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Chemistry Questions

Total questions: 85

Worksheet time: 43mins

Name
Class
Date
1.

What type of reaction is:

2Mg + O2 --> 2MgO

a)

synthesis

b)

decomposition

c)

single replacement

d)

neutralization

2.

What type of reaction is:

Mg + O2 --> MgO

a)

single replacement

b)

decomposition

c)

combustion

d)

precipitate

3.

What type of reaction is:

Al2(SO4)3 + KOH --> Al(OH)3 + K2SO4

a)

single replacement

b)

double replacement

c)

synthesis

d)

neutralization

4.

What type of reaction is:

H2O2 --> H2O + O2

a)

synthesis

b)

decomposition

c)

combustion

d)

decomposition & combustion

5.

What type of reaction is:

AgNO3 (aq) + NaCl(aq) --> AgCl(s) + NaNO3 (aq)

Chose all that apply

a)

double replacement

b)

precipitate

c)

neutralization

d)

single replacement

6.

What type of reaction is

Mg(s) + Zn(NO3)2(aq) --> Mg(NO3)2(aq) + Zn(s)

Choose all that apply

a)

single replacement

b)

double replacement

c)

precipitate

d)

neutralization

7.

What type of reaction is:

HCl + NaOH --> NaCl + H2O

Choose all that apply

a)

single replacement

b)

double replacement

c)

precipitate

d)

neutralization

8.

How many significant figures?

1000

a)

1

b)

2

c)

3

d)

4

9.

How many significant figures?

1010

a)

1

b)

2

c)

3

d)

4

10.

How many significant figures?

1001.00

a)

2

b)

4

c)

6

11.

How many significant figures?

0.001010

a)

1

b)

2

c)

3

d)

4

12.

What is the independent variable?

a)

% with college degree

b)

gender

c)

age

d)

birth year

13.

What is the dependent variable?

a)

enzyme activity

b)

pH

14.

Research question: If students spend more time on social media, do they read fewer books?

What is the independent variable?

a)

time on social media

b)

books read

15.

Research question: If I take a nap in the afternoon, does my focus increase the rest of the day?

What is the dependent variable?

a)

napping

b)

focus level

16.

This graph shows which type of relationship?

a)

direct

b)

indirect

c)

inverse

d)

no relationship

17.

This graph shows which type of relationship?

a)

direct

b)

indirect

c)

no relationship

18.

Balance the following equation:

KOH + H3PO4 --> K3PO4 + H2O

a)

2:1:1:3

b)

1:1:1:1

c)

4:2:1:3

d)

3:1:1:3

19.

Balance the following equation:

CaCl2 + Na3PO4 --> Ca3(PO4)2 + NaCl

a)

1:1:1:1

b)

3:2:1:6

c)

2:3:2:3

d)

1:4:2:2

20.

What is the correct way to write:

aluminum nitrate

a)

AlNO3

b)

Al(NO3)2

c)

AlN2

d)

Al(NO3)3

21.

Which is the correct way to write:

Iron (II) selenide

a)

FeSe

b)

Fe2Se

c)

Fe2Se3

d)

FeSe2

22.

Which is the correct way to write:

MgCl2

a)

magnesium chlorate

b)

magnesium chlorite

c)

magnesium (II) chloride

d)

magnesium chloride

23.

Which is the correct way to write:

HBr

a)

hydrogen bromide

b)

hydrobromic acid

c)

bromic acid

d)

hydrogen bromous

24.

Which is the correct way to write:

lead (II) nitrate

a)

PbNO3

b)

Pb(II)NO3

c)

PbNO2

d)

Pb(NO3)2

25.

Which is the correct way to write:

nickle (II) hydroxide

a)

NiH

b)

NiOH

c)

Ni(OH)2

d)

NiH2

26.

Which is the correct way to write:

H2SO4

a)

hydrogen sulfate

b)

sulfuric acid

c)

sulfurous acid

d)

hydrosulfuric acid

27.

Which is the correct way to write:

H2SO3

a)

sulfuric acid

b)

hydrogen sulfate

c)

hydrosulfurous acid

d)

sulfurous acid

28.

Which is the correct way to write:

BrO2

a)

bromic oxide

b)

bromine oxide

c)

bromine dioxide

d)

monobromine dioxide

29.

Which is a diatomic molecule?

a)

bromine

b)

hydroxide

c)

carbon

d)

gallium

30.

Which is a polyatomic molecule?

a)

bromine

b)

hydroxide

c)

oxygen

d)

carbon

31.

Which is ionic?

a)

magnesium oxide

b)

sodium chloride

c)

zinc sulfide

d)

all of the above

32.

How would you write 340,000 in scientific notation?

a)

3.4 x 10^5

b)

.34 x 10^6

c)

3.4 x 10^-5

d)

3.4 x 10^6

33.

Convert 12 mL into deciliters.

a)

1200

b)

120

c)

0.012

d)

0.12

34.

Convert 75 pounds to to decigrams. (1 lb=0.454 kg)

a)

34.05

b)

3.41

c)

340500

d)

3405

35.

Convert 2.3 m/s to km/hr

a)

8.3

b)

3.68

c)

0.061

d)

221

36.

Which of the following is the correct Lewis dot structure for calcium?

a)
b)
c)
d)
37.

Covalent bonds form between _____.

a)

metals & metals

b)

nonmetals & nonmetals

c)

metals & nonmetals

d)

all of the above

38.

Nonpolar covalent bonds will always form between diatomic molecules.

a)

true

b)

false

39.

What type of bond will form between carbon (EN=2.55) and hydrogen (EN=2.2)?

a)

polar covalent

b)

nonpolar covalent

c)

ionic

d)

metallic

40.

Which type of bond will form between oxygen (EN=3.44) and hydrogen (EN=2.2)?

a)

polar covalent

b)

nonpolar covalent

c)

ionic

d)

metallic

41.

This molecule is ____.

a)

polar

b)

nonpolar

42.

Predict the shape?

a)

bent

b)

trigonal pyramidal

c)

tetrahedral

d)

trigonal planar

43.

Predict the shape:

a)

bent

b)

trigonal pyramidal

c)

tetrahedral

d)

trigonal planar

44.

Predict the shape:

a)

bent

b)

linear

c)

trigonal planar

d)

trigonal pyramidal

45.

How many moles of aluminum are needed to react completely with 1.2 mol of FeO?

2Al + 3FeO → 3Fe + Al2O3

a)

1.6

b)

1.2

c)

2.4

d)

0.8

e)

4.8

46.

How many grams of beryllium are needed to produce 36.0 g of hydrogen? (Assume an excess of water)

Be + 2H2O → Be(OH)2 + H2

a)

161

b)

4.00

c)

648

d)

36

47.

Identify the limiting reactant when 11 mol CS2 reacts with 18 mol O2.

CS2 + 3O2 → CO2 + 2SO2

a)

CS2

b)

O2

c)

CO2

d)

SO2

48.

What would be your percent yield if only 12 grams of water were produced in the lab, and the reaction started with 30 g of oxygen with an excess of hydrogen?

2H2 + O2 --> 2H2O

a)

36%

b)

14%

c)

55%

d)

5%

49.

Carbon-12, Carbon-13, and Carbon-14 all have the same number of neutrons.

a)

true

b)

false

50.

One mole of H2O has the same mass as one mole of NaCl.

a)

true

b)

false

51.

1 mole of sodium has the same number of particles as 1 mole of calcium.

a)

true

b)

false

52.

Find the molar mass of calcium hydroxide.

a)

57.1 g/mol

b)

74.1 g/mol

c)

641.2 g/mol

53.

How many protons does fluorine-19 have?

a)

9

b)

10

c)

19

54.

How many neutrons does a neutral atom of iodine have?

a)

53

b)

127

c)

74

55.

How many electrons does a neutral atom of carbon have?

a)

6

b)

12

c)

7

56.

Radium has 2 common isotopes. Rubidium-85 has an abundance of 72.2% and Rubidium-87 has an abundance of 27.8%. What is the average atomic mass of rubidium?

a)

1495 atm

b)

8573 atm

c)

85.6 amu

d)

101.1 amu

57.

The correct abbreviated designation for the electron configuration 1s22s2p6 is:

a)

[He]

b)

[He]

c)

[Ne]

d)

[Ar]

58.

The correct electron configuration for iron is:

a)

1s22s22p63s23p64s23d6

b)

1s22s22p63s23p64s23d4

c)

1s22s22p63s23p6

d)

1s22s22p63s23p64s2

59.

What is the relationship between wavelength and frequency?

a)

direct

b)

indirect

c)

no relationship

60.

Which elements are in the mixture?

a)

lithium & cadmium

b)

cadmium & strontium

c)

strontium & lithium

d)

all of the elements are included in the mixture

61.

Which bright line spectra best represents the wavelength chart at the bottom?

a)

H

b)

He

c)

Ne

d)

Na

e)

Hg

62.

Which has the greatest wavelength?

a)

gamma rays

b)

red light waves

c)

ultraviolet rays

d)

violet light waves

63.

This orbital diagram represents ____.

a)

boron

b)

carbon

c)

nitrogen

d)

oxygen

64.

Which of the following is the correct orbital diagram for carbon?

a)
b)
c)
d)
65.

Which of the following describes a chemical property?

a)

reacts with water

b)

blue color

c)

high luster

d)

high melting point

66.

Which of the following is a physical property?

a)

reacts with an acid

b)

is soluble in water

c)

is flammable

d)

has a low density

67.

Which letters on the diagram represent a phase change?

a)

A, C, and E

b)

B and D

c)

C

d)

A and E

68.

Which letter represents the melting point?

a)

A

b)

B

c)

C

d)

D

69.

Gold is which type of matter?

a)

homogeneous mixture

b)

heterogeneous mixture

c)

element

d)

compound

70.

Black coffee is classified as which type of matter?

a)

homogeneous mixture

b)

heterogeneous mixture

c)

element

d)

compound

71.

If temperature is constant, the relationship between pressure and volume is:

a)

direct

b)

indirect

c)

no relationship

72.

One way to increase the pressure on a gas is to:

a)

decrease temperature

b)

increase volume

c)

increase number of particles of gas

d)

lower the kinetic energy

73.

The pressure of a gas is 750 mmHg when its volume is 400.0 mL. Calculate the pressure (in atm) if the gas is allowed to expand to 600.0 mL at constant temperature.

a)

0.660 atm

b)

1.48 atm

c)

500.0 atm

d)

1125 atm

74.

The volume of a gas is increased from 150 mL to 350 mL by heating it. If the original temperature of the gas was 25 °C, what will its final temperature be?

a)

146°C

b)

10.7°C

c)

58.3°C

d)

422°C

75.

A gas exerts a pressure of 1 atm at standard temperature (273K). What must the temperature be adjusted to for the gas to exert a pressure of 4.00 atm?

a)

-205°C

b)

68.3°C

c)

819°C

d)

1092°C

76.

A quantity of gas has a volume of 250 L at 17°C and 3 atm of pressure. To what volume must the gas be increased for the gas to be under STP (1 atm and 273K)?

a)

78.4 L

b)

88.5 L

c)

706 L

d)

771 L

77.

Which of the following gases has the greatest density (g/L) at STP?

a)

N2

b)

O2

c)

F2

d)

Ne

78.

Avogadro stated that equal volumes of gases under the same conditions of temperature and pressure have equal ___.

a)

number of molecules

b)

number of grams

c)

molar masses

d)

kinetic energy

79.

What volume of O2, collected at 22 °C and 728 mmHg would be produced by the decomposition of 8.15 g KClO3? (do stoich then ideal gas law)

2KClO3(s) --> 2KCl(s) + 3O2(g)

a)

1.12 L

b)

1.48 L

c)

2.23 L

d)

2.52 L

80.

At 18°C, 34.7 grams of carbon dioxide gas creates a pressure of 613 mmHg, what is the volume of the gas? (get into correct units before plugging into equation)

a)

23.3 L

b)

42.9 L

c)

25.8 L

d)

102.3 L

81.

What volume will 2.00 mol of oxygen gas occupy at STP?

a)

0.089 L

b)

44.8 L

c)

569 L

d)

25.6 L

82.

If you dilute 175 mL of a 1.6 M solution of LiCl to 1.0 L, determine the new concentration of the solution.

a)

2.1 M

b)

3.6 M

c)

280 M

d)

0.28 M

83.

How many mL of 5.0 M copper (II) sulfate solution must be added to water to create 200 mL of a 0.30 M copper (II) sulfate solution?

a)

55 mL

b)

12 mL

c)

34 mL

d)

20 mL

84.

How many moles of Na are needed to make 4.5 L of a 1.5 M Na solution?

a)

6.75 mol

b)

0.33 M

c)

0.33 mol

d)

3 M

85.

What is the molarity of 50 g of NaCl dissolved in 150 mL of water?

a)

0.33 M

b)

0.006 M

c)

5.7 M

d)

10.2 M

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