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GC Chapter 8 Bonding

Total questions: 35

Worksheet time: 3hrs 55mins

Name
Class
Date
1.
Which of the following has a full valence shell?
a)
Oxygen
b)
Neon
c)
Barium
d)
Carbon
2.
An ionic bond forms when atoms ___________ electrons.
a)
gain
b)
share
c)
increase
d)
transfer
3.
Which type of bond has an equal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
4.
Which type of bond has an unequal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
5.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
6.
What is the number of valence electrons for Oxygen?
a)
8
b)
6
c)
2
d)
1
7.
How many valence electrons in this structure?
a)
6
b)
5
c)
4
d)
7
8.
Atoms joined together by SHARING electrons are?
a)
Ionic bonds
b)
Covalent bonds
c)
Metallic Bonds
d)
James Bonds
9.
Covalent bonds tend to happen between two
a)
metals
b)
nonmetals
c)
metal and nonmetal
10.
Outer shell electrons are called
a)
outer electrons
b)
valence electrons
c)
negatives
11.
Atoms want
a)
A full outer shell of electrons
b)
One electron short of a full shell
c)
kit kats
12.
How many more electrons are needed to fill an outermost energy level of a Carbon atom?
a)
its already full, 0 needed
b)
2
c)
4
d)
carbon is a nonmetal, it has no electrons
13.
How many more valence electrons does Oxygen need to be stable?
a)
6
b)
2
c)
4
d)
It's already stable with 8
14.
Valence electrons are the...
a)
Innermost electrons
b)
Middle electrons
c)
Outermost electrons
d)
Any electrons
15.

How many valence electrons does carbon have?

a)

4

b)

5

c)

6

d)

7

16.

USE THE PERIODIC TABLE

How many valence electrons does sodium have?

a)

1

b)

2

c)

3

d)

4

17.

USE THE PERIODIC TABLE

How many valence electrons does Phosphorus have?

a)

31

b)

5

c)

15

d)

4

18.
How many valence electrons are in an atom of Ba?
a)
2
b)
8
c)
4
d)
1
19.
How many electrons should Lithium have around its Lewis dot model?
a)
1
b)
2
c)
3
d)
4
20.
How many electrons should Flourine have around its Lewis dot model?
a)
5
b)
6
c)
7
d)
8
21.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
22.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
23.

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

a)

8

b)

4

c)

2

d)

3

24.

NH3 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

25.

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

26.

How many valence electrons does Hydrogen 'want' to have?

a)

1

b)

2

c)

8

d)

6

27.

Which of the following elements are exceptions to the octet rule? (more than one answer possible)

a)

Carbon

b)

Beryllium

c)

Boron

d)

Hydrogen

28.

How do you determine if a bond is polar covalent or nonpolar covalent?

a)

Guess

b)

Add the electronegativites of the two atoms

c)

Subtract the electronegativities of the two atoms

d)

Look for perfect symmetry. If the molecule is symmetrical, the bonds are nonpolar.

29.

How do you determine if a molecule is polar or nonpolar?

a)

Guess

b)

Add the electronegativities of all the atoms

c)

Subtract the electronegativities of all the atoms

d)

Look for perfect symmetry. If the atom has perfect symmetry, it is nonpolar.

30.
Choose the correct shape for this molecule:
a)
linear
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
31.

Determine the molecular geometry of the given structure.

a)

Trigonal Pyramidal

b)

Trigonal Bipyramidal

c)

Trigonal Planar

d)

Tetrahedral

32.

What is the geometry of this molecule?

a)

linear

b)

trigonal planar

c)

trigonal pyramid

d)

bent of angular

33.

What is the geometry of this molecule?

a)

trigonal pyramid

b)

linear

c)

bent

d)

angular

34.
What is the shape of H2O?
a)
linear
b)
tetrahedral
c)
bent
d)
trigonal pyramidal
35.

What is the molecular geometry of CO2?

a)

Bent

b)

Trigonal planar

c)

Trigonal pyramidal

d)

Linear

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