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Chemistry Test #3 Review

Total questions: 85

Worksheet time: 3hrs 7mins

Name
Class
Date
1.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
2.
What do atoms that form positive ions tend to do?
a)
Tend to lose electrons 
b)
Tend to lose protons
c)
Tend to gain electrons
d)
Tend to gain protons
3.
What usually forms the positive ion?
a)
Metal
b)
Non Metals
c)
None
4.
What usually forms the negative ion?
a)
nonmetals
b)
metal
c)
none
5.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
6.
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
7.
What happens when an atom loses an electron?
a)
Neutral (no charge)
b)
Positive charge
c)
Negative charge
8.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
9.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 or more nonmetals
c)
metal
d)
none of the above
10.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
c)

Metallic

11.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
c)

Metallic

12.
Predict the bond that will form between Sr and S.
a)
Ionic
b)
Covalent
c)

Metallic

13.
Copper (II) oxide
a)
Ionic
b)
Covalent
c)

Metallic

14.
Carbon dioxide
a)
ionic 
b)
covalent
c)

Metallic

15.

Silver (I) Nitride

a)
ionic 
b)
covalent
c)

Metallic

16.

Predict the bond that will form between Pb and Sn.

a)
Ionic
b)
Covalent
c)

Metallic

17.
If Magnesium (Mg+2) and Fluorine (F-1)  form an ionic bond, what is the chemical formula for that compound?
a)
Mg2F
b)
MgF2
c)
F2Mg3
18.
What is the chemical formula for copper (II) oxide?
a)
CuO
b)
Cu2O
c)
CuO2
19.
What is the chemical formula for carbon tetrachloride?
a)
CCl
b)
C4Cl
c)
CCl4
20.
What is the name of PF3?
a)
Monophosphorous trifluoride
b)
Phosphorous fluoride
c)
Phosphorous trifluoride
d)
Monophosphorous fluoride
21.

Cu and Cu bonds

a)
Ion
b)
Ionic bonding
c)
Metallic bonding
d)
Covalent bonding
22.
Which makes a double bond?
a)

N2

b)

CO

c)

Cl2

d)

O2

23.
Which makes a triple bond?
a)

nitrogen gas

b)
carbon dioxide
c)

chlorine gas

d)

oxygen gas

24.
How many electrons are shared in a double bond?
a)
2
b)
4
c)
6
d)
8
25.
Which is polar?
a)
water
b)
carbon dioxide
c)
chlorine
d)
methane
26.
Geometry of carbon dioxide
a)
linear
b)
bent
c)
trigonal planar
d)
trigonal pyramidal
27.
Geometry of methane
a)
linear
b)
tetrahedral
c)
trigonal planar
d)
trigonal pyramidal
28.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
29.
What do we call a covalent bond where electrons are shared UNEVENLY or UNEQUALLY?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
30.

If a molecule contains polar bonds, the molecule MUST be polar overall. 

a)
True 
b)
False
31.

In a POLAR bond, one atom pulls on the shared electrons more than the other atom. 

a)
True
b)
False
32.

Molecules with three bonds like this have this shape:

a)
linear
b)
trigonal planar
c)
trigonal pyramid
d)
bent of angular
33.

Molecules that have two shared pairs have this shape:

a)
trigonal pyramid
b)
linear
c)
bent
d)
angular
34.
Choose the correct shape for this molecule:
a)
Bent
b)
Linear
c)
Tetrahedral
d)
Trigonal pyramidal
35.
Electronegativity is a measurement of the ability of a nucleus to...
a)
attract bonding electrons
b)
attract other nuclei
c)
attract elenece in the non-valence energy levels
36.
In general, substances with stronger intermolecular forces have ___________  boiling points than those with weaker intermolecular forces
a)
higher
b)
lower
37.
How many electrons should Oxygen have around its Lewis dot model?
a)
5
b)
6
c)
7
d)
8
38.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
39.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
40.
In the correct Lewis structure for CH4, how many unshared electron pairs surround the carbon?
a)
2
b)
8
c)
0
d)
4
41.
This is the correct dot diagram for sodium (Na)
a)
true
b)
false
42.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
43.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
44.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
45.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core 
c)
Valence
d)
Stable
46.
Each line in a Lewis Structure represents __________ electron(s).
a)
3
b)
2
c)
1
d)
4
47.
The theory that is used to predict the arrangement of atoms about a central atom is called?
a)
Valence shell repulsion
b)
Valence shell electron sharing
c)
Valence shell electron pair repulsion
d)
Valence electron shell repulsion pair
48.
 Lone electron pairs in a molecule...
a)

never exist

b)

are lost in space

c)

creates an isotope

d)

repel the bonded atoms

49.
What is the correct name for C4H6?
a)
Carbon Hexahydride
b)
Pentacarbon Pentahydride
c)
Hexacarbon Tetrahydride
d)
Tetracarbon Hexahydride
50.
What is the formula for Tricarbon Octahydride?
a)
Ca3O
b)
C2H8
c)
C3H8
d)
Ca3H8
51.
Phosphorous trichloride
a)
PCl3
b)
P3Cl
c)
P3Cl3
d)
PCL
52.
P2O5
a)
Phosphorus Oxide
b)
Pentaphosphorus Dioxide
c)
Diphosphorous pentoxide
d)
Phosphoric Oxygen
53.

Which of the following is the chemical formula for sulfur hexachloride?

a)

SCl6 

b)

S6Cl

c)

S6Cl6

d)

S1Cl6

54.

Name the ionic compound SnSe2

a)

Tin diselenide

b)

Tin (IV) Selenide

c)

Tin selenide

d)

Tin (II) triselenide

55.

Name the following ionic compound: Cs2S

a)

cesium sulfide

b)

cesium sulfate

c)

cesium (II) sulfate

d)

cesium (II) sulfide

56.

Name the following ionic compound: BeCl2

a)

beryllium chlorine

b)

beryllium (II) chloride

c)

beryllium chloride

d)

beryllium dichloride

57.

When naming a compound, which of these is written first?

a)

Metal

b)

Nonmetal

c)

Anion

d)

Cation

58.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

59.

What is the name of the compound Sc(OH)3?

a)

Scandium (III) hydroxide

b)

Scandium (I) hydroxide

c)

Scandium (II) hydroxide

d)

Scandium hydroxide

60.

The name of the compound Ca3(PO4)2

a)

calcium phosphate

b)

tricalcium diphosphate

c)

calcium phosphorus oxide

d)

calcium phosphide

61.

How many Hydrogen atoms are in 4H2O?

a)

6

b)

8

c)

2

d)

4

62.

How many Magnesium atoms are in 10MgCl2?

a)

10

b)

5

c)

20

63.

How many atoms are there TOTAL in H2SO4 ?

a)

6

b)

5

c)

7

d)

3

64.

How many Nitrogen atoms are in (NH₄)₂CrO₄?

a)

1

b)

2

c)

8

d)

16

65.

How many Oxygen atoms are in Al₂(SO₄)₃?

a)

4

b)

12

c)

7

d)

24

66.

A subscript is the small number below the element symbol that tells the number of _______ of that element.

a)

atoms

b)

valence electrons

c)

protons

d)

elements

67.

How many Aluminum atoms are in Al2O3?

a)

3

b)

2

c)

5

d)

1

68.

How many atoms are present if there is no subscript following the element symbol?

a)

0

b)

2

c)

only 1

d)

1 million

69.

What is the oxidation state of Cl in CaCl2 ?

a)

0

b)

+1

c)

-1

d)

+2

70.

What is the oxidation state of Cu in Cu2+?

a)

-1

b)

-2

c)

+2

d)

0

71.

What is the oxidation state of Pb in PbO ?

a)

+2

b)

+4

c)

0

d)

-2

72.
What is the oxidation number of Fe in FeO?
a)
+1
b)
-1
c)
+2
d)
-2
73.

What is the oxidation number of Be in BeO?

a)

+2

b)

-1

c)

+4

d)

-2

74.

What is the basis of a metallic bond?

a)

the attraction of neutral metal atoms.

b)

the attraction between protons and neutrons.

c)

the attraction between positive metal ions and interlocking electrons.

d)

the attraction between positive metal ions and free moving electrons.

75.

The dashed lines represent

a)

hydrogen bonds

b)

covalent bonds

c)

ionic bonds

d)

delta

76.

A molecule that has a partial positive end and a partial negative end because of unequal sharing of electrons is a _______________.

a)

nonpolar molecule

b)

polar molecule

c)

ionic compound

d)

metalic compound

77.

Polar molecules have

a)

no charges.

b)

slight positive and negative charges on opposite ends of the molecules.

c)

only positive charges.

d)

either positive or negative charges, but not both.

78.

Phosphorus has an electronegativity value of 2.1. Chlorine's electronegativity value is 3.0. What type of bond will these two elements form?

a)

ionic

b)

nonpolar covalent

c)

polar covalent

d)

metallic

79.
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
80.

Calculate ΔEN for Pb-S

a)

1.1

b)

-0.6

c)

0.6

d)

4.4

81.

Calculate ΔEN for Na-Br

a)

1.9

b)

0.9

c)

2.8

d)

1.0

82.

SiCl4 is a ______ molecule.

a)

polar

b)

non-polar

83.

H2O is a _____ molecule.

a)

polar

b)

non-polar

84.

HCl is a _____ molecule.

a)

polar

b)

non-polar

85.

H2 is a ____ molecule.

a)

polar

b)

non-polar

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