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Chemistry S1 Review

Total questions: 150

Worksheet time: 3hrs 19mins

Name
Class
Date
1.

This subatomic particle identifies the element

a)

proton

b)

neutron

c)

electron

2.

This subatomic particle stabilizes the nucleus

a)

proton

b)

neutron

c)

electron

3.

This subatomic particle determines the reactivity of the element

a)

proton

b)

neutron

c)

electron

4.

These subatomic particles are located in the nucleus (Select all that apply)

a)

proton

b)

neutron

c)

electron

5.

These subatomic particles determine the mass of the atom (Select all that apply)

a)

proton

b)

neutron

c)

electron

6.

This subatomic particle has a positive charge

a)

proton

b)

neutron

c)

electron

7.

This subatomic particle has no charge

a)

proton

b)

neutron

c)

electron

8.

This subatomic particle has a negative charge

a)

proton

b)

neutron

c)

electron

9.
What is the mass of an atom if it has 11 protons, 12 neutrons, and 11 electrons?
a)
22
b)
11
c)
34
d)
23
10.
If an atom has 10 protons, 10 neutrons, and 10 electrons, what is the mass of the atom?
a)
10
b)
20
c)
30
11.
If an atom has 12 positively charged subatomic particles, which of the following must it also have to be considered a neutral atom?
a)
12 neutrons
b)
12 electrons
c)
12 protons
d)
24 protons and neutrons
12.
The smallest particle of any type of matter is known by which of the following terms?
a)
Element
b)
Compound
c)
Atom
d)
Chemical
13.
What is the atomic number for an element with three protons?
a)
2
b)
1
c)
3
d)
6
14.

How many neutrons are in the atom "K"?

a)
7
b)
2
c)
39
d)
20
15.

What is the number of protons that the element in this image contains?

a)
14
b)
7
c)
15
d)
18
16.
John Dalton stated:
a)
elements are made of atoms
b)
atoms of a given element are identical
c)
atoms cannot be subdivided, created, nor destroyed
d)
all of the above
17.
How did Rutherford discover the proton?
a)
Cathode tube ray experiment
b)
Gold Foil Experiment
c)
Planetary Model
d)
Plum Pudding Model
18.
The scientist responsible for "discovering" the nucleus is:
a)
Bohr
b)
Rutherford
c)
Schroedinger
d)
Einstein
19.
What scientist is best known for his "Plum Pudding" model of the atom?
a)
J.J. Thomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
20.

He discovered the electron using cathode ray tube experiment.

a)

J.J. Thomson

b)

John Dalton

c)

Ernest Rutherford

d)

Robert Millikan

21.
Who came up with the model of an atom pictured?
a)
J.J. Thompson
b)
Ernest Rutherford
c)
Neils Bohr
d)
James Chadwick
22.
Who's model is this? 
a)
Millikan
b)
Rutherford
c)
Thomson
d)
Bohr
23.
Four isotopes of lead include lead-204, lead-206, lead-207, and lead-208.  The average atomic mass of lead is 207.2.  Which isotope of lead is likely to be the most abundant.
a)
204
b)
206
c)
207
d)
208
24.
Negative ions are called
a)
Cations
b)
Electrons
c)
Anions
d)
Neutrons
25.

When an atom loses a valence electron, it becomes a(n) _____________ ion.

a)

positive

b)

negative

c)

neutral

26.
Ions are: 
a)
atoms with a positive or negative charge
b)
atoms with no charge
c)
atoms with ONLY a positive charge
d)
atoms with ONLY a negative charge
27.
A negative ion is a 
a)
cation
b)
anion
28.
What charge does an atom have if it GAINS an electrons?
a)
Positive (+)
b)
Negative (-)
29.
What is the definition of isotope?
a)
atoms of an element with different numbers of neutrons.
b)
materials break down over time at a very consistent rate
30.
What are the names of the horizontal rows on the periodic table?
a)
The periods
b)
The Groups
c)
The Non-Metals
d)
Ionization Energies
31.

Valence electrons are:

a)

Electrons on the ring farthest away from the nucleus

b)

Electrons on the ring closest to the nucleus

c)

Electrons that just come and go - they don't stay with the atom

32.

Why are ions formed?

a)

To make our lives difficult

b)

Because atoms want empty or full outer shells

c)

Because atoms have the same number of protons and electrons

d)

Because atoms gained neutrons

33.

What is the charge of a sodium ion?

a)

+2

b)

+1

c)

-1

d)

-2

34.
Group 17 always has ions with a charge of 
a)
+1
b)
+2
c)
-1
d)
-2
35.
What charge will an Oxygen ion have? 
a)
+1
b)
-1
c)
+2
d)
-2
36.
If an element has 3 valence electrons, what charge will likely form on its ion ?
a)
+3
b)
+5
c)
-3
d)
-5
37.
Which of the following has a -3 charge?
a)
Boron
b)
Fluorine
c)
Nitrogen
d)
Neon
38.
charge of lithium ion
a)
-2
b)
-1
c)
+1
d)
+2
39.
charge of beryllium ion
a)
-2
b)
-1
c)
+1
d)
+2
40.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
41.
Different isotopes have...
a)
different masses
b)
different atomic numbers
c)
different electrons
d)
different protons
42.
How many neutrons does a Carbon 13 atom have?
a)
6
b)
5
c)
7
d)
8
43.
How many neutrons does an Oxygen-19 isotope have?
a)
19
b)
8
c)
11
d)
10
44.
What is the name of the pictured isotope?
a)
Copper-29
b)
Copper-63
c)
Copper-34
d)
CopperWopperHopperBopper
45.
What is the name of the pictured isotope?
a)
Chlorine-Schmorine
b)
Chlorine-17
c)
Chlorine-35
d)
Chlorine-18
46.
An element has two naturally occurring isotopes. One is 10.013 amu and is 19.9% abundant. The other is 11.01 amu and is 80.1% abundant. What is the average atomic mass? What element is it?
a)
9.012, Beryllium
b)
12.011, Carbon
c)
6.941, Lithium
d)
10.812, Boron
47.

What is the unit for mass?

a)

Grams (g)

b)

Milliliters (mL)

c)

Grams/Milliliter (g/mL)

48.

What is the unit for volume?

a)

Grams (g)

b)

Milliliters (mL)

c)

Grams/Milliliter (g/mL)

49.

What is the unit for Density?

a)

Grams (g)

b)

Milliliters (mL)

c)

Grams/Milliliter (g/mL)

50.

What is the equation to find density?

(a)  

51.

Calculate the density of the cube.

a)

2 g/cm3

b)

4 g/cm3

c)

6 g/cm3

d)

8 g/cm3

52.
What is the density of a liquid that has a mass of 27g and a volume of 30ml?
a)
0.9 g/ml
b)
3 g/ml
c)
57 g/ml
d)
810 g/ml
53.

what is the volume of the cube?

a)

123

b)

144

c)

244

d)

150

54.
A bar of copper has a mass of 216g and a volume of 24cm3. What is the density of copper?  
a)
9g/cm3
b)
.11g/cm3
c)
5184g/cm3
d)
322mL
55.
What is the volume of Object X?
a)
10.0 cm3
b)
15.0 cm3
c)
20.0 cm3
d)
25.0 cm3
56.
Two classifications of a pure substance are
a)
homogeneous and heterogeneous
b)
atoms and elements
c)
elements and compounds
d)
solutions and colloids
57.
A substance that is made up of only one kind of atom is a(an)
a)
compound
b)
homogeneous mixture
c)
element
d)
solution
58.
Coloured water is an example of a
a)
homogeneous mixture
b)
heterogeneous mixture
59.
Salad is an example of a
a)
homogeneous mixture
b)
heterogeneous mixture
60.
What type of mixture is this?
a)
heterogeneous 
b)
homogeneous
61.
What type of mixture is this?
a)
heterogeneous 
b)
homogeneous
62.
What type of mixture is this?
a)
heterogeneous 
b)
homogeneous
63.
What does it mean if a mixture is homogeneous?
a)
you can see the different parts
b)
cannot tell one part from another
c)
chunks of particles
d)
made of elements
64.
What does it mean if a mixture is heterogeneous?
a)
you can see the different parts
b)
cannot tell one part from another
c)
very well blended
d)
made of elements
65.

Freezing

a)

Solid to gas

b)

Liquid to solid

c)

Gas to solid

66.

Boiling

a)

liquid to gas

b)

gas to solid

c)

gas to liquid

67.
Which state of matter has a definite shape?
a)
solid
b)
liquid
c)
gas
68.

What is happening when my ice cream changes from a solid to a liquid?

a)

freezing

b)

melting

c)

burning

69.

The state of matter that has no definite size or shape is

a)

Solid

b)

Liquid

c)

Gas

70.

Particles in a ______________________ move quickly and are far apart.

a)

gas

b)

solid

c)

liquid

71.

Solid to Gas

a)

Deposition

b)

Sublimation

c)

Evaporation

72.

What is condensation?

a)

gas to solid

b)

gas to liquid

c)

liquid to solid

73.

Definite shape and definite volume

a)

Solid

b)

Liquid

c)

Gas

74.

Has a definite volume but not a definite shape

a)

Solid

b)

Liquid

c)

Gas

75.

Liquid to Gas

a)

Condensation

b)

Evaporation

c)

Sublimation

76.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
77.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
78.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
79.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
80.

What do you start all electron configurations with?

a)

1s2

b)

1d10

c)

1f14

d)

1p6

81.

The 4 orbitals are

a)

s, p, d, f

b)

a, b, c, d

c)

2, 4, 6, 8

82.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
83.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
84.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
85.
What noble gas should be used to write the shorthand configuration for Te?
a)
Ar
b)
Kr
c)
Xe
d)
Sb
86.

What is the noble gas configuration for silicon?

a)

[Ne] 3s2 3p1

b)

[Ar] 4s1

c)

[Kr] 5s1

d)

[Ne] 3s2 3p2

87.

Which element is depicted from this orbital diagram?

a)

Fluorine (9)

b)

Neon (10)

c)

Chlorine (17)

d)

Argon (18)

88.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
89.
How many electrons can the s sublevel hold?
a)
14
b)
10
c)
2
d)
6
90.

Write the electron configuration

a)

1s22s22p6

b)

1s12s12p3

c)

1s22s22p63s2

d)

1s22s22p63s3

91.
How many electrons can the p sublevel hold?
a)
14
b)
10
c)
2
d)
6
92.

The electron configuration for Nitrogen is 1s22s22p3. What would the electron configuration of the ion look like if Nitrogen has a -3 charge?

a)

1s22s22p6

b)

1s22s2

c)

1s22s22p3

d)

1s22s22p5

93.

The electron configuration for Cobalt is 1s22s22p63s23p64s23d7. What would the ion configuration look like if Cobalt has a +2 charge?

a)

1s22s22p63s23p64s23d7

b)

1s22s22p63s23p63d7

c)

1s22s22p63s23p64s23d5

d)

1s22s22p63s23p64s23d10

94.

A wave with a large wavelength will have a ______ frequency and _____ energy

a)

high, low

b)

high, high

c)

low, high

d)

low, low

95.
High frequency waves have _________ wavelength.
a)
varying
b)
high
c)
the same
d)
low
96.
An argon ion laser emits light at 488 nm. What is the frequency of this radiation? (1 nm = 1x10-9m)
a)
4.07 x 10-19 Hz
b)
6.15 x 1014 Hz
c)
1.46 x 102 Hz
d)
2.05 x 106 Hz
97.
The distance between two crests or two troughs of a wave is called:
a)
frequency
b)
amplitude
c)
wavelength
d)
hertz
98.
What is the frequency of a photon whose energy is 3.4x10-19J?
a)
8.8x1026 Hz
b)
5.1x1014 Hz
c)
1.9x10-15 Hz
d)
2.3x10-52 Hz
99.

The frequency of violet light is 7.5x1014 Hz. What is its wavelength?

a)

4.0x10-7 m

b)

4.0x107 m

c)

2.25x1023m

d)

2.25x1023 Hz

100.

What is the speed of light?

a)

3.0x108 ms

b)

3.0x108 m/s

c)

6.626x10-34 Js

d)

6.626x10-34 J/s

101.
A common infrared laser operates at 1.06 x 103 nm. What is the energy of a photon with this wavelength? (1 nm = 1x10-9m)
a)
7.02 x 10^-40 J
b)
6.25 x 10^-28 J
c)
3.54 x 10^-15 J
d)
1.87 x 10^-19 J
102.

Energy is measured in........

a)

Wavelength

b)

Meters

c)

Joules

d)

Frequency

103.

What is 78.5 rounded to one significant figure?

a)

79

b)

78.5

c)

70

d)

80

104.

Round 0.010229 to four significant figures

a)

1022

b)

1023

c)

0.01023

d)

0.01022

105.

What is 0.658 rounded to 1 significant figure?

a)

0

b)

0.66

c)

0.7

d)

0.658

106.

What is 7.555 rounded to two significant figures?

a)

7.6

b)

7.5

c)

70

d)

76

e)

7.60

107.
How many significant figures: 216 m
a)
1
b)
2
c)
3
d)
0
108.
How many significant figures: 2016 m
a)
1
b)
2
c)
3
d)
4
109.
How many significant figures: 153.0 mL
a)
1
b)
2
c)
3
d)
4
110.
How many significant figures: 0.012 km
a)
1
b)
2
c)
3
d)
4
111.
How many significant figures: 1000 mL
a)
1
b)
2
c)
3
d)
4
112.
How many significant figures: 100.000 cL
a)
1
b)
3
c)
5
d)
6
113.

Calculate and round to the correct number of significant digits.

a)
b)
c)
d)
114.

To which decimal place would you round the answer in order to be considered correct: 230 + 4.88 - .0643

a)

Ones

b)

Tenths

c)

Hundredths

d)

Thousandths

115.

Calculate and round to the correct number of significant digits.

a)

332.6

b)

333

c)

330

d)

33

116.

Calculate, giving the answer in the correct number of significant digits.

9.3 – 2.003 = ?



(a)  

117.

Calculate, giving the answer in the correct number of significant digits.

84.93 ÷ 2.01 = ?



(a)  

118.

Round 1.00059832 to 4 significant figures.

(a)  

119.

Round 890.6319 to 3 significant figures.



(a)  

120.

Round 0.0529 to 1 significant figure.



(a)  

121.

What is the correct formula for potassium oxide?

a)

KO2

b)

KO

c)

K2O

d)

OK2

122.

What is the correct name for SrF2?

a)

fluoride strontium

b)

strontium fluorine

c)

strontium diflluoride

d)

strontium fluoride

123.

What is the correct name for VBr3?

a)

vanadium(III) bromide

b)

vanadium bromide

c)

vanadium(III) bromate

d)

vanadium tribromide

124.

What is the correct name for CrO?

a)

chromium monoxide

b)

chromium(I) oxide

c)

chromium(II) oxide

d)

chromium oxide

125.

What is the formula for copper(II) phosphide?

a)

Cu2P3

b)

Cu3P2

c)

Cu3(PO4)2

d)

Cu2P

126.

What is the correct name for Zn(CN)2?

a)

zinc cyanide

b)

zinc dicyanide

c)

zinc carbide

d)

zinc(I) cyanide

127.

What is the correct name for (NH4)2CO3?

a)

diammonium carbonate

b)

nitrogen hydrogen carbon oxide

c)

ammonium carbonate

d)

ammonium carbide

128.

What is the correct name for Al2(SO4)3?

a)

aluminum(II) sulfate

b)

dialuminum trisulfate

c)

aluminum sulfide

d)

aluminum sulfate

129.

What is the correct formula for iron(III) permanganate?

a)

FeMnO4

b)

Fe(MnO4)3

c)

Fe3MnO4

d)

FeMn3O12

130.

What is the correct name for NiSO3?

a)

nickel(I) sulfite

b)

nickel(II) sulfite

c)

nickel(II) sulfate

d)

nickel(I) sulfate

131.
Sliver Phosphide
a)
Ag3P
b)
Ag3PO4
c)
Ag3PO3
d)
AgP
132.
Li2Cr2O7
a)
Lithium Dichromate
b)
Lithium Chromate
c)
Dilithium Dichromate
d)
Dilithium Dichromium Heptoxide
133.
Cu3PO4
a)
Copper I Phosphate
b)
Copper II Phosphate
c)
Copper Phosphide
d)
Copper I Phosphite
134.
What is the charge of Ni in NiBr3?
a)
+2
b)
+3
c)
-3
d)
+6
135.
The roman numeral in a compound name indicates ___________________.
a)
the number of metal ions
b)
the charge of the metal ion
c)
nothing
d)
the number of total ions
136.
Magnesium ion would take a charge of
a)
1+
b)
2+
c)
3+
d)
0
137.
In the compound TiO2, titanium has a charge of
a)
4+
b)
2+
c)
2-
d)
4-
138.
What is the ionic compound formed between LI and N?
a)
Li3N
b)
Li2N2
c)
Li3N2
d)
LiN3
139.
What is the ionic compound formed between Ca and Br?
a)
CaBr
b)
CaBr2
c)
Ca2Br
d)
Ca2Br
140.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
141.
How are ionic bonds formed?
a)
Transfer of electrons
b)
Sharing of electrons
142.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
143.
Where are metals located on the periodic table?
a)
Blue
b)
Green
c)
Red
144.

Anions

a)

Gain electrons, has an overall positive charge

b)

Lose electrons, has an overall positive charge

c)

Lose electrons, has an overall negative charge

d)

Gain electrons, has an overall negative charge

145.

Cations

a)

Gain electrons, has an overall positive charge

b)

Lose electrons, has an overall positive charge

c)

Lose electrons, has an overall negative charge

d)

Gain electrons, has an overall negative charge

146.

Shares electrons:

a)

Ionic Bonds

b)

Covalent Bonds

147.

What type of chemical bonds occur when atoms transfer electrons (gains or loses)?

(a)  

148.

Gains or loses electrons:

a)

Ionic Bonds

b)

Covalent Bonds

149.

7,000 g = ____ kg

a)

70

b)

700

c)

7

d)

0.07

150.

648 g = ____ mg

a)

6,480

b)

64,800

c)

648,000

d)

64.8

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