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Covalent Bonds

Total questions: 81

Worksheet time: 3hrs 19mins

Name
Class
Date
1.
Name the following compound: 
N2O4
a)
dinitrogren tetraoxide
b)
tetranitrogen dioxide
c)
nitrogen oxide
d)
dinitrogen tetraoxygen
2.
Name the following compound: 
CO2
a)
monocarbon dioxide
b)
carbon oxide
c)
carbon dioxide
d)
oxygen carbonide
3.
Name the following compound: 
CCl4
a)
monocarbon quadchloride
b)
carbon tetrachloride
c)
carbon chloride
d)
monocarbon quadchloide
4.
Write the formula for:
dinitrogen tetroxide
a)
N2O4
b)
NO2
c)
NO
d)
N4O8
5.
In an electron dot diagram, two pairs of shared electrons represents a ...
a)
single bond
b)
double bond
c)
triple bond
d)
quadruple bond
6.
A Nitrogen molecule (N2) has one triple bond. How many electrons do the nitrogen atoms share?
a)
1
1
b)
3
c)
4
d)
6
7.
Compared to ionic compounds, molecular compounds generally have...
a)
stronger chemical bonds
b)
poor conductivity
c)
a high melting point
d)
lower densities
8.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
9.
silicon dioxide
a)
SO2
b)
NaO2
c)
SiO2
d)
SiO
10.

hexaboron monosilicide

a)

B6Si

b)

BSi

c)

BSi6

d)

B6Si6

11.
Is hydrogen considered a metal or a non-metal?
a)
A metal
b)
Nonmetal
c)
Metalloid
12.
Covalent bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
13.
What is a valence electron?
a)
The sum of neutrons and protons.
b)
The # of electrons in the last shell.
c)
A type of bond.
d)
A popular compound.
14.
Atoms are most stable when their outer shell is complete.
a)
true
b)
false
15.
What do we call a covalent bond where electrons are shared UNEVENLY or UNEQUALLY?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
16.

This is the displayed formula for what covalent compound?

a)

Water

b)

Hydrogen peroxide

c)

Hydrogen oxide

d)

Ethanol

17.

This is the displayed formula for what covalent molecule?

a)

Water

b)

Chlorine

c)

Chloride

d)

Ethanol

18.

The red dots indicate ______________________.

a)

lone pairs

b)

bond pairs

19.
Compared to ionic compounds, molecular compounds generally have...
a)
stronger chemical bonds
b)
poor conductivity
c)
a high melting point
d)
lower densities
20.

How many valence electrons does Oxygen (O) have?

a)

6

b)

8

c)

15

d)

16

21.

How many atoms of hydrogen are in a sugar molecule with the formula C6H12O6

a)

12

b)

6

c)

24

d)

18

22.

Atoms that are _____________ will form bonds.

a)

stable

b)

unstable

23.

The weakest covalent bond is a _____________.

a)

single bond

b)

double bond

c)

triple bond

d)

polar bond

24.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
25.

Which is the correct molecular structure for carbon dioxide CO2?

a)
b)
c)
d)
26.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
27.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

28.

How many total valence electrons are participating in bonding in the molecule above?

a)

8

b)

4

c)

2

d)

3

29.

__________ bonds involve an unequal sharing of electrons, while __________ bonds involve an equal sharing of electrons.

a)

Nonpolar, polar

b)

Polar, metallic

c)

Metallic, nonpolar

d)

Polar, nonpolar

30.

According to the Octet Rule, atoms of elements react with each other in order to attain ____ electrons in their outermost energy level or shell.

a)

2

b)

4

c)

6

d)

8

e)

10

31.

Electronegativity is...

a)

The ability for an atom to ATTRACT electrons

b)

the ability of an atom to LOSE electrons

c)

the energy required to remove an electron from an atom

d)

how easy it is to make friends.

32.
How many electrons should Lithium have around its Lewis dot model?
a)
1
b)
2
c)
3
d)
4
33.
How many electrons should Boron have around its Lewis dot model?
a)
1
b)
3
c)
5
d)
7
34.
How many electrons should Oxygen have around its Lewis dot model?
a)
5
b)
6
c)
7
d)
8
35.
This is the correct dot diagram for nitrogen (N)
a)
true
b)
false
36.

CO₂

(a)  

37.

PCl₃

(a)  

38.

P₂O₅

(a)  

39.

I₂O₇

(a)  

40.

carbon tetrahydride

(a)  

41.

dihydrogen monoxide

(a)  

42.

Covalent bonds form between: ​

a)

two nonmetals

b)

two metals

c)

a metal and a nonmetal

d)

two alkali metals

e)

A metal and a noble gas

43.

Due to similarities in electronegativities, atoms involved in covalent bonds __________ valence electrons

a)

"share"

b)

"transfer"

c)

"don't have any"

d)

do not "share"

44.
Disulfur trioxide
a)
S3O2
b)
SO
c)
S2O3
d)
S2O
45.
Bromine monoflouride
a)
Br1F1
b)
BrF
c)
Br2F
d)
BrF2
46.
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
47.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
48.
What is the prefix for nine?
a)
nina
b)
nona
c)
nuevo
d)
nuna
49.
The prefix for 10 is?
a)
deca
b)
diaz
c)
dozen
d)
tena
50.

What is a triple bond?

a)

A bond that involves the sharing of two pairs of electrons between two atoms.

b)

A covalent bond that involves the sharing of three pairs of electrons between two atoms.

c)

A bond formed by the transfer of electrons from one atom to another.

d)

A bond that occurs between three different atoms.

51.

What is a molecular formula?

a)

A molecular formula shows the number and type of atoms in a molecule, but does not show how they are arranged.

b)

A molecular formula indicates the arrangement of atoms in a molecule.

c)

A molecular formula is a graphical representation of a molecule.

d)

A molecular formula only shows the total number of atoms in a molecule.

52.

What is the difference between polar and nonpolar covalent bonds?

a)

Polar covalent bonds occur when electrons are shared equally between atoms.

b)

Nonpolar covalent bonds occur when electrons are shared unequally between atoms.

c)

Polar covalent bonds occur when electrons are shared unequally between atoms, while nonpolar covalent bonds occur when electrons are shared equally.

d)

Both polar and nonpolar covalent bonds involve equal sharing of electrons.

53.

What is a double bond?

a)

A bond that involves the sharing of one pair of electrons between two atoms.

b)

A covalent bond that involves the sharing of two pairs of electrons between two atoms.

c)

A bond formed by the transfer of electrons from one atom to another.

d)

A bond that occurs between two identical atoms only.

54.

What is a single bond?

a)

A covalent bond that involves the sharing of one pair of electrons between two atoms.

b)

A bond formed by the transfer of electrons from one atom to another.

c)

A bond that involves the sharing of three pairs of electrons between two atoms.

d)

A weak interaction between molecules that does not involve electron sharing.

55.

What is a Lewis Structure?

a)

A diagram that shows the bonding between atoms of a molecule and the lone pairs of electrons that may exist in the molecule.

b)

A method for calculating the molecular weight of a compound.

c)

A type of chemical reaction that involves the transfer of electrons.

d)

A graphical representation of the three-dimensional shape of a molecule.

56.

How do you determine the central atom in a Lewis Structure?

a)

The most electronegative atom

b)

The least electronegative atom or the atom that can form the most bonds

c)

The atom with the highest atomic number

d)

The atom that is a metal

57.

What is a diatomic molecule?

a)

A molecule that consists of two atoms of the same element.

b)

A molecule that consists of two atoms, which can be of the same or different elements.

c)

A molecule that consists of three atoms of different elements.

d)

A molecule that consists of one atom of each of two different elements.

58.

What is a lone pair of electrons?

a)

A pair of valence electrons that are shared between two atoms.

b)

A pair of valence electrons that are not involved in bonding.

c)

A pair of valence electrons that are involved in forming a double bond.

d)

A pair of valence electrons that are not shared with another atom and are not involved in bonding.

59.

What is electronegativity?

a)

A measure of an atom's ability to attract and hold onto electrons in a bond.

b)

The energy required to remove an electron from an atom.

c)

The tendency of an atom to lose electrons in a chemical reaction.

d)

The measure of an atom's size in a molecule.

60.

What is a structural formula?

a)

A structural formula shows the arrangement of atoms in a molecule and the bonds between them.

b)

A structural formula is a type of chemical equation that represents the reactants and products.

c)

A structural formula is a graphical representation of the molecular weight of a compound.

d)

A structural formula indicates the physical state of a substance at room temperature.

61.

Is the Lewis structure for CO2 correct or incorrect?

a)

Correct

b)

Incorrect

62.

Is the Lewis structure for F2 correct or incorrect?

a)

Correct

b)

Incorrect

63.

Is the Lewis structure for H2O correct or incorrect?

a)

Correct

b)

Incorrect

64.

Is the Lewis structure for CCl4 correct or incorrect?

a)

Correct

b)

Incorrect

65.

_____________ is an exception to the rule of 8 because it only needs two valence electrons to fill the outermost shell.

a)

Hydrogen (H)

b)

Chlorine (Cl)

c)

Nitrogen (N)

d)

Sulfur (S)

66.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
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.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
69.

Which of the following compounds has only single bonds?

a)

I only

b)

II only

c)

III only

d)

I and III

e)

III and IV

70.
Which of the following is the correct Lewis structure for CH2O?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
71.

Valence electrons are located _____________ the nucleus of an atom

a)

close to

b)

farthest from

c)

randomly around

72.

How strongly an atom attracts electrons towards itself in a bond is called... ______. If the EN difference is under 0.4, it is a _____ bond.

a)

Ionization energy; polar covalent

b)

Electronegativity; pure covalent

c)

Electricity; radioactive

d)

Nuclear force; ionic

73.

Which of the following is the correct Lewis structure for the compound PBr3 because halogens can only form ___ bond.

a)

structure A; double

b)

structure B; ionic

c)

structure C; triple

d)

structure D; single

74.
Which of the following is NOT formed by a covalent bond?
a)
K2S
b)
H2O
c)
I2
d)
CO2
75.
Is hydrogen considered a metal or a non-metal?
a)
A metal
b)
Nonmetal
c)
Metalloid
76.
Atoms are most stable when their outer shell is complete.
a)
true
b)
false
77.
Why do elements bond?
a)
To be friends
b)
To create a new element
c)
To become stable
78.
Ionic or covalent?
NaBr
a)
Ionic
b)
Covalent
79.
Ionic or covalent?
H2O
a)
Ionic
b)
Covalent
80.
What molecule could this be? 
a)
H2O
b)
CCl4
c)
PCl5
d)
NaCl
81.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3

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