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Name_________________________________________Period__________Pre-AP Chemistry
TURN IN BEFORE YOU TAKE YOUR CBA FOR EXTRA CREDIT
CBA #1 REVIEW
STATES OF MATTER
Draw conceptual drawings of 16 circles representing particles in the solid, liquid and gaseous states. List
four properties of each of these states. (page 9)
Solid
Liquid
Gas
INTENSIVE AND EXTENSIVE PROPERTIES
Define - Use your own words to define the following terms. (page 14, see CBA resouces)
Intensive Properties –
Extensive Properties-
Classification - Describe each of the following properties and either intensive (I) or extensive (E).
1. Mass ______
2. Density _______
3. Length _________
4. Color ______
5. Reactivity ______
6. Volume ________
7. Malleability _______
8. Luster _______
9. Weight ________
SIGNIFICANT FIGURES
Round the number at left to the number of significant figures stated in each column. ( pages 41-45)
Number
84.631
0.94500
7.95310
2,058,268
Four significant
figures
Three significant
figures
Two significant
figures
One significant
figure
ISOTOPES

Isotopes - atoms of the same element (having the same number of protons) with different
numbers of neutrons. (page 20-22)
Atomic Mass
Identify the following for the isotope
Atomic Number
Atomic Number:___
Protons: _____
Neutrons: ______
Electrons: ______
13
6C
Mass Number: ______
Calculate the average atomic mass of the following
isotope: carbon-12 which exists 98.93% of the time in
nature and carbon -13 which exists 1.07% of the time.
A = atomic number =
P = protons =
E = electrons
M = Mass number –
A = Atomic Number =
N = Number of Neutrons
Give the relative abundance of the two isotopes of neon when neon – 20 has a mass of 20 and neon – 22
has a mass of 22 a.m.u.
ELECTRON CONFIGURATION
Complete the following: (pages 27-39)
Atom
Atomi
c#
Short hand
Electron
Configurati
on
# of
proton
s
# of
e-
Valence
Electro
n
Calcium
Electron
s lost or
gained
# of elost or
gained
Cation
or
Anion
2
cation
1
Anion
Ion
Not.
Lost
[Ne]3s23p6
8
Group
18
INERT
Gain
9
Page | 2
Match the following (pages 19-33)
A. Electron configuration
B. Bohr Model
C. Isotope
D. Atomic Number
E. Cation
F. Short hand electron configuration
G. Bohr electron configuration
H. Isotope Symbol
I. Atomic Mass
J. Anion
 [Ne] 3s23p5
 1s22s22s63s23p5
 different
number of
neutrons
 Number of
Protons =
number of
electrons
 Lose of electrons
 Gain of
electrons
 2-8-7



Cl-
 Number of Protons and
Neutrons


Label the following: (page 31)
How do you write the short hand electron configuration?
1) Step 1:
2) Step 2:
Complete the following for Iodine:
Electron Configuration: _________________________________________
Short hand Electron Configuration:
Valence Electrons:
Lewis Dot:
Page | 3
How can you determine valence electrons using the periodic table:
Write the Electron configuration, short hand, Lewis dot, Bohr Model, Bohr electron configuration for the
following elements:
F
Mg
HISTORY OF THE ATOM:
Identify the following with the name of the scientist and name of the experiment (page 23)
1.
Postulates:______________________
All elements are composed of tiny indivisible particles called atoms
Atoms of the same element are identical & atoms of different elements are different
Atoms combine in predictable ratios to make compounds
Atoms are rearranged in chemical reactions
2. Experimented with cathode ray tube (Plum pudding Model) ________________________________
By adding a electric field , he found that the moving pieces were negative
Discovered that every atom has a negative particles called electrons
Proposed the plum pudding model
3. Said electrons travel in orbits
_________________________________
a. Central nucleus with electrons located in rings
b. Considered the Hydrogen atom
4. Matter is not infinitely divisible – smallest particles called atomos
__________________________________
5. Measured the mass of a electron
_________________________________
a. 1/1840 the mass of a hydrogen atom
b. Oil Drop Experiment
6. Gold Foil Experiment (Nuclear Atom Model)
__________________________________
a. Shot alpha (+) particles at a thin gold foil
b. Most of the particles traveled straight through but some were deflected
7. Showed there was a second particle in the nucleus
a. Neutron – no charge
__________________________________
Page | 4
Name the scientist that correlates with the experiment
________________
__________
___________
_______________
______________
PROPERTIES OF THE PERIODIC TABLE
Fill in the following table: (page 13-17)
Family Name
Properties
 Group 1A
 Lose 1 electron and form cations
 Shinny, silver and soft
 React explosively with water
 Not found in Nature
 Cesium is the least electronegative
 Examples include: sodium, potassium
 Group 2
 Lose 2 electrons and form cations
 Silver and react mildly in water
 Not as soft as alkali metals
 Examples include: calcium, magnesium






Groups 3-12
Lose electrons and form cations
High reactivity
Mostly solids except: mercury (liquid)
High conductivity
Examples Include: copper, silver, gold







Group 17
Gains electrons and forms anions
Corrosive and strong odor
Salt – formers
Non-metallic
Are diatomic
Fluorine is the most electronegative



Group 18
Colorless, odorless, and Tasteless
Non – reactive or inert
Page | 5
Vertical columns are called: ____________________________________________________
Horizontal rows are called:______________________________________________________
Dimitri Mendeleev is known as the __________________________________.
He arranged the periodic table based on the following:
1.
2.
3.
Henry Moseley arranged the periodic table based on:
Fill in the following table: (pages 13-17)
Type of elements
Metals
Properties
Non-metals
Metalloids
THE ELECTROMAGNETIC SPECTRUM AND PLANCK’S CONSTANT
Electromagnetic radiation is energy that travels in waves. Two types of electromagnetic waves are
microwaves and gamma rays. Gamma rays have a shorter wavelength than microwaves. Which of
these statements is true?(page 47)
a.
b.
c.
d.
Gamma
Gamma
Gamma
Gamma
rays travel faster than microwaves.
rays have more energy than microwaves do.
rays have a lower frequency than microwaves do.
rays, but not microwaves, can travel through a vacuum.
What is the relationship between frequency and wavelength for electromagnetic waves? (page 47)
a.
b.
c.
d.
A. Frequency equals wavelength.
B. As frequency increases, wavelength increases.
C. As frequency increases, wavelength decreases.
D. The relationship depends on the speed of the wave
Page | 6
Microwaves are used to transmit information. What is the wave length of a microwave having a
frequency of 3.44x109 Hz. Record bubble your answer to the thousandth place in the griddable below.
(page 51)
Tiny water drops in the air disperse the white light of the sun into a rainbow. What is the energy of a
photon from the violet portion of the rainbow if it has a frequency of 7.23x10 -4 s-1? (page 51)
Fill in the following table: You must show all your work for full credit. (page 51)
Wavelength (m)
Frequency (Hz)
Energy (J)
0.001
7.0 x 1013
5.0 x 10-7
Electron configuration(Page 34)
Write the electron configuration for copper and chromium and explain why copper and chromium are
exceptions.
Page | 7