unit review

Unit Test Setup

The test is the first unit test:
20 matching on the vocabulary (7 from ch. 4, 7 from ch. 5, and 6 from ch. 6)
20 multiple choice on the objectives (6 from ch. 4, 7 from ch. 5, and 7 from ch. 6)

Short Answers (Complete any two).
List the number protons, neutrons, and electrons in the following isotopes: Zn-65 and Ar-38.
Identify the elements described below. Use the atomic symbol to answer:

Configuration = 1s22s22p63s23p4
Contains a full second energy level
Contains only two electrons in its fifth energy level
Contains seven electrons in its fourth energy level
Contains three unpaired electrons in its third energy level

Arrange the following elements in order of increasing atomic size: Li, C, K, F, Cs
Give the group numbers of each of the following families: alkaline earth metals, halogens, noble gases. and alkali metals.
Name the rule and two principles used to do an energy level diagram.
Essays (Complete any two).
Explain how the isotopes of one element are alike and how they are different. Give two examples of each.
Distinguish between the Bohr model and the quantum mechanical model of an atom in terms of the positions of the
electrons in an atom.
Explain why elements with high first ionization energies typically also have high electronegativity values.
Explain the shielding effect and effective nuclear charge.
Positive ions are smaller than the atoms from which they are formed, but negative ions are larger than the atoms from
which they are formed. Explain why this is so.



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Unit Review Materials

Chapter 4 vocabulary Review

Match the correct vocabulary term to each numbered statement. Write the letter of the correct term on the line.

Column A Column B

1. defined as 1 the mass of a carbon-12 atom a. isotopes
12 b. neutrons

2. central core of an atom, which contains most of
the atom’s mass

3. a vertical column of elements in the periodic c. atom
table d. electrons
e. atomic number
4. subatomic particles with no charge

5. positively charged subatomic particles

6. the smallest particle of an element that retains its f. atomic mass unit
identity in a chemical reaction

7. the number of protons in the nucleus of an g. group
element

8. negatively charged subatomic particles h. nucleus

9. atoms with the same number of protons but i. periodic table
different numbers of neutrons

10. an arrangement of elements according to j. protons
similarities in their properties

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Chapter 5 vocabulary Review

Choose the term from the following list that best matches each description.

quantum Hund’s rule
photons atomic emission spectrum
hertz photoelectrons
Pauli exclusion principle Aufbau principle
wavelength quantum mechanical model

1. The lowest-energy arrangement of electrons in a subshell is obtained by putting electrons into separate orbitals of the subshell
before pairing electrons.

2. packets/quanta of electromagnetic energy

3. the SI unit of frequency

4. An atomic orbital can hold no more than two electrons.

5. the amount of energy required to move an electron from its present energy level to the next higher one

6. the modern description of the location and energy of electrons in an atom

7. This principle states that electrons enter orbitals of lowest energy first.

8. the distance between two adjacent crests of an electromagnetic wave

9. This is produced by passing the light emitted by an element through a prism.

10. These are sometimes produced when light shines on metals.

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Chapter 6 vocabulary review

Match the correct vocabulary term to each numbered statement. Write the letter of the correct term on the line.

Column A Column B

1. The highest occupied s and p sublevels a. representative elements
are partially filled.

2. The highest occupied s sublevel and a b. electronegativity
nearby d sublevel contain electrons.

3. metals having only 2 electrons in the c. atomic radius
highest occupied energy level

4. one half the distance between the d. metals
nuclei of two atoms of the same element

when the atoms are joined

5. decreases for cations and anions from e. ionization energy
left to right across a period

6. measures the ability of an atom to f. cation
attract electrons when the atom is in a g. noble gases
compound h. alkali metals
i. inner transition metals
7. an atom or group of atoms that has a j. nonmetals
positive or negative charge

8. elements in which the highest occupied
s and p sublevels are filled

9. nonmetals of Group 7A

10. The highest occupied s sublevel and a
nearby f sublevel contain electrons.

11. energy required to remove an electron k. ionic radius
from an atom

12. positively charged ion l. ion
m. Group 2A
13. Group 1A elements n. transition metal
o. halogens
14. good conductors of heat and electric p. anion
current

15. negatively charged ion

16. poor conductors of heat and electric
current

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Unit Review – Chapters 4, 5, and 6
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