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CCR Chem A Final Review (Units 1-5)

Total questions: 128

Worksheet time: 2hrs 44mins

Name
Class
Date
1.

Which compound from the list is ionic?

a)

MgO

b)

NO2

c)

CO

d)

CCl4

2.

How does a lithium atom become a +1 ion?

a)

gain a proton

b)

lose a proton

c)

gain an electron

d)

lose an electron

3.

Classify this bond: CrF3

a)

nonpolar covalent

b)

polar covalent

c)

ionic

4.

Classify this bond: CS2

a)

nonpolar covalent

b)

polar covalent

c)

ionic

5.

Which types of elements make ionic compounds?

a)

metal and nonmetal

b)

2 metals

c)

2 nonmetals

d)

metal and metalloid

6.

How many valence electrons are in Carbon's outer shell?

a)

2

b)

4

c)

6

d)

there is no way to determine that number

7.

Classify this bond: SO3

a)

nonpolar covalent

b)

polar covalent

c)

ionic

8.

What is the formula for dinitrogen tetroxide?

a)

NO4

b)

NO2

c)

N2O4

d)

NO

9.

Which element will not form a bond because it already has a full valence shell?

a)

Ar

b)

As

c)

Ag

d)

Al

10.

The name for Fe2S3 is:

a)

rion (II) sulfide

b)

iron (II) sulfite

c)

iron (III) sulfate

d)

Iron (III) sulfide

11.

Classify this bond: CaBr2

a)

nonpolar covalent

b)

polar covalent

c)

ionic

12.

How does an atom of sulfur become a sulfide ion?

a)

gain 2 electrons

b)

lose 2 electrons

c)

gains 2 protons

d)

lose 2 protons

13.

An atom of calcium has how many valence electrons?

a)

1

b)

2

c)

4

d)

6

14.

Which of the following is a property of ionic compounds?

a)

low boiling points

b)

soft solids

c)

gases at room temperature

d)

can conduct electricity when melted

15.

What do we call the particles of an ionic compound?

a)

atoms

b)

formula units

c)

molecules

16.

The name for K2O is:

a)

dipotassium monoxide

b)

potassium monoxide

c)

dipotassium oxide

d)

potassium oxide

17.

Which of these compounds is molecular?

a)

KCl

b)

K2O

c)

CO

d)

NaCl

18.

What is the name for Na3N?

a)

trisodium nitride

b)

sodium nitride

c)

trisodium mononitride

d)

sodium nitrogen

19.

The name for Pb(NO2)2 is:

a)

lead (II) nitrate

b)

lead (II) nitrite

c)

iron (II) nitrate

d)

iron (II) nitrite

20.

What is the charge on the tin in SnCO3?

a)

+1

b)

+2

c)

+3

d)

+4

21.

In ionic bonding, the electrons are:

a)

shared

b)

transferred

c)

free to roam in a sea of electrons

22.

In a polar covalent bond, the electrons are:

a)

shared equally

b)

shared unequally

c)

transferred

d)

free to roam in an electron sea

23.

Name P2O5

a)

dipotassium pentoxide

b)

dipotassium pentaoxide

c)

diphosphorus pentaoxide

d)

diphosphorus pentoxide

24.

In metallic bonding, the valence electrons are:

a)

shared

b)

transferred

c)

free to roam in an electron sea

25.

Which of the following is a property of molecular compounds?

a)

gases at room temperature

b)

hard rigid solids

c)

good conductors of heat

d)

high melting point

26.

What is the formula for sulfur hexafluoride?

a)

SF4

b)

SF6

c)

S2F6

d)

SF2

27.

Which element is most likely to form a cation?

a)

Oxygen

b)

Chlorine

c)

Sodium

d)

Argon

28.

What is the charge on the iron in FeCl3?

a)

+1

b)

+2

c)

+3

d)

+4

29.

What is the charge on the copper in CuSO4?

a)

+1

b)

+2

c)

+3

d)

+4

30.

Which of these elements is most likely to form an anion?

a)

Fluorine

b)

Magnesium

c)

Aluminum

d)

Potassium

31.

What is the formula for phosphorus pentachloride?

a)

PCl3

b)

PCl5

c)

P2Cl5

d)

P2Cl3

32.

How many bonds are in the structural formula for CO2?

a)

1

b)

2

c)

3

d)

4

33.

Consider the molecule CCl4. Work out its structural formula. Select the answer that completes this sentence the best: The bonds in CCl4 are _____________ and the molecule is ____________ because it is symmetrical in shape.

a)

polar, polar

b)

polar, nonpolar

c)

nonpolar, polar

d)

nonpolar, nonpolar

34.
Which of the following is NOT an ionic compound:
a)
CaO
b)
NaOH
c)
BaCl2
d)
Br2
35.

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

36.

How many sig figs in the number 90.080?

a)

1

b)

2

c)

3

d)

4

e)

5

37.

The distance to the moon is 239,000 miles. Put that number in proper scientific notation.

a)

2.39E3

b)

2.39E-3

c)

2.39E5

d)

2.39E-5

38.

Complete the calculation and select the answer with the appropriate number of sig figs:

2.00 x 3.0E4 =

a)

6E4

b)

6.0E4

c)

6.00E4

d)

60,000

39.

Complete the calculation and select the answer with the appropriate number of sig figs:

65.17 - 31.9 =

a)

33

b)

33.27

c)

33.3

d)

33.2

40.

How many sig figs in the number 0.000370

a)

2

b)

3

c)

5

d)

6

41.

Convert 35 km to meters

a)

0.035 m

b)

0.35 m

c)

350 m

d)

3500 m

e)

35000 m

42.

Complete the calculation and select the answer with the right sig figs:

3.88E-6 / 2.2E4 =

a)

1.76E-2

b)

1.76E10

c)

1.8E-10

d)

1.7E2

43.

You calculate your answer and get 0.3955 km. Round that answer to 3 sig figs.

a)

0.400

b)

0.39

c)

0.396

d)

0.395

44.

You calculate an answer and get 817.65. Round that answer to 3 sig figs.

a)

817

b)

817.6

c)

817.650

d)

818

e)

818.0

45.

A Nascar record set in 1987 was 212.8 miles per hour. Determine that speed in km/min.

a)

5.720 km/min

b)

5720 km/min

c)

20590 km/min

d)

2.199 km/min

46.

The side of a cube is 4.70 cm. Calculate its volume.

a)

103.8 cm3

b)

22 cm3

c)

14.1 cm3

d)

104 cm3

47.

A piece of metal with a mass of 7.95 g is placed in a graduated cylinder holding 15.0 mL of water. After the metal is placed in the cylinder, the water level rises to 17.9 mL. Calculate the density of the metal.

a)

2.74 g/mL

b)

0.53 g/mL

c)

183 g/mL

d)

2.7 g/mL

e)

2.3 g/mL

48.

Convert 13.2 Mg to g.

a)

1.32E7 g

b)

1.32E6 g

c)

1.32E-7 g

d)

1.32E-6 g

49.

Round the number 30.068 to 2 sig figs.

a)

30.0

b)

30

c)

30.

d)

30.07

50.

Select the answer having 4 sig figs:

a)

4800

b)

4800.

c)

4.8E103

d)

4.80E3

51.

A student measures the density of silver to be 10.1 g/mL and the true value is 10.5 g/mL. Determine their % error and report the answer with the right sig figs.

a)

3% error

b)

-3.8 % error

c)

3.8% error

d)

-4% error

e)

4% error

52.

A cube measures 33 mm on each side. Determine its volume.

a)

99 mm3

b)

36000 mm3

c)

9.9 cm3

d)

36 cm3

53.

Determine the volume of a cylinder with a diameter of 2.8 cm and a height of 8.0 cm.

a)

4.9 cm3

b)

49 cm3

c)

197 cm3

d)

22.4 cm3

54.

There are 454 g in 1 lb. Convert 3.45 lb to mg. Report the answer with the right sig figs.

a)

1.6E6 mg

b)

1.57 mg

c)

1.57E6 mg

d)

1.32E4 mg

e)

7.6 mg

55.

The cost of a velvet ribbon is $1.95 per foot. Calculate the price per meter and report the answer with the right sig figs.

a)

$6.40/m

b)

$0.59/m

c)

$921/m

d)

$41.3/m

56.

Which phase of matter has a definite volume but no definite shape?

a)

solid

b)

liquid

c)

gas

57.

Which phase of matter fills its container because there is very little attraction between neighboring particles?

a)

solid

b)

liquid

c)

gas

58.

Which of the following changes is a chemical change?

a)

boiling water

b)

burning wood

c)

melting wax

d)

separating iron using a magnet

59.

Select the physical change from this list:

a)

Condensing Steam

b)

Silver tarnishing

c)

Burning a candle

d)

Decomposing Water into hydrogen and oxygen

60.

Select the intensive physical property from this list:

a)

mass

b)

flammability

c)

melting point

d)

length

61.

Select the chemical property from this list:

a)

boiling point

b)

density

c)

volume

d)

pyrophoric

62.

A compound, XY, is formed by reacting 10.0 g of X with 4.0 g of Y. When the reaction is complete, 2.5 g of X remains. How many grams of XY were formed?

a)

12.5 g

b)

14.0 g

c)

11.5 g

d)

16.5 g

63.

When 12.0 g of carbon and 4.0 g of hydrogen react, they form methane. What is the percentage of hydrogen in methane?

a)

33.3 % H

b)

25.0 % H

c)

75.0 % H

d)

there is insufficient info to answer this question.

64.

Which law indicates compounds have a set composition?

a)

The Law of Conservation of Mass

b)

The Law of Definite Proportions

c)

The Law of Multiple Proportions

65.

When 4.6 g of sodium reacts with chlorine, 11.6 grams of salt (NaCl) is formed. Calculate the amount of chlorine that reacted.

a)

16.2 g chlorine

b)

7.0 g chlorine

c)

53 g chlorine

d)

There is not enough information to answer the question.

66.

When ethane burns it reacts with oxygen to produce carbon dioxide and water. If 224 g of oxygen reacted and the products were 176 g CO2 and 108 g of water, determine how much ethane was burned.

a)

60 g ethane

b)

292 g ethane

c)

508 g ethane

d)

156 g ethane

67.

Classify paint

a)

element

b)

compound

c)

homogeneous mixture

d)

heterogeneous mixture

68.

Check all that apply. Which properties are intensive physical?

a)

density

b)

volume

c)

malleability

d)

toxicity

69.

Check all that apply. Which are chemical changes?

a)

iron rusting

b)

dissolving salt in water

c)

fireworks exploding

d)

digesting lunch

e)

removing iron using a magnet

70.

Classify brass

a)

element

b)

compound

c)

homogeneous mixture

d)

heterogeneous mixture

71.

Classify baking soda

a)

element

b)

compound

c)

homogeneous mixture

d)

heterogeneous mixutre

72.

Classify air

a)

element

b)

compound

c)

homogeneous mixture

d)

heterogeneous mixture

73.

Select all of the heterogeneous mixtures

a)

water

b)

salt water

c)

muddy water

d)

bubbly soda

e)

granite

74.

Select all of the compounds on this list:

a)

bronze

b)

carbon dioxide

c)

salt

d)

steel

e)

air

75.

Which technique is most useful to separate sand and salt from one another if they are mixed with water?

a)

filtration

b)

chromatography

c)

distillation

76.

Separating a mixture uses what type of change?

a)

physical

b)

chemical

c)

it depends on the situation

77.

Cl is a member of which family?

a)

alkali metal

b)

Transition element

c)

halogen

d)

noble gas

78.

Which rule is not obeyed in the pictured orbital diagram?

a)

The Aufbau Principle

b)

Hund's Rule

c)

The Pauli Exclusion Principle

d)

The Law of Conservation of Mass

79.

Which of the following atoms is not likely to form an ion in a chemical reaction?

a)

Cr

b)

Kr

c)

Br

d)

Sr

80.

How many valence electrons would an alkaline earth metal possess in its outer shell?

a)

1

b)

2

c)

5

d)

8

81.

Select the atom or ion with the largest radius from this list.

a)

Se-2

b)

Se

c)

O-2

d)

O

82.

How many valence electrons are shown in this orbital diagram?

a)

2

b)

3

c)

5

d)

7

83.

This is the electron configuration for what element?

a)

fluorine

b)

phosphorus

c)

argon

d)

chlorine

e)

bromine

84.

Select the atom with the largest ionization energy.

a)

Mg

b)

P

c)

Ba

d)

Cl

85.

Select the atom that is most likely to form a cation in a chemical reaction.

a)

Mg

b)

Si

c)

Cl

d)

Ar

86.

The properties of an unknown are tested and it is found to be malleable and is able to conduct electricity. This unknown is most likely a:

a)

metal

b)

nonmetal

c)

metalloid

d)

noble gas

87.

The properties of an unknown are tested and it is found to be a good semiconductor. What is the most likely identity of the unknown from these possibilities?

a)

K

b)

Cu

c)

Ge

d)

Ne

88.

Bromine has how many valence electrons and will form which kind of ion?

a)

5, cation

b)

5, anion

c)

7, cation

d)

7, anion

89.

The properties of an unknown gas are tested and it is unreactive. Which gas is most likely the identity of the unknown?

a)

N

b)

Cl

c)

He

d)

H

90.

How many valence electrons are shown in this configuration?

a)

2

b)

4

c)

6

d)

8

91.

Which element would make a good insulator because it is not a good conductor?

a)

Cu

b)

Ca

c)

Si

d)

Kr

92.

This is an orbital diagram for what element?

a)

Nitrogen

b)

Iron

c)

Zinc

d)

NIckel

e)

Palladium

93.

Which family has a full valence shell of electrons?

a)

alkali metals

b)

lanthanide series

c)

halogens

d)

noble gases

94.

In which region of the periodic table is uranium located?

a)

metal

b)

nonmetal

c)

metalloid

95.

Which element from the list is most likely to form an anion?

a)

Ar

b)

S

c)

Sr

d)

Li

96.

Which element on this list has the highest electronegativity?

a)

F

b)

Fe

c)

Fr

d)

Zn

97.

How many valence electrons are shown in this orbital diagram?

a)

8

b)

10

c)

6

d)

2

98.

Which rule is not obeyed in the pictured orbital diagram?

a)

The Aufbau Principle

b)

Hund's Rule

c)

The Pauli Exclusion Principle

d)

The Law of Conservation of Mass

99.

THere are 2 natural isotopes of nitrogen, Nitrogen-14 and Nitrogen-15. Consult the periodic table and predict which isotope is more abundant in nature.

a)

Nitrogen-14 is more abundant

b)

Nitrogen-15 is more abundant

c)

They are of equal abundance in nature.

d)

There is no way to predict this from the information given.

100.

The name for an atom with a positive charge is _____________.

a)

isotope

b)

anion

c)

cation

101.

Light has properties like ____________.

a)

a wave.

b)

a particle.

c)

Both a wave and a particle

d)

neither a wave nor a particle.

102.

The name for all of the forms of energy that move at the speed of light is _______________________.

a)

visible light.

b)

radio waves.

c)

the electromagnetic spectrum.

d)

invisible radiation.

103.

Which scientist discovered the nucleus with his gold foil experiment?

a)

Dalton

b)

Rutherford

c)

Bohr

d)

Thompson

104.

Which scientist created equations in which electrons moved in waves around the nucleus? What was the name of his model of the atom?

a)

Schrodinger/Plum Pudding

b)

Rutherford/Gold Foil

c)

Rutherford/Solid Sphere

d)

Schrodinger/Quantum Mechanical

105.

Determine the number of protons in an atom of iron.

a)

26

b)

30

c)

56

106.

How did Rutherford describe the nucleus of an atom? Check all that apply!

a)

empty space

b)

small

c)

positive

d)

negative

e)

dense

107.

When an isotope of Carbon-14 gives off a beta particle, what will it form?

a)

carbon-12

b)

nitrogen-14

c)

nitrogen-12

d)

beryllium-12

108.

When an isotope of uranium-238 gives off an alpha particle, what does it form?

a)

thorium-234

b)

thorium-238

c)

plutonium-242

d)

neptunium-239

109.

How many electrons are in the structure of the Br-1 ion?

a)

34

b)

35

c)

36

d)

80

e)

81

110.

Which of the following forms of radiation can be stopped by a piece of paper?

a)

alpha particle

b)

beta particle

c)

gamma ray

111.

An atom of arsenic has how many neutrons?

a)

33

b)

75

c)

42

d)

there is no way to know from the information given

112.

Light in the form of a mass-less particle that has discrete amount of energy is called a

a)

Charm

b)

Photon

c)

Exciton

d)

Muon

113.

The _______________ determines the color of visible light.

a)

wavelength (and frequency)

b)

speed

c)

amplitude

d)

particles of the medium

114.

All electromagnetic waves travel at the speed of light.

a)

True

b)

False

115.
How many protons does He have?
a)
4
b)
2
c)
6
d)
0
116.
The top number in this isotope notation is
a)
the mass number
b)
the atomic number
c)
the atomic mass
d)
the neutron number
117.
The bottom number in this isotope notation is
a)
the mass number
b)
the atomic number
c)
the atomic mass
d)
the neutron number
118.

The photo shows which isotope?

a)

Calcium

b)

Silicon

c)

Carbon-13

d)

Copper

e)

Carbon-14

119.
Which of the following is the proper equation for determining the number of neutrons for a given isotope?
a)
mass # - atomic #
b)
atomic mass - protons
c)
protons + electrons
d)
mass # + protons
120.

According to the atomic notation for copper-63, how many neutrons are present in this type of atom?

a)

29

b)

34

c)

63

d)

92

121.

UV light has a higher frequency than IR light. How will the energies compare?

a)

UV has a higher energy than IR

b)

UV has a lower energy than IR

c)

UV and IR have the same energy

d)

There is no way to compare UV and IR

122.

How is the wavelength of light related to the energy?

a)

They are inversely related

b)

They are directly related

c)

They are neither inversely nor directly related

d)

They are both inversely and directly related at the same time.

123.

Select all of the statements that are true about atomic emission spectra:

a)

Two different elements can have the same spectra

b)

it is the fingerprint for an element

c)

it is created when electrons move from higher to lower energy levels

d)

It is created when electrons move from lower to higher energy levels

124.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
125.

How many electrons are in a Ca+2 ion?

a)

16

b)

18

c)

20

d)

22

e)

38

126.

What color of visible light has the greatest energy per photon?

a)

Red

b)

Green

c)

Blue

d)

Violet

127.

Red light has a higher wavelength that purple light. How will the frequency of red light compare to purple light?

a)

Red will have a higher frequency

b)

Red and Purple have the same freqency

c)

Red will have a lower frequency

128.

Which of these is the correct way to write oxygen-18?

a)

A

b)

B

c)

C

d)

D

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