CHAPTER 1 : MATTER

CHAPTER 1: MATTER C1 C2 C3 C4
√
1.1 DEFINITION AND CLASSIFICATION
√
Learning outcomes
(a) Define matter
(b) Classify matter into pure substances (elements and compounds)

and mixture (homogeneous and heterogeneous)

MATTER
 Definition: Matter is anything that has mass and takes up space.
 Example: air, earth, animals, trees, atoms
 The three states of matter are solid, liquid and gas
 Chemistry is the study of the properties of matter and how matter changes.

CLASSIFICATION OF MATTER

Matter

Mixtures Separation by physical method Pure Substances

Homogeneous Heterogeneous Compounds Separation Element
Mixtures Mixtures by chemical

method

 All matter can be classified based on its composition. It is either a MIXTURES or a PURE
SUBSTANCE.

1

MIXTURES
 Definition: A mixture is a combination of two or more kinds of matter each of which retains its

own composition and properties.

Mixture

Homogeneous Mixture Heterogeneous Mixture

Characteristics Of A Mixture :

1. Mixtures can be either heterogeneous or homogeneous.

2. The different types of matter which make up the mixture can be separated by physical changes.

3. The separated matter has basically the same characteristic properties and identities as found in
the mixture. The properties of a mixture therefore, are a combination of the properties of the
different kinds of matter it contains.

4. The composition of a mixture can contain varying amounts of different kinds of matter, within
the same sample or from one sample of the mixture to another. This shows that mixtures have
variable composition.

Homogeneous mixtures Heterogeneous mixtures
Heterogeneous or non-uniform mixtures are
 Homogeneous or uniform mixtures are ones in  those in which the composition varies
which the composition is same throughout. throughout and can be easily separated into
individual substances.
 Another name for homogeneous is a solution, For example, mixing sand with iron fillings.
which is made up of a solvent, usually taken to be
the substances present in larger amount, and one  Mixture of iron fillings and sand
or more solutes.

 Most commonly, the solvent is a liquid, whereas
solute may be solids, liquids or gases. For instance,
dissolving a spoonful of sugar in water.

Example of homogeneous mixture (a) (b)

(a) Illustration of uniform distribution of components

in homogeneous mixture
(b) Uniform distribution of components in

heterogeneous mixture

2

PURE SUBSTANCES
 Definition: A pure substance is a homogeneous sample of matter that always has the same
composition and properties, regardless of its source. Substances can only be homogeneous and
have constant composition. They are classified as either compounds or elements
 A compound is a homogeneous substance made up of two or more elements chemically
combined.

Characteristics of Compound :
1. Elements in a compound are combined in a definite proportion (ratio) by mass. This
proportion is the same in all samples of the compound—constant composition.
2. The chemical and physical properties of a compound are different from the individual
components which form the compound.
3. Compounds can be formed or decomposed by chemical changes. When decomposed, some
breakdown into elements, others into elements and simpler compounds. For instance, molten
sodium chloride can be broken down into metallic sodium and chlorine gas through
electrolysis

Figure: Different properties of sodium metal and chlorine gas in comparison with sodium chloride
compound formed when combining sodium metal and chlorine gas together chemically.

3

ELEMENT

 Definition: An element is a pure substance that cannot be broken down into any other
substance by chemical or physical means.

 Elements are the simplest substances. Each element can be identified by its specific physical
and chemical properties.

 Particles of Elements - An atom is the basic particle from which all elements are made. All
matter is composed of some combination of elements

 When Atoms Combine - When atoms combine, they form a chemical bond, which is a force of
attraction between two atoms. In many cases, atoms combine to form larger particles called
molecules-groups of two or more atoms held together by chemical bonds.

 Examples of elements: gold, oxygen, copper

(a) (b)
Figure: (a) Illustration of composition of gold atoms in gold coin.

(b) Illustration of oxygen molecules.

4

EXAMPLES:

Classify each of the materials below. In the center column, state whether the material is a pure
substance or a mixture. If the material is a pure substance, further classify it as either an element or
compound in the right column. Similarly, if the material is a mixture, further classify it as
homogeneous or heterogeneous in the right column.

Material Pure Substance Element, Compound,
or Mixture Homogeneous, Heterogeneous
concrete Mixture
sugar + pure water Mixture Heterogeneous
(C12H22O11 + H2O)
Pure Substance Homogeneous
iron filings (Fe) Pure Substance
Element
limestone (CaCO3) Mixture Compound
Mixture Heterogeneous
orange juice (w/pulp) Mixture Heterogeneous
Pure Substance Homogeneous
Pacific Ocean Pure Substance
Pure Substance Element
air inside a balloon Mixture Element
Mixture Compound
aluminum (Al) Pure Substance Homogeneous
Pure Substance Heterogeneous
magnesium (Mg) Mixture Compound,
Mixture Element,
acetylene (C2H2) Pure Substance Heterogeneous
Mixture
tap water in a glass Mixture Homogeneous
Pure Substance
soil Compound
5 Heterogeneous
pure water (H2O)
Homogeneous
chromium (Cr)
Compound
Chex mix
salt + pure water

(NaCl + H2O)
benzene (C6H6)

Muddy water
brass

(Cu mixed with Zn)
baking soda (NaHCO3)

EXERCISES :

1. Classify each of the following as either substance or mixture. If it is a substance, write element
or compound in the appropriate column. If it is a mixture, write heterogeneous or
homogeneous in the appropriate column.

Type of matter Substance Mixture
Chlorine (Cl2)
Water (H2O)
Lucky Charms
Salt water
Nitrogen (N2)
Salt (NaCl)
Rocky road ice cream
Rubbing Alcohol
Pure air
Iron (Fe)
bronze
Spaghetti and meatballs

2. Compare and contrast a mixture and a compound. How are they alike? How are they
different?

6

3. State a difference between a compound and a solution.

4. Label each substance listed below as an element (E), compound (C), heterogeneous mixture
(He), or homogeneous mixture (Ho)
a. _______ Barium (Ba)
b. _______ Carbon Monoxide (CO)
c. _______ Soil
d. _______ Kool-Aid
e. _______ Brass (CuZn)
f. ________ Air
g. _______ Vegetable soup
h. _______ Carbon (C)
i. _______ Baking Soda (NaHCO3)
j. _______ Jello with fruit
k. _______ Gold (Ag)
l. _______ Milk
m. _______ Sand
n. _______ Orange juice w/o pulp
o. _______ Orange juice w/pulp

7

1.2 STATES OF MATTER C1 C2 C3 C4
√√
Learning outcomes

(a) Explain the general properties of solid, liquid and gas in terms of
arrangement of particles, shape, density and compressibility.

MATTER

 In facts, all matter that exist naturally on earth can be classified as one of these physical forms,
which are called states of matter.

 Matter can exist in three physical forms/states: solid, liquid and gas.
 So, each of the three common states of matter can be distinguished by the way it fills it

container.

Matter exists in 3 Physical State

Solid Liquid Gas

SOLID
 A solid is a form of matter that has its own definite/fixed shape and volume.
 Because its shape is definite, a solid might not conform to the shape of the container in which it is
placed. If you place a rock in a container, the rock will not take the shape of the containers.
 Examples: Wood, iron, paper and sugar
 The particles of matter in a solid are tightly packed or are held closely together in orderly manner and
at fixed positions with little freedom of motion (particles vibrate about fixed positions)

 The tight packing of particles in solid makes it incompressible, that is it cannot be pressed into a smaller
volume.

 Incompressible materials will maintain their density. So solid particles have a high density.

8

LIQUID
 A liquid is a form of matter that has a constant/definite volume and takes the shape of
container. Common examples of liquids include water, blood and mercury.
 Particles in a liquid are close together but are not held so rigidly in position and can move past
one another or slide past one another freely. This property allows liquid to flow and take the
shape of containers.

 Because of the way the particles of a liquid are packed, liquid is virtually incompressible or can
be compressed slightly.

 Liquid has a high density because the particles in liquid are free and can move around, but the
density of liquid less dense than solid.

GAS
 A gas is a form of matter that not only flows to conform to the shape of its container but also
fills the entire volume of its container. Thus, gas does not have fixed shape and volume.
 In a gas, the particles are far apart and move in random motion. Because of the significant
amount of space between particles of gases are easily compressed.

 Gases have lower density than other states of matter, such as solids and liquids

9

COMPARISON BETWEEN SOLID, LIQUID AND GAS

PROPERTIES OF MATTER SOLID LIQUID GAS

Arrangement of particles Closely packed in Closely packed in an Far apart in random
arrangement
an orderly disorderly

arrangement arrangement

Shape Fixed Not Fixed Not Fixed
Density Very Dense Least Dense
Compressibility Dense Compressible
Not Compressible
Not
Compressible

EXERCISES :
1. a) Each particles of argon can be represented by a circle. Draw the particles to show solid

argon, liquid argon and argon gas in the box below.

Solid Liquid Gas

b) i. If the particles a move around quickly in any direction within the container, the argon

is __________________

ii. If the particles are very close together in definite pattern and can only vibrate in

position, the argon is ________________

iii. If the particles are close together but not always touching and can move in any

direction, the argon is __________________

2. There are three states of matter: solid, liquid and gas.
a) Give one property that liquids and gases have in common.

b) Give one property in which liquids and gases differ.

10

3. Complete the table below

Solid Liquid Gas

Does it have its own
shape?

Does it have a
definite volume?

How are the
particles arranged?
How are the density

of particles ?
Does it can be
compressed?

11