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Chemistry Bonding Review

Total questions: 42

Worksheet time: 46mins

Name
Class
Date
1.

Using a periodic table, how many unpaired electrons are in the Lewis Structure of Ga (gallium)?

a)

1

b)

2

c)

3

d)

4

e)

14

2.

How many lone pairs for P (phosphorus)?

a)

0

b)

1

c)

2

d)

3

e)

4

3.

Noble gasses have how many lone pairs?

a)

1

b)

2

c)

3

d)

4

4.

How many unpaired electrons are in a halogen?

a)

0

b)

1

c)

2

d)

3

e)

7

5.

How many lone pairs does calcium have?

a)

0

b)

1

c)

2

d)

3

6.

Carbon has how many unpaired electrons?

a)

1

b)

2

c)

3

d)

4

7.

If nitrogen lost one electron, how many electrons would it have?

a)

4

b)

5

c)

6

d)

-

e)

+

8.

In a Lewis structure, bonds typically form between

a)

Unpaired electrons

b)

Lone Pairs

c)

Like Charges

9.

If a bond forms with an electron from a lone pair, the Lewis Structure has become

a)

resonance

b)

ionic

c)

hypervalent

d)

translucent

10.

What is the definition of hypervalent?

(a)  

11.

How many bonds can carbon make?

a)

1

b)

2

c)

3

d)

4

12.

A double bond is...

a)

Two connections leading to the same atom

b)

Two connections from the same atom

c)

Both

d)

Neither

13.

In organic notation, a bond is represented by...

a)

A single dot

b)

A pair of dots

c)

A straight line

d)

A circle

14.

How many carbons?

a)

5

b)

2

c)

3

d)

4

15.

How many hydrogens are in this compound?

a)

1

b)

3

c)

4

d)

5

16.

If this was converted to a Lewis structure, how many lone pairs would there be?

a)

0

b)

2

c)

8

d)

6

17.

What is this oxygen double-bonded to?

a)

Oxygen

b)

Carbon

c)

Hydrogen

d)

Nitrogen

18.

What is the problem with forgetting lone pairs when drawing a Lewis structure?

a)

Lone pairs affect what a molecule will react with

b)

Lone pairs don't matter

c)

Lone pairs are capable of teleportation

d)

Lone pairs are unstable; having too many will break a molecule

19.

What kind of bond has electrons that don't belong to any particular atom?

a)

Hydrogen bonding

b)

Covalent

c)

Ionic

d)

Metallic

20.

What kind of bond has electrons that belong to an atom but are shared with a different atom?

a)

Hydrogen bonding

b)

Covalent

c)

Ionic

d)

Metallic

21.

What kind of bond has electrons that belong to an atom but have been stolen by an electronegative atom?

a)

Hydrogen bonding

b)

Covalent

c)

Ionic

d)

Metallic

22.

What kind of bond has a hydrogen's electron being fought over by two electronegative atoms?

a)

Hydrogen bonding

b)

Covalent

c)

Ionic

d)

Metallic

23.

What kind of bonding is this?

a)

Covalent

b)

Hydrogen

c)

Ionic

d)

Metallic

24.

What kind of bonding is this?

a)

Covalent

b)

Hydrogen

c)

Ionic

d)

Metallic

25.

What kind of bonding is this?

a)

Covalent

b)

Hydrogen

c)

Ionic

d)

Metallic

26.

Which of the following isn't electronegative enough to participate in hydrogen bonding?

a)

O

b)

C

c)

F

d)

N

27.

Which of the following shapes is used by an atom with four other atoms bonded to it?

a)
b)
c)
d)
28.

Methane, CH4, will likely take what shape?

a)
b)
c)
d)
29.

Sulfur hexafluoride (SF6) will likely take what shape?

a)
b)
c)
d)
30.

What shape is octahedral?

a)
b)
c)
d)
31.

Water has what shape?

a)

Linear

b)

Tetrahedral

c)

Bent

d)

Octahedral

32.

Ammonia (NH3) has what shape?

a)

Bent

b)

Tetrahedral

c)

Trigonal Pyramidal

d)

Trigonal Planar

33.

Carbon dioxide has what shape?

a)

Linear

b)

Bent

c)

Curved

d)

Trigonal Planar

34.

What is the name of this VSEPR shape?

a)

Linear

b)

Bent

c)

Tetrahedral

d)

Trigonal Planar

35.

What is the name of this VSEPR shape?

a)

Trigonal Planar

b)

T-shaped

c)

Trigonal pyramidal

d)

Trigonal Bipyramidal

36.

What charge is arsenic most likely to create (that is, which charge gets it to noble gas configuration)?

a)

+1

b)

-1

c)

+5

d)

-3

e)
37.

If this element ionizes to reach noble gas configuration, how many electrons will it lose?

a)

8

b)

7

c)

2

d)

1

38.

If this element lost all its valence electrons, what charge would it have?

a)

+1

b)

-1

c)

+2

d)

-2

39.

If this element ionized to reach noble gas configuration, what charge would it have?

a)

+1

b)

-1

c)

+2

d)

-2

40.

If this atom lost all its valence electrons, what charge would it have?

a)

+1

b)

+3

c)

+5

d)

+7

41.

A covalent bond forms between a(n) ___ and a(n) ___ atom

a)

highly electronegative; low electronegative

b)

highly electronegative; highly electronegative

c)

low electronegative; low electronegative

d)

Electronegativity cannot predict bonding type

42.

A metallic bond forms between a(n) ___ and a(n) ___ atom

a)

highly electronegativity; low electronegativity

b)

highly electronegativity; highly electronegativity

c)

low electronegativity; low electronegativity

d)

Electronegativity cannot predict bonding type

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