Chemistry CPA Unit 2 Test Study Guide
Test Date: Wednesday, November 6, 2013
Unit 2 Materials – make sure you have the materials below completed and that you
refer to them while you study:

Do-Nows and Exit Passes (questions and answers on the website)

Unit 2 notes – blue packet

Unit 2 worksheet packet – purple packet

Study Guide - Assignment 7 of purple packet (pp. 29-30)

Textbook – Chapter 2

Labs – Atomic Target Practice, “Candium”, Flame Tests
Topics:

Atomic Theory – Know the scientists and their theories and atomic models

Atomic Structure – Know the properties and location of protons, neutrons, and
electrons within an atom

Know that the atomic number identifies an atom and is also the same as the
number of protons

Isotopes and Ions – Know how and why they form

Know the difference between the mass number and the average atomic mass

Be able to calculate the average atomic mass given the mass numbers and
percent abundance of multiple isotopes

Electron Energy and the Electromagnetic Spectrumo Know the connection between electron energy and light
o Know the Electromagnetic Spectrum and be able to correctly label each
region, including where the energy, frequency, and wavelength is the
greatest and the least
Unit 2 Study Guide p. 1
Callahan, Pengitore & Ricafort – Fall 2013
Practice – Answer the following questions. Do not use this as your only study
guide. You must be reviewing your notes, the work you have done, and the labs you
have performed in this unit.
1. Atomic Theory
Fill in the Graphic Organizer below. Put the scientists into chronological order, starting
with the earliest scientist:
Scientist and Year
Experiment
Theory
Model (Draw or
Sketch)
Unit 2 Study Guide p. 2
Callahan, Pengitore & Ricafort – Fall 2013
Unit 2 Study Guide p. 3
Callahan, Pengitore & Ricafort – Fall 2013
Atomic Structure
2. Define atomic number:
3. Define mass number:
4. Define average atomic mass:
5. Fill in the chart below:
Particle
Charge
Location in
Relative Mass
atom
Role in an
atom
6. Fill in the chart below:
Element
Element Atomic # #
name
Symbol
Mass #
Neutrons
Tellurium
Isotope
Hyphen
Notation
Notation
128
N
7
28
31
Potassium-39
F
19
7. When atoms differ by protons they are called:
8. When atoms differ by neutrons they are called:
9. When atoms differ by electrons they are called:
Unit 2 Study Guide p. 4
Callahan, Pengitore & Ricafort – Fall 2013
Electrons – Bohr and Lewis Dot Structures
10. Draw both the Bohr Model and Lewis Dot Diagram for the following elements
below. Assume they are all neutral (equal number of protons and electrons):
Element and Placement
Bohr
Lewis
of electrons
Argon
Level 1:___
Level 2:___
Level 3:___
Silicon
Level 1:___
Level 2:___
Level 3:___
Boron
Level 1:___
Level 2:___
Level 3:___
Calcium
Level 1:___
Level 2:___
Level 3:___
Magnesium
Level 1:___
Level 2:___
Level 3:___
Unit 2 Study Guide p. 5
Callahan, Pengitore & Ricafort – Fall 2013
Ions
11. Fill in the chart below:
Ion
Atomic Number
Number of Protons
Number of Electrons
Ca+2
Ni+3
Br-1
Li+1
O-2
Ba+2
B+3
N-3
12. Write the chemical symbol (like above) for the ion with 12 protons and 10 electrons.
13. Write the chemical symbol for the ion with 53 protons and 54 electrons.
14. Write the chemical symbol for the ion with 88 protons and 86 electrons.
15. Write the chemical symbol for the ion with 15 protons and 18 electrons.
16. How many protons, neutrons, and electrons are present in the 59Ni+2 ion?
28
17. How many protons, neutrons, and electrons are present in the 91Zr+4 ion?
40
18. How many protons, neutrons, and electrons are present in the 79Se-2 ion?
34
Unit 2 Study Guide p. 6
Callahan, Pengitore & Ricafort – Fall 2013
19. How many protons, neutrons, and electrons are present in the 13C-4 ion?
6
20. Write the complete chemical symbol (like in the problems above) for the ion with 84
protons, 125 neutrons, and 80 electrons.
21. Write the complete chemical symbol for the ion with 27 protons, 32 neutrons, and
25 electrons.
22. Write the complete chemical symbol for the ion with 73 protons, 108 neutrons, and
68 electrons.
23. Write the complete chemical symbol for the ion with 31 protons, 39 neutrons, and
28 electrons.
Unit 2 Study Guide p. 7
Callahan, Pengitore & Ricafort – Fall 2013
Atomic Number, Isotopes, and Ions
Identify the following sets of numbers as either different elements, isotopes, and/or ions:
24.
25.
26.
27.
28.
Atomic number: 9
Neutrons: 10
Electrons: 9
Atomic number: 9
Neutrons: 10
Electrons: 10
Atomic number: 31
Neutrons: 39
Electrons: 31
Atomic number: 31
Neutrons: 31
Electrons: 31
Atomic number: 6
Neutrons: 6
Electrons: 6
Atomic number: 7
Neutrons: 6
Electrons: 7
Atomic number: 30
Neutrons: 35
Electrons: 30
Atomic number: 30
Neutrons: 35
Electrons: 28
Atomic number: 8
Neutrons: 8
Electrons: 8
Atomic number: 8
Neutrons: 10
Electrons: 8
Unit 2 Study Guide p. 8
Callahan, Pengitore & Ricafort – Fall 2013
The Electromagnetic Spectrum
29. Which wave has the:
highest energy?
lowest energy?
30. Which wave has the:
highest frequency?
lowest frequency?
31. Which wave has the:
longest wavelength?
shortest wavelength?
32. Describe the three main properties of photons.
33. What change occurs within atoms when it emits light?
34. How does the modern electron cloud model of the atom differ from Bohr’s original
planetary model of the atom?
Unit 2 Study Guide p. 9
Callahan, Pengitore & Ricafort – Fall 2013
Average Atomic Mass
35. Argon has three naturally occurring isotopes: argon-36, argon-38, and argon-40.
Based on argon’s reported atomic mass, which isotope do you think is the most
abundant in nature? Explain.
36. Copper is made of two isotopes. Copper-63 is 96.17% abundant and Copper-65 is
30.83% abundant. What is the average atomic mass of these two isotopes?
37. Gallium has two naturally occurring isotopes. Gallium-69 is 60.108% abundant and
gallium-71 is 39.892% abundant. What is the average atomic mass of these two
isotopes?
38. Calculate the average atomic mass of lead. The four lead isotopes with their
percent abundances are: lead-204, 1.4% abundant; lead-206, 24.1% abundant, lead207, 22.1% abundant; and lead-208, 52.4% abundant.
Unit 2 Study Guide p. 10
Callahan, Pengitore & Ricafort – Fall 2013