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Unit 5 Bonding Review

Total questions: 145

Worksheet time: 4hrs 43mins

Name
Class
Date
1.

What is a positive ion called?

a)

anion

b)

cation

c)

isotope

d)

covalent

2.

What is a negative ion called?

a)

anion

b)

cation

c)

covalent

d)

isotope

3.

How many electrons would a Nitrogen ion gain/lose? If it has 5 valence electrons.

a)

lose 5

b)

gain 5

c)

lose 3

d)

gain 3

4.

What is the ion formed from Sulfur? If it has 6 valence electrons.

a)

S+2

b)

S-2

c)

S+6

d)

S-6

5.

How many electrons would a Calcium ion gain/lose? If it has 2 valence electrons.

a)

lose 1

b)

gain 1

c)

lose 2

d)

gain 2

6.

If an atom loses electrons, the charge will be positive.

a)

true

b)

false

7.

A Bromine ion gains 1 electron, which of the following is the correct symbol for a Bromine ion?

a)

Br-1

b)

Br+1

c)

Br+7

d)

Br-7

8.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
9.

An atom with 2 protons, 3 neutrons, and 4 electrons has a charge of ____.

a)

+2

b)

-2

c)

+3

d)

0

10.

Na has 1 valence electron. It will have a charge of _______

a)

+1

b)

+2

c)

-1

d)

-2

11.

Be has 2 valence electron. It will have a charge of _______

a)

+1

b)

+2

c)

-1

d)

-2

12.

Al has 3 valence electron. It will have a charge of _______

a)

+3

b)

-3

c)

+2

d)

-2

13.

P has 5 valence electron. It will have a charge of _______

a)

+3

b)

-3

c)

+2

d)

-2

14.

S has 6 valence electron. It will have a charge of _______

a)

-2

b)

-1

c)

+1

d)

+2

15.

Iodine has 7 valence electron. It will have a charge of _______

a)

-2

b)

-1

c)

+1

d)

+2

16.

Oxygen has 6 valence electron. It will have a charge of _______.

a)

+1

b)

-1

c)

+2

d)

-2

17.

The transfer of electrons from calcium atoms to chlorine atoms results in the formation of

a)

coordinate covalent bonds

b)

polar covalent bonds

c)

nonpolar covalent bonds

d)

ionic bonds

18.

A certain solid, when it is in the liquid state, will conduct electricity. In the solid state it will also conduct electricity. This solid must contain

a)

coordinate covalent bonds

b)

covalent bonds

c)

ionic bonds

d)

metallic bonds

19.

What type of bond exists in a molecule of I2?

a)

coordinate covalent bonds

b)

polar covalent bonds

c)

nonpolar covalent bonds

d)

ionic bonds

20.

The atoms in a molecule of HCl are held together by

a)

dipole-dipole attraction

b)

polar covalent bonds

c)

nonpolar covalent bonds

d)

ionic bonds

21.

Which type of bonding involves positive ions surrounded by a sea of mobile electrons?

a)

metallic bonds

b)

polar covalent bonds

c)

nonpolar covalent bonds

d)

ionic bonds

22.

A solid substance is soft, has a low melting point, and is a poor conductor of electricity. The substance is most likely a(n)

a)

molecular solid

b)

network solid

c)

metallic solid

d)

ionic solid

23.

A compound formed from potassium and bromine will have

a)

a molecular crystal structure

b)

a high melting point

c)

good heat conductivity in the solid state

d)

poor electrical conductivity in solution

24.

Which compound contains ionic bonds?

a)

NaH

b)

CH4

c)

H2O

d)

C6H12O6

25.

Which compound has the lowest melting point?

a)

HCl

b)

LiCL

c)

NaCl

d)

KCl

26.

A certain substance is a poor conductor of heat and electricity and has a high melting point. The substance is most likely

a)

Hg

b)

He

c)

CO2

d)

SiO2

27.

Which atom will form the most polar bond with hydrogen?

a)

F

b)

Cl

c)

Br

d)

I

28.

Which formula represents a molecular solid?

a)

NaCl(s)

b)

C6H12O6(s)

c)

Cu(s)

d)

KF(s)

29.

A solid substance has a melting point of 1074 K, conducts electricity when dissolved in water, but does not conduct electricity in the solid phase. The substance is most likely a(n)

a)

molecular solid

b)

network solid

c)

metallic solid

d)

ionic solid

30.

The relative tendency of an atom to attract electrons to itself when it is bonded to another atom is _____

a)

ionization energy

b)

electronegativity

c)

electron affinity

d)

electromotive force

31.

Which type of bond is created between C-N?

a)

Polar Covalent

b)

Non-polar Covalent

c)

Ionic

d)

Metallic

32.

Based on the electronegativity difference, what type of bond is this?

a)

nonpolar covalent

b)

polar covalent

c)

ionic

d)

none of the above

33.

In a polar covalent bond, which atom will have a partial positive charge? (choose 2 correct answers)

a)

The atom that lower attraction for electrons

b)

The atom with the greater electronegitivity

c)

The atom that has the greater attraction for electrons

d)

The atom with the lower electronegativity

34.

A diatomic molecule like O2 is always _____ because electrons are shared _____

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

35.
Which formula represents an ionic compound?
a)
CaCl2
b)
CH3OH
c)
CH4
d)
H2
36.
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
37.
Which formula represents an covalent compound?
a)
CO2
b)
Ag
c)
FeCl3
d)
Cs3P
38.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
39.
Does HCl have hydrogen bonding?
a)
yes
b)
no
40.
Does CH4 have hydrogen bonding?
a)
yes
b)
no
41.

Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

42.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
43.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
44.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

45.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

46.
Which of the following statements correctly explains why hydrogen bonding is such a strong intermolecular force?
a)
There is an attraction between a small, weakly electronegative hydrogen atom and a large, strongly electronegative atom of fluorine, nitrogen, or oxygen
b)
There is an attraction between a small, highly electronegative hydrogen atom and a large, highly electronegative fluorine atom
c)
There is an attraction between the hydrogen and oxygen atoms, only
d)
There is an attraction between the hydrogen and nitrogen atoms, only
47.

Water has an unusually high boiling point for a molecular compound because it has

a)

hydrogen bonding

b)

ion-ion attractions

c)

a high density

d)

a large gram formula mass

48.

Which of the following will NOT have hydrogen bonding?

a)
b)
c)
d)
49.
Does HF have hydrogen bonding?
a)
yes
b)
no
50.

In a polar covalent bond, the electrons gather around...

a)

Mostly the atom with the greatest electronegativity

b)

The atom with the lowest electronegativity

c)

Each atom equally

d)

Only the atom with the greatest electronegativity

51.

In a nonpolar covalent bond, the electrons gather around...

a)

Mostly the atom with the greatest electronegativity

b)

The atom with the lowest electronegativity

c)

Each atom Equally

d)

Only the atom with the greatest electronegativity

52.

The polarity of a bond is determined by...

a)

The sum of the electronegativities of the two atoms

b)

The difference in the electronegativities of the two atoms

c)

The charges of the atoms

d)

The number of electrons shared in the bond

53.
Rank these in order of strength:
covalent bond
London forces
hydrogen bond
dipole-dipole attraction
a)
dipole-dipole>covalent bond>hydrogen bond>London
b)
London>dipole-diple>hydrogen bond>covalent bond
c)
covalent bond>hydrogen bond>dipole-dipole>London
d)
hydrogen bond>dipole-dipole>London>covalent bond
54.

When new chemical bonds form, energy ____________.

a)

is taken into the system.

b)

is released from the system.

c)

stays the same in the system.

55.

Does breaking bonds require energy, release energy, or not involve energy at all?

a)

requires energy to break

b)

releases energy when broken

c)

No energy involved

56.

An exothermic reaction...

a)

requires energy

b)

releases energy

c)

is unrelated to energy

57.

An endothermic reaction...

a)

requires energy

b)

releases energy

c)

is unrelated to energy

58.

Forming a chemical bond...

a)

requires energy

b)

releases energy

c)

is unrelated to energy

59.

Breaking a chemical bond...

a)

requires energy

b)

releases energy

c)

is unrelated to energy

60.

Name the following: MgO

a)

Magnesium Oxide

b)

Monomagnesium monoxide

c)

Magnesium monoxide

d)

Magnesium (II) oxide

61.

Name the following: NO2

a)

Nitrogen oxide

b)

Mononitrogen dioxide

c)

Nitrogen dioxide

d)

Nitrogen (II) oxide

62.

Name the following: CF4

a)

Carbon fluoride

b)

Monocarbon tetrafluoride

c)

Carbon tetrafluoride

d)

Carbon fluorate

63.

Name the following: N2O5

a)

Nitrogen oxide

b)

Dinitrogen pentoxide

c)

Nitrous oxide

d)

Nitrogen pentoxide

64.

Name the following: CuO

a)

Copper oxide

b)

Copper (II) oxide

c)

Monocopper monoxide

d)

Copper monoxide

65.

Name the following: C3H8

a)

Tricarbon octahydride

b)

Carbon hydride

c)

Carbon octahydride

d)

Tricarbon hydride

66.

Name the following: NH3

a)

Nitrogen hydrogen

b)

Nitrogen trihydrogen

c)

Mononitrogen trihydride

d)

Nitrogen trihydride

67.

Is the following compound ionic or covalent?

Cl2

a)

Ionic

b)

Covalent

68.

Is the following compound ionic or covalent?

Ag2O

a)

Ionic

b)

Covalent

69.

Is the following compound ionic or covalent?

BaI2

a)

Ionic

b)

Covalent

70.

Is the following compound ionic or covalent?

A material that contains two nonmetals

a)

Ionic

b)

Covalent

71.

Is the following compound ionic or covalent?

A material that LOSES and GAINS electrons

a)

Ionic

b)

Covalent

72.
Elements combine to form __________.
a)
compounds
b)
atoms
c)
positive ions
d)
negative ions
73.

What is the formulas for sodium nitride?

a)

NaN

b)

Na2N

c)

Na3N

d)

NaN3

74.

Which of the following pair of elements is most likely to form an ionic compound?

a)

Magnesium and fluorine

b)

Nitrogen and sulfur

c)

Oxygen and chlorine

d)

Sodium and aluminum

75.

Which of these elements does not exist as a diatomic molecule?

a)

Ne

b)

F

c)

H

d)

I

76.
When metals bond with non-metals they form what type of bonds
a)
covalent
b)
ionic
c)
cooperative
d)
lewis
77.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
78.
How do the following two elements bond together?
Al3+  O2-         
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
79.
AgF
a)
silver fluoride
b)
silver fluorine
c)
monosilver monofluoride
d)
silver monofluorine
80.
When a nonmetal gains electrons, it becomes this type of ion.
a)
Anion
b)
Cation
81.
When a metal loses electrons, it becomes this type of ion.
a)
anion
b)
cation
82.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
83.

How many valence electrons does Tin (Sn) have?

a)

8

b)

7

c)

5

d)

4

84.

When atoms share 2 pairs of electrons, a _______ bond is formed.

a)

single

b)

double

c)

triple

85.

According to the diagram below, how many bonds will this atom be able to make?

a)
1
b)
2
c)
3
d)
4
86.
This could be the dot diagram of 
a)
Ne
b)
Si
c)
Al
d)
Be
87.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
d)

Ionic bond

88.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
89.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
90.

This atom would be considered stable.

a)

False

b)

True

91.

How many bonds could this atom form?

a)

1

b)

2

c)

3

d)

4

92.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
93.

At the beginning of the unit we discussed properties of metals. Why are metals excellent conductors of electricity?

a)
Metals have free electrons that can move easily through the metal lattice.
b)
Metals have a high resistance to electricity.
c)
Metals have positive charges that attract electrons.
d)
Metals have insulating properties that prevent the flow of electricity.
94.

Why do covalent compounds not conduct a current?

a)
Covalent compounds do not conduct a current because they have a low melting point.
b)
Covalent compounds do not conduct a current because they are not soluble in water.
c)
Covalent compounds do not conduct a current because there are no free ions or charged particles to carry the current.
d)
Covalent compounds do not conduct a current because they have a high electrical resistance.
95.

A substance that can conduct a current in solution due to moving ions contains what type of bonding?

a)
ionic
b)
covalent
c)
metallic
d)
polar
96.
What is the first thing you need to do when drawing Lewis Structures?
a)
Draw your bonds
b)
Count the number of valence electrons
c)
Subtract to make the valence number even
d)
Add to make the valence number even
97.
After drawing in your bonds, what do you do if you don't have enough electrons to get each atom to its octet?
a)
Place dots until everything has eight
b)
Place dots only around the terminal atoms
c)
Add a multiple bond
d)
Have eight only around the central atom
98.
How many electrons do atoms need to be stable?
a)
1
b)
2
c)
6
d)
8
99.
How many covalent bonds does carbon need to form in order to have a full octet?
a)
2
b)
3
c)
4
d)
5
100.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
101.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
102.
Which molecule would have this molecular geometry?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
103.
In a polar bond, the more electronegative element will assume a partial ________ charge.
a)
positive
b)
negative
104.

Hydrogen Bonding occurs when the negative _______ of one H2OH_2O  molecule attracts the positive ______ of another H2OH_2O  molecule.

a)

oxygen, hydrogen

b)

hydrogen, oxygen

c)

hydrogen, hydrogen

d)

oxygen, oxygen

105.

Oxygen attracts most of the _____ towards its end and away from the hydrogen.

a)

n0n^0  

b)

p+p^+  

c)

e−e^-  

106.

H2OH_2O  is a ________ molecule.

a)

polar

b)

nonpolar

c)

ionic

d)

metallic

107.

Use your knowledge and electronegativity sheet to predict what the following compound is classified as.

a)

polar covalent

b)

nonpolar covalent

c)

ionic

d)

metallic

108.

Use your knowledge and electronegativity sheet to predict what the following compound is classified as.

a)

nonpolar covalent

b)

polar covalent

c)

ionic

d)

metallic

109.

Use your knowledge and electronegativity sheet to predict what the following compound is classified as.

a)

non-polar covalent

b)

polar covalent

c)

ionic

d)

metallic

110.

Use your knowledge and electronegativity sheet to predict what type of bond would form between calcium and bromine.

a)

non-polar covalent

b)

polar covalent

c)

ionic

d)

metallic

111.

Use your knowledge and electronegativity sheet to predict what type of bond would form between phosphorus and fluorine.

a)

non-polar covalent

b)

polar covalent

c)

ionic

d)

metallic

112.
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
113.

The electronegativity difference in the bonds of CH4 is:

a)

0.4

b)

5.9

c)

-0.4

d)

1.7

114.

A covalent bond usually forms between:

a)

a metal and a nonmetal

b)

either metals or nonmetals

c)

two metals

d)

two nonmetals

115.

A diatomic molecule like O2 is always_______ because electrons are shared ________.

a)

nonpolar; equally

b)

polar; equally

c)

nonpolar; unequally

d)

nonpolar; unequally

116.

What causes a partial charge on a molecule?

a)

unequal sharing of electrons

b)

an electronegativity difference between 0.4 and 1.8.

c)

the shape of the molecule

d)

all of the above

117.
Polar, nonpolar, or ionic?
a)
Nonpolar
b)
Polar
118.
Polar, nonpolar, or ionic?
a)
nonpolar
b)
polar
119.

Polar or nonpolar?

a)

Nonpolar

b)

Polar

120.

Polar or Nonpolar

a)

Polar

b)

Nonpolar

121.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

122.

Classify the following molecule.

a)

polar

b)

nonpolar

123.

Classify the following molecule.

a)

polar

b)

nonpolar

124.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

125.

Is the following molecule polar or nonpolar?

a)

polar

b)

nonpolar

126.

What is the goal of the Lewis Dot Structure?

a)

To determine the electron position.

b)

To show the element's valence electrons & bonding capabilities.

c)

To find the atomic mass of an element.

d)

To search for the number of electrons in an individual atom.

127.

This is a correct dot diagram for nitrogen (N)

a)

true

b)

false

128.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

129.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
130.

Which is the correct Lewis structure for carbon dioxide?

a)
b)
c)
d)
131.

How many valence electrons are in the compound N2O?

(a)  

132.
What element is represented in this Bohr Model? 
a)
Carbon
b)
Hydrogen
c)
Aluminum
d)
Lithium
133.
How many valence electrons are in Phosphorus?
a)
15
b)
4
c)
5
d)
31
134.
The majority of an atom's mass exists where?
a)
In the nucleus
b)
In the electron cloud
c)
In the space between the nucleus and the electrons
d)
In the neutrons
135.
How many electrons are in the outer shell of Sodium (Na)?
a)
3
b)
1
c)
2
d)
4
136.

What Element does this Bohr Model show?

a)

Helium

b)

Hydrogen

c)

Argon

d)

Silver

137.

Ionic bonding involves

a)

transfer of electrons

b)

sharing of electrons

c)

holding onto electrons

d)

electrons are not involved

138.

What usually forms a positive ion?

a)

metal

b)

nonmetal

c)

metalloid

d)

there is no way to tell

139.

Covalent compounds

a)

contain a sea of electrons

b)

share electrons

c)

transfer electrons

d)

conduct electricity

140.

Nonmetals tend to

a)

gain electrons

b)

lose electrons

141.

Metals tend to

a)

gain electrons

b)

lose electrons

142.

a)

ionic

b)

covalent

c)

metallic

d)

acid

143.
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.
144.
How many valence electrons in this structure?
a)
6
b)
5
c)
4
d)
7
145.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above

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