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Final Practice

Total questions: 91

Worksheet time: 3hrs 5mins

Name
Class
Date
1.
How many significant figures: 216 m
a)
1
b)
2
c)
3
d)
0
2.
How many significant figures: 2016 m
a)
1
b)
2
c)
3
d)
4
3.
How many significant figures: 153.0 mL
a)
1
b)
2
c)
3
d)
4
4.
How many significant figures: 0.012 km
a)
1
b)
2
c)
3
d)
4
5.
How many significant figures: 1000 mL
a)
1
b)
2
c)
3
d)
4
6.
How many significant figures: 100.000 cL
a)
1
b)
3
c)
5
d)
6
7.
How many significant figures: 0.001 g
a)
4
b)
3
c)
2
d)
1
8.
How many significant figures: 4.20 cm
a)
1
b)
2
c)
3
d)
4
9.
How many significant figures: 0.010 L
a)
1
b)
2
c)
3
d)
4
10.

How many significant figures: 450 m

a)

3

b)

2

c)

1

d)

0

11.
How many sig figs are there?
100000000
a)
1
b)
9
c)
10
12.

3.05 + 0.013

a)

3.063

b)

3.06

c)

3.1

d)

3

13.

432.521 + 3.50

a)

436.021

b)

436.02

c)

436.0

d)

436

14.

340.123 - 63.02

a)

277.103

b)

277.10

c)

277.1

d)

277

15.

100 + 30.6

a)

130.6

b)

131

c)

130

d)

100

16.

5.9 x 6.01

a)

35.459

b)

35.46

c)

35.5

d)

35

17.

7.8 x 5.501

a)

42.9078

b)

42.908

c)

42.91

d)

42.9

e)

42

18.

2.1/5.1

a)

0.4118

b)

0.412

c)

0.41

d)

0.40

19.

0.9/2.3

a)

0.391

b)

0.39

c)

0.40

d)

0.4

20.

Convert 2.38 meters to millimeters.

a)

2380 mm

b)

0.2380 mm

c)

23.8 mm

d)

0.000238 mm

21.

Convert 12.54 liters to hectoliters.

a)

.1254 hL

b)

125.4 hL

c)

1254 hL

d)

0.01254 hL

22.

Convert 2.39 kilograms to grams.

a)

2390 g

b)

0.2390 g

c)

23.9 g

d)

239 g

23.

Convert 732 milliseconds to seconds.

a)

0.732 s

b)

73.2 s

c)

7.32 s

d)

7320 s

24.

Convert 7.5 kilograms to milligrams

a)

7500000 mg

b)

750000000000 mg

c)

750 mg

d)

0.75 mg

25.

Use dimensional analysis to convert the following:

Convert 3867 seconds to minutes. (Hint: 1 minute = 60 seconds)

a)

64.45 min

b)

45 min

c)

62.85 min

d)

7.32 min

26.

How many minutes are in a school year, 190 days?

a)

269,000 minutes

b)

11,400 minutes

c)

16,156 minutes

d)

273,600 minutes

27.
How would you write 564,000,000 in scientific notation?
a)
5.64 x 10-7
b)
5.64 x 106
c)
5.64 x 108
d)
56.4 x 107
28.
How do you write
1001
in scientific notation?
a)
1.0001 x 104
b)
1.01 x 105
c)
1.001 x 103
d)
10.1 x 103
29.
Express the following in scientific notation:
.000457
a)
457 x 106
b)
457 x 10-6
c)
4.57 x104
d)
4.57 x 10-4
30.
Put the following in scientific notation:
23,948
a)
23.948 x 103
b)
2.3948 x 104
c)
2.3948 x 10-4
d)
0.23948 x 105
31.
Which of these elements has the greatest atomic radius? 
a)
H
b)
N
c)
Cl
d)
Cs
32.
The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest electronegativity?

a)
W
b)
X
c)
Y
d)
Z
33.
The Periodic Table of the Elements is useful for revealing patterns and trends in the elements. Which statement accurately describes a pattern in the size of atomic radii in the Periodic Table of the Elements?
a)
Atomic radii decrease from left to right across a period and decrease from top to bottom in a group.
b)
Atomic radii increase from left to right across a period and increase from top to bottom in a group.
c)
Atomic radii decrease from left to right across a period and increase from top to bottom in a group.
d)
Atomic radii increase from left to right across a period and decrease from top to bottom in a group.
34.
Fluorine, chlorine, bromine, and iodine all have the same number of valence electrons and have a tendency to gain electrons. Which element has the greatest ionization energy and electronegativity?
a)
fluorine
b)
chlorine 
c)
bromine 
d)
iodine 
35.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
36.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
37.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
38.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
39.
How do the following two elements bond together?
K1+  S2- 
a)
KS
b)
K8S
c)
K6S3
d)
K2S
40.
What is the formula for magnesium chloride?
a)
MgCl
b)
Mg2Cl
c)
MgCl2
d)
Mg(ClO3)2
41.
What is the name of the compound Li(OH)?
a)
lithium hydrogen oxide
b)
lithium hydroxide
c)
lithium hydride
d)
lithium oxide hydride
42.
Name this compound: 
Ca(CO3)
a)
Calcium carbon oxide
b)
Calcium (II) carbonate
c)
Calcium carbonate
d)
Carbonate (I) calcide
43.
What is the formula for sodium nitrate?
a)
Na3(NO)
b)
Na(NO)
c)
Na3(NO3)
d)
Na(NO3)
44.
The name of FeCl₂ is
a)
iron chloride
b)
iron (II) chloride
c)
iron (I) chloride
d)
iron dichloride
45.
The name of Cu₃N₂ is
a)
copper (III) nitride
b)
copper (II) nitride
c)
copper nitride
d)
tricopper dinitride
46.

Name the compound: SO3

a)

sulfur trioxide

b)

sulfite ion

c)

sulfur oxide

d)

sodium trioxide

47.

Name the compound: CF4

a)

carbon tetrafluoride

b)

monocarbon tetrafluoride

c)

carbon fluoride

d)

chlorine tetrafluoride

48.

Name the compound: P4O8

a)

tetraphosphorus octoxide

b)

phosphorus oxide

c)

tetrapotassium octoxide

d)

potassium oxide

49.

Name the compound: SF6

a)

sulfur heptafluoride

b)

sulfur hexafluoride

c)

monosulfur hexafluoride

d)

monosulfur heptafluoride

50.

If an atom has 3 valence electrons, what charge will it have as an ion?

a)

+3

b)

-3

c)

+5

d)

-5

51.

If an atom gains 3 electrons, what charge will it have as an ion?

a)

+3

b)

-3

c)

+5

d)

-5

52.

If an atom has 1 valence electron, what charge will it have when it becomes an ion?

a)

+1

b)

-1

c)

+7

d)

-7

53.

If an element gains 2 electrons, what charge will it have when it becomes an ion?

a)

+2

b)

-2

c)

-6

d)

-6

54.

If an atom has 6 valence electrons, what charge will it have when it becomes an ion?

a)

+2

b)

-2

c)

+6

d)

-6

55.

Valence electrons are those electrons that are...

a)

closest to the nucleus.

b)

freely floating between atoms.

c)

farthest from the nucleus

d)

unable to become involved in chemical bonding.

56.

Oxygen has 6 valence electrons. When forming an ion, oxygen will

a)

lose six electrons and have a charge of +6.

b)

lose six electrons and have a charge of -6.

c)

gain two electrons and have a charge is +2.

d)

gain two electrons and have a charge of -2.

57.

Look at the periodic table. What should be the charge on the ion formed by calcium?

a)

+1

b)

+2

c)

-1

d)

-2

58.

Most elements are most stable when their valence shell has ________ electrons.

a)

4

b)

6

c)

8

d)

18

59.

What is the molecular shape of water?

a)

Tetrahedral

b)

Linear

c)

Octahedral

d)

Bent or V-shaped

60.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Bent
d)
Tetrahedral
61.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
62.
*
a)
trigonal pyramid
b)
linear
c)
bent
d)
angular
63.

What 3-D shape would this molecule have?

a)

Trigonal planar

b)

Pyramidal

c)

Tetrahedral

d)

Bent

64.

What 3-D shape would this molecule have?

a)

tetrahedral

b)

trigonal planar

c)

trigonal pyramid

d)

bent

65.

What is the formula for percent yield?

a)

ActualTheoretical×100\frac{Actual}{Theoretical}\times100

b)

TheoreticalActual×100\frac{Theoretical}{Actual}\times100

c)

Actual×Theoretical100\frac{Actual\times Theoretical}{100}

d)

100Actual×Theoretical\frac{100}{Actual\times Theoretical}

66.

When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

67.
CH4  +  2O2  →  CO2  +  2H2O
24 grams of CH4 was added to the above reaction. Calculate the theoretical yield of CO2.
a)
66 grams
b)
132 grams
c)
33 grams
d)
8.72
68.

2Fe2O3 + C → Fe + 3CO2

You add 28 grams of carbon. You find the actual yield to be 181.2 grams of CO2. What is the percent yield of CO2? (Hint: calculate theoretical yield of CO2 first)

a)

58.83%

b)

308%

c)

6435%

d)

15.5

69.
P4 + 6Cl2 --> 4PCl3 
The reaction of 75.0g P4 with excess chlorine gas produces 110g PCl3 in lab. Find the theoretical yield and calculate percent yield for the reaction. 
a)
78%
b)
64%
c)
27%
d)
33%
70.

What is the mass (g) of 2.5 moles of water (H2O)?

Molar mass of H2O = 18 g/mol

a)

45 g

b)

7.2 g

c)

0.16 g

d)

5 g

71.

Calculate the molar mass for Al(OH)3

a)

78.0 g/mol

b)

72 g/mol

c)

28 g/mol

d)

25 g/mol

72.

How many moles are there in 2.00 x 1023 atoms of oxygen?

a)

0.33 mol

b)

1.2 mol

c)

3.01 mol

73.

How many atoms are contained in 25 g of NaBr? (Atomic mass of Na = 23, Br = 35)

a)

102.96 molecules

b)

0.24 molecules

c)

1.45x1023 molecules

d)

2.34 x 1020molecules

74.
How many atoms are in 1.50 moles of Hg?
a)
9.03x1023 atoms Hg
b)
9.03x1024 atoms Hg
c)
903 atoms of Hg
d)
9.03 atoms of Hg
75.
Uranium-238  decays into  Thorium-234  by emitting .........
a)
an alpha particle
b)
a beta particle
c)
gamma rays
d)
visible light
76.

In the equation, 146C --> 147N + 0-1B, the _______ decay of radioactive carbon-14 results in the creation of a new nitrogen-14 atom.

a)

Gamma

b)

Beta

c)

Alpha

77.
If we start off with element 24X50 after an alpha decay we get another element Y that looks like
a)
22Y50
b)
22Y46
c)
20Y48
d)
26Y54
78.

24094Pu —› ____ + 42He

a)

23692U

b)

24796Cm

c)

24493Np

d)

24295Am

79.
Complete the nuclear equation and determine the type of decay that is occurring in this reaction. 
a)
alpha
b)
beta
c)
gamma
d)
none
80.

If some Protactinium (Pa) decays by alpha it would become...


[The large number at the top is the atomic number]

a)

Actinium (Ac)

b)

Thorium( (Th)

c)

Uranium (U)

d)

Neptunium (Np)

e)

Plutonium (Pu)

81.

If some Protactinium (Pa) decays by beta it would become...


[The large number at the top is the atomic number]

a)

Actinium (Ac)

b)

Thorium( (Th)

c)

Uranium (U)

d)

Neptunium (Np)

e)

Plutonium (Pu)

82.

The large number before a molecule is called a _______________.

a)

Subscript

b)

Capital Number

c)

Coefficient

83.

Balance the following equation--> What coefficient would need to be put in front of HCl to balance this equation. CH4 + 4 Cl2 → CCl4 + _____ HCl

a)

2

b)

3

c)

4

d)

5

84.

Which coefficients would balance this chemical equation? _Fe2O3 ---> _Fe + _O2

a)

2,1,2

b)

2,4,3

c)

1,1,1

d)

1,3,2

85.

Which coefficients would balance this chemical equation? _K + _Cl2 ---> _KCl

a)

1,1,1

b)

1,2,2

c)

1,1,2

d)

2,1,2

86.
CxHy +O2 --> H2O + CO2
a)
Decomposition
b)
Double replacement
c)
Combustion
d)
Single Replacement
87.
One reactant into several products.
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
88.
KOH + H3PO4 --> K3PO4 + H2O
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
89.
Si + S8 --> Si2S4
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
90.
Pb(NO3)2 --> PbO + NO2 + O2
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Combustion
91.

3 Pb + 2 H3PO4 ----> 3 H2 + 1 Pb3(PO4)2

a)

Synthesis (or combination)

b)

Decomposition

c)

Single replacement

d)

Double replacement

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