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chemical bonding

Total questions: 44

Worksheet time: 27mins

Name
Class
Date
1.

Typically, atoms are more stable when they are

a)

bonded together

b)

apart from each other

2.

Why do atoms bond?

a)

They typically don't bond

b)

To add or take away energy levels

c)

To have a full valance shell.

d)

To have a full inner shell

3.

Covalent bonding is between a

a)

nonmetal and nonmetal

b)

metal and nonmetal

c)

metal and metal

d)

It depends on the situation

4.

What do positive ions tend to do?

a)

lose electrons

b)

gain electrons

c)

lose protons

d)

gain protons

5.

What happens when magnesium loses 2 electrons?

a)

It stabilizes to a net charge of 0

b)

It turns into an atom

c)

It becomes negatively charged

d)

It becomes positively charged

6.

Predict the bond between Mg and Cl

a)

covalent

b)

ionic

c)

metallic

d)

none of the above

7.

Which is the correct Lewis Structure for oxygen?

a)
b)
c)
d)
8.

What is the correct Lewis structure for BF3?

a)
b)
c)
d)

BF3 (The formula is the Lewis Structure)

9.

What is the chemical formula for Lithium Nitride?

a)

Li3N

b)

LiN3

c)

NLi3

d)

N3Li

10.

What is the ionic formula for a bond between Calcium and Phosphorus?

a)

Ca2P3

b)

Ca3P2

c)

Ca2P5

d)

P5Ca2

11.

What category of element usually forms a positive ion?

a)

Metals

b)

Nonmetals

c)

metalloids

d)

Noble gases

12.

CaCl2 is an example of what type of bond?

a)

Covalent

b)

Metallic

c)

Ionic

13.

Valence electrons are

a)

neutral (no charge)

b)

found in the outer most energy level of the atom

c)

equal to the number of protons

14.

Which type of bonds create compounds?

a)

covalent bonds

b)

ionic bonds

c)

metallic bonds

d)

all type of bonds

15.

How many valence electrons does Oxygen have?

a)

0

b)

16

c)

6

d)

8

16.

How many different elements are in the C6H12O6

a)

3

b)

6

c)

12

d)

24

17.

How many oxygen atoms on each side of C3H8 + 5O2 = 4H2O + 3CO2

a)

2

b)

3

c)

5

d)

10

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.
Which of the following shapes has an unshared pairs of electrons on the central atom? 
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
21.
Which molecule would have this molecular geometry?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
22.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
23.
What molecule could this be? 
a)
H2O
b)
CCl4
c)
PCl5
d)
NaCl
24.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
25.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
26.
Who could this be?
a)
H2O
b)
NH3
c)
CO2
d)
CH4
27.

What molecular geometry would PH3 have?

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Bent

d)

Linear

28.
How many lone pairs of electrons are on the P atom in PF3?
a)
1
b)
2
c)
3
d)
0
29.
Determine the electron geometry (eg) and molecular geometry (mg) of XeF4 (Lewis structure is shown) .
a)
eg = tetrahedral, mg = tetrahedral
b)
eg = linear, mg = linear
c)
eg = octahedral, mg = square planar
d)
eg = trigonal bipyramidal, mg = tetrahedral
30.
Consider the molecule below.  Determine the molecular geometry at each of the 2 labeled carbons.
a)
C1 = tetrahedral, C2 = linear
b)
C1 = trigonal planar, C2 = bent
c)
C1 = bent, C2 = trigonal planar
d)
C1 = trigonal planar, C2 = tetrahedral
31.

Is this molecule polar?

a)

Yes

b)

No

32.

Is this molecule polar?

a)

No

b)

Yes

33.
VSEPR theory is to
a)
determine the number of bonding and lone pairs electrons
b)
determine the number of ECC
c)
determine the shape and geometry of molecule
d)
determine the lewis structure of molecule
34.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
35.
What is the measure of a tetrahedral bond angle?
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
36.
Which molecule would have this shape?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
37.
Which of the following molecular shapes would have a bond angle of 180 Degrees?
a)
Bent
b)
Trigonal Planar
c)
Tetrahedral
d)
Linear
38.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
39.
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
40.
What is the shape of H2O?
a)
linear
b)
tetrahedral
c)
bent
d)
trigonal pyramidal
41.

SiCl4 has what shape?

a)

trigonal planar

b)

pyramidal

c)

tetrahedral

d)

trigonal pyramidal

42.
VSEPR stands for ________ theory.
a)
Valence Structure of Electron Pyramids and Regression
b)
Varied Structures of Electrons Paired and Replaced
c)
Varied Shell Energy of Protons and Radiation
d)
Valence Shell Electron Pair Repulsion
43.

The shape that is made when you only have two atoms (NaCl)

a)

tetrahedral

b)

trigonal planar

c)

linear by default

d)

bent

44.

What shape would this have?

a)

Trigonal planar

b)

Pyramidal

c)

Tetrahedral

d)

Bent

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