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Covalent Bonding Test Review

Total questions: 85

Worksheet time: 1hrs 4mins

Name
Class
Date
1.

If the atoms that share electrons have an unequal attraction for the electrons, the bond is called

a)

nonpolar

b)

polar

c)

ionic

d)

dipole

2.

A neutral group of atoms held together by covalent bonds is a

a)

molecular formula

b)

chemical formula

c)

molecule

d)

monoatomic ion

3.

Elements that form multiple covalent bonds include

a)

oxygen

b)

carbon

c)

nitrogen

d)

all of the above

4.

What is the formula for dioxygen pentachloride?

a)

OCl4

b)

O2Cl5

c)

O5Cl2

d)

O4Cl

5.

Why do most atoms form bonds?

a)

to be more stable by completing the octet

b)

to be less stable

c)

to add more electrons

d)

to carry out physical changes

6.

If two covalently bonded atoms are identical, the bond is

a)

coordinate covalent

b)

polar covalent

c)

dipole covalent

d)

nonpolar covalent

7.

What are shared in a covalent bond?

a)

ions

b)

Lewis structures

c)

dipoles

d)

electrons

8.

The B-F bond in BF3 (electronegativity for B is 2.0; electronegativity for F is 4.0) is

a)

polar covalent

b)

ionic

c)

nonpolar covalent

d)

metallic

9.

In a molecule of fluorine, the two shared electrons give each fluorine atom how many electron(s) in the outer energy level?

a)

1

b)

2

c)

8

d)

32

10.

The following molecules contain polar bonds. The only polar molecule is

a)

CCl4

b)

CO2

c)

NH3

d)

CH4

11.

Name the compound CF4.

a)

calcium fluoride

b)

carbon fluoride

c)

carbon tetrafluoride

d)

monocalcium quadrafluoride

12.

How are atoms held together in covalent bonds?

a)

By gaining and losing electrons

b)

By sharing electrons

13.

If the bond between two atoms, both of which are nonmetals, has the electronegativity difference of 0.4, what type of bond do the atoms have?

a)

Ionic

b)

Polar Covalent

c)

Non-polar covalent

14.

What types of elements combine to form ionic bonds?

a)

Metals and metalloids

b)

Metals and non metals

c)

Non metals only

d)

Metalloids only

e)

Metals only

15.

When diatomic fluorine creates a molecule, what type of bond is used? (Hint, you may have to draw the Lewis structure)

a)

Single bond

b)

Double bond

c)

Triple bond

16.

Which of the following is NOT one of the seven diatomic molecules?

a)

Hydrogen

b)

Carbon

c)

Bromine

d)

Iodine

e)

Oxygen

17.

What type of bond will N - H form?

a)

Polar Covalent

b)

Non-polar Covalent

c)

Ionic

18.

If the bond between two atoms has an electronegativity difference of 0.6, what type of bond do the atoms have?

a)

Ionic

b)

Polar Covalent

c)

Non-polar Covalent

19.

Which group has no electronegativity value?

a)

Halogen

b)

Transition Metals

c)

Noble Gases

d)

Alkaline Earth Metals

20.

Which element is an exception to the octet rule?

a)

K

b)

H

c)

N

d)

O

21.

What type of bond is present in the compound Co3N?

a)

Covalent

b)

Ionic

22.

What type of bond does NO2 have?

a)

Ionic

b)

Covalent

23.

How many atoms of oxygen are in the compound Al2(SO4)3

a)

2

b)

3

c)

4

d)

7

e)

12

24.

How many electrons are shared between two atoms in a double covalent bond?

a)

1

b)

2

c)

4

d)

6

25.

Which of the following has the greatest electronegativity?

a)

O

b)

S

c)

Br

d)

Si

26.

If a bond between two atoms has an electronegativity difference of 1.9, we can assume that bond is ________________

a)

Ionic

b)

Polar Covalent

c)

Non Polar Covalent

27.

The compound CBr4 has a tetrahedral shape, what is the molecular polarity?

a)

Polar

b)

Nonpolar

28.

What is the molecular geometry (shape) of NH3?

a)

Bent

b)

Trigonal Planar

c)

Trigonal Pyramidal

d)

Tetrahedral

e)

Linear

29.

What is the correct molecular geometry AND molecular polarity of HCN?

a)

Tetrahedral, nonpolar

b)

Tetrahedral, polar

c)

Bent, polar

d)

Linear, polar

e)

Linear, nonpolar

30.

Which of the following bonds is the most polar?

a)

O-F

b)

N-F

c)

H-F

d)

S-F

31.

When drawing the structure of diatomic oxygen (O2), what type of bond is used?

a)

single

b)

double

c)

triple

d)

quadruple

32.

How many valence electrons are in an atom with a 1s22s22p3 electron configuration?

a)

1

b)

2

c)

3

d)

5

33.

Which family on the periodic table is unreactive because of the octet rule?

a)

Noble gases

b)

Alkaline Earth

c)

Alkali Earth

d)

Transition Metals

34.

Electrons are ______________ in ionic bonds

a)

shared

b)

buried

c)

transferred

35.

A substance has a high boiling point and conducts electricity. Is this an ionic or covalent substance?

a)

ionic

b)

covalent

36.

Write the formula for dihydride monoxide.

a)

HMo

b)

HO

c)

HO2

d)

H2O

37.

How many electrons are shared in a triple bond?

a)

2

b)

3

c)

4

d)

6

38.

Polar bonds exist because a difference in

a)

electronegativity

b)

ion charges

c)

atomic radius

d)

magnetism

39.

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

a)

metal

b)

ionic

c)

covalent

d)

polar

40.

In an ionic bond the metal wants to ______ electrons.

a)

lose

b)

gain

c)

share

41.

When a metal loses an electron(s) it becomes a ...

a)

positive ion

b)

negative ion

c)

metalloid

d)

nonmetal

42.

Carbon and Oxygen will make a ___________ bond.

a)

ionic

b)

covalent

c)

metallic

43.

Sodium and Bromine will make a _____ bond.

a)

ionic

b)

covalent

c)

metallic

44.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
45.
CH4 is a covalent compound, please select the proper name of that formula. 
a)
Carbon hydride
b)
Carbon tetrahydride
c)
Tetracarbon hydrogen
d)
Carbon tetrahydroxide
46.
Phosphorus trichloride is a covalent compound. What is the proper formula?
a)
PCl3
b)
P3Cl
c)
PCl
d)
PCl2
47.

Which of the following names matches the chemical formula N2O3?

a)

Dinitrogen triople oxide

b)

Nitrogen oxide

c)

Dinitrogen trioxide

d)

Trioxide nitrogen

48.

How many atoms are in this molecule? C6H12O6

a)

6

b)

12

c)

18

d)

24

49.
Which of the following elements wants to bond 3 times
a)
Oxygen
b)
Phosphorous
c)
Fluorine
d)
Germanium
50.
Which of the following is a Diatomic Molecule 
a)
K2
b)
C2
c)
S2
d)
N2
51.

When trying to figure out how many electron shells an atom has, do you look at the Period (rows) or the Group (columns)?

a)

Period (Rows)

b)

Group (Columns)

52.

When trying to figure out how many valence electrons an atom has, do you look at the Period (rows) or the Group (columns)?

a)

Period (Rows)

b)

Group (Columns)

53.

Which 2 elements have the same number of valance electrons?

a)

Aluminum (AL) and Sulfur (S)

b)

Nitrogen (N) and Silicone (Si)

c)

Oxygen (O) and Sulfur (S)

54.

In forming covalent bonds, why do atoms share electrons?

a)

To achieve noble-gas notation

b)

To become charged

c)

To form ions

55.

What are atoms used to complete an octet but not used in bonding called?

a)

Shared pair

b)

Lone pair

c)

Bonded pair

d)

unshared pair

56.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
57.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
58.
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
59.
In the correct Lewis structure for water, how many unshared pairs of electrons will oxygen have?
a)
1
b)
4
c)
3
d)
2
60.
Which of the following is the correct Lewis structure for CH2O?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
61.
How many valence electrons do elements in Group 2A have?
a)
12
b)
4
c)
1
d)
2
62.
How many electrons does each line indicate are shared?
a)
1
b)
2
c)
3
d)
4
63.

When drawing a Lewis structure, after drawing in your bonds and lone pairs, 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

64.
How many covalent bonds does carbon need to form in order to have a full octet?
a)
2
b)
3
c)
4
d)
5
65.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
66.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

67.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

68.
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
69.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
70.

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

71.

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

72.

Which sample has hydrogen bonding?

a)

H2S

b)

CH4

c)

NH3

d)

HI

73.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonds

74.
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
75.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

76.
Does H2S have hydrogen bonding?
a)
yes
b)
no
77.
Does HF have hydrogen bonding?
a)
yes
b)
no
78.
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
79.
Which is the second strongest intermolecular force, after hydrogen bonding?
a)
dipole-dipole attraction
b)
London forces
80.
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
81.
What information do we look for on the periodic table if we  want to examine intermolecular forces?
a)
atomic mass
b)
atomic number
c)
electronegativity
d)
ionization 
82.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
83.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
84.
Intermolecular force present in CHF3
a)
H bond
b)
dipole dipole
c)
dispersion
d)
ionic
85.
Which of these is not an intermolecular force?
a)
covalent bonding
b)
hydrogen bonding
c)
London dispersion forces
d)
dipole-dipole forces

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