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Bonding

Total questions: 45

Worksheet time: 44mins

Name
Class
Date
1.

What is the number of valence electrons for Carbon (Group 14)?

a)

1

b)

2

c)

3

d)

4

2.

A covalent bond forms when atoms ___________ electrons.

a)

gain

b)

share

c)

increase

d)

transfer

3.
Which type of bond has a transfer of an electron from on atom to another?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
4.
How many valence electrons in this structure?
a)
6
b)
5
c)
4
d)
7
5.

Ionic bonding is between a

a)

nonmetal and nonmetal

b)

metal and nonmetal

c)

metal and metal

d)

Depends on the situation

6.

Which category of elements usually form negative ions?

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

7.

Predict the bond between Mg and Cl

a)

covalent

b)

ionic

c)

metallic

d)

none of the above

8.
Which of the following is ionic?
a)
NO2
b)
MgO
c)
CO
d)
CH4
9.

What charge would a potassium (K) ion have?

a)

+1

b)

-1

c)

+2

d)

-2

10.

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

a)

Ionic Compound

b)

network solid

c)

metallic solid

d)

covalent solid

11.
 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
12.
The bond between N & H.   Ionic or covalent?
a)
Ionic
b)
Covalent
13.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
14.

In metallic bonds the electrons:

a)

are shared between atoms

b)

move freely around positive ions

c)

are transferred from one atom to another

15.
At room temperature, most metals are
a)
liquid
b)
solid
c)
gas
d)
an alloy
16.

Which of the following would be held together by the metallic bond?

a)

Atoms of iron (Fe)

b)

Molecules of CH4

c)

Atoms of sulfur (S)

d)

Formula units of NaCl

17.

A substance which has a high melting point, conducts electricity when dissolved in water, has a crystalline structure, but does not conduct electricity as a solid probably has what type of bond?

a)
Ionic
b)
Metallic
c)
Covalent
d)
Crystalline
18.
What type of bond is illustrated above?
a)
Metallic
b)
Ionic
c)
Covalent
d)
Wiggly
19.
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
20.

Ionic compounds are held together by

a)

intermolecular forces

b)

electrostatic forces

c)

magnetic forces

d)

nuclear forces

21.

Which compound would have a very low melting point?

a)

sodium chloride

b)

copper (II) sulfate

c)

sulfur dioxide

d)

aluminum

22.

Which solid would be a good conductor?

a)

sodium chloride

b)

copper (II) sulfate

c)

glucose

d)

aluminum

23.
Which of the following gives the correct chemical formula for the compound Calcium Nitride?
a)
Ca2N3
b)
CaN
c)
Ca3N2
d)
CaN2
24.

Which of the following gives the correct chemical formula for the compound Magnesium Fluoride?

a)

Mg2F

b)

MgF

c)

MgF2

d)

Mg2F2

25.
Given the picture, what type of bond is  holding the atoms together in this molecule?
a)
polar covalent bond
b)
nonpolar covalent bond
c)
ionic bond
d)
metallic bond
26.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
27.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Linear
28.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
29.
Choose the correct shape for this molecule:
a)
Tetrahedral
b)
Trigonal pyramidal
c)
Bent
d)
Trigonal planar
30.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
31.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
32.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
33.
Electronegativity is a measurement of the ability of a nucleus to...
a)
attract bonding electrons
b)
attract other nuclei
c)
attract elenece in the non-valence energy levels
34.
How many electrons are represented by a single straight line in a Lewis structure?
a)
1
b)
2
c)
4
d)
6
35.
The most electronegative atom in the periodic table is:
a)
Fluorine
b)
Helium
c)
Neon
d)
Francium
36.

This is an example of a __________ bond.

a)

non-polar covalent

b)

polar covalent

c)

ionic

d)

metallic

37.

Partial charges like the ones shown here are called:

a)

dipoles

b)

deltas

c)

ions

d)

magnetic poles

38.
Which molecule contains bonds of GREATER polarity?
a)

H2O

b)

OF2

39.
Which molecule contains bonds with a GREATER polarity?
a)
HCl
b)

CCl4

40.
A bond with a partially negative end and a partially positive end is:
a)
ionic
b)
polar
c)
non-polar
d)
isometric
41.

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

a)
nonpolar; equally
b)
polar; equally
c)
nonpolar; unequally
d)
nonpolar; unequally
42.
If Bromine bonds with Hydrogen, a ____________ bond forms.
a)
polar covalent
b)
nonpolar covalent
c)
metallic
d)
ionic
43.
When you are asked to find bond polarity, compare EN values of each bonding atom to the central atom
a)
true
b)
false
44.

The electronegativity difference in the bonds of CH4 (methane) is:

a)
0.4
b)
5.9
c)
-0.4
d)
1.7
45.

The electronegativity difference in the bonds of CCl4 (carbon tetrachloride) is:

a)
0.4
b)
0.5
c)
9.5
d)
5.5

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