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SHS Chemistry Final Exam Review

Total questions: 109

Worksheet time: 4hrs 38mins

Name
Class
Date
1.

Convert 0.00527 km into cm.

1000m = 1 km

100 cm = 1 m

a)

0.0527

b)

52.7

c)

527

d)

5270

2.

A student does a calculation using her calculator and the number 280.27163 is shown there should only be four significant figures, how should she round the final answer?

a)

280

b)

280.00

c)

280.3

d)

280.27

3.

A cylinder is weighed empty and with a liquid

What is the density of the liquid?

density = mass/volume

a)

13 g/mL

b)

5.7 g/mL

c)

7.4 g/mL

d)

1.7 g/mL

4.

Classify each observation as a physical or chemical property and tally them.

Observation 1: Bubbles form on a piece of metal when it is dropped into acid.

Observation 2: The color of a crystalline substance is yellow.

Observation 3: A shiny metal melts at 650°C

Observation 4: The density of a solution is 1.84 g/cm^3

a)

2 chemical properties and 2 physical

b)

3 chemical properties ad 1 physical

c)

1 chemical property and 3 physical properties

d)

4 chemical properties

5.

All the following are characteristic properties of phosphorus. Which one is a chemical property?

a)

Both red phosphorus and white phosphorus exist in solid allotropic forms.

b)

The red form melts at about 600°C and the white form melts at 44°C

c)

The white form is soluble in liquid carbon disulfide but is insoluble in water.

d)

When exposed to air, white phosphorus will burn spontaneously, but red phosphorus will not.

6.

"The wire was 5.3 cm long." This statement is a...

a)

qualitative observation

b)

quantitative observation

c)

conclusion

d)

hypothesis

7.

362 mL is the same volume as:


1000mL=1L

a)

0.00362 Liters

b)

0.362 Liters

c)

3.62 Liters

d)

362000 Liters

8.

Which of the following measurements is written with four significant figures?

a)

353.0000 m

b)

8200 ft

c)

8.000 s

d)

all of the above

9.

Which of the following is NOT a physical property of water?

a)

It has a boiling point of 100 C

b)

It is a colorless liquid

c)

It is composed of hydrogen and oxygen

d)

Sugar dissolves in it

10.

Which of the following is a physical change?

a)

corrosion

b)

explosion

c)

evaporation

d)

rotting of food

11.

Which of the following CANNOT be classified as a pure substance?

a)

table salt (compound)

b)

nitrogen (element)

c)

air (mixture)

d)

gold (element)

12.

Which of the following is a heterogeneous mixture?

a)

air

b)

steel

c)

salt water

d)

soil

13.

Which of the following is NOT an element?

a)

gold

b)

silver

c)

copper

d)

steel

14.

Which of the following measurements is expressed to three significant figures?

a)

0.007 m

b)

7077 mg

c)

7.30 km

d)

0.070 mm

15.

What is the density of an object having a mass of 8.0g and a volume of 25 mL?

density = mass/volume

a)

3.1 g/mL

b)

0.32 g/mL

c)

2/0 g/mL

d)

200 g/mL

16.

A ring is believed to be made of silver. The ring has a mass of 13.9 grams and a volume of 1.7 mL. Is the substance silver? If not, what is it?

a)

Yes

b)

No, it's platinum

c)

No, it's steel

d)

No, it's white gold

17.

Moves very quickly around the nucleus

a)

Proton

b)

Neutron

c)

Electron

d)

Proton and Neutron

18.

Located in the nucleus

a)

Proton

b)

Neutron

c)

Electron

d)

Proton and Neutron

19.

Has a charge of -1

a)

Proton

b)

Neutron

c)

Electron

d)

Proton and Neutron

20.

Defines the volume of the atom

a)

Proton

b)

Neutron

c)

Electron

d)

Proton and Neutron

21.

Which of the following is an isotope of the element with 20 protons (p=20) and 22 neutrons (n=22)?

a)

titanium-22

b)

calcium-42

c)

zirconium-40

d)

titanium-48

22.

Refer to an isotope with a mass of 31, protons 16, and a charge of 2-

The atomic number is ____.

a)

14

b)

15

c)

16

d)

18

23.

Refer to an isotope with a mass of 31, protons 16, and a charge of 2-

The isotope contains ___ electrons.

a)

14

b)

15

c)

16

d)

18

24.

Refer to an isotope with a mass of 31, protons 16, and a charge of 2-

The nucleus contains __ neutrons.

a)

14

b)

15

c)

16

d)

18

25.

Refer to an isotope with a mass of 31, protons 16, and a charge of 2-

The element is ___.

a)

Si (Silicon)

b)

P (Phosphorus)

c)

S (Sulfur)

d)

Ar (Argon)

26.

Which of the following diagrams represents the correct electron configuration for a Nitrogen atom?

a)
b)
c)
d)
27.

The modern periodic table has the elements arranged in order of increasing

a)

electron energy

b)

atomic size

c)

atomic number

d)

molar mass

28.

Which element would be the best conductor?

a)

Sn (Tin)

b)

As (Arsenic)

c)

S (Sulfur)

d)

P (Phosphorus)

29.

Properties of metals include:

a)

brittleness

b)

poor conductivity

c)

dull surface

d)

can be pounded into sheets

30.

Which one of the following elements is correctly matched with its symbol?

a)

Ag, Gold

b)

Ni, Nickel

c)

Fl, Fluorine

d)

Mg. Manganese

31.

Which of the following is a metalloid?

a)

Ag (Silver)

b)

As (Arsenic)

c)

S (Sulfur)

d)

Pb (Lead)

32.

Which is very unreactive?

a)

halogen family

b)

alkaline earth metal family

c)

alkali metal family

d)

noble gas family

33.

Which forms 2+ ions

a)

halogen family

b)

alkaline earth metal family

c)

alkali metal family

d)

noble gas family

34.

Which reacts with water?

a)

halogen family

b)

alkaline earth metal family

c)

alkali metal family

d)

noble gas family

35.

Which family includes Ca (Calcium), Mg (Magnesium), and Ba (Barium)?

a)

halogen family

b)

alkaline earth metal family

c)

alkali metal family

d)

noble gas family

36.

Which of the following is a transition metal?

a)

Cl (Chlorine)

b)

Ni (Nickel)

c)

P (Phorsphous)

d)

Ca (Calcium)

37.

Which of the following is an alkali metal?

a)

Mg (Magnesium)

b)

Kr (Krypton)

c)

K (Potassium)

d)

Al (Aluminium)

38.

An atom has 6 protons, 7 electrons, and 8 neutrons. What is the atom described?

a)

Carbon

b)

Nitrogen

c)

Oxygen

d)

Fluorine

39.

Which of the following is NOT a solid at room temperature?

a)

Gallium

b)

Indium

c)

Zinc

d)

Mercury

40.

How many valence electrons does nitrogen have?

a)

4

b)

14

c)

5

d)

7

41.

Identify the line in the table that is INCORRECT.

a)

A

b)

B

c)

C

d)

D

42.

An atom has 6 protons, 10 electrons, and 8 neutrons. What is the mass of the atom described?

a)

13

b)

14

c)

15

d)

21

43.

An atom has 6 protons, 10 electrons, and 8 neutrons. What is the charge of the atom described?

a)

-4

b)

-1

c)

0

d)

+2

44.

Barium forns an ion with a charge of:

a)

-3

b)

0

c)

+1

d)

+2

45.

Which one of the following is the correct formula for aluminum oxide?

a)

AlO

b)

Al2O3

c)

Al6O6

d)

Al3O2

46.

What is the name of the compound CF4?

a)

fluorocarbonate

b)

carbon tetrafluoride

c)

tricarbo fluoride

d)

carbon difluorate

47.

Sodium nitride has the formula Na3N. What is the formula for magnesium nitride?

a)

Mg2N

b)

Mg3N2

c)

Mg3N

d)

Mg2N3

48.

What is the formula of the ionic compound between Mg and Br?

a)

MgBr

b)

Mg2Br

c)

Mg2Br3

d)

MgBr2

49.

The correct formula for dinitrogen tetroxide is:

a)

No2

b)

NO3

c)

N2O4

d)

(N2O)4

50.

What is the name of the SO3^2- ion?

a)

sulfate

b)

sulfur trioxate

c)

hydrogen sulfate

d)

sulfite

51.

When a metal and a nonmetal react, the ___ tends to lose electrons and the ____ gains electrons.

a)

nonmetal, nonmetal

b)

metal, nonmetal

c)

nonmetal, metal

d)

none of the above, these elements share electrons

52.

Which substance exhibits ionic bonding rather than covalent bonding?

Ionic (metal + nonmetal)

Covalent (nonmetal+nonmetal)

a)

CO2

b)

N2O4

c)

SiO2

d)

Ca(OH)2

53.

The colecule NF3 has how many lone pairs of electrons on the centra atom?

a)

0

b)

1

c)

2

d)

3

54.

What is the geometrical arrangement of electron pairs in H2O?

a)

linear

b)

trigonal bipyramidal

c)

bent

d)

tetrahedral

55.

The halogens, alkali metals, and alkaline earth metals have _____ valence electrons.

a)

7, 4, and 6

b)

1, 5, and 7

c)

8, 2, and 3

d)

7, 1, and 2

56.

The molecular geometry of the CS2 molecule is _____.

a)

linear

b)

bent

c)

tetrahedral

d)

trigonal planar

57.

Of the following molecules, only _____ is polar.

a)

BF3

b)

CBr4

c)

SiH2Cl2

d)

Cl2

58.

How does calcium obey the octet rule when reacting to form compounds?

a)

It gains electrons

b)

It gives up electrons

c)

It does not change its number of electrons

d)

Calcium does not obey the octet rule

59.

Sodium and chlorine form a bond. What type of bond is formed and how is it formed?

a)

Ionic: sodium and chlorine share an electron

b)

Covalent: sodium and chlorine share an electron

c)

Ionic: sodium donated an electron to chlorine

d)

Ionic: chlorine donated an electron to sodium

60.

Cadmium forms the ion Cd^2+. What type of ion is formed? How was it formed?

a)

This ion is neutral. It naturally occurs like this.

b)

This is a cation. The cadmium loses two electrons

c)

This is an anion. The cadmium gains two electrons.

d)

Cadmium cannot form this ion.

61.

Calcium and bromine combine to form a neutral ionic compound with the formula:

a)

CaBr

b)

Ca2Br

c)

CaBr2

d)

Ca2Br2

62.

Which of the following is a polatomic ion?

a)

Bromide, Br-

b)

Oxide, O2-

c)

Hydroxide, OH

d)

Calcium, Ca2-

63.

Which of the following is a correct application of the octet rule? (Note: Check the charges of these elements, how many do they lose/gain?)

a)

Sodium loses 1 electron to have a cmplete octete with 8 electrons

b)

Beryllium loses 2 electrons to have a complete octet with 0 electrons

c)

Aluminum gains 3 electrons to have a complete octet with 8 electrons

d)

Silicon loses 3 electrons to have a complete octet with 0 electrons

64.

Which of the following is an example of an ionic compound?

a)

CO2

b)

CCl4

c)

FeO

d)

CH

65.

Name his compound: FeO

a)

Iron oxide

b)

Iron (I) oxide

c)

Iron (II) oxide

d)

Iron monoxide

66.

Name this compound: Fe(OH)3

a)

Iron hydroxide

b)

Iron (II) hydroxide

c)

Iron (III) hydroxide

d)

Iron trihydroxide

67.

Name this cmpound: KCl

a)

Potassium chlroine

b)

Potassium chloride

c)

Potassium chlorate

d)

Potassium chlorite

68.

Write this formula: dicarbon tetrahydride

a)

C2H4

b)

C2H2

c)

CH

d)

C4H2

69.

Which set of coefficients balances the equation for the complete combustion of ethane, C2H6?

a)

1, 3, 2, 3

b)

2, 6, 4, 5

c)

1, 6, 2, 6

d)

2, 7, 4, 6

70.

When this equation is balanced, what is the coefficient of O2?

a)

6

b)

12

c)

9

d)

18

71.

During an experiment, an acid was neutralized by the following reaction:

This reaction would be classified as...

a)

synthesis

b)

decomposition

c)

double replacement

d)

single replacement

72.

Which reaction below could be classified as a decomposition reaction?

a)
b)
c)
d)
73.

What gas is formed when Zn metal is mixed with hydrochloric acid, HCl?

a)

CO2

b)

O2

c)

He

d)

H2

74.

In the chemical equation the H2O2 is a ____.

a)

catalyst

b)

product

c)

solid

d)

reactant

75.

If you rewite the word equation as a balanced equation, what will the coefficient for fluorine be?

nitrogen trifluroide ➜ nitrogen + fluorine

a)

6 F

b)

6 F2

c)

F2

d)

3 F2

76.

What are the coefficients that will balance the equation:

a)

1, 3, 1, 3

b)

1, 1, 1, 3

c)

3, 1, 3, 1

d)

1, 3, 3, 1

77.

In the reaction, the (g) stands for:

a)

gas

b)

given

c)

gravimetric

d)

grams

78.

The reaction is an example of which type of reaction?

a)

combustion reaction

b)

single-replacement reaction

c)

synthesis reaction

d)

decomposition reaction

79.

What must occur for a change to be a chemical reaction?

a)

There must be a change in chemical properties

b)

There must be a change in physical preoperties

c)

The change must involve a change in mass

d)

The change must involve a change in volume

80.

What is the molar mass of CaCO3? (Note: add the atomic mass of each element together)

a)

68.1 g/mol

b)

106.0 g/mol

c)

312.2 g/mol

d)

100.1 g/mol

81.

The molar mass of aluminum sulfate, Al2(SO4)3, is...

a)

342 g

b)

150 g

c)

246 g

d)

123 g

82.

Milk of magnesia contains the chemical, magnesium hydroxide, Mg(OH)2. If a bottle contains 35.0 g of Mg(OH)2, how many molecules does it contain?

(Hint: Mg(OH)2 = 58.3 g/mol)

a)

6.02 x 10^23

b)

1.00 x 10^24

c)

5.80 x 10^22

d)

3.61 x 10^23

83.

How many moles are in 3.25 x 10^25 atoms?

a)

54 moles

b)

1.96 x 10^49 moles

c)

0.019 moles

d)

5.4 x 10^47 moles

84.

What is the molar mass of iron (II) oxide, FeO

a)

55.845 g/mol

b)

72.844 g/mol

c)

34 g/mol

d)

15.999 g/mol

85.

What is the volume of 2.8 moles of Cl2 gas?

a)

0.125 L

b)

62.72 L

c)

8.0 L

d)

0.14 L

86.

How many grams of lithium are in 6.7 mole of lithium?

a)

97 grams

b)

1.03 grams

c)

46.5 grams

d)

1.11 grams

87.

Calculate the percentage composition or boron, B, in the compound boron trifluoride, BF3

a)

15.9%

b)

19.0%

c)

25.0%

d)

56.9%

88.

What is the percent nitrogen in ammonium carbonate, (NH4)2CO3?

a)

14.53%

b)

27.83%

c)

29.16%

d)

33.34%

89.

Calculate the mass of hydrogen formed when 25 g of aluminum reacts with excess hydrochloric acid.

a)

0.41 g

b)

1.2 g

c)

0.92 g

d)

2.8 g

90.

What quantity of sulfur diocide, SO2 (64.0 g/mol), is produced when 245 g of dulfuric acid, H2SO4 (98.0 g/mol) reacts completely with zinc metal?

a)

64.0 g

b)

128 g

c)

80.0 g

d)

160 g

91.

At STP, how many liters of oxygen gas react with 4.0 moles of PH3 according to this equation?

a)

32.0

b)

134

c)

89.6

d)

146

92.

How many moles of FeS2 are required to produce 64 grams of SO2 according to the equation?

a)

0.40

b)

3.2

c)

0.50

d)

4.5

93.

In the reaction 2A + B → A2B, if 4 grams of A and 3 grams of B are used, how many grams of A2B will you make?

a)

3

b)

4

c)

7

d)

11

94.

Consider the following equation. If 2 moles of H2O2 are used, how many moles of O2 are produced?

a)

1

b)

2

c)

3

d)

4

95.

How does the gas propellant move when an aerosol can is used?

a)

from a region of high pressure to a region of lower pressure

b)

from a region of high pressure to a region of equally high pressure

c)

from a region of low pressure to a region of lower pressure

d)

from a region of low pressure to a region of equally low pressure

96.

At constant pressure, what happens to the temperature of a gas when it is compressed?

a)

the temperature increases

b)

the temperature does not change

c)

the temperature decreaes

d)

the temperature becomes unpredictable

97.

When the Kelvin temperature of an enclosed gas doubles, the particles of the gas ___.

a)

moves faster

b)

strike the walls of the containter with less force

c)

decrease in average kinetic energy

d)

decrease in volume

98.

As the temperature of a fixed volume of gas increases, the pressure will ___.

a)

vary iversely

b)

increase

c)

decrease

d)

not change

99.

If a sealed syring is plunged into cold water, in which direction will the syringe piston slide?

a)

in

b)

out

c)

no movement will occur

d)

the direction cannot be predicted

100.

A gas occupies a volume of 2.4 L at 14.1 kPa. What volume will the gas occupy at 84.6 kPa?

a)

497 L

b)

2.5 L

c)

14 L

d)

0.40 L

101.

A sample of gas ccupies 17 mL at -112°C. What volume does the sample occupy at 70°C?

a)

10.6 mL

b)

27 mL

c)

36 mL

d)

8.0 mL

102.

A solution of sugar water may be defined as a

a)

heterogeneous imxture

b)

homogeneous mixture

c)

compound

d)

element

103.

Which of the following is a base?

a)

KOH

b)

CO2

c)

HBr

d)

Na2SO4

104.

Which of the following is an acid?

a)

CaCO3

b)

KClO3

c)

CuNO3

d)

H3PO4

105.

What volume of 0.123 M NaOH solution contain 0.625 mol of NaOH?

a)

0.0769 L

b)

0.197 L

c)

5.08 L

d)

625 L

106.

What is the molarity of the solution that results when 1.5 mol NaOH is added to enough water to make 0.500 L of solution?

a)

1.33 M

b)

1.50 M

c)

3.00 M

d)

8.00 M

107.

What is the molarity of the solution that results when 1.24 mol HCl is added to enough water to make 0250 L of solution?

a)

1.46 M

b)

1.80 M

c)

3.24 M

d)

4.96 M

108.

A solution of vinegar has a pH of 4.7. Is the solution acidic, basic, or neutral?

a)

Acidic

b)

Basic

c)

Neutral

109.

Julia makes a pitcher of sweet tea by mixing 50 grams of sugar in a pitched of unsweetened tea. What is the solute?

a)

the sweetened tea

b)

the unsweetened tea

c)

the sugar

d)

the pitcher

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