe a clue for chemical change, you can be certain that a
chemical change has taken place.
9. Define precipitate.
Conservation of Mass
10. During a chemical reaction, the mass of the products is always equal to the mass of the
.
11. The law of conservation of mass states that in any physical change or chemical reaction,
mass is neither nor .
12. Look at Figure 2.16. How do you know that mass was conserved?
Before After
14
Chemical
and
Physical
Changes
worksheet
1. Label each process as a physical or chemical
change:
___a. perfume evaporating on your skin 5. If a certain mixture is homogeneous, you would
___b. butter melting properly conclude that the physical properties and the
___c. wood rotting composition:
___d. charcoal heating a grill a. are different from one part of the sample to another
___e. autumn leaves changing color b. vary smoothly from top to bottom of the sample
___f. a hot glass cracking when placed in cold water c. are the same in every small volume element from
___g. melting copper metal the sample
___h. burning sugar d. none of these
___i. mixing sugar in water 6. Label each process as a physical or chemical
___j. digesting food change:
2. Which of the following would NOT be a physical ___a. Moth balls gradually vaporize in a closet
change? ___b. hydrofluoric acid attacks glass (used to etch
glassware)
a. freezing water to make ice cubes ___c. A chef making a sauce with brandy is able to
b. melting gold to make jewelry burn off the alcohol from the brandy, leaving just the
c. burning gasoline in a lawnmower brandy flavoring
d. boiling water for soup ___d. Chlorine gas liquefies at -35 °C under normal
pressure
e. tearing a piece of aluminum foil ___e. hydrogen burns in chlorine gas
3. Which of the following is NOT a physical change? 7. Label each process as a physical or chemical
change:
a. grating cheese
b. melting cheese ___a. fogging a mirror with your breath
___b. breaking a bone
c. fermenting of cheese ___c. mending a broken bone
d. mixing two cheeses in a bowl ___d. burning paper
___e. slicing potatoes for fries
4. Which are physical and which are chemical ___f. mixing sugar with coffee
changes? ___g. frying chicken
___h. a nail rusting
___a. boil ___k. oxidize ___i. paper ripping
___b. burn (combustion) ___l. tarnish ___j. wood burning
___c. condense ___m. explode ___k. mixing water and food coloring
___d. corrode ___n. grind ___l. food molding (rotting)
___m. writing on paper
___e. crumple ___o. rot ___n. dyeing fabric
___f. ferment ___p. vaporize
___g. melt ___q. photosynthesis
___h. rust ___r. sublimation
___i. crush
___j. freeze
15
2.4
Homework
1-3 - Matching
a. mixture d. reactant
b. product e. chemical reaction
c. phase
__1. a substance formed in a chemical reaction
__2. starting substance in a chemical reaction
__3. process in which substances are changed into
different substances
4-20 - Multiple Choice __10. Which of the following processes involves a
__4. Which of the following is a chemical property? change in physical properties?
a. color a. rusting
b. hardness b. fermenting
c. freezing point c. boiling
d. ability to react with oxygen d. burning
__5. In the chemical reaction in which sucrose is heated __11. A chemical change occurs when a piece of wood
and decomposes to form carbon dioxide and water, a. splits.
which of the following is a reactant? b. is painted.
a. sucrose c. decays.
b. carbon dioxide __12. Which of the following is a chemical property of
c. water water?
d. heat a. its color
b. its state
__6. What must occur for a change to be a chemical c. its temperature
reaction? d. its ability to decompose into hydrogen and oxygen
a. There must be a change in chemical properties.
b. There must be a change in physical properties. __13. What must be done to be certain that a chemical
c. The change must involve a change in mass. change has taken place?
d. The change must involve a change in volume. a. Check for the production of bubbles before and after
__7. Which of the following is a chemical change? the change.
a. grating cheese b. Demonstrate that a release of energy occurred after
b. melting cheese
c. fermenting of cheese the change.
d. mixing two cheeses in a bowl c. Check the composition of the sample before and
__8. Which of the following changes to a metal is a after the change.
chemical change? d. Demonstrate that energy was absorbed by the
a. bending
b. melting reactants after the change.
c. rusting
d. polishing __14. When paper turns yellow-brown upon exposure to
sunlight, what type of change is likely taking place?
__9. Which of the following involves a chemical a. a physical change
change? b. a chemical change
a. mixing c. neither a physical change nor a chemical change
b. melting d. both a physical change and a chemical change
c. grinding
d. decomposing __15. Which of the following indicates that a chemical
change has happened during cooking?
a. The food darkens.
b. Bubbles form in boiling water.
c. Butter melts.
d. Energy is transferred from the stove to a pan.
16
Chapter
2
Study
Guides
2.1:
PROPERTIES
OF
MATTER
–
Study
guide
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms that are introduced in this
section. Each blank can be completed with a term, short phrase, or number.
Properties used to describe matter can be classified as 1.
2.
___1____ or ___2____. The ____3___ of an object is a 3.
4.
measure of the amount of matter the object contains. The 5.
6.
___4____ of an object is a measure of the space occupied by 7.
8.
the object. An extensive property is one that depends on the 9.
10.
___5____ of matter. An intensive property is one that depends 11.
on the _____6__ of matter.
A ___7____ is matter that has uniform and definite
composition. A solid has a definite ___8____ and ____9___. A
liquid has a definite volume, but takes the ___1_0___ of its
container. A ____11___ takes both the shape and volume of its
container.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
11. Matter has mass and occupies space.
12. A liquid has a definite shape.
13. Heating a solid to 200°C will cause it to change to a liquid.
14. Gases are easier to compress than liquids.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A Column B
15. volume a. a quality or condition of a substance that can be observed or
measured without changing the substance’s composition
16. mass
17. substance b. matter that takes both the shape and volume of its container
18. physical property c. matter that has a uniform and definite composition
19. solid d. measure of the space occupied by an object
20. liquid e. matter that has a definite volume and takes the shape of its container
21. gas f. a change to a material that does not change its composition
22. vapor g. gaseous state of a substance that generally exists as a liquid or solid
23. physical change
24. extensive property at room temperature
25. intensive property h. matter that has a definite shape and volume
i. the amount of matter that an object contains
j. depends on the type of matter in a sample
k. depends on the amount of matter in a sample
17
2.2:
MIXTURES
–
Study
guide
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank
can be completed with a term, short phrase, or number.
A physical blend of two or more substances is a ___1____. A 1.
mixture has a composition that varies. Mixtures may be identified 2.
as ____2___ or ___3____. Homogeneous mixtures are also known as 3.
___4____ and have uniform properties. Any part of a sample with 4.
uniform composition and properties is called a ___5____. 5.
6.
Many mixtures can be separated into their components by 7.
___6____ methods. ___7____ is a method of separation that involves
boiling a liquid, which is then condensed.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
8. Homogeneous mixtures can be separated by distillation.
9. A solution has a uniform composition.
10. A heterogeneous mixture contains two or more phases.
11. Solutions are liquids.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A Column B
12. mixture a. a mixture that has a uniform composition throughout
13. heterogeneous mixture b. any part of a sample that has uniform composition and
14. homogeneous mixture properties
15. solution
16. phase c. a mixture that is not uniform in composition
17. distillation
18. filtration d. separation of a liquid by boiling followed by condensation
e. another name for a homogeneous mixture
f. a physical blend of two or more components
g. a method for separating a solid from a liquid in a heterogeneous
mixture
18
2.4:
CHEMICAL
REACTIONS
–
Study
guide
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank
can be completed with a term, short phrase, or number.
Substances change into new substances du1ring a(n) _______ 1.
2.
reaction. A change in which the properties of a substance change, 3.
but not its composition, is a ___2____ change. If the composition 4.
changes, then a ____3___ change has occurred. In a chemical reaction, 5.
___4____ are converted to products. The only way to be sure a 6.
___5____ change has occurred is to test the ___6____ composition of a 7.
sample before and after a change. The law of ____7___ states that 8.
mass is conserved in any physical change or chemical reaction. In
other words, ___8____ is neither created nor destroyed.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
9. A physical change is reversible.
10. In a chemical reaction, reactants are changed into products.
11. The amount of matter present appears to change during a chemical reaction.
12. Matter can be created during a chemical reaction.
13. The substances formed in a chemical reaction are called reactants.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A Column B
14. chemical reaction a. solid that forms and settles out of a liquid mixture
15. reactants b. starting substances in a chemical reaction
16. product c. ability of a substance to undergo a specific chemical change
17. chemical property d. substance formed in a chemical reaction
18. precipitate e. process in which one or more substances change into one or more
new substances
19
Chapter
2
Practice
Quiz
1-10. Multiple choice. Place the letter that best answers the question in the space to the left of the number.
__1. Select the best statement. __6. If a liquid contains 60% sugar and 40% water
A. Physical changes may be reversed by changing the throughout its composition then what is it called?
temperature. A. solute
B. Physical changes alter the composition of the B. compound
substances involved. C. homogeneous mixture
C. Physical properties are not valid characteristics for D. heterogeneous mixture
identifying a substance. E. solvent
D. Physical properties are mostly extensive in nature.
E. Physical changes are usually accompanied by __7. Which of these is an example of a physical
chemical changes. property?
A. corrosiveness of sulfuric acid
__2. Which of the following is a chemical change? B. toxicity of cyanide
A. boiling of water C. flammability of gasoline
B. melting wax D. neutralization of stomach acid with an antacid
C. broiling a steak on a grill E. lead becoming a liquid when heated to 601°C
D. condensing water vapor into rainfall
E. carving a piece of wood __8. Select the best statement.
A. Chemical changes provide the only valid basis for
__3. Which of the following is an extensive property identification of a substance.
of oxygen? B. Chemical changes are easily reversed by altering
A. boiling point the temperature of the system.
B. temperature C. Chemical changes always produce substances
C. average kinetic energy of molecules different from the starting materials.
D. density D. Chemical changes are associated primarily with
E. mass extensive properties.
E. Chemical changes are accompanied by changes in
__4. Which of the following cannot be classified as a the total mass of the substances involved.
substance?
A. table salt __9. Which one of these represents a physical
B. iron change?
C. air A. Water, when heated, forms steam.
D. sulfur B. Bleach turns hair yellow.
E. carbon dioxide C. Sugar, when heated, becomes brown.
D. Milk turns sour.
__5. Which of the following cannot be separated into a E. Apples, when exposed to air, turn brown.
simpler substance by chemical means?
A. element __10. Which one of these represents a chemical
B. emulsion change?
C. compound A. boiling water to form steam
D. homogeneous mixture B. turning hair yellow with bleach
E. heterogeneous mixture C. melting butter
D. mixing charcoal and oxygen at room temperature
E. cutting a bar of sodium metal with a knife
20
11-14. True or Fix-it. If the statement is true, write TRUE in the space provided; otherwise change
the underlined word(s) to make the statement true.
_______________________11. The ripening of fruit is an example of physical change.
_______________________12. The density of a substance is an intensive property.
_______________________13. Boiling point and melting point are extensive properties.
_______________________14. Rusting of a piece of iron is a chemical change.
15-19. Classify the following properties of hydrogen gas as either Intensive or Extensive.
__15. the mass of the gas sample
__16. the average speed of a molecule in the sample
__17. temperature
__18. density
__19. number of molecules present
20-25. Write a short essay for the following.
Distinguish between physical changes and chemical changes and give one example of each.
Then, list three clues that are often indications of chemical changes.
_________________________________________________________________________________
_________________________________________________________________________________
_________________________________________________________________________________
_________________________________________________________________________________
_________________________________________________________________________________
_________________________________________________________________________________
_________________________________________________________________________________
_________________________________________________________________________________
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21
Chapter
9
-‐
Chemical
Names
and
Formulas
9.1 – Naming Ions
Objectives
• Determine the charges of monatomic ions by using the periodic table and write the names of
the ions
• Define a polyatomic ion and write the names and formulas of the most common polyatomic
ions
• Identify the two common endings for the names of most polyatomic ions.
Vocabulary
• monatomic ions
• polyatomic ions
9.2 – Naming and Writing Formulas for Ionic Compounds
Objectives
• Apply the rules for naming and writing formulas for binary ionic compounds
• Apply the rules for naming and writing formulas for compounds with polyatomic ions
Vocabulary
• binary compound
9.3 – Naming and Writing Formulas for Ionic Compounds
Objectives
• Interpret the prefixes in the names of molecular compounds in terms of their chemical formulas
• Apply the rules for naming and writing formulas for binary molecular compounds
22
9.1
Naming
Ions
After reading Lesson 9.1, answer the following questions.
Monatomic Ions
1. What are monatomic ions?
_________________________________________________________
2. How is the ionic charge of a Group 1A, 2A, or 3A ion determined?
__________________________________________________________
3. How is the ionic charge of a Group 5A, 6A, or 7A ion determined?
__________________________________________________________
Metals That Form More Than One Ion
4. Many of the transition metals (Groups 1B-8B) form more than one cation with __________________
ionic charges.
5. The of naming
transition metal cations uses a Roman numeral in
parentheses to indicate the numeric value of the ionic
charge.
6. An older naming system uses the suffix -ous to name
the cation with the ___________________ charge, and
the suffix -ic to name the cation with the
________________ charge.
7. What is a major advantage of the Stock system over the
old naming system?
23
Polyatomic Ions
8. What is a polyatomic ion?
9. Is the following sentence true or false? The names of polyatomic anions always end in -ide.
10. What is the difference between the sulfite and sulfate anions?
11. Look at Polyatomic ions table. Circle the letter of a polyatomic ion that is a cation with a +1 charge.
a. ammonium b. acetate c. oxalate d. phosphate
12. Look at Polyatomic ions table. Circle the letter of a polyatomic ion that is a cation with a +2 charge.
a. ammonium b. peroxide c. mercury (I) d. thiosulfate
Polyatomic Ions
-1 -2 -3
Formula Name Formula Name Formula Name
H2PO4– HPO42– PO43–
C2H3O2– dihydrogen phosphate C2O42– hydrogen phosphate PO33– phosphate
HSO3– acetate SO32– oxalate BO33– phosphite
hydrogen sulfite SO42– sulfite AsO43– borate
S2O32– sulfate AsO33– arsenate
HSO4− hydrogen sulfate SiO32–
**HCO3– CO32– thiosulfate arsenite
NO2– hydrogen carbonate CrO42– silicate
NO3– nitrite Cr2O72– carbonate +1
CN– nitrate O22– chromate NH4+ = ammonium
cyanide dichromate
SCN– peroxide
thiocyanate
OH– hydroxide
MnO4–
ClO– permanganate +2
hypochlorite Hg22+ = mercury (I)
ClO2–
ClO3– chlorite ** If hydrogen is in the name, it can be replaced
ClO4– chlorate by the prefix bi– ; HCO3– (hydrogen carbonate)
IO3– perchlorate can be bicarbonate
IO4– iodate
periodate
24
9.1
Homework
1-8. Match the charge of the ion with the element. Some can
be used more than once and some may not be used at all.
__1. oxygen A. 0
__2. iodine B. 1-
__3. sodium C. 1+
__4. aluminum D. 2-
__5. magnesium E. 2+
__6. sulfur AB. 3-
__7. phosphorus AC. 3+
__8. calcium AD. 4-
__9. Sn+2 is called __. B. tin(II) anion
D. tin(II) cation
A. tin cation
C. tin anion
__10. Cl- is called __. B. chloride anion
A. chlorine cation D. chlorine(I) cation
C. chloride(I) anion
__11. Mg+2 is called __.
A. magnesium ion B. magnesium anion __18. In which of the following are the symbol and name for
the ion given correctly?
C. manganese ion D. magnesium (II) cation A. Fe+3: ferrous ion; Fe+2: ferric ion
B. Sn+4: stannic ion; Sn+1: stannous ion
__12. Iron has two ions with charges +2 and +3. Fe+3 is called C. Co+2: cobalt(II) ion; Co+2: cobaltous ion
D. Pb+: lead ion; Pb+4: lead(IV) ion
__.
A. ferrous ion B. ferric ion
C. ironous ion D. ironic ion
__13. Single atom ions are called __. 19. The __19. Ions formed by nonmetals in Groups 6A and 7A
A. have a numerical charge that is found by subtracting the
A. monatomic ions B. polyatomic ions group number from 8.
B. have a numerical charge that is found by subtracting 8 from
C. diatomic ions D. cations the group number.
C. all have a numerical charge of –1.
__14. A positively charged ion is called a(n) __. D. all have a name that ends in -ate.
A. cation B. anion
C. both A and B D. neither A nor B
__15. What type of ions have names ending in –ide? __20. Which of the following determines that an element is a
metal?
A. cations B. anions A. the magnitude (size) of its charge
B. the molecules that it forms
C. metal ions D. gaseous ions C. when it is a Group A element
D. whether it loses valence electrons
__16. When group 2A elements form ions, they __.
A. lose 2 p+ B. gain 2 p+
C. lose 2 e- D. gain 2 e-
__21. What is the Stock name for the chromic ion?
__17. When a transition metal ion can have more than one A. chromium(I) ion B. chromium(II) ion
charge, it is indicated by a __. C. chromium(III) ion D. chromium(IV) ion
A. prefix B. suffix __22. An –ate or –ite at the end of a compound name usually
C. Roman numeral D. superscript after the name indicates that the compound contains __.
A. fewer e- than p+ B. neutral molecules
C. only two elements D. a polyatomic ion
25
9.2
Naming
and
Writing
Formulas
for
Ionic
Compounds
Ionic Name to Formula Practice
- 1st element is a metal or polyatomic ion
if charge is not in name, find it on PT and then write formula and charge (if in name, write formula/charge)
- 2nd element is a nonmetal or polyatomic ion
look up charge on naming sheet and write formula and charge as superscript
- If charge numbers are different, cross charge numbers and reduce if necessary
(if you cross a number over to the polyatomic ion, place the formula of the polyatomic ion in parentheses)
1. mercury(II) phosphate Hg3(PO4)2
Hg+2 PO43- = Hg3(PO4)2
2. iron(III) chloride FeCl3
Fe+3 Cl- = FeCl3
3. potassium permanganate
4. manganese(II) nitride
5. strontium chloride
6. cobalt(III) oxide
7. barium iodide
8. beryllium bromide
9. calcium fluoride
10. aluminum sulfide
11. gold(III) oxide
12. ammonium nitrate
13. mercury(II) fluoride
14. manganese(III) chloride
15. manganese (III) hydroxide
16. gold(III) bromide
17. silver carbonate
18. potassium perchlorate
19. calcium acetate
20. zinc perchlorate
21. aluminum nitride
22. manganese(II) oxide
26
Ionic Formula to Name Practice
- If symbol of first element is a metal with one oxidation number (or polyatomic ion), write the name of the
cation followed by the anion (Ex. NaCl = sodium chloride)
- If the first element is a metal with multiple oxidation numbers, write the possible charges above the cation and
the charge of the anion above the anion.
- Multiply the subscript on the anion by the charge of the anion to get the total negative charge
- Choose the cation that balances the negative total charge and put that oxidation number in parentheses after the
name of the metal and name the cation and anion.
1. Cu(ClO3)2 Cu +1,+2 (ClO3-1)2, 2×(-1) = -2,
+2 balances, so it is copper (II) chlorate
Sn +2,+4 F-14, 4×(-1) = -4,
2. SnF4 +4 balances, so it is tin (IV) fluoride
3. SrS
4. Li2S
5. PbBr4
6. Na2CrO4
7. KBr
8. Mg3(PO4)2
9. FeO
10. NaBr
11. MnSO4
12. PbO2
13. SrF2
14. Sr3P2
15. CuS
16. MgS
17. NaHCO3
18. Mn2O3
19. Al2Se3
20. NH4NO3
27
Binary Ionic Compounds
1. Traditionally, common names were based on some of a compound or
its .
2. What is the general name for compounds composed of two elements? They are
.
3. When writing the formula for any ionic compound, the charges of the ions must .
4. What are two methods for writing a balanced formula?
a.
b.
5. What are the formulas for the compounds formed by the following pairs of ions?
a. Fe2+, Cl− ______ b. Cr3+, O2− _______ c. Na+, S2− _______
6. What are the formulas for these compounds?
a. lithium bromide _______ b. copper(II) nitride _______ c. magnesium chloride _______
7. The name of a binary ionic compound is written with the name of the first, followed
by the name of the .
8. How can you tell that cobalt(II) iodide is a binary ionic compound formed by a transition metal with more than
one ionic charge?
9. Write the names for these binary ionic compounds.
a. PbS
b. MgCl2
c. Al2Se3
Compounds With Polyatomic Ions
10. What is a polyatomic ion?
11. How do you write the formula for a compound containing a polyatomic ion?
12. Why are parentheses used to write the formula Al(OH)3?
13. Complete the table for these ionic compounds containing polyatomic ions.
Cation Anion Name Formula
NH4+ S2–
Fe3+ iron(III) carbonate AgNO3
NO3– KCN
potassium cyanide
28
9.3
Naming
and
Writing
Formulas
for
Molecular
Compounds
Molecular Name to Formula Practice Problems
1st element is a nonmetal (or metalloid) other than H
1a. look up nonmetal symbol and write it
1b. if contains a prefix, look up prefix and write it as a subscript for this element
2nd element nonmetal written as anion (-ide)
1a. look up nonmetal symbol and write it
1b. if contains a prefix, look up prefix and write it as a subscript for this element
1. sulfur trioxide SO3
S O3 P4O10
2. tetraphosphorus decoxide
P4 O10
3. chlorine monoxide
4. oxygen difluoride
5. boron monophosphide
6. dinitrogen monoxide
7. nitrogen trifluoride
8. sulfur tetrachloride
9. xenon trioxide
10. carbon dioxide
11. diphosphorus pentoxide
12. phosphorus trichloride
13. sulfur dioxide
14. bromine pentafluoride
15. disulfur dichloride
16. boron trifluoride
17. tetraarsenic decoxide
18. silicon tetrachloride
19. krypton difluoride
20. chlorine monoxide
21. silicon dioxide
22. boron trichloride
29
Molecular Formula to Name Practice Problems
First element is a nonmetal or metalloid,
1. Look up the name and write it; if the element has a subscript, write the proper prefix.
2. Look up name of second element write the proper prefix and end it as if it were an anion (-ide).
If a-o or o-o vowel combinations MUST lose first vowel (tetraoxide is tetroxide)
1. BN BN
boron mononitride
2. N2O3 dinitrogNe2nOt3rioxide
3. NI3
4. SF6
5. XeF4
6. PCl3
7. CO
8. PCl5
9. P2O5
10. S2Cl2
11. ICl2
12. SO2
13. P4O10
14. N2H4
15. OF2
16. ClO2
17. SiO2
18. BF3
19. N2S5
20. CO2
21. SO3
22. XeF6
23. KrF2
24. BrCl5
30
Binary Molecular Compounds
1. To name a molecular compound, name the first element, add the root of the second element plus -ide, then add
given by the formula’s subscripts.
2. To write the formula of a molecular compound, write the symbol of each element, then
write given by prefixes in the name of the compound.
3. Circle the letter of the type(s) of elements that form binary molecular compounds.
a. two nonmetallic elements b. a metal and a nonmetal c. two metals
4. Is the following sentence true or false? Two nonmetallic elements can combine in only one way.
5. What method is used to distinguish between different molecular compounds that contain the same elements?
WRITE the number each prefix indicates.
6. octa-
7. tetra-
8. hepta-
9. nona-
10. What are the names of the following compounds?
a. BF3
b. N2O4
c. P4S7
11. What are the formulas for the following compounds?
a. carbon tetrabromide
b. nitrogen triiodide
c. iodine monochloride
d. tetraiodine nonoxide
9.2/9.3
Homework
(GRADECAM
BOX
ON
NEXT
PAGE)
__1. What is the formula for the ionic compound C. NK2 D. K3N
formed by calcium ions and nitrate ions?
A. Ca3N2 B. Ca(NO3)2 __5. Which is the correct formula for copper(II)
C. Ca2NO3 D. Ca2NO2
phosphate?
__2. What is the formula for the ionic compound A. Cu2PO4 B. Cu3(PO4)2
formed by calcium and selenium? C. Cu2PO3 D. Cu(PO4)2
A. CaSe B. Ca2Se __6. The formula for magnesium sulfate is
C. CaSe2 D. Ca3Se A. MnS. B. MgS.
__3. What is the formula for the ionic compound C. MnSO3. D. MgSO4.
formed by magnesium and iodine? __7. The formula for sodium sulfide is
A. MgI B. Mg2I A. NaS. B. K2S.
C. MgI2 D. MgI3 C. NaS2. D. Na2S.
__4. What is the formula for the binary compound
formed by potassium and nitrogen?
A. KN B. K2N
31
__8. The correct name for NH4NO3 is __18. The name for Ga2O3 is
A. ammonium nitrate. A. gallium oxide.
B. ammonium nitrogen trioxide. B. digallium trioxide.
C. ammonia nitrogen oxide. C. gallium(VI) oxide.
D. hydrogen nitrogen oxide. D. gallium(II) trioxide.
__9. The correct name for Ba(OH)2 is __19. What is the name of PCl3?
A. barium hydrogen oxide. A. phosphorus chloride
B. boron hydroxide. B. phosphoric chloride
C. barium hydroxide. C. phosphorus trichlorate
D. beryllium hydroxide. D. phosphorus trichloride
__10. The correct name for KHCO3 is __20. The compound, P4S10, is used in the manufacture
A. calcium bicarbonate. of safety matches. What is its name?
B. potassium hydrogen carbonate. A. phosphorus sulfide
C. potassium carbonate. B. phosphoric sulfide
D. calcium hydrogen carbon trioxide. C. phosphorus decasulfide
D. tetraphosphorus decasulfide
__11. The Stock system name for Mn2O7 is __21. Diiodine pentoxide is used as an oxidizing agent
A. dimanganese heptaoxide.
B. magnesium oxide. that converts carbon monoxide to carbon dioxide. What
C. manganese(VII) oxide.
D. manganese(II) oxide. is its chemical formula?
__12. The molecular name for As2S5 is A. I2O5 B. IO5
A. arsenic(V) sulfide. C. 2IO5 D. I5O2
B. diarsenic pentasulfide.
C. arsenic(III) sulfide. __22. What is the name of P4Se3?
D. arsenic(V) sulfate. A. phosphorus selenide
B. phosphorus triselenide
C. tetraphosphorus selenide
D. tetraphosphorus triselenide
__13. Consistent with vanadium being a transition __23. Tetrasulfur dinitride decomposes explosively
metal, the name for VSO4 should be
A. vanadium sulfide. when heated. What is its formula?
B. vanadium (I) sulfite.
C. vanadium (I) sulfate. A. S2N4 B. S4N2
D. vanadium (II) sulfate. C. 4SN2 D. S4N
__14. Which is the correct formula for lead(IV) __24. The name of S4N4 is
A. sulfur nitride.
chloride? B. sulfur tetranitride.
C. tetrasulfur nitride.
A. Pb4Cl B. PbCl2 D. tetrasulfur tetranitride.
C. PbCl3 D. PbCl4
__15. The chemical formula for iron(II) nitrate is __25. The name of XeF4 is
A. xenon tetrafluoride.
A. Fe2(NO3)3. B. Ir(NO2)2. B. xenon fluoride.
C. Fe2N3. D. Fe(NO3)2. C. monoxenon tetrafluoride.
D. monoxenon fluoride.
__16. The Stock system name for CrSO3 is
A. chromium sulfide.
B. chromium(II) sulfite.
C. chromium(II) sulfate.
D. chromium(III) sulfite.
__17. The Stock system name for CrO3 is
A. chromium oxide.
B. chromium(II) oxide.
C. chromium(III) trioxide.
D. chromium(VI) oxide.
32
Chapter
9
Study
Guides
9.1:
NAMING
IONS
–
Study
guide
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms that are introduced in this
section. Each blank can be completed with a term, short phrase, or number.
Ions that consist of a single atom are called ___1____ ions. 1.
Metallic elements tend to ___2____ electrons. Group 1A ions have a 2.
3.
____3___ charge, whereas Group 2A metals form ions with a ____4___ 4.
5.
charge, and Group 3A metals form ions with a ____5___ charge. 6.
The charge of a Group A nonmetal ion is determined by 7.
8.
subtracting ____6___ from the group number. For example, the Group 9.
10.
7A elements form ions with a charge of __7_____. 11.
Many of the ____8___ have more than one common ionic charge. 12.
13.
These ions are named using either the ____9___ system or the
___1_0___ naming system.
Ions containing more than one atom are called ____1_1__ ions. The
names of most common polyatomic ions end in either ___1_2___ or
___1_3___.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
14. The names of polyatomic ions end in -ite or -ate.
15. In polyatomic ions for which there is an -ite/-ate pair, the -ite ending will always indicate one less oxygen
atom than the -ate ending.
16. Polyatomic ions are anions.
17. The charge on Group A metal ions is determined by subtracting the group number from 8.
18. The Group 6A ions have a charge of 2–.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A Column B
19. monatomic ions a. negatively charged ions
20. polyatomic ions b. ions formed from single atoms
21. cations c. a traditional way of naming transition metal cations
22. anions d. positively charged ions
23. classical naming system e. ions formed from groups of atoms
33
9.2
NAMING
AND
WRITING
FORMULAS
FOR
IONIC
COMPOUNDS
-‐
Study
Guide
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank
can be completed with a term, short phrase, or number.
Binary ionic compounds are named by writing the name of the ____1___ 1.
2.
followed by the name of the ____2___. Names of binary compounds end in 3.
4.
_____3__. For example, NaI is __4_____. 5.
6.
When a cation has more than one ionic charge, a ___5____ is used in the 7.
8.
name.
Compounds with polyatomic ions whose names end in -ite or -ate contain
6 ___7____.
a polyatomic _______ that includes In writing the formula of an ionic
compound, the net ionic charge must be ___8____.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
9. The systematic name for baking soda (NaHCO3) is sodium bicarbonate.
10. In writing a formula for an ionic compound, the net ionic charge of the formula must be zero.
11. Anions that contain oxygen end in -ite or -ate.
12. The cation name is placed first when naming ionic compounds.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A Column B
13. binary compounds a. ions that consist of a single atom
14. monatomic ions b. ionic compounds composed of two elements
15. polyatomic ions c. Group B metals, many of which have more than one common ionic charge
16. transition metals d. ions that consist of more than one atom
Part D Questions and Problems
Answer the following in the space provided.
17. Name the following compounds and tell what type of compound they are (binary ionic or ionic with a polyatomic ion).
a. FeBr3 ____________________________________________________________________________________________________________
b. KOH
c. Na2Cr2O7
18. Write the formulas for the following compounds.
a. sodium chlorate ________________________________________________________________________________________________
b. lead(II) phosphate
c. magnesium hydrogen carbonate
34
9.3
NAMING
AND
WRITING
FORMULAS
FOR
MOLECULAR
COMPOUNDS
-‐
Study
Guide
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank
can be completed with a term, short phrase, or number.
Binary molecular compounds are composed of two ___1____ elements. 1.
The name of this type of compound ends in _______. Pref2ixes are used to show 2.
how many _______ of each element are p3resent in a molecule of the 3.
compound. For example, the name of As2S5 is _______. 4.
4
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
5. Binary molecular compounds contain carbon.
6. Charges must be balanced when writing formulas for molecular compounds.
7. CO2 is named monocarbon dioxide.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A Column B
8. binary molecular compound a. used to indicate the relative number of atoms of an element in a
molecular compound
9. prefix
10. mono- b. prefix indicating one atom of an element in a molecule
11. tetra-
c. prefix indicating four atoms of an element in a molecule
d. nonionic compound containing atoms of two elements
Part D Questions and Problems
Answer the following in the space provided.
12. Name each of the following compounds.
a. PCl5
b. SO2
c. P4S10
13. Write formulas for the following compounds.
a. carbon tetrabromide
b. dinitrogen tetroxide
35
Chapter
9
Practice
Quiz
1-20. Using the example in each table, give the name when the formula is supplied or vice versa.
Ex. sodium sulfide Na2S
potassium selenide
aluminum fluoride
calcium sulfide
gallium phosphide
Ex. magnesium and oxygen MgO
lithium and phosphorus
gallium and bromine
strontium and nitrogen
rubidium and fluorine
Ex. SrSO3 strontium sulfite
CaHPO4
Mg(MnO4)2
In(ClO)3
Ex. Fe(OH)3 iron (III) hydroxide
CuCN
Bi2(S2O3)3
Au(NO3)3
Ex. P2O3 diphosphorus trioxide
SiS2
SF6
Se2Cl2
Ex. carbon dioxide CO2
nitrogen trifluoride
disulfur dichloride
tetraphosphorus triselenide
36
Ch.
15
-‐
Aqueous
Systems
Ch.
16
-‐
Solutions
15.2 – Homogeneous Aqueous Systems (p. 494-495)
Objectives
• Distinguish between a solvent and a solute
• Describe what happens in the solution process
Vocabulary • solute • solvent • solvation
• aqueous solution
16.1 – Properties of Solutions
Objective
• Identify the factors that determine the rate at which a solute dissolves
16.2 – Concentration of Solutions
Objectives
• Solve problems involving the molarity of a solution
• Define what is meant by percent by volume [%(v/v)] and percent by mass
[%(m/m)]
Vocabulary • concentrated solution • dilute solution • molarity (M)
• concentration
Key Equations
• Molarity (M ) = moles of solute
liters of solution
• Percent by volume [%(v/v)] = volume of solute × 100%
volume of solution
• Percent by mass [%(m/m)] = mass of solute × 100%
mass of solution
37
15.2
Homogeneous
Aqueous
Systems
(only
pages
494-‐495)
After reading pages 494-495, answer the following questions.
Solutions
• Solutions are __________________ mixtures.
• Solvents and solutes may be __________, liquids, or solids.
• In a solution, the ____________ medium is the solvent.
• __________ is the solvent in an aqueous solution.
• The dissolved particles in a solution are the ___________.
• The solution is named after the ____________.
• An solution is water that contains dissolved substances.
• Solute particles can be atoms, ions, or ________________.
• The solute becomes dispersed in the ______________.
• If the solute is ionic, it ________________ (splits into ions of the compound
Ex. NaCl becomes Na+ and Cl-)
• If the solute is ________________, it dissolves (individual molecules break off
from solid and float freely)
• A solvent ________________ the solute.
• If you filter a solution through filter paper, both the ________________ and
________________ pass through the filter.
Substances that dissolve most readily in
water include _________________
compounds and polar
__________________ compounds.
• ___________ solvents such as water
dissolve ionic compounds and polar
compounds.
• Nonpolar solvents such as gasoline
dissolve _____________ compounds.
This relationship can be summed up in the expression
“like dissolves like.”
Nonpolar covalent compounds, such as methane, and compounds found in oil,
___________, and gasoline, do not dissolve in water. However, oil and grease
will dissolve in _______________.
38
The Solution Process
• A water molecule is polar, with a
partial negative charge on the
___________ atom and partial positive
charges on the ______________ atoms.
• As individual solute ions break away from the
_____________, the negatively and positively charged
ions become _________________ by solvent molecules
and the ionic crystal dissolves.
• The process by which the positive and negative ions of an ionic solid become
surrounded by solvent molecules is called _______________.
39
15.2
Homework
Matching: Match the term on the right with the description on the left. Some may be used more than once, and some
may not be used at all.
__1. a solution is named after the __ a. aqueous solution
__2. breaking off of individual molecules to float freely in the solution b. dissociating
__3. dissolved particles in a solution c. dissolving
__4. dissolving medium d. nonpolar covalent
__5. homogeneous mixture e. polar covalent
__6. methane, oil, and grease dissolve in gasoline because gasoline is a __ compound ab. solute
__7. most ionic and __ compounds dissolve in water ac. solution
__8. splitting of ionic compound into ions ad. solvation
__9. the process by which the positive and negative ions of an ionic solid become surrounded by ae. solvent
solvent molecules
__10. water that contains dissolved substances bc. water
Label the water molecule and use the letters to answer the questions about the water molecule in solution.
__11. hydrogen atom
__12. oxygen atom
__13. partial negative “end”
__14. partial positive “end”
__15. Using the diagram, which “end” of multiple water molecules would surround
sodium ions in solution
__16. Using the diagram, which “end” of multiple water molecules would surround
chloride ions in solution
__17. When a solution of Pb(NO3)2 and KI are mixed, the yellow precipitate formed was __ and the compound that
stayed in solution was __.
a. PbI2/KNO3 b. KNO3/PbI2 c. Pb(NO3)2/KI d. KI/Pb(NO3)2
__18. Decompression sickness is commonly called the __ and to avoid this, scuba divers must come up from deep water
__.
a. bubbles/quickly b. bends/slowly c. bubbles/slowly d. bends/quickly
__19. The greenhouse gas (when dissolved in sea water) that can effect oyster shell growth is __.
a. O2 b. H2O c. CO2 d. all of the above
__20. The total dissolved solids in hot brew coffee was __ than that of cold brew coffee.
a. higher b. lower c. the same as d. colder
40
16.1
Properties
of
Solutions
After reading Lesson 16.1, answer the following questions.
Solution Formation
Granulated sugar dissolves _________ than sugar cubes (a), and both granulated sugar
and sugar cubes dissolve faster when you _______ the tea (b) or in ______ tea (c).
Figure 16.1
Temperature (a) - Temperature influences the ________ at which a solute
dissolves.
• Sugar dissolves much more rapidly in _____ tea than in iced tea.
• At higher temperatures, the _______________ energy of water molecules is
greater, so the molecules move ______________.
• The more rapid motion of the solvent molecules leads to an ____________ in the
frequency of the force of the collisions between water molecules and the
________________ of the sugar crystals.
Agitation (b) - If the contents of the glass are _________, the crystals dissolve
more quickly.
• The dissolving process occurs at the ______________ of the sugar crystals.
• Stirring speeds up the process because fresh solvent (the ____________) is
continually brought in contact with the surface of the _______________ (sugar).
Agitation (stirring or ________________) affects only the rate at which a solid solute
dissolves.
• It does not influence the ______________ of solute that will dissolve.
• An _________________ substance remains undissolved regardless of how
vigorously or for how long the solvent/solute system is agitated. Ex. CaCO3 will
not dissolve in water.
41
Particle size of solute (c) - The rate at which a solute dissolves also depends
upon the size of the solute particles.
• The smaller particles in granulated sugar expose a much greater ___________ area
to the colliding water molecules.
• The more surface area of the solute that is exposed, the _________ the rate of
dissolving.
16.2
Concentrations
of
Solutions
After reading Lesson 16.2, answer the following questions.
Molarity
The of a solution is a measure of the amount of solute
dissolved in a given quantity of solvent.
• A solution that contains a relatively small amount of solute is a
solution.
•A solution contains a large amount of solute.
In chemistry, the most important unit of concentration is molarity.
• (M) is the number of moles of solute dissolved in one liter of
solution.
• Molarity is also known as ____________ concentration.
To calculate the molarity of a solution, divide the number of moles of solute by the
volume of the solution in liters.
Molarity (M) = moles of solute
liters of solution
The figure below illustrates the procedure for making a 0.5M, or 0.5-molar, solution.
Add 0.5 mol of solute to a Swirl the flask carefully to Fill the flask with water
1-L __________ flask half dissolve the __________. ____________ to the 1-L
filled with distilled water. mark.
42
Percent Solutions
Percent by volume of a solution is the ratio of the volume of solute to the volume of
solution.
• Isopropyl alcohol (2-propanol) is sold as a ____% solution by volume.
• You could prepare such a solution by diluting 91 mL of __________ isopropyl
alcohol with enough water to make _______ mL of solution.
• The concentration is 91 percent by volume, 91 percent (volume/volume), or 91%
(v/v).
volume of solute
Percent by volume (%(v/v)) = volume of solution × 100%
Calculating Percent by Volume
What is the percent by volume of ethanol (C2H6O, or ethyl alcohol) in the final
solution when 85 mL of ethanol is diluted to a volume of 250 mL with water?
1 – Analyze: List the knowns and the unknown.
Use the known values for the volume of solute and volume of solution to calculate
percent by volume.
KNOWNS volume of solution = ____ mL
volume of solute = ____ mL ethanol
UNKNOWN
Percent by volume = ?% ethanol (v/v)
2 – Calculate: Solve for the unknown.
State the equation for percent by volume.
Percent by volume [%(v/v)] = volume of solute × 100%
volume of solution
Substitute the known values into the equation and solve.
Percent by volume [%(v/v)] = __mL ethanol × 100%
___ mL solution
= __ % ethanol (v/v)
Another way to express the concentration of a solution is as a percent by mass, or
percent (mass/mass). mass of solute
Percent by mass of a solution is the ________ Percent by mass (%(m/m)) = mass of solution × 100%
of the mass of the solute to the mass of the
solution.
43
16.1/16.2
Homework
(I
will
grade
#s
12/13
before
you
scan
your
homework)
1-5: Matching: Match the term on the right with the description on the left.
__1. The number of moles of solute a. concentrated
dissolved in one liter of solution b. concentration
__2. A substance that remains
undissolved regardless of how c. dilute
vigorously or for how long the d. insoluble
solvent/solute system is agitated e. molarity
__3. A solution that contains a
relatively small amount of solute
__4. A solution that contains a
relatively large amount of solute
__5. A measure of the amount of
solute dissolved in a given quantity of
solvent.
__6. Increasing the temperature of a liquid–solid solution will:
a. often decrease the amount of crystalline solute that dissolves.
b. always increase the rate at which a crystalline solute dissolves.
c. both a and b d. neither a nor b
__7. Which of the following operations usually makes a substance dissolve faster in a solvent?
a. agitation b. raising the temperature c. crushing the substance to a powder d. all of the above
__8. Sugar dissolves __ rapidly in __ tea due to increased kinetic energy.
a. more/cold b. less/cold c. more/hot d. less/hot
__9. Stirring speeds up the process of dissolving because fresh solvent (__) is continually brought in contact with the
surface of the solute (__).
a. water/water b. sugar/sugar c. water/sugar d. sugar/water
__10. Agitation is __ and __ the rate of solid solute dissolving.
a. raising temperature/decreases b. raising temperature/increases
c. shaking or stirring/increases d. shaking or stirring/decreases
__11. __ particles in granulated sugar exposes a much __ surface area to collide with water molecules, therefore it will
form a solution at a faster rate.
a. smaller/greater b. larger/lesser c. larger/greater d. smaller/lesser
12. What is the molarity of a 0.400-L solution in which 0.200 mole of sodium bromide is dissolved?
(YOU MUST SHOW YOUR WORK – worth two answers)
a. 0.400 M b. 0.200 M c. 0.500 M d. 2.00 M
13. What is the % (m/m) of a solution that contains 60 g of calcium chloride and the solution has a mass of 400 g?
(YOU MUST SHOW YOUR WORK – worth two answers)
a. 6% b. 40% c. 6.7% d. 15%
44
Chapters
15
and
16
Review
15.1 Review - Complete the following in the space provided.
1. Distinguish between a solution in general and an aqueous solution.
2. In the formation of a solution, how does the solvent differ from the solute?
3. Identify the solvent and solute in a sugar solution.
4. Suppose an aqueous solution contains both table sugar and table salt. Can you separate either of
the solutes from the water by filtration. Explain your reasoning.
5. Describe the process of solvation using NaCl as the solute. Explain both ions in your explanation.
6. Why is water an excellent solvent for most ionic and polar covalent compounds but not for
nonpolar compounds?
7. Explain why gasoline does not dissolve in water?
8. Which of the following substances dissolve well in water? Give reasons for your choices.
a. methane d. grease
b. K2SO4 e. oil
c. NaI f. CaCO3
45
Chapter 16 (16.1/16.2) Review - Complete the following in the space provided.
1. Name and distinguish between the two components of a solution.
2. Explain why the dissolved component does not settle out of a solution.
3. Knowing the molarity of a solution is more meaningful than knowing whether a solution is dilute
or concentrated. Define each and explain why this is so.
4. Calculate the molarity of each solution. Show your work. Also, name the solution.
a. 1.0 mol KCl 0.750 L of solution
b. 0.50 mol MgCl2 in 1.5 L of solution.
c. 0.517 L of a solution containing 0.0044 mol of Ca(NO3)2.
5. What is the percent by mass of sodium chloride in the following solutions (you must add the
solute and solvent to get the total mass of the solution). Show your work.
a. 44 g NaCl in 756 g H2O
b. 15 g NaCl in 485 g H2O
c. 135 g NaCl in 765 g H2O
c. 333 g NaCl in 667 g H2O
46
Chapter
16
Study
Guides
16.1:
PROPERTIES
OF
SOLUTIONS
–
Study
guide
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms that are introduced in this
section. Each blank can be completed with a term, short phrase, or number.
Changes in the temperature of a system and ___1____ of a solute 1.
2.
alter the __2_____ at which a solute dissolves. The extent to which a gas 3.
dissolves in a liquid is proportional to the ____3___ of the gas in 4.
5.
accordance with ___4____ law. The solubility of a gas decreases with 6.
increasing ____5___. A solution that contains the maximum amount of 7.
solute at a given temperature is said to be ___6____. Two liquids that 8.
are mutually soluble in each other are said to be ___7____. Generally the 9.
____8___ of a solid in water ___9____ with increasing temperature, but 10.
there are exceptions. A(n) ____1_0__ solution holds more solute than is
theoretically possible.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
11. The rate at which a solute dissolves can be increased by grinding.
12. As the temperature of a solvent decreases, the solubility of a solute increases.
13. Stirring a solute when adding it to a solvent should increase the rate of its dissolving.
14. Henry’s law states that the solubility of a gas in a liquid is a function of temperature.
15. Two liquids that dissolve in each other are miscible.
Part C Matching
Match each description in Column B to the correct term in Column A. NOT ALL CHOICES WILL BE USED.
Column A Column B
16. saturated solution a. the amount of a substance that dissolves in a given quantity of solvent
17. solubility at a given temperature
18. unsaturated solution
19. miscible b. The solubility of a gas in a liquid is directly proportional to the
20. immiscible pressure of the gas above the liquid.
21. supersaturated solution
c. solution that contains the maximum amount of solute for a given
amount of solvent at a constant temperature
d. a solution containing more solute than it can theoretically hold at a
given temperature
e. description of two liquids that dissolve in each other
f. a solution that contains less solute than possible at a given temperature
g. description of two liquids that do not dissolve in each other
47
16.2:
CONCENTRATIONS
OF
SOLUTIONS
–
Study
guide
Part A Completion
Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank
can be completed with a term, short phrase, or number.
The relative amounts of solute and ___1____ in a ____2___ can 1.
be described qualitatively as ____3___ or concentrated. Quantitative 2.
units of concentration include molar concentration, percent by 3.
volume, and percent by mass. 4.
5.
Molarity, the most important unit of concentration in 6.
chemistry, is expressed as ____4___ of solute per ____5___ of 7.
solution. 8.
Solutions of different concentrations can be prepared by
___6____ a stock solution. In dilution, the moles of ____7___ remain
the same, while the amount of ___8____ changes.
Part B True-False
Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT.
9. One hundred mL of 1.0M sodium hydroxide solution is more concentrated than 1.0 L of 5M sodium
hydroxide solution.
10. The amount of sodium hydroxide in 100 mL of 1.0M NaOH is less than that in 1.0 L of 5M NaOH
solution.
11. Fifty mL of a 32% solution (v/v) of ethyl alcohol in water would contain 42 mL of water.
12. A dilute solution is a quantitative expression of concentration.
Part C Matching
Match each description in Column B to the correct term in Column A.
Column A Column B
13. concentration a. number of moles of solute dissolved in 1 L of solution
14. dilute solution b. measure of the amount of solute that is dissolved in a given
15. concentrated solution
16. molarity quantity of solvent
c. solution that contains a low concentration of solute
17. percent solution d. concentration expressed as volume of solute over volume of
solution × 100%
e. solution that contains a high concentration of solute
48
Chapter
15/16
Practice
Quiz
Matching: Match the term on the right with the description on the left. Some may be used more than once and some may note be used
at all.
__1. __ solvents dissolve ionic compounds A. aqueous solution
__2. __ solvents dissolve nonpolar compounds B. dissociates
__3. a molecular solute __ in the solvent C. dissolves
__4. an ionic solute __ in the solvent (splits into the ions of the compound) D. negative
__5. the dissolved particles in a solution E. nonpolar
__6. the dissolving medium in a solution AB. polar
__7. the hydrogen atoms in water have a partial __ charge AC. positive
__8. the oxygen atom in water has a partial __ charge AD. solute
__9. the process where the ions of an ionic solid become surrounded by solvent particles is called __. AE. solvation
__10. water that contains dissolved substances BC. solvent
__11. a measure of the amount of solute dissolved in a given quantity of solvent A. percent by mass
__12. a solution with a large amount of solute is a(n) __ solution B. percent by volume
__13. a solution with a relatively small amount of solute is a(n) __ solution C. concentrated
__14. a substance that remains undissolved in the solvent is a(n) __ substance D. concentration
__15. ratio of the mass of solute to the mass of the solution E. dilute
__16. ratio of the volume of solute to the volume of solution AB. insoluble
__17. the number of moles of solute in a liter of solution AC. molarity
Multiple Choice: Choose the answer that best completes the statement.
__18. Solute particles can be __. __22. Stirring speeds up the process of dissolving sugar
A. atoms
C. ions B. molecules because fresh __ is brought in contact with the surface of the
D. all of the above
sugar.
A. solute B. solvent
__19. In a solution, the __ is dispersed in the __. C. solution D. none of the above
A. solute/solution B. solvent/solute
C. solute/solvent D. solution/solvent __23. Agitation speeds up the rate in which a solid solute
dissolves, but __.
__20. If you filter a solution, the __ will pass through the filter. A. it does not influence the amount of solute that will dissolve
B. it will cause the solute to become insoluble
A. solute and solvent B. solvent C. it will cause the water to become nonpolar
D. none of the above
C. solute D. none of the above
__21. Sugar dissolves faster in __ tea than in __ tea.
A. iced/hot B. hot/iced __24. Methane, oil, and grease are nonpolar and will readily
C. both A and B D. neither A nor B dissolve in __.
A. water B. gasoline
C. both A and B D. neither A nor B
Problems: Show all work and circle your final answer.
25. If a solution contains 5.0 moles of solute in 2.5 L of solution, what is the molarity of the solution?
26. If a solution contains 40 mL of solute and a total volume of 90 mL of solution, what is the % v/v?
49
Chemical
and
Physical
Changes
Lab
Introduction:
There are two kinds of changes matter can go through, physical and chemical changes. In a physical change, the
matter only changes its appearance. Examples of physical changes are melting, freezing, dissolving, grinding, or
evaporation, just to name a few. In a chemical change, one or more “new” substances are formed. The substances formed
by a chemical change will have different properties than the original substances. Burning and rusting are examples of
chemical changes.
Materials for Part A: magnesium (Mg) lighter
hydrochloric acid (HCl) table salt (NaCl)
Water (H2O) test tubes with screw caps silver nitrate sol’n (AgNO3)
candle
scoop
Procedure for Part A:
1. Light a candle. Allow the candle to burn for the remainder of time you are at this
station. Record your observations for the burning candle in the space provided in the
observations section.
2. Add a very small scoop of NaCl (just enough to cover the tip of the scoop) to a test tube
that has been half filled with tap water. Put the screw cap on the test tube and shake to
dissolve the salt. Record your observations. Using the dropper bottle of AgNO3, add 5
drops to the salt water. Record your observations.
3. Place one small piece of magnesium in a test tube. Add 5 drops of HCl to the test tube.
Record your observations. DO NOT put the screw cap on the test tube. Touch the
bottom of the test tube with your fingertips. Record your observations.
Materials for Part B: sodium chloride (NaCl) beaker
Water (H2O) sand (SiO2) stirring rod
iron (Fe) citric acid (C6H8O7) copper (II) chloride (CuCl2)
sulfur (S) sodium bicarbonate (NaHCO3) aluminum foil (Al)
pennies
scoop
vinegar (CH3COOH)
filter paper
petri dish
Procedure for Part B: (each step is separate and you must clean up between steps)
1. Place a small sample of iron and a small sample of sulfur on a petri dish. Mix the two thoroughly together. Record
your observations in the observation section. Place the cover on the petri dish. Move a magnet under the covered
dish, below the mixture. Record your observations.
2. Place a small sample of sand and salt onto another piece of filter paper. Mix the two together, and record your
observations. Place the mixture into a test tube that has been half filled with water. Put the screw cap on the test
tube and shake the test tube. Record your observations.
3. Place a small sample of citric acid and sodium bicarbonate onto another piece of filter paper. Mix the two together,
and record your observations. Place the mixture into a beaker that has been half filled with water (do this over a
sink). Record your observations.
50
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