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Chemistry Final Exam Review

Total questions: 120

Worksheet time: 3hrs 6mins

Name
Class
Date
1.

What happens to the atoms of a substance in a physical change?

a)

Atoms get bigger

b)

Atoms change their arrangement and motion

c)

Atoms get smaller

d)

Atoms bond together differently

2.

What happens to the atoms of a substance in a chemical change?

a)

Atoms get bigger

b)

Atoms change their arrangement and motion

c)

Atoms get smaller

d)

Atoms bond together differently

3.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number
4.
What quantities vary between isotopes of an element?
a)
protons, electrons, and atomic mass
b)
protons, electrons, and atomic number
c)
neutrons and electrons
d)
neutrons and atomic mass
5.
What does the 1.00794 stand for?
a)
Hydrogen
b)
atomic number
c)
average atomic mass
d)
mass number
6.
What particle decides the identity of an atom/element?
a)
proton
b)
neutron
c)
electron
d)
All of the above.
7.
If X is the symbol for an element, which of the following two symbols represent    isotopes of the same element?    
a)
I and II
b)
III and IV
c)
I and IV
d)
I and III
8.

Which of the following are examples of chemical changes?

a)

Burning paper

b)

Cutting paper

c)

Iron rusting

d)

Wrinkling paper

9.

Determine the molecular geometry of the given structure.

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Trigonal Planar

d)

Tetrahedral

10.

What intermolecular forces would exist between molecules of HF?

a)

London Dispersion Forces

b)

Dipole-Dipole Forces

c)

Hydrogen Bonding

d)

All of the above

11.

Which of the following would experience dipole-dipole forces of attraction between molecules?

a)
b)
c)
d)
12.

Which of the following has T-shape molecular geometry?

a)
b)
c)
d)
13.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

14.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
15.
In this Lewis structure, the symbol above F means...
a)
electrons are being transferred to Fluorine
b)
electrons are less attracted to F than H
c)
electrons are more attracted to F than H
d)
Fluorine has formed a cation
16.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

17.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

18.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

19.
What geometry will this molecular structure have?: PH3
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
20.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
21.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
22.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
23.

Which is true of this molecule? (select ALL that apply)

a)

bent, 109.5o bond angles

b)

bent, 120o bond angles

c)

linear, 180o bond angles

d)

polar

e)

nonpolar

24.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
25.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
26.

Ionic bonds have an electronegativity difference of...

a)

Under 1.7

b)

Over 1.7

c)

Between .4 and 1.7

d)

Under .4

27.

What is electronegativity?

a)

An electron's charge

b)

The same as atomic bonding

c)

Whether they can easily repel electrons

d)

How easily elements can attract electrons to themselves

28.

If a molecule is trigonal pyramidal, how is that different from a tetrahedral?

a)

A trigonal pyramidal has 1 lone pair and 3 atoms around the central atom ... a tetrahedral has 4 atoms around the central atom and no lone pairs

b)

A trigonal pyramidal has 4 atoms around the central molecule and no lone pairs, and a tetrahedral has one lone pair and three atoms

c)

A trigonal pyramidal has 2 lone pairs and 2 atoms around the central molecule ... a tetrahedral has 4 atoms and no lone pairs

d)

Trick question, they aren't different.

29.

Why do lone pairs affect molecular geometry?

a)

They don't affect molecular geometry.

b)

Lone pairs pull the atoms bonded to the central atom towards them.

c)

Lone pairs are made of electrons, which repel other electrons in the molecule (such as the ones in the bonds)

d)

Lone pairs are made of protons, which repel the protons in the atoms around the central atom

30.

How do you take the electronegativity difference?

a)

Subtract the two electronegativity values from each other

b)

Divide the larger electronegativity value by the smaller one

c)

Add the two electronegativity values

d)

Multiply the electronegativity values

31.

What are the bond angles between each H in BeH2?

a)

90

b)

120

c)

109.5

d)

180

32.

What are the bond angles between each H in CH4?

a)

109.5

b)

120

c)

180

d)

360

33.

If there are 2 atoms bonded around the central atom, and an unknown number of lone pairs, what is its molecular geometry?

a)

Linear

b)

Bent

c)

Trigonal Pyramidal

d)

We can't know without knowing if there are lone pairs.

34.

What type of bond would H2S have, if H has an electronegativity of 2.2 and S has an electronegativity of 2.58?

a)

Polar

b)

Nonpolar

c)

Ionic

d)

None of the above

35.

The polarity of a bond between two elements can be best determined by

a)

The difference in electronegativity between the elements

b)

The difference in first ionization energy between the elements

c)

The number of electrons shared in the bond

d)

The difference in atomic radius between the elements

36.
What are the formal charges on the boron and nitrogen in the compounds BF3 and NH3? 
a)
-2 and +2
b)
+2 and –2                             
c)
0 and 0
d)
+1 and –1
37.
In the diagram shown, what is the total number of electrons shared in the bond between the two carbon atoms?
a)
2
b)
3
c)
4
d)
6
38.
This molecule has______bond and is a _________molecule.
a)
non-polar; non-polar
b)
polar, polar
c)
polar,
non-polar
d)
non-polar; polar
39.

What is the electron-domain and molecular geometry of the pictured compound, respectively?

a)

Trigonal Bipyramidal; See Saw

b)

Octahedral; Square Pyramidal

c)

Trigonal Bipyramidal; Trigonal Bipyramidal

d)

Octahedral; T-shaped

40.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
41.

Which is the correct Lewis structure for carbon dioxide?

a)
b)
c)
d)
42.

Which of the following best explain how to determine the shape of the molecule above?

a)

there are 3 atoms bonded to the central atom and 2 lone pairs

b)

there are single bonds

c)

there are 3 atoms bonded to the central atom and 0 lone pairs of electrons on the central atom

43.

Which of the following bonds is least polar?

a)

C--O

b)

O--H

c)

S--Cl

d)

Br--Br

e)

I--F

44.

Choose the electron dot formula that most accurately describes the bonding in CS2.

a)
b)
c)
d)
e)
45.

In the Lewis structure for ICl2–, how many lone pairs of electrons are around the central iodine atom?

a)

0

b)

1

c)

2

d)

3

e)

4

46.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

47.
The force of attraction between nonpolar molecules:
a)
Hydrogen Bonding
b)
Dipole - Dipole Forces
c)
LDF
d)
Ionic Forces
48.
The strength of temporary dipoles:
a)
increases with the size of molecules
b)
is greater than intremolecular forces
c)
is the strongest intermolecular force
49.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

50.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

51.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

52.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

53.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

54.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

55.

Which type of IMF is responsible for the attraction pictured above?

a)

Dipole-Dipole Interaction

b)

Ion-Dipole Interaction

c)

Hydrogen Bonds

d)

Covalent Bond

e)

Ionic Bond

56.

Intermolecular forces are attractions between ______.

a)

Cations and anions

b)

Atoms within a molecule

c)

Neighboring molecules

d)

Protons and electrons

57.

Which of the following might cause a hydrogen bond to form?

a)

Carbon

b)

Phosphorus

c)

Sulfur

d)

Oxygen

58.

Intermolecular forces are responsible for which of the following properties?

a)

State of matter

b)

Color

c)

Odor

d)

Conductivity

59.

Which of the following gives the correct chemical formula for the compound Magnesium Phosphide?

a)

Mg2P3

b)

MgP

c)

Mg3P2

d)

MgP2

60.
Which of the following gives the correct chemical formula for the compound Dinitrogen Monoxide?
a)
NO
b)
N2O
c)
N2O2
d)
O2N2
61.

What is the correct chemical name for the ionic compound: Na2O

a)

Sodium oxide

b)

Sodium (II) oxide

c)

Disodium monoxide

d)

Disodium oxide

62.

What is the correct chemical name for the ionic compound: Fe3N2

a)

Iron nitride

b)

Iron (III) nitride

c)

Iron (II) nitride

d)

TriIron dinitride

63.

What is the correct chemical name for the molecular compound: CS2

a)

Carbon Sulfide

b)

Carbon diSulfide

c)

diCarbide diSulfide

d)

Carbon (II) Sulfide

64.
What type of atoms make a covalent bond?
a)
only Nonmetals
b)
Metal and a Nonmetal
c)
only Metals
d)
only Noble Gases
65.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
66.
What is H2SO4 
(Sulfuric Acid) made up of?
a)
2 hydrogen, 1 sulfur, 4 oxygen
b)
1 hydrogen, 2 sulfur, 4 oxygen
c)
2 hydrogen & 4 sodium
d)
1 hydrogen & 6 sodium
67.
What type of bond forms when electrons are transferred from one atom to another?
a)
ionic bond
b)
atomic bond
c)
covalent bond
d)
metallic bond
68.

What is the correct chemical name for the molecular compound: SF4

a)

Sulfur Fluoride

b)

Sulfur TetraFluoride

c)

TetraSulfide Fluoride

d)

Sulfur (IV) Fluoride

69.

What do atoms that form positive ions tend to do?

a)

Tend to lose electrons

b)

Tend to lose protons

c)

Tend to gain electrons

d)

Tend to gain protons

70.

Titanium(IV) oxide has the formula

a)

Ti4O

b)

TiO4

c)

Ti(IV)O

d)

TiO2

e)

Ti4O2

71.

The substance ClO3– is best described as

a)

a molecule

b)

a polyatomic ion

c)

a polyatomic molecule

d)

a mixture

72.

Which part of the atom is responsible for chemical bonding?

a)

Core Electrons

b)

Valence Electrons

c)

Protons

d)

Neutrons

73.
A solid substance is an excellent conductor of electricity. The chemical bonds in this substance are most likely?
a)
ionic, because the valence electrons are shared between atoms
b)
covalent, because the valence electrons are mobile
c)
metallic, because the valence electrons are stationary
d)
metallic, because the valence electrons are mobile
74.

Ionic compounds are held together by

a)

intermolecular forces

b)

electrostatic forces

c)

magnetic forces

d)

nuclear forces

75.

A compound that is a poor conductor and has low melting and boiling points is most likely

a)

ionic

b)

metallic

c)

covalent

76.

High Melting & Boiling Points

a)

Ionic

b)

Network Covalent

c)

Metallic

d)

Molecular Covalent

77.

When writing the chemical formula of a compound that contains more than one of a particular polyatomic ion, _____ must be used.

a)

ionic charges

b)

parenthesis

c)

Greek prefixes

d)

lower case letters.

78.

If there is no subscript, there is ______ atom(s) of that element present in the compound

a)

0

b)

2

c)

only 1

d)

1 million

79.

What is the charge of an aluminum ion that has 13 protons and 10 electrons?

a)

3+

b)

3 -

c)

no charge

80.

Which is the correct lewis dot structure for calcium chloride?

a)

A

b)

B

c)

C

81.

Horizontal row in the periodic table

a)

group

b)

valence electrons

c)

period

d)

family

82.

type of element that is a good conductor of energy

a)

nonmetal

b)

metalloid

c)

metal

d)

transition metal

83.

Each period in the periodic table corresponds to a(n)

a)

principle energy level

b)

energy sublevel

c)

orbital

d)

suborbital

84.

Which statement is true about electronegativity

a)

electronegativity is the ability of an anion to attract another anion

b)

electronegativity generally increases as you move from top to bottom within a group

c)

electronegativity generally is higher for metals than for non metals

d)

electronegativity generally increases from left to right across a period

85.

For groups 13 through 18, the number of valence electrons is equal to the group number

a)

plus 1

b)

plus the period number

c)

minus the period number

d)

minus 10

86.

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

a)

it tends to decrease

b)

it tends to increase

c)

it first increases, then decreases

d)

it first decreases, then increases

87.

Which of the following will have a larger radius than Zinc (Zn)?

a)

Gallium (Ga)

b)

Aluminum (Al)

c)

Magnesium (Mg)

d)

Strontium (Sr)

88.
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
89.
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.
90.

All elements found on the left side of the Periodic Table of the Elements have what properties in common?

a)

They conduct heat and electricity

b)

They are all gases

c)

They are brittle and dull

d)

They are radioactive

91.

Based on their locations in the periodic table, which element has chemical properties most similar to those of calcium, Ca?

a)

beryllium, Be

b)

potassium, K

c)

titanium, Ti

d)

yttrium, Y

92.
What are the electrons in the outer most energy level called?
a)
Halogens
b)
Metals
c)
Oxidation Number
d)
Valence Electrons
93.
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
94.

As you move across the periodic table atoms tend to get smaller because, ______________.

a)

the atoms have more mass.

b)

the atoms have more protons and increased electron shielding.

c)

the atoms have more protons and electrons are added to the same energy level.

d)

the atoms have more protons, electrons, and increased electron shielding.

95.

The most dominant factor affecting the attraction between the outermost electrons and the nucleus is the

a)

distance between the nucleus and outermost electrons.

b)

none of these are correct.

c)

total number of electrons.

d)

number of protons/ nuclear charge.

96.

What kind of element can conduct electricity, but be brittle (not malleable)?

a)

some nonmetals

b)

metalloids

c)

some metals

d)

all nonmetals

97.

Chlorine has 17 electrons. According to the modern atomic theory, how many electrons are found in n = 2, the second energy level?

a)

7

b)

2

c)

8

d)

17

98.

According to the Bohr model, what may happen when an atom gains energy?

a)

The electron moves to a higher energy level.

b)

The electron moves to a lower energy level.

99.

What atom matches this electron configuration?

1s2 2s2 2p6 3s2

a)

Neon

b)

Magnesium

c)

Aluminum

d)

Potassium

100.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
101.

What is this element?

1s22s22p63s23p64s23d104p6

a)

Argon

b)

Krypton

c)

Selenium

d)

Bromide

102.

What is the shorthand electron configuration for Sulfur atom?

a)

[Ar] 3p4

b)

[He] 3s23p4

c)

[Ne] 3s23p4

d)

[Na] 3s23p3

103.

Which element is pictured?

a)

neon - 1s22s22p6

b)

fluorine - 1s22s22p5

c)

magnesium - 1s22s22p63s2

d)

argon - 1s22s22p63s23p6

104.

Identify the element in Period 5 that has 1 valence electron?

a)

Rb

b)

Nb

c)

Ag

d)

Sb

105.

What element in Period 4 has 5 valence electrons?

a)

Zr

b)

As

c)

V

d)

Sb

106.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
107.

Which element is depicted from this orbital diagram

a)

Fluorine - 1s22s22p5

b)

Neon - 1s22s22p6

c)

Chlorine - 1s22s22p63s23p5

d)

Argon - 1s22s22p63s23p6

108.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
109.
Which orbital shows a violation of Hund's Rule?
a)
A
b)
B
c)
C
d)
D
110.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
111.

When atoms _____________ energy, their electrons move to higher energy levels. These electrons _____________ energy by emitting light when they return to lower energy levels.

a)

lose, absorb

b)

absorb, lose

c)

lose, lose

d)

absorb, absorb

112.

What is the difference in a 1s orbital and a 2s orbital?

a)

The shape of the orbital

b)

The size of the orbital

c)

The number of electrons it can hold

d)

None of the above

113.
If distance remains the same, as the number of protons increases, the force of attraction
a)
remains the same
b)
increases
c)
decreases
d)
is divided by 1/2
114.

Why does Ca have a larger radius than Se?

a)

It has more energy levels

b)

It has fewer energy levels

c)

It has a more effective nuclear charge

d)

It has a less effective nuclear charge

115.

Why is S smaller than Te?

a)

It has more energy levels.

b)

It has fewer energy levels.

c)

It has a more effective nuclear charge.

d)

It has a less effective nuclear charge.

116.

Which of the following elements has the most "shielding" electrons?

a)

nitrogen (N)

b)

phosphorus (P)

c)

arsenic (As)

d)

bismuth (Bi)

117.
If a laboratory fire erupts, immediately
a)
notify your instructor
b)
 run for the fire extinguisher
c)
throw water on the fire
d)
 open the windows
118.
Approved eye protection devices (such as goggles) are worn in the laboratory
a)
 to avoid eye strain
b)
to improve your vision
c)
only if you don’t have corrective glasses
d)
 any time chemicals, heat or glassware are used
119.
You are heating a substance in a test tube. Always point the open end of the tube 
a)
away from all people
b)
toward another classmate
c)
toward your lab partner
d)
toward yourself
120.
You have accidentally broken a test tube and spilled a chemical on the table. Which of the following best explains what you should do?
a)
Quickly dispose of the glass, wipe up the spill with the nearest cloth, and hope nobody notices.
b)
Throw the glass into the nearest trash bin and let the spill air-dry.
c)
Use water and paper towels to clean up the spill; place the broken test tube in the disposal container specified for sharp objects.
d)
Caution your lab partners to avoid the area while you inform the teacher of the small accident.

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