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End Of Quarter 3 Test

Total questions: 101

Worksheet time: 2hrs 7mins

Name
Class
Date
1.
How do covalent bonds form?
a)

Donating & receiving valence e- between atoms.

b)

Opposite slight charges attract each other between compounds.

c)

Scientists are still not sure how they form.

d)

Sharing valence e- between atoms.

2.
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

3.
Which of the following is NOT considered a diatomic element?
a)

Carbon

b)

Nitrogen

c)

Chlorine

d)

Iodine

4.

Name the following compound:

N2O4

a)

dinitrogren tetroxide

b)

tetranitrogen dioxide

c)

nitrogen oxide

d)

dinitrogen tetraoxygen

5.
Name the following compound: 
CCl4
a)

monocarbon quadchloride

b)

carbon tetrachloride

c)

carbon chloride

d)

monocarbon quadchloide

6.

tetraphosphorus heptoxide

a)

K₄O₁₀

b)

P₄O7

c)

KO

d)

P₁₀O₄

7.

In the formation of a covalent bond, electrons are

a)

shared

b)

transferred

c)

lost

8.

How many lone pairs are in this molecule?

a)

1

b)

2

c)

3

d)

4

9.

Which of the following is an ionic compound? (metal + nonmetal)

a)

CO

b)

NH4

c)

NaCl

d)

CCl4

10.

Is this an ionic or covalent compound?

a)

Ionic

b)

Covalent

11.

Is this an ionic or covalent compound?

a)

Ionic

b)

Covalent

12.

Write the formula for this molecule

a)

Carbon Chloride

b)

Carbon Chlorine

c)

Monocarbon Tetrachloride

d)

Carbon Tetrachloride

13.

What is the formula AND name of this structure?

a)

Xenon Fluoride XeF4

b)

Xenon Tetrafluoride XeF4

c)

Monoxenon Tetrafluoride XeF4

d)

Xenon Trifluoride XeF3

14.

What does VSEPR stand for?

a)

Valence Shell Electron Repulsion Pair Model

b)

Very shiny eels pair really modestly

c)

Valence Shell Electron Pair Repulsion Model

d)

Valence Shell Electron Partial Repulsion Model

15.
Who could this be?
a)

H2O

b)

NH3

c)

CO2

d)

CH4

16.
What is the molecular shape of CH3Cl?
a)

trigonal pyramidal

b)

trigonal bipyramidal

c)

tetrahedral

d)

not enough information

17.
The bond angle for a trigonal planar molecule is 
a)

90 Degrees

b)

109.5 Degrees

c)

120 Degrees

d)

180 Degrees

18.
Who could this be? 
a)

CO2

b)

NH3

c)

H2S

d)

CH4

19.
What molecular shape is the structure shown here? (H2O)
a)

tetrahedral

b)

trigonal planar

c)

bent

d)

trigonal pyramidal

20.

Which geometry is this?

a)

Tetrahedral

b)

Octahedral

c)

Square planar

d)

Trigonal planar

21.
Which molecule would have this shape?
a)

BF3

b)

CH4

c)

PCl5

d)

CO2

22.
What is the following shape?
a)

Trigonal Pyrimidal

b)

Trigonal Planar

c)

Tetrahedral

d)

Triagonal

23.

Is this molecule polar?

a)

No

b)

Yes

24.
Will this molecule be polar or nonpolar? PH3
a)

polar

b)

nonpolar

25.
Will this molecule be polar or nonpolar? CS2
a)

polar

b)

nonpolar

26.
In a polar bond, the more electronegative element will assume a partial ________ charge.
a)

positive

b)

negative

27.
There are _____ sigma bond(s) and _____ pi bond(s) in 1 molecule of H2CO (formaldehyde).
a)

1, 2

b)

2, 3

c)

3, 1

d)

4, 0

28.
This is an example of a __________ bond.
a)

non-polar covalent

b)

polar covalent

c)

ionic

d)

metallic

29.

How many pi bonds are in the following compound?

a)

0

b)

1

c)

2

d)

5

e)

6

30.

Look at the center atom and all the atoms around it. Predict the bond type for the whole molecule.

a)

nonpolar covalent

b)

polar covalent

c)

ionic

d)

metallic

31.

In a polar covalent bond, electrons are shared:

a)

equally

b)

unequally

c)

between two metals

d)

between a metal and a non-metal

32.
Which of the following geometries could be nonpolar?
a)

bent

b)

tetrahedral

c)

trigonal pyrimidal

d)

none of the above

33.

Is this molecule polar

a)

Yes, and you draw the dipole moment pointing between the two chlorine atoms.

b)

No

c)

Yes, and you draw the dipole moment pointing between the two hydrogen atoms.

34.

How many sigma bonds are in the following molecule?

a)

0

b)

1

c)

2

d)

5

e)

6

35.

Name the following compound: XeF6

a)

Monoxenon hexafluoride

b)

Xenon fluoride

c)

Xenon hexafluoride

d)

Xenon tretrafluoride

36.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

37.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

38.

Which of the following combinations would need roman numerals in the name?

a)

potassium + fluorine

b)

beryllium + oxygen

c)

boron + iodine

d)

lead + oxygen

39.

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

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

40.
What is the correct formula for Sodium Oxide?
a)

NaO

b)

NaO2

c)

Na2O

d)

Na2O2

41.

What is the correct molecular formula for barium hydroxide?

a)

Ba(OH)2

b)

Ba2OH

c)

BaOH

d)

Ba2OH

42.
What is the formula for copper(I) sulfate?
a)

CuSO3

b)

CuSO4

c)

Cu2SO3

d)

Cu2SO4

43.

Which of these combinations is an ionic compound made of?

a)

Metal and Metal

b)

Nonmetal and Nonmetal

c)

Metal and Nonmetal

d)

Cation and Cation

44.

When naming ionic compounds with transition metals you need to include roman numerals to show the _____ of the metal..

a)

atomic number

b)

mass number

c)

charge

d)

ionization energy

45.
Which of the following is the correct name for the chemical formula Ca(NO2)2?
a)

cadmium nitride

b)

calcium nitrate

c)

calcium nitrite

d)

cadmium nitrite

46.
Metals tend to 
a)

gain electrons

b)

lose electrons

47.
Nonmetals tend to 
a)

gain electrons

b)

lose electrons

48.
If I gain electrons I become
a)

Positive because I've added to my atom

b)

negative because I've added electrons

c)

same because i'm balanced

d)

equal because now I have electrons

49.
How do the following two elements bond together?
Cr3+  O2-         
a)

CrO

b)

Cr3O2

c)

Cr2O3

d)

CrO3

50.
When a nonmetal gains electrons, it becomes this type of ion.
a)

Anion

b)

Cation

51.
When a metal loses electrons, it becomes this type of ion.
a)

anion

b)

cation

52.
What is the formula for barium phosphate?
a)

BaPO4

b)

Ba3PO3

c)

Ba3(PO4)2

d)

Ba4(PO2)3

53.

Name this acid with the formula HF

a)

hydrofluoric acid

b)

hypofluoric acid

c)

hydrogen fluorine acid

d)

fluoric acid

54.

What is the formula for hydrochloric acid?

a)

HCl

b)

HClO

c)

H3ClO3

d)

HClO3

55.

carbonic acid

a)

H2CO3

b)

H2CrO4

c)

H2C2O4

d)

HCO3

56.

H3PO4

a)

hydrophsophorus acid

b)

phosphoric acid

c)

hydrogen phosphorous

d)

phosphori hydroxide

57.
What coefficient should be used to make the following equation balanced?
N2+O2--> _NO 
a)

1

b)

2

c)

3

d)

4

58.

Which equation is balanced?

a)

PbO2 + 2H2

b)

SO2 + H20 --> H2SO4

c)

2Na + 2H2O --> 2NaOH + H2

59.
How many HCl molecules do you need to balance this equation? 
Mg +  __HCl --->  MgCl2 + H2
a)

1

b)

2

c)

3

d)

4

60.

What law governs the balancing of chemical equations?

a)

Law of Energy

b)

Law of Conservation of Matter/Mass

c)

Law of Gravity

d)

Law of Matter Movement

61.
What is the total number of atoms present in 5Na3PO4
a)

5

b)

40

c)

55

d)

8

62.

Balance this equation

_Al +_HCl --> _H2 +_AlCl3

a)

2,6,3,2

b)

it's already balanced

c)

4,12,3,4

d)

2,1,4,5

63.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__CO + __Fe2O3--> __Fe + __CO2
a)

3,1 --> 2,3

b)

3,2 --> 1,1

c)

3,2 --> 2,4

d)

3,2 --> 2,1

64.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

65.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

66.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

67.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

68.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

69.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

70.

Identify the type of chemical reaction

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

71.
Which of the following describes a precipitate?
a)

a liquid forms when a block of metal is heated

b)

a solid forms when one liquid is poured into another

c)

a gas forms when a solid is placed in a liquid

d)

bubbles form when an acid is poured on a rock

72.

What are the products of this reaction?

Cu+ AgNO3 -->

a)

Cu(NO3)2+Ag

b)

Cu + NO3 + Ag

c)

CuAg+NO3

d)

Cu+ AgNO3

73.

According to the activity series, which of the following single replacement reactions can occur?

a)

Ca + Al2(SO4)3

b)

Fe + NaOH

c)

Ni + MgSO4

d)

Al + KOH

74.
If an element is diatomic it should have a subscript of___
a)

2, always

b)

2, only when it is by itself

c)

it shouldn't have a subscript, it should have a coefficent

75.

Based on the activity series, which metal could X represent in the reaction below?

X + Ca (NO3)2 --> Ca + X (NO3)2

a)

Sr

b)

Na

c)

Mg

d)

Zn

76.
In writing a chemical equation that produces hydrogen gas, the correct representation of hydrogen gas is
a)

2H

b)

OH

c)

H

d)

H2

77.
To predict if a single replacement reaction will take place you should use a(n)
a)

Activity series

b)

Solubility Chart

c)

Periodic Table

d)

Metal chart

78.
What is the name for the solid formed during a reaction?
a)

Precipitate

b)

Rocks

c)

Bubbles

d)

Aqueous 

79.

What is the oxidation state of Cl in ClO- ?

a)

0

b)

+1

c)

-1

d)

+2

80.

What is the oxidation state of Pb in PbO ?

a)

+2

b)

+4

c)

0

d)

-2

81.

H in NaH ?

a)

+1

b)

0

c)

-1

d)

None of the above

82.
What is the oxidation number of Fe in FeO?
a)

+1

b)

-1

c)

+2

d)

-2

83.
What is the oxidation number of O in CO2?
a)

+2

b)

-1

c)

+4

d)

-2

84.
What is the oxidation of C in CH4?
a)

-4

b)

-1

c)

+4

d)

+1

85.
What is the oxidation number of Ca in Ca3N2?
a)

+3

b)

+2

c)

-3

d)

-2

86.
What is oxidation number of Cr in
Cr2O72-?
a)

-2

b)

+2

c)

+6

d)

+12

87.
What is oxidation number of P in K3PO4?
a)

+1

b)

+5

c)

-2

d)

0

88.

Oxidation number of O in its stable elemental form, O2:

a)

0

b)

-1

c)

-2

d)

+2

89.

Oxidation number of Fe in Fe2+ ion:

a)

0

b)

-2

c)

+2

d)

+3

90.
Oxygen always has an oxidation number of...
a)

-1

b)

1

c)

2

d)

-2

91.
Is calcium oxidized or reduced in the following reaction? 
2CaO--> 2Ca + O2
a)

Oxidized

b)

Reduced

92.
     In the reaction Zn + H2O --> ZnO2 + H2
 which element, if any, is oxidized? 
a)

Zinc

b)

Hydrogen

c)

Oxygen

d)

None

93.
Another name for a "oxidation-reduction" reaction is
a)

chemical reaction

b)

neutralization reaction

c)

redox reaction

d)

nuclear reaction

94.
What substance is oxidized in the following reaction?
4Fe + 3O2 --> 2Fe2O3
a)

Iron

b)

Fluorine

c)

Oxygen

95.
If an atom loses electrons during a chemical reaction, the atom was:
a)

Oxidized

b)

Reduced

c)

Neutralized

d)

Precipitated

96.
What is oxidation number of O in O2 ?
a)

0

b)

-2

c)

+1

d)

+2

97.

Which of following is incorrect about oxidation?

a)

Addition of oxygen

b)

Loss of electron

c)

Increase in oxidation state

d)

Addition of electopositive element

98.

The reduction process involves

a)

Increase in oxidation number

b)

Decrease in oxidation number

c)

No change in oxidation number

d)

Sometimes increase and sometimes decrease in oxidation number

99.

If an atom is reduced in a redox reaction, what must happen to another atom in the system?

a)

It must be oxidised.

b)

It must be reduced.

c)

It must be neutralised.

d)

Nothing needs to happen to another atom in the system.

100.

Substance that oxidizes another substance by accepting its electrons.

a)

reducing agent

b)

oxidation number

c)

combustion

d)

oxidizing agent

101.

Substance that reduces another substance by losing electrons.

a)

reducing agent

b)

half-reaction

c)

electronegative atom

d)

oxidizing agent

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