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CHEM 101 Practice

Total questions: 70

Worksheet time: 2hrs 33mins

Name
Class
Date
1.

A pure substance is:

a)

Composed of two or more different types of atoms or molecules combined in variable proportions

b)

Composed of only one type of atom or molecule

c)

Composed of two or more regions with different compositions

d)

Composed of two or more different types of atoms or molecules that has constant composition

e)

None of the above

2.

Which of the following items is a physical property?

a)

The corrosive action of acid rain on granite

b)

The odor of spearmint gum

c)

The combustion of gasoline

d)

The tarnishing of a copper statue

e)

None of the above

3.

What is the atomic symbol for tin?

a)

Sn

b)

Ti

c)

Tn

d)

Si

e)

None of the above

4.

Ions are formed when atoms

a)

gain or lose protons

b)

gain or lose electrons

c)

gain or lose neutrons

d)

each of these results in ion formation

e)

none of these results in ion formation

5.

How many protons and neutrons are in Cl-37

a)

20 protons, 17 neutrons

b)

17 protons, 37 neutrons

c)

17 protons, 20 neutrons

d)

37 protons, 17 neutrons

e)

none of the above

6.

In the number 48.93, which digit is estimated?

a)

4

b)

8

c)

9

d)

3

e)

none of the above, all digits are certain

7.

Determine the answer to the following equation with correct number of significant figures:


2.02 + 8.102 - 0.0297 = _________

a)

10.0923

b)

10.09

c)

10.1

d)

10.092

e)

none of the above

8.

Which state of matter has atomic spacing that is close together and indefinite shape?

a)

liquid

b)

solid

c)

gas

d)

plasma

e)

none of the above

9.

How would you classify sugar?

a)

pure substance - compound

b)

mixture - heterogenous

c)

pure substance - element

d)

mixture - homogenous

e)

none of the above

10.

Xe is a member of which family?

a)

Noble Gases

b)

Halogens

c)

Alkaline Earth Metals

d)

Alkali Metals

e)

None of the above

11.

The number of protons in the nucleus of an atom

a)

is called the atomic number

b)

is given the symbol "Z"

c)

identifies the atom as a particular element

d)

is the same for all isotopes of an element

e)

all of the above

12.

How would the number 1.09 x 101 be expressed in decimal form?

a)

109

b)

0.109

c)

1.09

d)

10.9

e)

none of the above

13.

Which state of matter has indefinite shape and is compressible?

a)

liquid

b)

solid

c)

gas

d)

plasma

e)

none of the above

14.

Which measurement below represents the heaviest atom?

a)

1 mg

b)

1 kg

c)

1 pg

d)

1 Mg

e)

1 dg

15.

The correct number of significant figures in the number 4.0 x 10-2 is:

a)

1

b)

2

c)

3

d)

Ambiguous

e)

None of the above

16.

Isotopes are:

a)

atoms of the same element that have different number of neutrons

b)

atoms of the same element that have different number of protons

c)

atoms of the same element that have different number of electrons

d)

atoms of the same element that have the same number of neutrons

e)

none of the above

17.

Group 7A (17) elements are called:

a)

noble gases

b)

halogens

c)

alkaline earth metals

d)

alkali metals

e)

none of the above

18.

Which of the following items is a chemical property?

a)

The paint color on a new red Corvette

b)

The odor of spearmint gum

c)

The melting and boiling point of water

d)

The tarnishing of a copper statue

e)

none of the above

19.

What is the density of 96 mL of a liquid that has a mass of 90.5 g?

a)

0.94 g/mL

b)

1.1 g/mL

c)

186.5 g/mL

d)

28.4 g/mL

e)

none of the above

20.

How many significant figures are in the number 2903?

a)

2

b)

5

c)

4

d)

3

e)

none of the above

21.

Suppose a thermometer has marks at every one degree increment and the mercury level on the thermometer is exactly between the 25 and 26 degree Celsius marks. We should properly report the temperature measurement as:

a)

25oC

b)

26oC

c)

25.5oC

d)

25.50oC

e)

25.55oC

22.

Which of the following elements has only 12 protons?

a)

C

b)

Zn

c)

Mg

d)

O

e)

None of the above

23.

When elements combine to form compounds,

a)

their properties are an average of all elements in the compound.

b)

their properties change completely.

c)

their properties do not change.

d)

their properties are completely random.

e)

none of the above are correct

24.

How many grams of chlorine gas are needed to make 117 g of sodium chloride (NaCl)?

Given the reaction:

2 Na + Cl2 → 2 NaCl

a)

71.0 g

b)

142 g

c)

35.5 g

d)

48.2 g

e)

Not enough information

25.

A 7.96 g sample of silver (Ag) reacts with oxygen to form 8.55 g of the metal oxide. What is the formula of the oxide?

a)

AgO

b)

AgO2

c)

Ag2O

d)

Ag3O

e)

None of the above

26.

How many of each type of atom are there in the formula Ca3(PO4)2?

a)

Ca = 3; P = 1; O = 4

b)

Ca = 3; P = 2; O = 4

c)

Ca = 3; P = 2; O = 8

d)

Ca = 3; P = 1; O = 8

e)

None of the above

27.

Before a chemical reaction can be written, one must know

a)

the atomic mass of all the elements involved.

b)

the molar mass of all the compounds.

c)

the symbols and formulas of all reactants and products.

d)

the number of moles of all reactants and products.

e)

none of the above

28.

How many waffles can be made from 1 dozen eggs, assuming you have enough of all other ingredients? Given:

2 cups flour + 3 eggs + 1 tbs oil → 4 waffles

a)

48

b)

12

c)

4

d)

16

e)

Not enough information

29.

What is the correct formula of a compound that has ten oxygen atoms and four phosphorus atoms?

a)

O10P4

b)

10 OP4

c)

4 PO10

d)

P4O10

e)

None of the above

30.

Which of the following equations is NOT balanced properly?

a)

2 Cr + 6 HCl → 2 CrCl3 + 3 H2

b)

2 NaHCO3 → Na2CO3 + CO2 + H2O

c)

Cr2(SO4)3 + 6 KOH → 2 Cr(OH)3 + 3 K2SO4

d)

4 NH3 + 14 O2 → 4 NO2 + 6 H2O

e)

None of the above

31.

Suppose a vodka martini contains 30% alcohol with the remaining portion of the drink composed of water. What is the solute in this type of martini?

a)

Water

b)

Alcohol

c)

Ice

d)

Olive

e)

None of the above

32.

What is the formula mass of copper(II) fluroide?

a)

101.55 g/mol

b)

146.10 g/mol

c)

90.00 g/mol

d)

165.10 g/mol

e)

none of the above

33.

What are the coefficients for the following reaction when it is properly balanced?

_____ O2 + _____ CH4 → _____ CO2 + _____ H2O

a)

2, 1, 3, 1

b)

2, 3, 2, 2

c)

1, 3, 2, 1

d)

2, 1, 1, 2

e)

None of the above

34.

If the theoretical yield of a reaction is 42.0 g of product and the percent yield is 75%. How many grams were actually produced?

a)

5,400 g

b)

56 g

c)

32 g

d)

1.8 g

e)

None of the above

35.

The mass of one mole of carbon dioxide is _____________ g.

a)

28.01

b)

384.4

c)

32.00

d)

44.01

e)

None of the above

36.

How many total atoms are in the formula Al2(CO3)3?

a)

8

b)

9

c)

12

d)

14

e)

None of the above

37.

What is the theoretical yield of waffles if you have 5 cups of flour, 9 eggs, and 3 tbs of oil? Given:

2 cups flour + 3 eggs + 1 tbs oil →4 waffles

a)

10

b)

12

c)

6

d)

4

e)

Not enough information

38.

What would the formula of diiodine pentasulfide be?

a)

I5S2

b)

I2S5

c)

I4S9

d)

I2S7

e)

None of the above

39.

When solid NaCl is stirred into water, which of the following is NOT true?

a)

Individual sodium and chloride ions are present.

b)

The solution will conduct electricity.

c)

The solution will taste salty.

d)

The NaCl will fail to dissolve.

e)

None of the above

40.

Given the balanced equation:

CH4 + 2 O2 → CO2 + 2 H2O

Which of the following is NOT a correct conversion factor?

a)

2 mol H2O = 18.02 g H2O

b)

1 mol O2 = 32.00 g O2

c)

1 mol CH4 = 2 mol H2O

d)

2 mol O2 = 1 mol CO2

e)

None of the above

41.

Which formula shows the proper use of parentheses?

a)

Ca(F)2

b)

Ca(SO4)

c)

(NH4)3(PO4)

d)

Ca(NO3)2

e)

None of the above

42.

How many valence electrons are in a chlorine atom?

a)

1

b)

17

c)

10

d)

7

e)

None of the above

43.

Substance A is a molecular compound that dissolves in gasoline but not in water. The molecules of A are very likely:

a)

metallic

b)

nonmetallic

c)

polar

d)

nonpolar

e)

none of the above

44.

How many electrons are unpaired in the orbitals of nitrogen?

a)

14

b)

5

c)

9

d)

3

e)

None of the above

45.

Which intermolecular force is the strongest?

a)

Dispersion Forces

b)

Dipole-dipole forces

c)

Hydrogen Bonding

d)

X-forces

e)

None of the above

46.

NaCl is which type of solid?

a)

Molecular solid

b)

Ionic solid

c)

Covalent atomic solid

d)

Nonbonding atomic solid

e)

Metallic atomic solid

47.

What do the alkali metals all have in common?

a)

They all undergo similar reactions.

b)

They all have similar physical properties.

c)

They all form +1 ions

d)

They all have the same number of valence electrons.

e)

All of the above

48.

The measure of the resistance to the flow of a liquid is called:

a)

vapor pressure

b)

sublimation

c)

viscosity

d)

condensation

e)

none of the above

49.

The ideal gas law is:

a)

PV = nRTPV\ =\ nRT

b)

P = nRTVP\ =\ \frac{nRT}{V}

c)

T =PVnRT\ =\frac{PV}{nR}

d)

V=nRTPV=\frac{nRT}{P}

e)

All of the above are forms of the ideal gas law

50.

Which state of matter has a high density and a definite volume?

a)

solids

b)

liquids

c)

gases

d)

both solids and liquids

e)

none of the above

51.

The opposite process of freezing is:

a)

evaporation

b)

sublimation

c)

boiling

d)

condensation

e)

none of the above

52.

A 325 mL of gas is initially at a pressure of 721 torr and a temperature of 32 oC. If this gas is compressed to a volume of 286 mL and the pressure increases to 901 torr, what will be the new temperature of the gas (reported to three significant figures in oC)?

a)

35.2 oC

b)

335 oC

c)

62.4 oC

d)

215 oC

e)

None of the above

53.

Which intermolecular force is present in all molecules and atoms?

a)

Dispersion forces

b)

Dipole-dipole forces

c)

Hydrogen Bonding

d)

X-forces

e)

None of the above

54.

Intermolecular forces are responsible for:

a)

The taste sensations

b)

The shape of protein molecules

c)

The function of DNA

d)

The existence of liquids and solids

e)

All of the above

55.

Charles' Law is expressed as:

a)

V is proportional to 1/P

b)

P is proportional to V

c)

V is proportional to 1/T

d)

V is proportional to T

e)

None of the above

56.

How many electrons can exist in an orbital?

a)

1

b)

2

c)

3

d)

4

e)

None of the above

57.

When a nonmetal bonds with a nonmetal

a)

a molecular compound forms.

b)

a covalent bond is involved.

c)

electrons are shared.

d)

all of the above are true

e)

none of the above are true

58.

To solve problems using Charles' Law, which mathematical equation should be used?

a)

V1T1=V2T2\frac{V_1}{T_1}=\frac{V_2}{T_2}

b)

T1V1=T2V2T_1V_1=T_2V_2

c)

P1V2=P2V1\frac{P_1}{V_2}=\frac{P_2}{V_1}

d)

P2V1=P1V2P_2V_1=P_1V_2

e)

None of the above

59.

Which of the following is NOT a property of acids?

a)

acids have a slippery feel

b)

acids have a sour taste

c)

acids turn litmus paper red

d)

acids dissolve many metals

e)

all of the above are properties of acids

60.

The Bronsted-Lowry definition of a base is:

a)

a proton donor

b)

a proton acceptor

c)

produces H+ in solution

d)

produces OH- in solution

e)

none of the above

61.

In the following reaction:

HCO3- + H2O →H2CO3 + OH-

a)

HCO3- is an acid and H2CO3 is its conjugate base

b)

H2O is an acid and OH- is its conjugate base

c)

HCO3- is an acid and OH- is its conjugate base

d)

H2O is an acid and H2CO3 is its conjugate base

e)

H2O is an acid and HCO3- is its conjugate base

62.

What is the concentration of the hydronium ions (H3O+) in an acidic solution?

a)

0.0 M

b)

1.0 x 10-7 M

c)

1.0 x 10-14 M

d)

Greater than 1.0 x 10-7 M

e)

Less than 1.0 x 10-7 M

63.

If the pH of an aqueous solution changed from 9.10 to 4.67, what happened to the hydronium ion concentration?

a)

It decreased

b)

It became zero

c)

It became less than zero

d)

It increased

e)

None of the above

64.

What is the [OH-] in a solution that has a pOH of 9.65?

a)

4.5 x 10-9 M

b)

4.5 x 105 M

c)

9.8 x 10-1 M

d)

2.2 x 10-10 M

e)

None of the above

65.

What is the pH of a solution that has a [H+] = 0.0045 M?

a)

1.35

b)

2.35

c)

3.35

d)

7.0045

e)

None of the above

66.

Determine the mass in grams of 3.00 x 1021 atoms of arsenic. (The mass of one mole of arsenic is 74.92 g.)

a)

2.25 x 1023 g

b)

6.65 x 10-5 g

c)

0.373 g

d)

37.3 g

e)

None of the above

67.

Determine the mass, in grams, of 0.400 mol Pb.

a)

0.00193 g

b)

82.88 g

c)

2.40 x 1023 g

d)

0.829 g

e)

None of the above

68.

How many grams of NO can be formed from 4.96 mol of NO2 in the reaction below?

3 NO2 + H2O → 2 HNO3 + NO

a)

0.4962 g

b)

446.5 g

c)

0.05509 g

d)

49.62 g

e)

None of the above

69.

How many grams of H2 can be formed from 54.6 g of NH3 in the following reaction?

2 NH3 → 2 H2 + N2

a)

9.71 g

b)

165 g

c)

4.32 g

d)

2.38 g

e)

None of the above

70.

If 24.7 g of NO and 13.8 g of O2 are used to form NO2, how many moles of excess reactant will be left over?

2 NO + O2 → 2 NO2

a)

0.431 mol

b)

0.412 mol

c)

0.823 mol

d)

0.020 mol

e)

None of the above

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