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Covalent compounds review

Total questions: 45

Worksheet time: 57mins

Name
Class
Date
1.
A covalent bond is formed when two atoms ____ electrons
a)
share
b)
lose
c)
transfer
d)
gain
2.
Write the formula for Dinitrogen Pentaoxide.
a)
N5O2
b)
N2O5
c)
(N2O)5
d)
O5N2
3.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
4.
How many bonds does carbon have to create in order to satisfy the octet rule
a)
1
b)
2
c)
3
d)
4
5.

Outer shell electrons are called

a)

outer electrons

b)

valence electrons

c)

negatives

d)

super electrons

6.
If electrons are shared unequally then the bond is....
a)
Non-polar covalent
b)
Ionic
c)
Non-polar ionic
d)
Polar covalent
7.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
8.
Which of the following is an acceptable Lewis structure for CH3Cl?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
9.
PBr5
a)
Phosphorus Bromide
b)
Phosphorus Pentabromide
c)
Pentaphosphorus bromide
d)
Phosphorus Bromine
10.
Phosphorous trichloride
a)
PCl3
b)
P3Cl
c)
P3Cl3
d)
PCL
11.
The molecule shown has been called "laughing gas" and has been used in dentistry as a pain killer. What is its chemical name?
a)
Nitrogen oxide
b)
dinitrogen dioxide
c)
dinitrogen oxide
d)
nitrogen dioxide
12.
What does the prefix tetra mean?
a)
Three
b)
Four
c)
Six
13.
a)
The number circled is called a subscript.
b)
The number circled is called a superscript.
c)
The number shows that the element is a coefficient.
14.
What is the prefix for 10?
a)
mono
b)
tetra
c)
dec
d)
hept
15.

When electrons are shared equally the compound is a what type of bond?

a)

Polar Covalent

b)

Polar Ionic

c)

Non-Polar Covalent

d)

None of the above

16.

How many electrons make up a single bond?

a)

2

b)

4

c)

6

d)

1

17.

How many electrons make up a double bond?

a)

2

b)

4

c)

6

d)

1

18.

How many electrons make up a triple bond?

a)

2

b)

4

c)

6

d)

1

19.
Why do atoms share electrons?
a)
To attain the electron configuration of a noble gas.
b)
To become ions and take a charge
c)
to increase the mass
d)
it's a nice thing to do.
20.

Which of the following is NOT covalently bonded?

a)

K2S

b)

H2O

c)

I2

d)

CO2

21.

Diatomic elements are defined as IDENTICAL elements that bond with each other (i.e. Oxygen with Oxygen). What type of bond should they form?

a)

Ionic

b)

Covalent

22.
With the ________ you must have 8 electrons on the outside ring.
a)
anions
b)
ionic bonds
c)
cations
d)
octet rule
23.

Which pair of atoms is most likely to form a covalent molecule?

a)

Hydrogen and lithium

b)

Phosphorus and sulfur

c)

Helium and neon

d)

Zinc and Boron

24.
Which will NOT form a diatomic molecule?
a)
fluorine
b)
nitrogen
c)
bromine
d)
boron
25.
Covalent compounds display which of these properties?
a)
They are hard, brittle solids.
b)
They have high melting and boiling points.
c)
They display luster.
d)
They are usually insoluble in water.
26.
How many bonds can halogens form?
a)
1
b)
2
c)
3
d)
4
27.
Which of the following is NOT a property/characteristic of covalent compounds?
a)
May be a liquid at room temperature.
b)
Poor conductors of electricity.
c)
Have high melting points.
d)
Solid forms are soft or brittle.
28.

Is the following compound ionic or covalent?

A material that has a low boiling point

a)

Ionic

b)

Covalent

29.
How are covalent bonds explained?
a)
When one atom takes the other atom's electron
b)
When the atom shares an electron with an another atom
c)
When the two nucleus merge
d)
When the neutrons leave the nucleus
30.

Which of these is NOT a chemical bond?

a)

Ionic bond

b)

Covalent bond

c)

Metallic bond

d)

Molecule bond

31.

Nonpolar bonds are when electrons are ______________ shared.

a)

equally

b)

nonequally

32.
Low melting point and low solubility in water are general properties of ______________________ compounds
a)
ionic
b)
covalent
c)
chemical
d)
glucose
33.

What are diatomic elements?

a)

Elements that form two-atom molecules when not combined in a compound.

b)

Two elements that combine with one atom from each element.

c)

Elements that are always in pairs no matter what.

34.

What are the seven diatomic elements?

a)

H2, Cl2, Br2, O2, N2, I2, F2

b)

H2, Cl2, I2, F2, Hg2, Br2, Fe2

c)

H2, Cu2, Ni2, B2, O2, I2, Fe2

35.

In an electron dot diagram, three lines connecting atoms represents a ...

a)

single bond

b)

double bond

c)

triple bond

d)

quadruple bond

36.

Compound X has a low melting point and is a poor conductor. When separated into its constituent elements, it's found to be made of nonmetals. Is the compound ionic or covalent?

a)

Ionic

b)

Covalent

37.
What is a double bond?
a)
a bond between two atoms
b)
one pair of electrons shared between two atoms
c)
two pairs of electrons shared between two atoms
d)
James Bond's brother
38.
How many electrons are shared in N2?
a)
3
b)
6
c)
7
d)
10
39.
chlorine monoxide
a)
ClO
b)
ClO-
c)
ClO2
d)
CO
40.
Which pair of elements will form a covalent bond between them? 
a)
Mg and Cl
b)
S and O
c)
Li and F
d)
Mg and S
41.
Compared to ionic compounds, molecular compounds generally have...
a)
stronger chemical bonds
b)
poor conductivity
c)
a high melting point
d)
lower densities
42.

Why do all bonds form?

a)

so the number of protons equals the number of electrons

b)

so an atom can become unstable

c)

to fill the outermost energy level

43.

Which of the following elements can form diatomic molecules held together by double covalent bonds?

a)

Carbon

b)

Oxygen

c)

Fluorine

d)

Nitrogen

44.

Which molecule has only single bonds?

a)

CO2

b)

Cl2

c)

CO

d)

N2

45.

Which Lewis structure below is correct for CH2Cl2?

a)
b)
c)
d)

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