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Honors Chemistry Unit 3 Review Questions

Total questions: 90

Worksheet time: 3hrs 28mins

Name
Class
Date
1.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
2.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p6
3.
How many d orbitals are there in a given sublevel?
a)
1
b)
3
c)
5
d)
7
4.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
5.
How many p orbitals are there in a sublevel?
a)
2
b)
1
c)
4
d)
3
6.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
7.
What is this element? 
1s22s22p63s23p6
4s23d104p6
a)
Argon
b)
Krypton
c)
Selenium
d)
Bromide
8.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
9.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
10.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
11.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
12.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
13.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
14.
What noble gas should be used to write the shorthand configuration for Te?
a)
Ar
b)
Kr
c)
Xe
d)
Sb
15.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
16.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
17.
This is the correct dot diagram for sodium (Na)
a)
true
b)
false
18.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
19.

What are valence electrons?

a)

The innermost electrons

b)

The outermost electrons

20.

What is the octet rule?

a)

Elements can only have 8 electrons in its outermost shell

b)

The elements must form an octopus like structure

21.

How many valence electrons does Carbon have

a)

1

b)

4

22.

Electron dot notation is . . . .

a)

A representation of an element in which only valence electrons of an atom are shown

b)

A representation of how compounds are formed.

23.
How many electrons should Helium have around its Lewis dot model?
a)
1
b)
2
c)
7
d)
8
24.

Which of the elements in the picture has correct electron dot notation?

a)

1

b)

2

c)

3

d)

4

25.
There are 4 different types of subshells (orbitals) s,p,d,f.
a)
true
b)
false
26.
Which periodic table family could have electrons filling orbitals in the s-block?
a)
Alkaine Earth 
b)
Halogens
c)
Noble Gases
d)
Transition Metals
27.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
28.
Which has the greater EN: 
N or C?
a)
C
b)
N
29.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
30.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
31.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
32.
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....
a)
decreases
b)
increases
c)
remains the same
d)
none of the above
33.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
34.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
35.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
36.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
37.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
38.
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
39.
Which statement correctly and completely identifies a trend?
a)
Atomic radius decreases across a period and increases down a group.
b)
Electronegativity decreases across a period and decreases down a group.
c)
Ionization energy increases across a period and increases down a group.
d)
Ionic radius increases across a period and increases down a group.
40.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
41.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
42.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
43.
What term is used to describe "an atom's tendency to attract electrons to itself when is is chemically combined with another element"
a)
electronation
b)
electron affinity
c)
electronegativity
d)
electrolysis
44.
What term is used to describe "The energy required to remove an electron from gaseous atoms"
a)
excitation energy
b)
ionization energy
c)
polarization energy
d)
electrolytic energy 
45.
What term is used to describe "A measure of the size of an atom"
a)
chemical reactivity
b)
atomic radius
c)
energy levels
d)
orbit
46.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

47.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium II chloride

c)

beryllium chloride

d)

beryllium dichloride

48.

The number that tells you if an ion has lost or gained electrons

a)

atomic number

b)

oxidation number

c)

mass number

d)

electron number

49.

If I gain electrons I become

a)

Positive because I've added to my atom

b)

negative because I've added electrons

c)

same because i'm balanced

d)

equal because now I have electrons

50.
Nonmetals tend to 
a)
gain electrons
b)
lose electrons
51.
Metals tend to 
a)
gain electrons
b)
lose electrons
52.
In most cases, when naming you change the ending of the second element to ________.
a)
-ate.
b)
-ite.
c)
-ide.
d)
-ine.
53.
Name this compound: 
KF
a)
Potassium fluoride
b)
Potassium fluorite
c)
Fluorine potasside 
d)
Potassium fluorate
54.
MgS 
a)
Magnesium sulfide
b)
Monomagnesium monosulfide
c)
Magnesium monosulfide
55.

Which of the following statement is/are true?


I. Shielding describes the decrease in attraction between an electron and the nucleus


II. Effective nuclear charge increases across a period from left to right


III. Effective nuclear charge decreases down a group

a)

I only

b)

II only

c)

II and III only

d)

I, II and III

56.

Across a period from left to right, the effective nuclear charge __________

a)

Increases

b)

Decreases

c)

Remains the same

57.

Down the group the electron shielding

a)

Increases

b)

Decreases

c)

Remains the same

58.

Across the period, electron shielding _______

a)

Increases

b)

Decreases

c)

remains the same

59.
Shielding electrons causes the force of attraction to the nucleus to 
a)
increase
b)
decrease
60.
When a new energy level is added to the atom, shielding
a)
increases
b)
decreases
61.

A wave with a large wavelength will have a ______ frequency and _____ energy

a)

high, low

b)

high, high

c)

low, high

d)

low, low

62.

High frequency waves have _________ wavelength.

a)

varying

b)

high

c)

the same

d)

short

63.

Given the frequencies, which color has the highest energy?

a)

Violet

b)

Red

c)

Green

64.

Given the frequencies, which color has the longest wavelength?

a)

Violet

b)

Red

c)

Green

65.

Which color has the highest frequency?

a)

green

b)

blue

c)

red

d)

yellow

66.

Energy of a photon is ___ proportional to frequency.

a)

directly

b)

inversely

67.

When wavelength increases...

a)

energy decreases

b)

energy increases

68.

the distance between peaks of adjacent electromagnetic waves is called:

a)

wavelength

b)

frequency

c)

energy

d)

amplitude

69.

Which of the following is a unit for frequency?

a)

Joules

b)

Hertz

c)

meters per second

d)

seconds

70.

A light particle is called a(n):

a)

electromagnetic wave

b)

photon

c)

electron

d)

atom

71.

The lower the frequency the ______ the energy.

a)

higher

b)

lower

c)

neither, stays the same

72.
Which type of light has the highest energy of this group?
a)
red
b)
yellow
c)
green
d)
blue
73.

What is the term used to describe the dual nature of light as both a particle and a wave?

a)

wave-particle duality

b)

particle-wave duality

c)

light duality

d)

quantum duality

74.
What is the energy of light whose wavelength is 4.06 x 10-11 m? 
a)
2.69 x 10-44 J
b)
1.63 x 10-23 J
c)
4.90 x 10-15 J
d)
8.97 x 10-53 J
75.
The equation that shows the relationship between the energy of light and frequency is: 
a)
c= λ⋅f
b)
E=h⋅f
76.
What is the typical units of measurement for the "E" in the following equation: 
Ephoton= h x f
a)
joules
b)
meters
c)
meters/seconds
d)
hertz
77.
Find the energy, in joules per photon, of microwave radiation with a frequency of 7.91 × 10 10 1/s.
a)
6.63 x 10-34 J
b)
5.25 x 1014 J
c)
5.24 x 10-23 J
d)
1.19 x 1044 J
78.

What is the speed of light?

a)

3.0x108 ms

b)

3.0x108 m/s

c)

6.626x10-34 Js

d)

6.626x10-34 J/s

79.

Red light has a wavelength of 675 x 10-9 m. What is its frequency?

a)

2.03x1011 m

b)

4.44x1014 Hz

c)

4.44x1014 nm

d)

2.03x1011 Hz

80.
What is the energy of a quantum of light with a frequency of 7.39x1014Hz.(E=Hv)
a)
4.88x1019
b)
4.88x10-19
c)
2.22x1023
d)
2.22x10-23
81.
What is the wavelength for a quantum of light with energy of 7.56x10-19J? (λ=hc/E) 
a)
2.62x10-7m
b)
2.62x107m
c)
2.64x10-45m
d)
2.64x1045m
82.

Light is emitted when an electron moves from the ________ state to the _________ state.

a)

excited, ground

b)

ground, excited

83.
Which would describe an electron that has gained energy and jumped to another shell?
a)
ground state
b)
excited state
c)
valence
d)
core
84.
The energy of an electron __________ as it moves further away from the nucleus
a)
increases
b)
decreases
85.
When an atom has all of its electrons in the lowest energy orbitals available, the atom is  
a)
in ground state
b)
in excited state
c)
giving off light energy
d)
unstable
86.
Every element has its own unique atomic spectra.
a)
True
b)
False
87.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
88.
Light is emitted when an electron moves from the ________ state to the _________ state
a)
excited, ground
b)
ground, excited
89.

What evidence led Niels Bohr to believe that electrons occupy specific energy levels in atoms?

a)

Excited electrons emit colored light at every possible wavelength.

b)

Excited electrons emit colored light at only certain wavelengths.

c)

Electrons emit colored light only when in an excited state.

d)

Electrons emit colored light only when in ground state.

90.

What is the reaction involved if the electron moves from position 1 to 2?

a)

Light will be emitted

b)

Light will be absorbed

c)

The electron will become less excited

d)

The electron will decrease a quantum

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