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Worksheets

Chmistry fall 2022

Total questions: 121

Worksheet time: 4hrs 17mins

Name
Class
Date
1.

What is important to remember when working with hot plates and burners?

a)

It's ok to walk away.

b)

Hot plates and burners are not dangerous.

c)

Hot plates and burners should not be left unattended.

d)

Hot plates and burners are fireproof.

2.

Lab waste materials can only poured down the drain, if

a)

you use a lot of water to wash them down.

b)

It is never ok to pour stuff down the drain.

c)

the teacher gives you permission to do so.

d)

they are clear liquids.

3.
240 cm = ___________ m
a)
2400
b)
24
c)
2.4
d)
0.24
4.
15.6 L = ___________ mL
a)
15,600
b)
156,000
c)
1,560,000
d)
15,600,000
5.
2804 mg = ___________ g
a)
0.2804
b)
2.804
c)
28.04
d)
280.4
6.
What is 416,000,000 in scientific notation?
a)
4.16 x 108
b)
4.16 x 109
c)
4.16 x 10-8
d)
4.16 x 10-9
7.
What is 2.8 x 10-4 in standard notation?
a)
28,000
b)
280,000
c)
.00028
d)
.000028
8.

A proton weighs 0.000429 milligrams. Which of the following shows the mass of the proton expressed in scientific notation?

a)

0.429 X 10-3

b)

429 X 10-3

c)

4.29 X 10-4

d)

42.9 X 10-4

9.

What is 5.5 x 1018 divided by 8 x 1017?

a)

6.8 x 100

b)

6.7 x 10-1

c)

6.88 x 100

d)

6.7 x 101

10.
How many significant figures does the following number have?
0.00345
a)
6
b)
5
c)
3
d)
Ambiguous: 3,4,5, or 6
11.

How many significant figures does the following number have?1.2500 x 10310^3  

a)
5
b)
3
c)

Ambiguous: 3 or 5

d)

7

12.
Round 1289 to three significant figures
a)
1290
b)
130
c)
1300
d)
1.29x103
13.
What is 98.907 rounded to 1 significant figure?
a)
98.9
b)
90
c)
100
d)
1x102
14.
Solve and give your answer with the correct number of significant figures
(12.470)(271)
a)
3366.9
b)
3.37x103
c)
3400
d)
3370
15.
Solve and give your answer with the correct number of significant figures
129.6/3
a)
43.0
b)
43
c)
 4x101
d)
40
16.
Solve and give your answer with the correct number of significant figures
24.28 + 12.5
a)
3.687 x 101
b)
36.8
c)
37
d)
3.70x101
17.
Solve and give your answer with the correct number of significant figures
1421-34
a)
1.39x103
b)
1387
c)
1390
d)

1400

18.
How many gallons are in a pool that holds 758,000 Liters?
(1 gallon = 3.79 Liters)
a)
200
b)
20,000
c)
200,000
d)
2,000,000
19.
How many minutes are in a year?
a)
I can't count that high.
b)
525,600min
c)
52,560min
d)
31,536,000min
20.

Convert 62 miles/hour to feet/second. (5,280 ft = 1 mi)

a)

5,456 ft/s

b)

.003 ft/s

c)

91 ft/s

d)

909 ft/s

21.
Gas costs $3.05 a gallon, and your car travels at 27 miles for each gallon of gas. How far can you travel in your car with $95 in your pocket?
a)
11 miles
b)
840 miles
c)
7800 miles
d)
870 miles
22.

A child weighs 40.0 lb and is to receive 0.10 mg of an antibiotic for each kg of body weight. How many milligrams of the antibiotic shall the child receive? (1 kg = 2.2 lbs)

a)

18.2 mg

b)

182 mg

c)

0.182 mg

d)

1.82 mg

23.
What is an example of a Chemical change?
a)
Ripped paper 
b)
boiled egg
c)
cracked egg
d)
sugar in water
24.
Which of the following is a sign that a chemical reaction has occurred?
a)
change in shape
b)
melting
c)
formation of a gas
d)
dissolving
25.

What is a physical property of these strawberries?

a)

Red

b)

Rotten

c)

Flammable

26.

What is a chemical property of paper?

a)

Flammable

b)

White

c)

Light

27.

How many protons are in Sodium?

a)

11

b)

22

c)

12

d)

33

28.

How many electrons are in Aluminium?

a)

40

b)

27

c)

13

d)

14

29.

How many neutrons are in Magnesium?

a)

36

b)

12

c)

24

d)

6

30.

Arsenic has a mass of _______

a)

33

b)

79

c)

75

d)

47

31.

The nucleus is made up of

a)

Protons and neutrons

b)

protons and electrons

c)

electrons and neutrons

d)

neutrons

32.

A proton is described as

a)

a positively charged particle in the nucleus

b)

a positively charged particle in the rings of an atom

c)

a neutrally charge particle in the nucleus

d)

a negatively charge particle in the nucleus

33.
Which scientist developed the atomic theory
a)
Aristotle
b)
Dalton
c)
Democritus
34.
What scientist is best known for his "Plum Pudding" model of the atom?
a)
J.J. Tomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
35.
J.J. Thomson provided evidence that an atom...
a)
is the smallest particle of matter
b)
contains negatively charged particles
c)
has an overall negative charge
d)
has an overall positive charge
36.
Rutherford's gold foil experiment provided evidence that...
a)
negative and positive charges are spread evenly throughout the atom.
b)
alpha particles have a positive charge.
c)
gold is not a dense as previously thought.
d)
there is a dense positively charged nucleus at the center of an atom.
37.
Electrons are not factored into atomic mass because:
a)
They are so small their mass is negligible
b)
They're not in the nucleus
c)
They're too big
d)
They move so quickly their mass is zero
38.

Which part of the atomic theory did Niels Bohr prove?

a)

there are electrons

b)

there is a nucleus

c)

electrons are in energy levels

d)

gold foil experiment

39.
Ions are: 
a)
atoms with a positive or negative charge
b)
atoms with no charge
c)
atoms with ONLY a positive charge
d)
atoms with ONLY a negative charge
40.
When an atom loses a valence electron, it becomes a(n) _____________ ion.
a)
positive
b)
negative
c)
neutral
d)
polyatomic
41.
When an atom gains a valence electron, it becomes a(n) _____________ ion.
a)
positive
b)
negative
c)
neutral
d)
polyatomic
42.
What is the charge of an atom that has gained one electron?
a)
-1
b)
-2
c)
+1
d)
+2
43.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
44.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
45.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
46.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
47.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
48.
How many valence electrons are in Phosphorus?
a)
15
b)
4
c)
5
d)
31
49.

Choose the correct shortcut configuration for iodine.

a)

[Ar]4s24d104p5

b)

[Kr]5s24d105p5

c)

[Xe]5s25d105p5

d)

none of the above

50.
What is the abbreviated electron configuration for barium?
a)
[Xe] 6s2
b)
[Rn] 6s2
c)
[Ar] 4s2 3d10 4p5
d)
[He] 2s2 3p1
51.

What is the shorthand configuration for Lead?

a)

[Xe]6s24f145d106p2

b)

[Xe]6s25d106p2

c)

[Rn]6s25d106p2

d)

[Rn]6s24f145d106p2

52.

The full range of frequencies of electromagnetic radiation is called

a)

visible light

b)

the electromagnetic spectrum

c)

radio waves

d)

invisible radiation

53.

The waves with the longest wavelengths in the electromagnetic spectrum

a)

Infrared rays

b)

gamma rays

c)

radio waves

d)

X-rays

54.

What happens to frequency when the energy increases?

a)

it increases

b)

it stays the same

c)

it decreases

55.

What part of the wave is shown at letter A?

a)

crest

b)

wavelength

c)

trough

d)

frequency

56.

What does a wave carry?

a)

boats

b)

energy

c)

matter

d)

water

57.

Which wave has a greater frequency?

a)

wave B

b)

wave C

58.

Select the correct order of waves on the EMS from low to high energy

a)

Radio wave, Microwave, Infrared, Visible, Ultraviolet, X-ray, Gamma

b)

Visible, Microwave, Infrared, Ultraviolet, X-ray, Gamma, Radio wave

c)

Gamma, X-ray, Ultraviolet, Visible, Infrared, Microwave, Radio wave

d)

Microwave, Radio wave, Visible, Infrared, Ultraviolet, X-ray, Gamma

59.

Utilized in treating cancer, the radiotherapy

a)

gamma ray

b)

x-ray

c)

visible light

d)

microwave

60.

What is the molar mass of fluorine gas, F2?

a)

18.998 g/mol

b)

38 g/mol

c)

9 g/mol

d)

18 g/mol

61.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
62.

Calculate the molar mass of Ba(C2H3O2)2

a)

255.3 g/mol

b)

237.3 g/mol

c)

228.3 g/mol

d)

196.3 g/mol

63.

Calculate the molar mass of Cu2O.

a)

37 g/mol

b)

45 g/mol

c)

79.5 g/mol

d)

143 g/mol

64.
In chemistry, a "mole" is:
a)
The mass of an atom
b)
a large number used to count particles
c)
based on the volume of a substance
65.
What would be the mass of 1.5mol H2O
a)
20
b)
27
c)
32
d)
40
66.
What is the mass of 0.75 moles of (NH4)3PO4?
a)
101.75 g
b)
121.75 g
c)
111.75 g
d)
131.75 g
67.
How many moles are there in 12.7g of CaF2?
a)
0.20 mol
b)
1,000.76 mol
c)
6.14 mol
d)
0.16 mol
68.
How many moles of (NH4)2O are present in 74.9 g?
a)
3,907.0  moles
b)
1.44 moles
c)
8.67x1023moles
d)
0.79 moles
69.

What percentage of the total atomic mass of carbon monoxide (CO) is composed of carbon?

a)

29%

b)

43%

c)

57%

d)

73%

70.

Lithium phosphide (three lithium atoms with one phosphorus atom) has a chemical formula of Li3P. If you look at the total atomic mass of Li3P, does lithium or phosphorus make up more of the mass?

a)

lithium

b)

phosphorus

c)

they are exactly the same

d)

it is impossible to tell

71.

What percentage of the total atomic mass of calcium nitrate (Ca(NO3)2) is composed of nitrogen? Hint - another way to think of calcium nitrate is Ca(NO3)(NO3).

a)

17%

b)

24%

c)

29%

d)

59%

72.
What is the percent composition by mass of sulfur in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
73.

A substance that conducts heat and electricity well, is shiny, and is malleable.

a)

metal

b)

nonmetal

c)

atom

d)

element

74.

A substance that does not tend to conduct heat and electricity, is dull, and tends to crumble, break, or shatter when pounded.

a)

nonmetal

b)

metal

c)

group

d)

period

75.

Elements in a group have the same number of ___________.

a)

valence electrons

b)

protons

c)

neutrons

d)

energy levels

76.

What are Group 1 elements known as?

a)

Alkali metals

b)

Transition elements

c)

Alkaline earth metals

d)

Inner transition elements

77.

Mendeelev's periodic table was arranged based on increasing?

a)

Atomic Mass

b)

Atomic Number

c)

Color

d)

Alphabetical Order

78.

The modern periodic table is arranged based on increasing?

a)

Atomic Mass

b)

Atomic Number

c)

Color

d)

Alphabetical Order

79.
Which of the following is an Alkali Metal? 
a)
Magnesium
b)
Chromium
c)
Sodium
d)
Fluorine 
80.
Which of the following is an Alkaline Earth Metal? 
a)
Calcium
b)
Lithium
c)
Phosphorus
d)
Copper 
81.
Which of the following is a transition metal? 
a)
Iron
b)
Oxygen
c)
Neon
d)
Barium
82.
Which of the following is a Halogen? 
a)
Bromine
b)
Rubidium
c)
Argon
d)
Beryllium
83.
Which of the following is a Noble Gas? 
a)
Krypton
b)
Chlorine
c)
Radium
d)
Gallium
84.
Which of the following is the most reactive group of metals? 
a)
Alkali
b)
Alkaline Earth
c)
Halogen
d)
Transition Metals
85.
Which of the following is the most reactive group of non-metals? 
a)
Alkali
b)
Alkali Earth
c)
Halogen
d)
Noble Gas
86.
Which of the following groups is inert? 
a)
Alkali
b)
Transition Metals
c)
Halogens
d)
Noble Gas
87.

Which of the following elements is a metalloid?

a)

Neon

b)

Selenium

c)

Mercury

d)

Antimony

88.

Lanthanide series, a series of metallic elements, included in the rare-earth metals , in _________ of the periodic table

a)

Group 1

b)

Group 2

c)

Group 3

d)

Group 5

89.
What element in Group 1 is not a metal but a nonmetal?
a)
Helium
b)
Lithium
c)
Hydrogen
d)
Oxygen
90.
Some students conducted a laboratory investigation to learn more about the physical properties of different elements. They observed four samples and recorded their observations in the table . Based on these observations, which sample is most likely a nonmetal?
a)
Sample 1
b)
Sample 2
c)
Sample 3
d)
Sample 4
91.

Strontium nitride

a)

SrN

b)

Sr3N2

c)

Sr2N3

d)

N3Sr2

92.

BeI2

a)

Beryllium (II) iodide

b)

Beryllium iodine

c)

Beryllium iodide

d)

Beryllium (I) iodide

93.

CuS

a)

copper sulfide

b)

copper (I) sulfide

c)

copper (II) sulfide

d)

copper (i) sulfate

94.

FePO4

a)

iron phosphite

b)

iron (III) phosphite

c)

iron (III) phosphate

d)

iron (II) phosphite

95.

Cr2O3

a)

chromium oxide

b)

chromium hydroxide

c)

chromium (II) oxide

d)

chromium (III) oxide

96.

iron (II) chlorate

a)

Fe2ClO3

b)

FeClO3

c)

Fe(ClO4)2

d)

Fe(ClO3)2

97.

NH4NO3

a)

ammonium nitrite

b)

hydrogen nitrate

c)

ammonium oxide

d)

ammonium nitrate

98.

Li3PO4

a)

lithium phosphate

b)

lithium (I) phosphate

c)

lithium (III) phosphate

d)

lithium phosphite

99.
Name the following ionic compound: MgSO4
a)
magnesium sulfoxide
b)
magnesium sulfide
c)
magnesium sulfate
d)
magnesium oxide
100.
Name the following compound: FeCl3
a)
iron chloride
b)
iron III chloride
c)
iron chlorate
d)
iron III chlorate
101.
Name the ionic compound SnSe2
a)
Tin diselenide
b)
Tin (IV) Selenide
c)
Tin selenide
d)
Tin (II) triselenide
102.
Cu2CO3
a)
copper carbonate
b)
copper II carbonate
c)
copper I carbonate
d)
copper carbon oxide
103.
Cu2CO3
a)
copper carbonate
b)
copper II carbonate
c)
copper I carbonate
d)
copper carbon oxide
104.

How many moles are in 19.82 g Mg?

a)

1.23 mol Mg

b)

481.70 mol Mg

c)

1.00 mol Mg

d)

0.82 mol Mg

105.

What is the percent composition by mass of sulfur (S) in the compound MgSO4?

a)

20.22%

b)

19.85%

c)

26.64%

d)

28.64%

106.

Determine the mass of 4.20 moles of C6H12

a)

354 g

b)

84 g

c)

337 g

d)

421 g

107.

How many grams are in 1.2 moles of Neon?

a)

0.05 grams

b)

16.6 grams

c)

21.2 grams

d)

24 grams

108.
What is the percent by mass of oxygen in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
109.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
110.
What is the percent composition by mass of oxygen in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
111.

What is the molar mass of lithium oxide? (Use 'g/mol' in your answer as your unit.)

(a)  

112.

What is the molar mass of PbSO4?

a)

303.27 g/mol

b)

255.27 g/mol

c)

163.87 g/mol

d)

372.27 g/mol

113.

Shivani measures out 3.0 moles of epsom salt (MgSO4) to put in her bath. How many grams of MgSO4 went in the bath?

a)

3.6 x 1024 g

b)

720 g

c)

0.050 g

d)

360 g

114.

Find the mass of 2.82 mol of MgCl2. Round to the nearest tenth.

a)

552.9 g

b)

495.8 g

c)

55.2 g

d)

268 g

115.

Find the mass of 3.0 mol of H2O. Round to the nearest tenth.

a)

57.9 g

b)

54.0 g

c)

68.4 g

d)

62.3 g

116.

Determine the number of moles of Mg3P2 that are in 583 g of the compound.

a)

2.9 mol

b)

6.1 mol

c)

4.3 mol

d)

1.7 mol

117.

Determine the number of moles of Mg3P2 that are in 583 g of the compound.

a)

2.9 mol

b)

6.1 mol

c)

4.3 mol

d)

1.7 mol

118.
What is the molar mass of AgF
a)
514.9g/mol
b)
99.7g/mol
c)
126.9 g/mol
d)
198.8g/mol
119.
What is the molar mass of NaBr
a)
381.9g/mol
b)
102.9 g/mol
c)
213.6g/mol
d)
93.0g/mol
120.
What is the molar mass of Ca(OH)2
a)
74.1 g/mol
b)
210.0g/mol
c)
98.9g/mol
d)
219.9g/mol
121.

Find the mass of 3.6 mol of Au.

a)

843.6 g

b)

709.2 g

c)

435.9 g

d)

196.9 g

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