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Module 3 Review

Total questions: 85

Worksheet time: 2hrs 34mins

Name
Class
Date
1.

Name the compound: N2O5.

a)

dinitrogen pentaoxide

b)

binitrogen pentaoxide

c)

nitrogen oxide

d)

pentanitrogen dioxide

2.

Name the compound: (NH4)2S

a)

ammonium sulfide

b)

nitrogen tetrahydrogen sulfide

c)

diammounium sulfate

d)

ammonium sulfate

3.

Name the compound: MgCl2

a)

magnesium chloride

b)

magnesium dichloride

c)

monomagnesium chloride

d)

manganese chloride

4.

Name the compound: Cu(NO3)2

a)

copper nitrate

b)

copper(II) nitrate

c)

copper(II) dinitrate

d)

copper dinitrogen hepaoxide

5.

Name the compound: SO3

a)

sulfur trioxide

b)

sulfite ion

c)

sulfur oxide

d)

sodium trioxide

6.

Name the compound: CF4

a)

carbon tetrafluoride

b)

monocarbon tetrafluoride

c)

carbon fluoride

d)

chlorine tetrafluoride

7.

Name the compound: P4O8

a)

tetraphosphorus octoxide

b)

phosphorus oxide

c)

tetrapotassium octoxide

d)

potassium oxide

8.

Name the compound: SF6

a)

sulfur heptafluoride

b)

sulfur hexafluoride

c)

monosulfur hexafluoride

d)

monosulfur heptafluoride

9.

Name the compound: AgNO3

a)

silver mononitrogen trioxide

b)

silver nitrate

c)

silver nitride

d)

monosilver mononitrogen trioxide

10.

Name the compound: Zn3P2

a)

zinc phosphide

b)

trizinc diphosphide

c)

zinc phosphate

d)

zinc phosphite

11.

Write the formula: potassium hydroxide

a)

KOH

b)

POH

c)

KH

d)

KO

12.

Write the formula: tetraarsenic decoxide

a)

As4O10

b)

As10O4

c)

As6O9

d)

AsO

13.

Write the formula: iodine heptafluoride

a)

IF7

b)

I2F14

c)

IHF7

d)

IF6

14.

Write the formula: nitrogen trichloride

a)

NCl3

b)

N1Cl3

c)

N1Cl5

d)

Cl3N

15.

Write the formula: carbon monoxide

a)

CO

b)

CO2

c)

OC

d)

C2O4

16.

Write the formula: tin(II) phosphite

a)

Sn3(PO3)2

b)

Sn3PO8

c)

Sn2PO4

d)

Sn3(PO4)2

17.

Lithium nitride

a)

Li3N

b)

LiN

c)

Li3(NO3)2

d)

LiNO3

18.

Write the formula: lead(IV) sulfite

a)

Pb2(SO3)4

b)

Pb(SO3)2

c)

Pb2(SO4)4

d)

Pb(SO4)2

19.

Write the formula: silver chlorate

a)

AgClO3

b)

AgCl

c)

AgCLO3

d)

AgCl3

20.

Write the formula: beryllium oxide

a)

BO

b)

BeO

c)

BeO2

d)

BO2

21.

Have a high melting point (1000°C-3000°C)

a)

ionic compounds

b)

covalent compounds

22.

Have a low melting point (< 200°C)

a)

ionic compounds

b)

covalent compounds

23.
usually hard but brittle
a)
ionic compounds
b)
covalent compounds
24.
usually soft
a)
ionic compounds
b)
covalent compounds
25.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
26.

Which of the following describes covalent bonds?

a)

Bonds form because of opposite charges

b)

electrons are shared to fill outer electron shells

c)

Electrons are transferred between atoms

d)

Covalent bonds are magical

27.

Which of the following is TRUE about ionic compounds?

a)

They have low melting and boiling points.

b)

They can conduct electricity in the solid state.

c)

They are stronger than covalent bonds.

d)

They are usually formed from 2 metals.

28.

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

29.

Compounds composed of a ______________ and _____________ like the compound CaCl2 , are ionic compounds.

a)

metal ... metal

b)

nonmetal ... nonmetal

c)

metal ... nonmetal

30.

Always dissolves in water

a)

ionic compound

b)

covalent compound

31.

The electrons in a polar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

32.

The electrons in a nonpolar covalent molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

33.

The electrons in an ionic molecule are shared...

a)

Evenly

b)

Unevenly

c)

Electrons are not shared

d)

None of the Above

34.

In a polar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

35.

In a nonpolar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

36.

In an ionic bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity Only

b)

The atom with the Lowest Electronegativity Only

c)

The atom with the Greatest Electronegativity Mostly

d)

The atom with the Lowest Electronegativity Mostly

37.

The polarity of a bond is determined by...

a)

The sum of the electronegativities of the two atoms

b)

The difference in the electronegativities of the two atoms

c)

The charges of the atoms

d)

None of the Above

38.

Partial charges are present in which type of bond?

a)

Ionic

b)

Nonpolar Covalent

c)

Polar Covalent

d)

Both Polar Covalent and Ionic

39.

Molecules that contain whole number charges on atoms (+1,-3, etc.) must be...

a)

Polar Covalent

b)

Nonpolar Covalent

c)

Ionic

d)

Polar Covalent or Ionic

40.

In a polar covalent bond, which atom will have a partial positive charge? (choose 2 correct answers)

a)

The atom that attracts fewer electrons

b)

The atom with the greater electronegitivity

c)

The atom that attracts more electrons

d)

The atom with the lower electronegativity

41.

What must the difference in electronegativity between two atoms be in order for the bond between them to be polar covalent?

a)

less than 0.5

b)

greater than 1.7

c)

between 0.5 and 1.7

d)

exactly 0

42.

What must the difference in electronegativity between two atoms be in order for the bond between them to be nonpolar covalent?

a)

less than 0.5

b)

greater than 1.7

c)

between 0.5 and 1.7

d)

exactly 0

43.

A diatomic molecule like O2 is always _____ because electrons are shared _____

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

44.

Order the types of bonds based on the charge of their molecules. (lowest amount of charge to greatest)

a)

Polar Covalent --> Ionic --> Nonpolar Covalent

b)

Ionic --> Nonpolar Covalent --> Polar Covalent

c)

Ionic --> Polar Covalent --> Nonpolar Covalent

d)

Nonpolar Covalent --> Polar Covalent --> Ionic

45.
How many valence electrons are in an atom of Se?
a)
2
b)
8
c)
6
d)
5
46.
How many valence electrons are in an atom of Ba?
a)
2
b)
8
c)
4
d)
1
47.
How many valence electrons are in an atom of Ar?
a)
2
b)
8
c)
4
d)
1
48.
How many valence electrons are in an atom of In?
a)
3
b)
8
c)
4
d)
1
49.
How many valence electrons are in an atom of K?
a)
3
b)
8
c)
4
d)
1
50.
How many valence electrons are in an atom of Sn?
a)
3
b)
8
c)
4
d)
1
51.
How many valence electrons are in an atom of P?
a)
4
b)
5
c)
2
d)
3
52.
How many valence electrons are found in atoms of group 1?
a)
7
b)
6
c)
4
d)
1
53.
How many valence electrons are found in atoms of group 15?
a)
4
b)
5
c)
2
d)
3
54.

How many valence electrons does an element with this electron configuration have?


1s22s22p63s1


(Only enter whole-number answers)

(a)  

55.

How many valence electrons does an element with this electron configuration have?


1s22s22p63s2


(Only enter whole-number answers)

(a)  

56.

How many valence electrons does an element with this electron configuration have?


1s22s22p63s23p1


(Only enter whole-number answers)

(a)  

57.

How many valence electrons does an element with this electron configuration have?


1s22s22p63s23p2


(Only enter whole-number answers)

(a)  

58.

How many valence electrons does an element with this electron configuration have?


1s22s22p63s23p3


(Only enter whole-number answers)

(a)  

59.

How many valence electrons does an element with this electron configuration have?


1s22s22p63s23p4


(Only enter whole-number answers)

(a)  

60.

How many valence electrons does an element with this electron configuration have?


1s22s22p63s23p5


(Only enter whole-number answers)

(a)  

61.

How many valence electrons does an element with this electron configuration have?


1s22s22p63s23p6


(Only enter whole-number answers)

(a)  

62.

What are valence electrons?

a)

The total number of electrons in an atom

b)

The number of electrons in the outermost shell

c)

The number of electrons in the second shell

d)

The number of protons in the outermost shell

63.
a)
2
b)
8
c)
3
d)
13
64.
a)
2
b)
3
c)
5
65.

How many valence electrons does carbon have?

a)

4

b)

5

c)

6

d)

7

66.
a)
12
b)
7
c)
8
d)
14
67.
a)
7
b)
8
c)
9
d)
10
68.
Which of the following is an example of a COVALENT COMPOUND?
a)
H2S
b)
KI
c)
CaCl2
d)
MgO
69.

Which of the following is NOT covalently bonded?

a)

K2S

b)

H2O

c)

I2

d)

CO2

70.

Which pair of atoms is most likely to form a covalent molecule?

a)

Hydrogen and lithium

b)

Phosphorus and sulfur

c)

Helium and neon

d)

Zinc and Boron

71.

What are the seven diatomic elements?

a)

H2, Cl2, Br2, O2, N2, I2, F2

b)

H2, Cl2, I2, F2, Hg2, Br2, Fe2

c)

H2, Cu2, Ni2, B2, O2, I2, Fe2

72.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
73.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
74.
How many electrons does each line indicate are shared?
a)
1
b)
2
c)
3
d)
4
75.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
76.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

77.

What is the goal of the Lewis Dot Structure?

a)

To determine the electron position.

b)

To show the element's valence electrons & bonding capabilities.

c)

To find the atomic mass of an element.

d)

To search for the number of electrons in an individual atom.

78.

This is a correct dot diagram for neon (Ne)

a)

true

b)

false

79.
This is the correct dot diagram for nitrogen, group 15.
a)
true
b)
false
80.

This is a correct dot diagram for nitrogen (N)

a)

true

b)

false

81.

This is a correct dot diagram for carbon (C)

a)

true

b)

false

82.
This could be the dot diagram of
a)
O
b)
B
c)
Li
d)
Ne
83.
This could be the dot diagram of 
a)
Ne
b)
Si
c)
Al
d)
Be
84.

How would you draw a Lewis dot diagram for Magnesium?

a)
b)
c)
d)
85.

Which of the following shows a correct Lewis dot structure?

a)
b)
c)
d)

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