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DC CHEM - UNIT 4 REVIEW

Total questions: 67

Worksheet time: 6hrs 35mins

Name
Class
Date
1.

Which of the below is an ionic compounds?

a)

Ni

b)

MgCl2

c)

H2O

d)

CH4

2.

Ionic bonds are formed between...

a)

Non - metals

b)

A metal and a non-metal

c)

Metals

3.

How is an ionic bond formed?

a)

Sharing of electrons

b)

Delocalised electrons

c)

Transfer of electrons

4.

An example of an ionic compound is Sodium Chloride, which is made from Na+ and Cl- ions. Why do these ions form an ionic bond?

a)

They have like charges

b)

They are from the same group

c)

They are from the same period

d)

They have opposite charges

5.
In the chemical formula for an ionic compound, which item is written first?
a)
positive ion
b)
negative ion
c)
subscript
d)
the female
6.

Which properties are all characteristics of ionic compounds?

a)

solids with high melting and boiling points

b)

soft solids which are highly malleable

c)

when solid, the ions are held in place so the compounds cannot conduct electricity

d)

conduct electricity when dissolved or molten

7.

What is the correct formula for aluminium oxide? Aluminium is in group 3 and oxygen is in group 6.

a)

Al₂O₃

b)

AlO

c)

AlO₄

d)

Al₂O

e)

Al₃O₂

8.
what type of bond is the strongest
a)
single
b)
Double
c)
coordination
d)
triple
9.
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
10.
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
11.
How many are shared in a single bond?
a)
2 pairs
b)
4
c)
2
d)
1
12.
How many are shared in a double bond?
a)
2
b)
4 pairs
c)
6
d)
4
13.
How many electrons are shared in a triple bond?
a)
6
b)
3
c)
6 pairs
d)
5
14.
Name the following compound: 
CO2
a)
monocarbon dioxide
b)
carbon oxide
c)
carbon dioxide
d)
oxygen carbonide
15.
How many valence electrons does oxygen have?
a)
2
b)
3
c)
6
d)
4
16.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
17.
How many valence electrons does hydrogen have?
a)
4
b)
3
c)
2
d)
1
18.
What is it called if there are three-pairs of electrons being shared?
a)
Triple bond
b)
Bond length
c)
Tribond
d)
Chocolate Mousse
19.
Atoms want
a)
A full outer shell of electrons
b)
One electron short of a full shell
c)
kit kats
20.
Outer shell electrons are called
a)
outer electrons
b)
valence electrons
c)
negatives
21.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
22.

How many valence electrons does Tin (Sn) have?

a)

8

b)

7

c)

5

d)

4

23.

According to the diagram below, how many bonds will this atom be able to make?

a)
1
b)
2
c)
3
d)
4
24.

Which of these is incorrect?

a)
b)
25.

Which of these is correct?

a)
b)
c)
26.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
27.

This atom would be considered stable.

a)

False

b)

True

28.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
29.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
30.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
31.

NH3 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

32.

3. Which is a correct Lewis structure for hydrogen cyanide, HCN?

a)
b)
c)
d)
33.

Why is this Lewis Structure incorrect? Choose all that apply.

a)

There are too many bonds around Si.

b)

There should only be single bonds in this Lewis Structure.

c)

The Structure is missing a triple bond.

d)

Chlorine only has 6 electrons surrounding it.

34.

What shape would CH4 have?

a)

Trigonal planar

b)

Pyramidal

c)

Tetrahedral

d)

Bent

35.
What is the best explanation of VSEPR theory?
a)

It explains the shapes that electrons make around atoms when they repel

b)

It explains how many electrons fit into an element's valent shell

c)

It explains why electrons pair up

d)

It explains why electrons repel each other

36.
Who could this be? 
a)

CO2

b)

NH3

c)

H2S

d)

CH4

37.
Who could this be?
a)

H2O

b)

NH3

c)

CO2

d)

CH4

38.

The atoms in a molecule of water adopt what kind of molecular geometry?

a)

Linear

b)

Tetrahedral

c)

Bent

d)

Trigonal planar

39.
Choose the correct shape for this molecule:
a)

linear

b)

Trigonal pyramidal

c)

Bent

d)

Tetrahedral

40.
Which formula represents a nonpolar molecule?
a)

HBr

b)

H2S

c)

CBr4

d)

PCl3

41.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

42.
In covalent bonds, electrons are ___________.
a)

transferred

b)

gained

c)

lost

d)

shared

43.
In this Lewis structure, the symbol above F means...
a)

electrons are being transferred to Fluorine

b)

electrons are less attracted to F than H

c)

electrons are more attracted to F than H

d)

Fluorine has formed a cation

44.

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

a)

nonpolar; equally

b)

polar; equally

c)

nonpolar; unequally

d)

nonpolar; unequally

45.

CO2 is...

a)

polar

b)

nonpolar

46.

Water is...

a)

polar

b)

nonpolar

47.

CF4 is...

a)

polar

b)

nonpolar

48.

Carbon monoxide, a deadly gas, has a chemical formula of CO (one carbon atom with one oxygen atom). If you look at the total atomic mass of CO, does carbon or oxygen make up more of the mass?

a)

carbon

b)

oxygen

c)

they are exactly the same

d)

it is impossible to tell

49.

What percentage of the total atomic mass of carbon monoxide (CO) is composed of carbon?

a)

29%

b)

43%

c)

57%

d)

73%

50.

What percentage of the total atomic mass of carbon monoxide (CO) is composed of oxygen?

a)

29%

b)

43%

c)

57%

d)

73%

51.

What percentage of the total atomic mass of magnesium bromide (MgBr2) is composed of magnesium?

a)

13%

b)

43%

c)

63%

d)

87%

52.

What percentage of the total atomic mass of calcium nitrate (Ca(NO3)2) is composed of nitrogen? Hint - another way to think of calcium nitrate is Ca(NO3)(NO3).

a)

17%

b)

24%

c)

29%

d)

59%

53.
A formula with the lowest whole # ratio of elements in a compound is called
a)

Molecular Formula

b)

Chemical Formula

c)

Empirical Formula 

d)

Distance Formula

54.

What is the empirical formula for C4H6?

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

55.

What is the empirical formula for N2S3?

a)

NS

b)

N3S2

c)

N2S3

d)

N1S1.5

56.
Which pair has the same empirical formula?
a)

NaCrO4 and Na2Cr2O7

b)

C2H4O2 and C6H12O6

c)

C3H6O3 and C2H6O2

d)

CH4 and C2H6

57.

What is the first step in calculating empirical formula?

a)

convert grams to moles

b)

change percent to grams

c)

divide by smallest number of moles

d)

multiply 'til whole

58.

How many moles are in 83.65 g of carbon?

a)

1,003.8

b)

6.965

c)

501.9

d)

83.65

59.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.
a)
SO
b)
SO2
c)
SO3
d)
SO4
60.

A formula with the lowest whole # molar ratio of elements in a compound is called

a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
61.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.
a)
SO
b)
SO2
c)
SO3
d)
SO4
62.
What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180.18?
a)
CH2O
b)
C2H4O2
c)
C4H8O4
d)
C6H12O6
63.
Which one is an empirical formula?
a)
H2O2
b)
C2H6O12
c)
CaCl2
d)
N2O8
64.

Glycerol has a molecular molar mass of 92.09g/mol. The empirical formula is C3H8O3. What is the molecular formula for glycerol?

a)
C2H3O2
b)
CH2O
c)
C2H4O2
d)
C3H8O3
65.

A sample contains 36.95 g of mercury (Hg) and 13.05 g of chlorine (Cl). What is the empirical formula for this compound?

a)

HgCl2

b)

Hg3Cl

c)

Hg17Cl36

d)

HgCl

66.
What is the empirical formula for C3H8
a)
CH
b)
C3H8
c)
C6H16
d)
CH2.7
67.

The Empirical Formula for a substance is CF2. The Molecular formula mass is 200. g/mol. What is the Molecular formula?

a)
C4F8
b)
C4F
c)
CF8
d)
C2F4

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