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EXAM REVIEW

Total questions: 140

Worksheet time: 4hrs 39mins

Name
Class
Date
1.

The mass of an object _______________.

a)

changes, depending on where it is located

b)

changes randomly

c)

changes, depending on temperature

d)

does not change

2.

How many significant figures are there in 2016 m?

a)

1

b)

2

c)

3

d)

4

3.

How many significant figures are there in 0.010 L?

a)

1

b)

2

c)

3

d)

4

4.

Match the following

a)

length

1.

meter

b)

mass

2.

kilogram

c)

volume

3.

m^3

d)

temperature

4.

kelvin

5.

1 meter = (a)   centimeters

6.

1.5 m equals to how many mm?

a)

0.0015

b)

0.015

c)

150

d)

1500

7.

Which unit is the smallest?

a)

km

b)

mm

c)

m

d)

cm

8.

The candy was sour.

a)

Qualitative

b)

Quantitative

9.

Molly investigated whether the age of students affects their driving skills. What is the dependent variable?

a)

Type of car

b)

Skill of driving

c)

Age of student

10.

Steve wanted to see if the type of fertilizer made sunflowers grow larger. What is the independent variable?

a)

Type of fertilizer

b)

Size of sunflower

c)

Type of sunflower

11.
How would you write 0.0005 in scientific notation?
a)
50 x 105
b)
5 x 10-4
c)
5 x 103
d)
0.5 x 103
12.

How would you write 4.3756 x 104 in standard form?

a)

437,560,000

b)

0.00043756

c)

43,756

d)

437,560

13.

Round 0.010229 to four significant figures

a)

1022

b)

1023

c)

0.01023

d)

0.01022

14.

What is the product of 4.2 and 16.32? (Consider significant figures)

a)

68.544

b)

68.54

c)

68.5

d)

69

15.

What is the measurement using the correct number of significant figures?

a)

39.5 mL

b)

40 mL

c)

39 mL

d)

40.0 mL

16.

What kind of relationship is this?

a)

Inverse

b)

Direct

17.
Zed went to the store and bought a bag of chips.  He estimated there would be 350 chips in the package, but realized there were only 210 chips in that package.  What was his percent error?
a)
35%
b)
67%
c)
85%
d)
92%
18.
This bullseye demonstrates...
a)
High Accuracy & High Precision
b)
High Accuracy & Low Precision
c)
Low Accuracy & High Precision
d)
Low Accuracy & Low Precision
19.

100 cm = 1 m.

What conversion factor would be used to convert 120 centimeters into meters?

a)

120 cm1 m\frac{120\ cm}{1\ m}  

b)

1 m120 cm\frac{1\ m}{120\ cm}  

c)

 100 cm1 m\ \frac{100\ cm}{1\ m}  

d)

100 m1 cm\frac{100\ m}{1\ cm}  

e)

1 m100 cm\frac{1\ m}{100\ cm}  

20.

A chemical change

a)

changes matter from one form to another.

b)

 destroys matter.

c)

creates matter

d)

does not change matter in any way.

21.

Which of the following is a physical change?

a)

 Iron is oxidized to iron oxide

b)

Aluminum metal is pounded into thin sheets

c)

Copper reacts with a strong acid

d)

Sodium metal explodes on contact with water

22.

Which of the following is an example of a chemical change?

a)

melting solid gold

b)

burning hydrogen gas

c)

dissolving sugar in water

d)

breaking a sheet of glass

23.

Substances that are made up of ONLY one type of atom (element) or compound.

a)

Heterogeneous mixture

b)

Pure substance

c)

Suspension

d)

Homogeneous mixture

24.

Which of the following is classified as a pure substance?

a)

Lemonade

b)

Fruit punch

c)

ketchup

d)

Hydrogen

25.

Which of the following is NOT a mixture?

a)

milk

b)

lemonade

c)

vegetable salad

d)

carbon

26.

True or False: Elements and compounds are pure substances.

a)

True

b)

False

27.

Identify which images are HETEROGENEOUS MIXTURES! (Check all that apply)

a)
b)
c)
d)
28.
What type of mixture is this?
a)
homogenous mixture
b)
chemical
c)
heterogeneous mixture 
d)
solid mix
29.
Which of the following is an Alkaline Earth Metal? 
a)
Calcium
b)
Lithium
c)
Phosphorus
d)
Copper 
30.

Which of the following is a Halogen?

a)

Bromine

b)

Rubidium

c)

Beryllium

31.
Which of the following is a transition metal? 
a)
Iron
b)
Oxygen
c)
Neon
d)
Barium
32.

Which of the following is a Noble Gas?

a)

Krypton

b)

Chlorine

c)

Gallium

33.
What group on the Periodic Table contains the elements of the alkaline earth family?
a)
1
b)
2
c)
17
d)
18
34.
How many valence electrons does a halogen have? 
a)
1
b)
2
c)
7
d)
8
35.

Matter is classified in...

a)

Elements & Compounds

b)

Homogeneous & Heterogeneous

c)

Colloids & Suspensions

d)

Pure substances & Mixtures

36.
a)
Alkali
b)
Alkaline
c)
Halogen
d)
Noble Gases
37.
a)
Alkali
b)
Alkaline Earth
c)
Halogen
d)
Noble Gases
38.

How many moles are in 8.30 X 1023 molecules of H2O?

a)

1.38 X 1023 moles H2O

b)

1.38 moles H2O

c)

2 moles H2O

d)

1 mole H2O

39.

How many molecules are there in 31.8 moles of water?

a)

5.28 x 10-23 molecules

b)

1.91 x 1025 molecules

c)

5.28x 10-25 molecules

d)

1.91 x 1023 molecules

40.

What is the conversion factor that should be used to determine how many molecules are there in 4.00 moles of glucose, C6H12O6?

a)
b)
c)
d)
41.

Which has the most particles?

a)

1 mole H2

b)

1 mole Na1+

c)

1 mole Al(OH)3

d)

These are all the same

42.

How many atoms are in 1 mole of Iodine (I)?

a)

6.022 x 1023

b)

4.022 x 1023

c)

6.022 x 1025

d)

4.022 x 1025

43.

What is the molar mass of H2O?

a)

6.02 x 1023 g/mol

b)

16 g/mol

c)

18 g/mol

d)

15.99999 g/mol

44.
How many moles are in 20 grams of Ca (Calcium)?
a)
0.5 
b)
1
c)
3
d)
20
45.

What is the molar mass when you have 4 moles of CO2?

a)

176 grams

b)

54 grams

c)

128 grams

d)

280 grams

46.

Calculate the mass of 4 mol of chlorine molecules. Cl2. (Cl =35.5)

a)

4

b)

35.5

c)

142

d)

284

47.
Negative ions are called
a)
Cations
b)
Electrons
c)
Anions
d)
Neutrons
48.

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

a)

positive

b)

negative

c)

neutral

d)

polyatomic

49.
How many protons are in this element?
a)
79
b)
196
c)
117
d)
Cannot be determined
50.
What is the number of neutrons?
a)
34
b)
79
c)
45
d)
35
51.
If you have 10 protons and 9 neutrons, what would the mass number be?
a)
19
b)
9
c)
10
d)
1
52.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number
53.

What is the mass number of bromine?

a)

35

b)

45

c)

80

d)

79.904

54.

How many neutrons does this bromine atom have?

a)

35

b)

45

c)

80

55.
J.J. Thomson used a cathode ray tube to find what particle in the atom?
a)
Proton
b)
Neutron
c)
Electron
56.
Idea was of an indivisible particle of matter he called "atomos"
a)
John Dalton
b)
Aristotle
c)
Democritus
d)
Plato
57.
What is the Law of Conservation of mass?
a)
Mass is created in a chemical reaction
b)
Mass is created in a physical change
c)
New chemicals formed from a chemical reaction have a larger overall mass than the original reactants
d)
Mass is never created or destroyed
58.

Place each part of the atom in its correct location.

a)

Proton

b)

Neutron

c)

Electron

1
2
3
1)
2)
3)
59.
This particle is found in the nucleus and has a positive charge
a)
Electron
b)
Proton
c)
Neutron
d)
Neutral
60.

Which wave has the highest energy?

a)

A

b)

B

c)

C

d)

You cannot tell from this diagram.

61.
What is the wavelength for a quantum of light with energy of 7.56x10-19J? (λ=hc/E) 
a)
2.62x10-7m
b)
2.62x107m
c)
2.64x10-45m
d)
2.64x1045m
62.
What is the energy of a quantum of light with a frequency of 7.39x1014Hz.(E=Hv)
a)
4.88x1019
b)
4.88x10-19
c)
2.22x1023
d)
2.22x10-23
63.

Match the following measurements to the correct unit.

a)

Wavelength

1.

meters

b)

Wave speed

2.

m/s

c)

Frequency

3.

Hz

d)

Energy

4.

J

64.

During a flame test, a lithium salt produces a characteristic red flame. This red color is produced when electrons in excited lithium atoms

a)

are gained by the atoms

b)

are lost by the atoms

c)

move to higher energy states within the atoms

d)

return to lower energy states within the atoms

65.

The light produced by signs using neon gas results from electrons that are

a)

being lost by the Ne(g) atoms

b)

being gained by the Ne(g) atoms

c)

moving from lower to higher principal energy level

d)

moving from higher to lower principal energy level

66.
Which drawing represents the process by which an emission line is formed?
a)
A
b)
B
c)
C
d)
D
67.

The ground state is the ______________ energy state of an atom.

a)

highest

b)

lowest

68.
Emission of light from an atom occurs when an electron
a)
drops from a higher to a lower energy level.
b)
   jumps from a lower to a higher energy level.   
c)
   moves within its atomic orbital.
d)
falls into the nucleus.
69.

The picture shows an atom in the ground state absorbing energy and the electron jumps to the excited state. Which state has higher energy?

a)

Ground State

b)

Excited State

70.

Which electromagnetic waves carry more energy?

a)

Waves with long wavelengths

b)

Waves with short wavelengths

c)

Waves with low frequency

d)

They all carry the same amount of energy

71.

In the image shown, which part of the wave is labeled A?

a)

Speed

b)

Frequency

c)

Amplitude

d)

Wavelength

72.

At the arrow, name that part

a)

trough

b)

amplitude

c)

crest

d)

hill

73.

The arrow is pointing to the

a)

trough

b)

wavelength

c)

amplitude

d)

equilibrium

74.

The height of a wave is

a)

Wavelength

b)

Amplitude

c)

Equilibrium

d)

Magnitude

75.

Which two variables of the electromagnetic spectrum have a direct relationship?

a)

Crests and trough

b)

energy and frequency

c)

wavelength and energy

d)

frequency and wavelength

76.

As the wavelength of an electromagnetic wave gets LONGER, the frequency gets ____________.

a)

Lower

b)

Higher

c)

does not change

d)

doubles

77.

________________ have the highest energy and shortest wavelength of all electromagnetic waves.

a)

Gamma

b)

X Ray

c)

Radio

d)

Microwaves

78.

What type of wave has the largest wavelength and the lowest frequency on the electromagnetic spectrum?

a)

Radio

b)

Micro

c)

Gamma

d)

X ray

79.

In the visible light waves what color has the highest frequency electromagnetic waves?

a)

Red

b)

Violet

c)

Green

d)

Yellow

80.
The energy of waves _______ as the wavelength gets shorter.
a)
increases
b)
decreases
c)
stays the same
81.
What is the number of waves that pass a point in one second?
a)
Amplitude
b)
Frequency
c)
Period
d)
Wavelength
82.

This shape is that of a...

a)

s orbital

b)

d orbital

c)

p orbital

d)

f orbital

83.

There may be a maximum of ____ p orbitals at a given energy level.

a)

2

b)

6

c)

3

d)

8

84.

The principle quantum number, n, represents the:

a)

spin value

b)

suborbital value

c)

energy level

d)

magnetic value

85.

How many electrons total are found in the d orbital?

a)

2

b)

6

c)

10

d)

14

86.

What does the 1 in "1s" stand for?

a)

energy level

b)

s orbitals

c)

p orbitals

d)

the number of electrons

87.

For a p sublevel, "L" equals ____.

a)

0

b)

1

c)

2

d)

3

88.

Which of the following sets of quantum numbers (n, l, ml, and ms) describes the valence electron of Na?

a)

2, 1, 0, -½

b)

2, 0, 0, -½

c)

3, 1, 1, +½

d)

3, 0, 0, +½

89.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
90.

Which values can (n) be?

a)

only 0

b)

0, 1, 2, 3...

c)

1,2,3,4...

d)

-2 < n < +2

91.

Which set of Quantum numbers is not allowed

a)

(3,1,1,-1/2)

b)

(2,1,-2,+1/2)

c)

(4,2,-1,-1/2)

92.

A subshell that contains 5 orbitals is ... subshell.

a)

d

b)

s

c)

f

d)

p

93.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
94.

What is the electron configuration of Sulfur using noble gas method

a)

[Ne]3s1

b)

[Ne]3s23p3

c)

[Ne]3s23p4

d)

[Ne]3s6

95.

Electrons will not pair up in a subshell until all other subshells (orientations) are full. This describes which theory of the quantum atomic model?

a)

Hund’s Rule

b)

Aufbau Principle

c)

Pauli Exclusion Principle

d)

Heisenberg's Uncertainty Principle

96.
Which type of orbital is shaped like a sphere?
a)
s orbital
b)
p orbital
c)
d orbital
d)
f orbital
97.

Which of the following elements is located in the "p" block of the periodic table?

a)

Sc

b)

Ca

c)

Se

d)

Sm

98.

Which of the following atoms is associated as having the final electron to fill it's orbitals with the following quantum numbers? n=3, l=0, ml=0

a)

Be

b)

K

c)

Mg

d)

Ca

99.

Which of the following atoms is associated as having the final electron to fill it's orbitals with the following quantum numbers? n=3, l=2, ml=0

a)

Cu

b)

Ti

c)

Ni

d)

Fe

100.

What are the possible values of ml if L=2

a)

0, 1, 2

b)

0, 1

c)

-2, -1, 0, 1, 2

d)

-1, 0, 1

101.

How many electrons can occupy a single orbital?

a)

1

b)

6

c)

2

d)

8

102.

How many orientations does a p orbital have?

a)

1

b)

2

c)

3

d)

5

103.

What is the formula for Sodium Bromide?

a)

NaBr

b)

NaBr2

c)

Na2Br

d)

SoBr

104.

What is the formula for diphosphorus pentoxide?

a)

P5O2

b)

PO5

c)

P2O5

d)

Po2O5

105.

What is the name for BrO3?

a)

bromine oxide

b)

monobromine trioxide

c)

bromine trioxide

d)

tribromine monoxide

106.

What is the chemical formula for an ionic compound of Potassium K +1and Oxygen O2- ?

a)

KO

b)

K2O

c)

K2O2

d)

KO2

107.

What is the name of transition metal compound- FeCl₂?

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

108.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
109.

What is the name of Br6F10 ?

a)

Bromium fluoride

b)

Hexabromine fluoride

c)

Bromium decafluoride

d)

Hexabromine decafluoride

110.

Name the following ionic compound: MgSO4

a)

Magnesium Sulfoxide

b)

Magnesium Sulfide

c)

Magnesium Sulfate

d)

Magnesium (II) Sulfate

111.

Aluminum is a group 3 metal. Which ion does Al typically form?

a)

Al 5-

b)

Al 3+

c)

Al3-

d)

Al5+

112.

What is the name of this compound:

Na2O

a)

Sodium oxide

b)

Disodium monoxide

c)

Sodium (I) oxide

d)

Sodium dioxide

113.

What is the formula for the following compound:

iron (III) oxide

a)

FeO3

b)

Fe3O2

c)

FeO

d)

Fe2O3

114.

Name the compound: (NH4)2S

a)

ammonium sulfide

b)

nitrogen tetrahydrogen sulfide

c)

diammounium sulfate

d)

ammonium sulfate

115.

Name the compound: Cu(NO3)2

a)

copper nitrate

b)

copper(II) nitrate

c)

copper(II) dinitrate

d)

copper dinitrogen hepaoxide

116.

Name the compound: AgNO3

a)

silver mononitrogen trioxide

b)

silver nitrate

c)

silver nitride

d)

monosilver mononitrogen trioxide

117.

Name the compound: Zn3P2

a)

zinc phosphide

b)

trizinc diphosphide

c)

zinc phosphate

d)

zinc phosphite

118.

Write the formula: potassium hydroxide

a)

KOH

b)

POH

c)

KH

d)

KO

119.

Write the formula: tin(II) phosphite

a)

Sn3(PO3)2

b)

Sn3PO8

c)

Sn2PO4

d)

Sn3(PO4)2

120.

Lithium nitride

a)

Li3N

b)

LiN

c)

Li3(NO3)2

d)

LiNO3

121.

Write the formula: lead(IV) sulfite

a)

Pb2(SO3)4

b)

Pb(SO3)2

c)

Pb2(SO4)4

d)

Pb(SO4)2

122.

Write the formula: beryllium oxide

a)

BO

b)

BeO

c)

BeO2

d)

BO2

123.

Write the formula: silver chlorate

a)

AgClO3

b)

AgCl

c)

AgCLO3

d)

AgCl3

124.

What is the name of the compound with the formula Ba3P2?

a)

barium phosphide

b)

barium diphosphide

c)

tribarium diphosphide

d)

barium phosphorous

125.

What is the formula for copper(I) sulfate?

a)

CuSO3

b)

CuSO4

c)

Cu2SO3

d)

Cu2SO4

126.
Find the percent composition of Cu2S?
a)
%Cu= 67.987 %S= 32.013
b)
%Cu= 79.854   %S= 20.145
c)
%Cu= 35.946   %S= 64.054
127.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
128.
What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180.18?
a)
CH2O
b)
C2H4O2
c)
C4H8O4
d)
C6H12O6
129.

What is the empirical formula if you have 36.84% nitrogen and 63.16% oxygen?

a)

NO

b)

N2O4

c)

N2O3

d)

N2O5

130.

What is the empirical formula for C4H6?

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

131.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
132.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
133.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
134.
The energy required to remove electrons is the definition of: 
a)
Electronegativity
b)
Atomic Number
c)
Atomic Radius
d)
Ionization
135.
Electronegativity is...
a)
the ability of an atom to attract/ accept 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. 
136.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
137.

Which has the smaller ionization energy?

a)

P

b)

Mg

138.

Which has the highest ionization energy?

a)

Ca

b)

As

c)

Br

139.

Which of the following will have a larger radius than Zinc?

a)

Gallium

b)

Aluminum

c)

Magnesium

d)

Strontium

140.
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)

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Honors Midterm Review (4 of 4)

136 questions

Honors Midterm Review (4 of 4)

quiz

Worksheet

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10th - 12th Grade

Review for Pre-AP Chemistry Part 2

145 questions

Review for Pre-AP Chemistry Part 2

quiz

Worksheet

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10th Grade - University