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Ap Chem Rev Pt 2

Total questions: 52

Worksheet time: 51mins

Name
Class
Date
1.
How many significant figures does the following number have: 0.002040
a)
6
b)
4
c)
3
d)
2
2.
How many significant figures does the following number have: 100.00210
a)
7
b)
5
c)
10
d)
8
3.
Round 1047.78 to three sig figs
a)
104
b)
105
c)
1050
d)
1050.00
4.
Round 0.010229 to four sig figs
a)
1022
b)
1023
c)
0.01023
d)
0.01022
5.
What is 78.5 rounded to one significant figure?
a)
79
b)
78.5
c)
70
d)
80
6.
55.78 + 4.6 =
a)
60.28
b)
55.32
c)
56.44
d)
60.38
7.
Calculate 1.23 m x 0.89 m and give your answer with the appropriate number of significant figures.
a)
1.0 m2
b)
1.1 m2
c)
1.0947 m2
d)
1.09 m2
8.
Believed that atoms of the same element are identical to each other
a)
Bohr
b)
Rutherford
c)
Dalton
d)
Thomson
9.
What contribution did John Dalton make to atomic theory? 
a)
He discovered that every atom was positively charged. 
b)
He discovered that every element consisted of one type of atom that couldn't be divided. 
c)
He discovered that atoms had nuclei. 
d)
He discovered that atoms could be divided into smaller parts. 
10.
All matter is made of what?
a)
energy 
b)
atoms 
c)
electrons 
d)
compounds 
11.
The word atom comes from a Greek word "atomos" that means
a)
Invisible
b)
Indivisible
c)
Undivided
d)
Indestructable 
12.

The percentage of copper and oxygen in samples of “CuO” obtained by different methods were found to be the same. This illustrates the law of:

a)

Constant proportions

b)

Conservation of mass

c)

Multiple proportions

d)

Reciprocal proportions

13.

If two or more compounds are composed of the same two elements, then the ratio of the masses of the second element that is combined with a certain mass of the first element is always a ratio of small whole numbers. This statement is called the law of

a)

definite proportions.

b)

conservation of mass.

c)

atomic theory.

d)

multiple proportions.

14.

The fact that every sample of a particular chemical compound contains the same elements in exactly the same proportions by mass is known as the law of

a)

conservation of energy.

b)

conservation of mass.

c)

atomic theory.

d)

definite proportions.

15.

Isotopes are atoms of the same element that have different

a)

masses.

b)

charges.

c)

numbers of electrons.

d)

atomic numbers.

16.

Hydrogen and oxygen combine in the ratio of 1:8 by mass to form water. Calculate the mass of oxygen required in the reaction to form water if 12g of hydrogen is given.

a)

108g

b)

63g

c)

96g

d)

7g

17.

An Example of the law of multiple proportions is the existence of ________________________.

a)

FeCl3 and Fe(SO4)3

b)

O2 and O3

c)

CO and CO2

d)

FeCl2 and Fe(NO3)2

18.

12 grams of carbon react with 32 grams of oxygen to form exactly 44 grams of carbon dioxide. This is a good example of Lavoisier's:

a)

Law of Definite Proportions

b)

Atomic Theory

c)

Law of Conservation of Mass

d)

Law of Multiple Proportions

19.

What is the percentage of hydrogen in methane (CH4) if carbon is 12. g/mol and hydrogen is 1.0 g/mol

a)

33%

b)

25%

c)

8.5%

d)

6.3%

20.

A decomposition reaction yields two different results for lead and oxygen.

Compound A: 2.98 g Pb, 0.461 g O.

Compound B: 9.89 g Pb, 0.763 g O.

For a given mass of oxygen, what is the lowest whole number mass ratio of lead in the two compounds?

a)

4:1

b)

3:1

c)

2:1

d)

1:1

21.

Name the compound: N2O5.

a)

dinitrogen pentaoxide

b)

binitrogen pentaoxide

c)

nitrogen oxide

d)

pentanitrogen dioxide

22.

Name the compound: (NH4)2S

a)

ammonium sulfide

b)

nitrogen tetrahydrogen sulfide

c)

diammounium sulfate

d)

ammonium sulfate

23.

Name the compound: MgCl2

a)

magnesium chloride

b)

magnesium dichloride

c)

monomagnesium chloride

d)

manganese chloride

24.

Name the compound: Cu(NO3)2

a)

copper nitrate

b)

copper(II) nitrate

c)

copper(II) dinitrate

d)

copper dinitrogen hepaoxide

25.

Name the compound: SO3

a)

sulfur trioxide

b)

sulfite ion

c)

sulfur oxide

d)

sodium trioxide

26.

Name the compound: CF4

a)

carbon tetrafluoride

b)

monocarbon tetrafluoride

c)

carbon fluoride

d)

chlorine tetrafluoride

27.

Name the compound: P4O8

a)

tetraphosphorus octoxide

b)

phosphorus oxide

c)

tetrapotassium octoxide

d)

potassium oxide

28.

Name the compound: SF6

a)

sulfur heptafluoride

b)

sulfur hexafluoride

c)

monosulfur hexafluoride

d)

monosulfur heptafluoride

29.

Name the compound: AgNO3

a)

silver mononitrogen trioxide

b)

silver nitrate

c)

silver nitride

d)

monosilver mononitrogen trioxide

30.

Name the compound: Zn3P2

a)

zinc phosphide

b)

trizinc diphosphide

c)

zinc phosphate

d)

zinc phosphite

31.

Write the formula: potassium hydroxide

a)

KOH

b)

POH

c)

KH

d)

KO

32.

Write the formula: tetraarsenic decoxide

a)

As4O10

b)

As10O4

c)

As6O9

d)

AsO

33.

Write the formula: tin(II) phosphite

a)

Sn3(PO3)2

b)

Sn3PO8

c)

Sn2PO4

d)

Sn3(PO4)2

34.

Lithium nitride

a)

Li3N

b)

LiN

c)

Li3(NO3)2

d)

LiNO3

35.

Write the formula: lead(IV) sulfite

a)

Pb2(SO3)4

b)

Pb(SO3)2

c)

Pb2(SO4)4

d)

Pb(SO4)2

36.

Write the formula: silver chlorate

a)

AgClO3

b)

AgCl

c)

AgCLO3

d)

AgCl3

37.
Nonmetals tend to 
a)
gain electrons
b)
lose electrons
38.
Metals tend to 
a)
gain electrons
b)
lose electrons
39.

What is oxidation

a)

gaining electrons

b)

Loosing electrons

c)

sharing electronsmonosilver monofluoride

d)

non of the above

40.

What is a cation?

a)

an atom

b)

an element

c)

a positive ion

d)

a negative ion

41.

Which compound contains a polyatomic ion

a)

NaCl

b)

Ba F

c)

CaSO4

d)

K2S

42.

Which compound contains monoatomic ions

a)

Li2CO3

b)

MgO

c)

KNO3

d)

Ba3(PO4) 2

43.
Name the following ionic compound: LiNO3
a)
lithium nitrate
b)
lithium III nitrate
c)
lithium nitride
d)
lithium oxide
44.
Name the following ionic compound: MgSO4
a)
magnesium sulfoxide
b)
magnesium sulfide
c)
magnesium sulfate
d)
magnesium oxide
45.
What would be the proper chemical formula for combining Al3+ and Cl- :
a)
AlCl3
b)
Al3Cl
c)
AlCl
d)
Al3Cl3
46.
The chemical formula of iron (III)bromide is
a)
FeBr
b)
Fe(III)Br
c)
FeBr₃
d)
Fe₂Br₃
47.
When naming ionic compounds you always write the name of the positive element  _______ .
a)
first
b)
second
c)
with "ide"
d)
with a prefix
48.
In most cases, when naming you change the ending of the second element to ________.
a)
-ate.
b)
-ite.
c)
-ide.
d)
-ine.
49.
What is the formula for calcium phosphide?
a)
CaP
b)
Ca2P3
c)
Ca3P2
d)
Ca2P
50.
What is the formula for copper(I) sulfate?
a)
CuSO3
b)
CuSO4
c)
Cu2SO3
d)
Cu2SO4
51.

_________ are the substances that are produced in a chemical reaction.

a)

Reactants

b)

Producer

c)

Reaction

d)

Product

52.

________ are the starting substances in a chemical equation.

a)

Reactants

b)

Producer

c)

Reaction

d)

Products

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