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Chemical Bonding Review

Total questions: 68

Worksheet time: 1hrs 16mins

Name
Class
Date
1.
Which part of the atom is responsible for chemical bonding?
a)
Inner/Core Electrons
b)
Outer/Valence Electrons
c)
Protons
d)
Neutrons
2.
What best describes valence electrons?
a)
Electrons in the inner-most shell.
b)
Electrons in the outer-most shell.
c)
Electron that became a beta particle.
3.
How many valence electrons do most atoms need to have a complete outer shell and be happy?
a)
1
b)
8
c)
10
d)
5
4.
Which two elements only need two valence electrons to be happy?
a)
Hydrogen and Helium
b)
Lithium and Neon
c)
Copper and Iron
d)
Californium and Berkelium
5.
How many valence electrons do elements in Group 1, the Alkali Metals, have?
a)
1
b)
2
c)
6
d)
7
6.
How many valence electrons do elements in Group 2, the Alkaline Earth Metals, have?
a)
1
b)
2
c)
6
d)
7
7.
How do ionic bonds form?
a)
Atoms share electrons to fill their valence shell.
b)
Atoms gain or lose electrons to fill their valence shell.
c)
Atoms donate electrons to a "sea" of electrons.
8.
How do covalent bonds form?
a)
Atoms share electrons to fill their valence shell.
b)
Atoms gain or lose electrons to fill their valence shell.
c)
Atoms donate electrons to a "sea" of electrons.
9.

Electronegativity ______ moving left to right on the Periodic Table.

a)

increases

b)

decreases

c)

stays the same

10.

What type of bond is illustrated in this image?

a)

Metallic

b)

Ionic

c)

Covalent

d)

James

11.
Which of the following is a covalent compound?
a)
LiF - Lithium Fluoride
b)
NH3 - Ammonia
c)
NaBr - Sodium Bromide
d)
CuCl - Copper(I) Chloride
12.
Which is an example a covalent compound?
a)
CO2
b)
NaCl
c)
AlF3
d)
MgO
13.

In an ionic bond, the metal atom

a)

gains electrons to form a cation

b)

loses electrons to form a cation

c)

gains electrons to form an anion

d)

loses electrons to form an anion

14.

Properties of _____ bonds include high melting points, good conductivity, poor solubility, and malleable.

a)

Covalent

b)

Ionic

c)

Metallic

15.

Properties of _____ bonds include low melting points, poor conductivity, poor solubility, and the weakest compared to other types.

a)

Covalent

b)

Ionic

c)

Metallic

16.

Properties of _____ bonds include high melting points, poor conductivity, good solubility, and form solid, crystalline substances.

a)

Covalent

b)

Ionic

c)

Metallic

17.

Which is the correct Lewis Dot Structure for H2S?

a)
b)
c)
18.
 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
19.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
20.
What is the measure of a tetrahedral bond angle?
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
21.
Which of the following molecular shapes would have a bond angle of 180 Degrees?
a)
Bent
b)
Trigonal Planar
c)
Tetrahedral
d)
Linear
22.
The bond angle for a trigonal planar molecule is 
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
23.
What molecular shape is the structure shown here? (BeCl2)
a)
linear
b)
bent
c)
trigonal planar
d)
tetrahedral
24.
What molecular shape is the structure shown here? (H2O)
a)
tetrahedral
b)
trigonal planar
c)
bent
d)
trigonal pyramidal
25.
What molecular shape is the structure shown here? (BCl3)
a)
linear
b)
trigonal planar
c)
tetrahedral
d)
trigonal pyramidal
26.
What is a cation? 
a)
a metal with a negative (-) charge
b)
a non-metal with a negative (-) charge 
c)
a metal with a positive (+) charge 
d)
a non-metal with a positive (+) charge
27.
What is a anion? 
a)
a metal with a negative (-) charge
b)
a non-metal with a negative (-) charge 
c)
a metal with a positive (+) charge 
d)
a non-metal with a positive (+) charge
28.
The octet rule means that all valence shells want to have the number...... 
a)
1
b)
9
c)
8
d)
16
29.

The chemical bond between a metal and a non-metal will be a _____ bond.

a)

metal

b)

ionic

c)

covalent

d)

polar

30.

The chemical bond between a non-metal and another non-metal will be a ________ bond.

a)

metal

b)

ionic

c)

covalent

d)

polar

31.

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

32.

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

33.

Using your electronegativity handout and the types of atoms involved, predict what type of bond would form between F and Cl.

a)

nonpolar covalent

b)

polar covalent

c)

ionic

d)

metallic

34.

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

a)

nonpolar; equally

b)

polar; equally

c)

nonpolar; unequally

d)

nonpolar; unequally

35.

This type of bond typically forms between a metal and another metal.

a)

covalent

b)

hydrogen

c)

metallic

d)

ionic

36.
Sliver Phosphide
a)
Ag3P
b)
Ag3PO4
c)
Ag3PO3
d)
AgP
37.
Na2S
a)
Sodium Sulfide
b)
Sodium Sulfate
c)
Sodium Sulfite
d)
Disodium Sulfide
38.
Manganese II Oxide
a)
MnO
b)
Mn2O
c)
Mn2O4
d)
MnO2
39.
The charge of V in V2O5 is?
a)
2+
b)
3+
c)
4+
d)
5+
40.
Which of the following elements would require Roman Numerals when it is named?
a)
Ga
b)
Ca
c)
B
d)
Au
41.
The formula for iron(III) oxide is
a)
FeO
b)
Fe3O
c)
Fe2O3
d)
Fe3O2
42.
What is the name of Li3P?
a)
Lithium potassium
b)
Lithium III Phosophide
c)
Lithium3 Phosphide
d)
Lithium Phosphide
43.
What is the formula for a compound made of Mg2+ and As3-?
a)
Mg3As2
b)
Mg2As3
c)
MgAs
d)
Mg6As4
44.
Ammonium Phosphate
a)
(NH4)3PO4
b)
NPO4
c)
NH4PO4
d)
NH4(PO4)3
45.
Sodium Bicarbonate
a)
NaHCO3
b)
Na2CO3
c)
Na2HCO3
d)
S(HCO3)2
46.

Which of the following is NOT a property of ionic compounds?

a)

They conduct electricity when molten

b)

They conduct electricity when in solution

c)

They have high boiling points

d)

They are insoluble in water

47.
A(n) _________ is an ion with a positive (+) charge.
a)
anion
b)
cation
c)
ion
d)
solute
48.
In what form can an ionic compound conduct electricity?
a)
when dissolved in water
b)
as a solid
c)
as a crystal
d)
when warmed slightly
49.

Dihydrogen Monoxide

a)

2HO

b)

H2O2

c)

H2O

d)

HO2

50.

Boron trichloride

a)

B3Cl

b)

B3Cl3

c)

BCl3

d)

3BCl

51.

Phosphorus pentachloride

a)

KCl5

b)

PCl5

c)

P5Cl

d)

5PCl

52.

XeF4

a)

Monoxenon tetrafluoride

b)

Xenon trifluoride

c)

Xenon tetrafluoride

d)

Xenon fluoride

53.

OF2

a)

Oxygen difluoride

b)

Oxygen fluoride

c)

Monoxide fluoride

d)

Fluorine dioxide

54.

Boron mononitride

a)

BNO3

b)

BNi

c)

BN

d)

BrN

55.

What characteristic differentiates covalent bonding from ionic bonding?

a)

Electrons are transferred from one atom to another to form a bond

b)

Electrons are shared in pairs from one atom to another to form a bond

56.

Which of the following compound is the least polar?

a)

NH3

b)

NCl3

c)

N2O5

d)

CH4

57.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

58.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

59.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

60.
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.
61.
Hydrogen bonding occurs when hydrogen is bonded to N, O, or F.  Which of the following has hydrogen bonding?
a)
CBr4
b)
NO2
c)
H2S
d)
NH3
62.
All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces.  Which of these has ONLY London forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
63.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
64.
How many electrons are shared between the nitrogen and each chlorine atom in a nitrogen trichloride molecule?
a)
1
b)
2
c)
3
d)
4
65.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
66.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
67.
Which of the following is an acceptable Lewis structure for CH3Cl?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
68.

Ionic bonds form between metals and ____.

a)

metalloids

b)

metals

c)

nonmetals

d)

protons

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