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CPA Q3 Exam Review

Total questions: 112

Worksheet time: 3hrs 58mins

Name
Class
Date
1.

What property of this wave is represented by the letter "A"

a)

amplitude

b)

crest

c)

trough

d)

wavelength

2.
What property of the wave is represented by the letter "B"?
a)
amplitude
b)
crest
c)
trough
d)
wavelength
3.
The number of wavelengths that pass a point each per second is:
a)
frequency
b)
period
c)
longitudinal 
d)
transverse wave 
4.
Which letter(s) represent the trough of the wave?
a)
A
b)
B & D
c)
D
d)
C & G
5.
Which letter(s) represent the crest of the wave?
a)
A
b)
B & D
c)
B & F
d)
F
6.
Which wave in the diagram has the greatest frequency?
a)
1
b)
2
c)
3
d)
4
7.
Which wave in the diagram has the greatest wavelength?
a)
1
b)
2
c)
3
d)
4
8.

Which wave has the longest wavelength?

a)

A

b)

B

c)

C

d)

None (same wavelength)

9.

What is the relationship between frequency and wavelength?

a)

high frequency --> short wavelength

b)

high frequency --> long wavelength

c)

low frequency --> short wavelength

d)

there is no relationship

10.
Which parts of the electromagnetic spectrum have a higher frequency than visible light?
a)
Infrared, microwaves, and radio waves
b)
Ultraviolet, X-ray, and gamma rays
11.
Which type of wave has the highest frequency?
a)
Gamma
b)
Radio
c)
Visible
d)
Infrared
12.
Which type of wave has the greatest energy?
a)
Gamma
b)
Radio
c)
Visible
d)
Infrared
13.
Which part of the electromagnetic spectrum can be seen by the human eye?
a)
Gamma
b)
Radio
c)
Visible
d)
Infrared
14.
What is the ground state electron configuration of Bromine?
a)
2-8-18-7
b)
2-8-18-8
c)
2-3
d)
2-8-17-8
15.
What are patterns made when excited electrons emit light of certain wavelengths?
a)
electromagnetic spectra
b)
atomic emission spectra
c)
spectroscopes
d)
prisms
16.
Lowest energy state of an atom
a)
Ground
b)
Excited
17.
How many valence electrons does Lithium have?
a)
1
b)
2
c)
3
d)
4
18.
How many valence electrons does Carbon have?
a)
4
b)
12
c)
6
d)
14
19.
How many valence electrons does Oxygen have?
a)
8
b)
2
c)
16
d)
6
20.
Which of the following must you do to draw a Lewis dot diagram?
a)
Decide if each atom shown will give up or accept neutrons.
b)
Determine if the elements involved are metals or nonmetals.
c)
Determine the number of electrons in the outermost energy level.
d)
Decide how many protons should be shown to represent a molecule.
21.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
22.
How many valence electrons does Chlorine have?
a)
1
b)
7
c)
17
d)
35
23.
How many electrons should Lithium have around its Lewis dot model?
a)
1
b)
2
c)
3
d)
4
24.
How many electrons should Nitrogen have around its Lewis dot model?
a)
1
b)
3
c)
4
d)
5
25.
The energy of an electron __________ as it moves further away from the nucleus
a)
increases
b)
decreases
26.
Every element has its own unique atomic spectra.
a)
True
b)
False
27.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
28.
Why are line emission spectrums useful?
a)
they allow us to identify elements
b)
they tell us how many protons there are in a nucleus
c)
they represent the true color of the element
d)
to draw straight lines in our cornell notebooks
29.
Which of the following elements make up the unknown sample?
a)
A and B
b)
B and C
c)
C and D
d)
B and C
30.

Which is a possible excited state electron configuration for Si?

a)

2-8-4

b)

1-9-4

c)

2-8-8

d)

2-8-3-1

31.

What is the ground state electron configuration of Na?

a)

2-8

b)

2-8-2

c)

2-8-1

d)

11

32.

Which of the following shows an excited state electron configuration?

a)

2-7-1

b)

2-4

c)

2-8-4

d)

2-8-1

33.

What is the maximum number of electrons allowed in the second shell?

a)

1

b)

2

c)

8

d)

3

34.
What element is represented in this Bohr Model? 
a)
Carbon
b)
Hydrogen
c)
Aluminum
d)
Lithium
35.
What is the mass number of this atom?
a)
1
b)
3
c)
4
d)
7
36.
Identify the element in the picture
a)
Boron
b)
Carbon
c)
Nitrogen
d)
Lithium
37.
What element is this?
a)
Helium
b)
Hydrogen
c)
Argon
d)
Silver
38.
What is the atomic number of this atom?
a)
2
b)
4
c)
6
d)
none of the above
39.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
None of these
40.
What group does this element belong to?
a)
Group 1: Alkali metals
b)
Group 18: Noble Gases
c)
Group 2: Alkaline-Earth Metals
d)
Group 17: Halogens
41.

How is the periodic table organized?

a)

Periods are horizontal and groups are vertical

b)

Periods and groups are horizontal

c)

Periods are vertical and groups are horizontal

d)

Periods and groups are vertical

42.

Which elements have the most similar chemical properties?

a)

K and Na

b)

K and Ca

c)

K and Cl

d)

K and S

43.

In a modern periodic table, elements are arranged in order of?

a)

atomic mass

b)

number of isotopes

c)

atomic number

d)

number of neutrons

44.

How many periods does the periodic table have?

a)

18

b)

7

c)

9

d)

5

45.

Which elements are in the same group or family?

a)

Na and Mg

b)

Na and H

c)

Li and Be

d)

K and Ca

46.

Which elements are in the same period?

a)

F and Cl

b)

N and P

c)

O and S

d)

N and O

47.

Most elements on the periodic table are

a)

gases

b)

metals

c)

liquids

d)

nonmetals

48.

A material is said to be ductile if it

a)

can be shaped

b)

can be pulled into wire

c)

conducts heat

d)

is a mixture of metals and nonmetals

49.

Most nonmetals are

a)

ductile

b)

mallable

c)

lusturous

d)

dull

50.

Elements have similar properties are in the same

a)

group

b)

row

c)

period

d)

none of these

51.

Which group of nonmetals are the LEAST reactive?

a)

group 1

b)

group 17

c)

group 18

d)

group 4

52.

Elements to the right of the zigzag line are most likely

a)

metals

b)

nonmetals

c)

metalloids

d)

quarks

53.

Each period in the periodic table corresponds to __.

a)

a principal energy level

b)

an orbital

c)

an energy sublevel

d)

a suborbital

54.

To what category of elements does an element belong if it is a poor conductor of electricity?

a)

transition elements

b)

nonmetals

c)

metalloids

d)

Metals

55.

How does atomic radius change from left to right across a period in the periodic table?

a)

It tends to decrease.

b)

It first increases, then decreases.

c)

It tends to increase.

d)

It first decreases, then increases.

56.

What element in the second period has the largest atomic radius?

a)

carbon

b)

neon

c)

lithium

d)

potassium

57.

What is the charge of a cation?

a)

a positive charge

b)

no charge

c)

a negative charge

d)

The charge depends on the size of the nucleus

58.

The __________ are touching or bordering the zig-zag 'staircase' on the Periodic Table.

a)

metals

b)

non-metals

c)

metalloids

59.

If an element is in group number 18 you know it is ______. (will not bond because it has a full valence shell of electrons)

a)

reactive

b)

very reactive

c)

stable

60.

The most reactive group of non-metals is group ____.

a)

1

b)

2

c)

17

d)

18

61.

What are these elements called?

a)

Transition metals

b)

Noble gases

c)

Alkali metals

d)

Alkaline metals

62.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
63.

Which statement correctly and completely identifies a trend?

a)

Atomic radius decreases across a period and increases down a group.

b)

Atomic radius increases across a period and increases down a group

c)

Ionization energy increases across a period and increases down a group

d)

Ionization energy decreases across a period and decreases down a group

64.

Atomic radius generally increases as we move __________.

a)

down a group and from right to left across a period

b)

up a group and from left to right across a period

c)

down a group and from left to right across a period

d)

up a group and from right to left across a period

65.
The energy required to remove electrons is the definition of: 
a)
Electronegativity
b)
Atomic Number
c)
Atomic Radius
d)
Ionization
66.

What is the trend for reactivity of the alkali metals as one moves down a group?

a)

Reactivity increases

b)

Reactivity decreases

c)

Reactivity is relatively the same for the whole group

d)

Alkali metals are generally unreactive

e)

The reactivity decreases then increases

67.

Which family of elements have 7 valence electrons?

a)

the alkali metal family

b)

the boron group

c)

the nitrogen group

d)

the halogen family

68.

What is the name of the family that is highlighted?

a)

Alkali Metal Family

b)

Halogen Family

c)

Noble Gas Family

d)

Transition Metal Family

69.

Which family of elements is characterized by having 2 valence electrons?

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

70.

Which family of elements is known for forming salts when combined with metals?

a)

Noble gases

b)

Halogens

c)

Alkali metals

d)

Alkaline earth metals

71.
Which has the greater EN: 
N or C?
a)
C
b)
N
72.

Define electronegativity.

a)

The ability of an electron to attract atom to itself.

b)

The ability of a molecule to attract electrons to itself.

c)

The ability of an atom to attract electrons to itself.

d)

The ability of an ion to attract electrons to itself.

73.

The trend of electronegativity ________ across the period and _________down the group?

a)

increases... increases

b)

decreases... decreases

c)

decreases... increases

d)

increases... decreases

74.

Which of the following ordered pairs of elements has the highest difference in electronegativity?

a)

Li and Be

b)

Li and F

c)

O and F

d)

F and F

75.

How does electronegativity affect the type of bond formed between two atoms?

a)

A large difference in electronegativity leads to a metallic bond

b)

A small difference in electronegativity leads to an ionic bond

c)

A large difference in electronegativity leads to an ionic bond

d)

Electronegativity has no effect on the type of bond formed

76.

Which of the following elements has the lowest electronegativity?

a)

Fluorine

b)

Francium

c)

Oxygen

d)

Nitrogen

77.

What is the molar mass of CO2?

a)

12 g/mol

b)

16 g/mol

c)

32 g/mol

d)

44 g/mol

78.
What is the molar mass of table salt (NaCl)?
a)
116.886 g/mol
b)
35.453 g/mol
c)
22.990 g/mol
d)
58.443 g/mol
79.
What are the units in molar mass?
a)
grams
b)
moles
c)
moles/gram
d)
grams/mole
80.
Find the molar mass of KCl
a)
36 g/mol
b)
78 g/mol
c)
74 g/mol
d)
178 g/mol
81.
What is the molar mass of fluorine gas, F2?
a)
18.998 g/mol
b)
38 g/mol
c)
9 g/mol
d)
18 g/mol
82.
What is the molar mass of AuCl3?
a)
96 g
b)
130 g
c)
232.5 g
d)
303.3 g
83.
What is the molar mass C6H12O6
a)
61.0g/mol
b)
95.7g/mol
c)
180.2 g/mol
d)
164.9g/mol
84.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
85.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
86.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)
pairs of electrons are shared between two nonmetal atoms.
d)
two nonmetal atoms are attracted to each other by opposite charges.
87.
An ionic bond forms when 
a)
Valence electrons are shared
b)
a sea of mobile electrons surround the cations
c)
valence electrons are transferred between atoms
d)
none of the above
88.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
89.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
90.
Predict the bond that will form between Sr and S.
a)
Ionic
b)
Covalent
91.

______ compounds conduct electricity best when dissolved in water, while ______ compounds conduct electricity best as solids.

a)

covalent, ionic

b)

ionic, metallic

c)

metallic, ionic

d)

ionic, covalent

92.

A compound dissolves in water, has a high melting point, and doesn't conduct electricity as a solid. What is it?

a)

Ionic

b)

Covalent

c)

Metallic

d)

A mystery

93.

A compound does not dissolve water, has a low melting point, and conducts electricity as a solid. What is it?

a)

Ionic

b)

Covalent

c)

Metallic

d)

A mystery

94.

A compound dissolves in water, has a medium melting point, and doesn't conduct electricity as a solid. What is it?

a)

Ionic

b)

Covalent

c)

Metallic

d)

A mystery

95.
What type of bond is illustrated above?
a)
Metallic
b)
Ionic
c)
Covalent
d)
Wiggly
96.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
97.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
98.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
99.
How many electrons can be used in the Lewis Structure for : NO3 -
a)
23
b)
20
c)
18
d)
24
100.

This is a correct dot diagram for nitrogen (N)

a)

true

b)

false

101.
How many electrons does each line indicate are shared?
a)
1
b)
2
c)
3
d)
4
102.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

103.

What is the correct Lewis structure for NH3?

a)
b)
c)
d)
104.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
105.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
106.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core 
c)
Valence
d)
Stable
107.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
108.

Is this the correct structure for CH2O?

a)

Yes

b)

No

109.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
110.
What is the formal charge for Oxygen
a)
+1
b)
-1
c)
0
d)
-2
111.
How many valence electrons are available for bonding in the sulfate ion (SO4-2)?
a)
30 electrons
b)
32 electrons
c)
28 electrons
d)
impossible to tell
112.

What is the formal charge on the bromine atom in this Lewis dot structure?

a)

-1

b)

+1

c)

-2

d)

+2

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