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Semester 1 Exam

Total questions: 100

Worksheet time: 3600secs

Name
Class
Date
1.

Which group of elements typically forms cations and has two valence electrons?

a)

Alkali metals

b)

Alkaline Earth metals

c)

Noble Gasses

d)

Halogens

2.

What type of ion is typically formed by copper?

a)

Anion

b)

Cation

c)

Neutral

d)

none are correct

3.

Which noble gas does not have a complete 8 valence electrons in its outer shell?

a)

He

b)

Ne

c)

Ar

d)

all of them

e)

none are correct

4.

Periods in the periodic table are:

a)

Vertical columns with varying properties

b)

Vertical columns with identical properties

c)

Horizontal rows with varying properties

d)

Horizontal rows with identical properties

5.

Which letter represents an atom in the noble gas group of elements?

a)

A

b)

B

c)

C

d)

D

e)

E

6.

Which letter represents an atom in the alkali metal group of elements?

a)

A

b)

B

c)

C

d)

D

e)

E

7.

Which letter represents an atom in the earth metals group of elements?

a)

A

b)

B

c)

C

d)

D

e)

E

8.

Which element is expected to have the smallest atomic radius based on periodic trends?

The atomic radius decrease as you move left to right on the P.T.

and increase as you move top to bottom on the P.T.

a)

Li

b)

F

c)

Si

d)

Cl

9.

Which of the following elements is not an alkali metal?

a)

Li

b)

Na

c)

B

d)

All are alkali metals

10.

Which of the following elements is not typically considered a metal?

a)

Helium

b)

Iron

c)

Copper

d)

All are metals

11.

Which subatomic particle carries a negative charge and orbits the nucleus?

a)

electron

b)

neutron

c)

proton

d)

nucleus

12.

How many valence electrons do most Halogens possess?

a)

0

b)

2

c)

6

d)

8

e)

7

13.

Which of the following describes isotopes?

a)

Atoms of the same element with different numbers of electrons

b)

Atoms of the same element with different numbers of neutrons

c)

Atoms of the same element with different numbers of protons

d)

All of the above describe isotopes

14.

What role do neutrons play in an atom?

a)

They add to the atom's mass and carry a positive charge

b)

They do not add to the atom's mass but carry a positive charge

c)

They add to the atom's mass and are neutral in charge

d)

They do not add to the atom's mass and are neutral in charge

15.

What is the electron configuration for Bromine (Atomic Number 35)?

a)

1s2 2s2 2p6 3s2 3p5

b)

[Ar] 4s2 3d10 4p5

c)

[Kr] 5s2 4d10 5p5

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

e)

1s2 2s2 2p6 3s2 3p5

16.

What is the electron configuration for Sulfur (Atomic number 16)?

a)

1s2 2s2 2p6 3s2 3p4

b)

1s2 2s2 2p6 3s2 3p5

c)

1s2 2s2 2p6 3s2 3d10 4s2 4p4

d)

1s2 2s2 2p6 3s2 3p3

17.

What is the electron configuration for Calcium (Atomic number 20)?

a)

1s2 2s2 2p6 3s2 3p6 4s2

b)

1s2 2s2 2p6 3s2 3p6 3d10 4s2

c)

1s2 2s2 2p6 3s2 3p6 4s2 4p6

d)

1s2 2s2 2p6 3s2 3p6 3d10 4p6

18.

What is the electron configuation for Iron (Atomic Number 26)?

a)

[Ne] 3s2 3p6 4s2 3d10

b)

[Ar] 4s2 3d10

c)

[Ar] 4s2 3d6

d)

[He] 2s2 2p6 3s2 3p6 4s2 3d6

19.

What is the electron configuration of Manganese (Mn)?

a)

1s²2s²2p⁶3s²3p⁶4s²3d⁴

b)

1s²2s²2p⁶3s²3p⁶4s¹3d⁵

c)

1s²2s²2p⁶3s²3p⁶4s²3d⁵

d)

1s²2p⁶3s²3p⁶4s²3d³

20.

How many protons, neutrons, and electrons are in Nitrogen - 14?

a)

14 protons, 17 neutrons, 11 electrons

b)

7 protons, 7 neutrons, 10 electrons

c)

17 protons, 7 neutrons, 17 electrons

d)

7 protons, 10 neutrons, 10 electrons

21.

How many protons does Fe - 56 contain?

a)

56

b)

26

c)

30

d)

55.85

22.

How many neutrons does Copper contain according to the Periodic Table?

a)

29

b)

35

c)

64

d)

63.55

23.

How many significant figures would be in 0.0402?

a)

2

b)

3

c)

4

d)

5

e)

none of the above

24.

The number 30.0152 rounded to five (5) significant figures is

a)

30.010

b)

30.015

c)

30.020

d)

30.01

e)

none are correct

25.

Convert 9830 grams to pounds. (1 lb = 453.6 grams)

a)

21.7 lbs

b)

0.0461 lbs

c)

4,460,000 lbs

d)

none of the above

26.

Convert 6.93 cm to inches. (2.54 cm = 1 inch)

a)

2.73 inches

b)

0.367 inches

c)

17.6 inches

d)

none of the above

27.

If a student found 1.25 kilograms of a substance, how many grams would they have just found? (1000 g = 1 kg)

a)

0.00125 grams

b)

0.0125 grams

c)

125 grams

d)

1250 grams

28.

An object has a mass of 40.1 grams and occupies a volume of 8.20 mL. The density of this object is? Hint (D = m/V)

a)

329 g/mL

b)

0.204 g/mL

c)

4.89 g/mL

d)

40.1 g/mL

29.

What volume would be occupied by a piece of aluminum (density 2.70 g/mL) weighing 85 grams?

a)

229.5 mL

b)

3.2 mL

c)

31 mL

d)

none of these

30.

What is the density (Density = mass / volume) of the following block? The mass of the block was measured to be 4.170 grams. (Volume = length x width x height)

a)

0.2 g/cm³

b)

0.25 g/cm³

c)

4.0 g/cm³

d)

3.972 g/cm³

31.

The speed of sound at sea level is said to be 3.4 x 10⁵ mm/sec, how fast is this in standard notation?

a)

0.0000034 mm/s

b)

340000 mm/s

c)

3.4 mm/s

d)

none of the above

32.

A lab experiment asks for 30 mL liquid in chemistry class, what volumetric piece of equipment would yield the most accurate result?

a)

25 mL graduated cylinder

b)

50 mL graduated cylinder

c)

40 mL graduated cylinder

d)

1000 mL graduated cylinder

33.

Calculate the mass of a substance which has a volume of 35.0 cm³ and a density of 0.50 g/cm³

a)

17.5

b)

70

c)

0.167

d)

35.5

34.

Which object(s) of the following densities will float on water? (Density of water = 1 g/mL)

a)

0.7

b)

0.9

c)

1.1

d)

1.3

e)

none of these

35.

How many significant figures should the answer have when calculating 4.5 x 3.786

a)

1

b)

2

c)

3

d)

4

e)

none of these

36.

How many decimal places should be in the result of 4.6 + 8.34?

a)

1

b)

2

c)

3

d)

4

e)

none of these

37.

What is the answer rounded to the correct number of significant figures for 3.76 x 1.456

a)

6.00

b)

5

c)

5.5

d)

5.47

38.

The law of conservation of energy states that:

a)

energy can be created and can be destroyed

b)

energy cannot be created but can be destroyed

c)

energy can be created and cannot be destroyed

d)

energy cannot be created and cannot be destroyed

39.

What is the formula for the compound Magnesium nitride?

a)

Mg3N2

b)

MgN

c)

Mg2N3

d)

none of the above

40.

What is the formula for potassium nitrite?

a)

KNO3

b)

K(NO3)2

c)

KNO2

d)

K(NO2)2

41.

The correct name for HgO is

a)

Mercury oxide

b)

Mercury (I) oxide

c)

Mercury (II) oxide

d)

Dimercury monoxide

42.

Name the chemical compound Li2CO3

a)

Lithium carbon oxide

b)

Dilithium monocarbon trioxide

c)

Lithium (II) carboxide

d)

Lithium carbonate

e)

Lithium carboxide

43.

The name of N₂S₃ is

a)

Nitrogen sulfide

b)

trinitrogen disulfide

c)
dinitrogen trisulfide
d)

none of the above

44.

Write the formula for Iron (III) sulfide.

a)

Fe₃Se₂

b)

Fe₃S₂

c)

Fe₂Se₃

d)

Fe₂S₃

45.

The name of N₃S₂ is .

a)

Nitrogen sulfide

b)
trinitrogen disulfide
c)

dinitrogen trisulfide

d)

None are correct

46.

Write the formula for dicarbon octahydride.

a)

C₂H₈

b)

C₈H₂

c)

C₂H₆

d)

C₈H₂

47.

What is the name of this acid: H₂SO4?

a)

Sulfuric Acid

b)

Sulfurous Acid

c)

Hydrosulfuric Acid

d)

Hydrosulfurous Acid

48.

Write the formula for Calcium Sulfide Tetrahydrate.

a)

CaS • 5H₂O

b)

CaS • 4H₂O

c)

CaSO₄ • 4H₂O

d)

CaSO₄ • 5H₂O

49.

When converting grams to moles, what number should we have for the amount of moles in the conversion?

a)

The value of the mole ratio.

b)

The value from in the answer.

c)

The value should always be one.

d)

The value does not matter.

50.

Which represents the greatest mass?

a)

1.0 mol of H

b)

1.0 mol of He

c)

1.0 mol of Li

d)

1.0 mol of Be

51.

What is the molar mass of sucrose, C₆H₁₂O₆?

a)

29.02 g/mol

b)

180.16 g/mol

c)

246.17 g/mol

d)

174.11 g/mol

52.

How many moles of carbon are in a 24 grams sample of carbon?

a)

0.5 moles

b)

1 moles

c)

2 moles

d)

4 moles

53.

How many moles would 1.204 x 1024 molecules of sodium chloride (NaCl) have?

a)

0.50 moles NaCl

b)

1 mole NaCl

c)

1.5 moles NaCl

d)

2.0 moles NaCl

54.

How many liters are in 2.4 moles of water (H2O)?

a)

53.76

b)

964.07

c)

1.45 x 10^24

d)

1.93 x 19^24

55.

How many atoms are in 4.56 grams of Mg(NO3)2?

a)

4.56

b)

676.4

c)

1.85

d)

1.85E22

e)

none of these

56.

What is the molar mass of carbonic acid, H2CO3?

a)

1,152 g/mol

b)

86 g/mol

c)

62 g/mol

d)

29 g/mol

57.

What percentage is Carbon in carbonic acid, H2CO3?

a)

12%

b)

14 %

c)

42 %

d)

58%

58.

What is the molar mass of Copper II Sulfate?

a)

159.62

b)

155

c)

319. 24

d)

224. 3

59.

What is the percent of oxygen in Magnesium Nitride Pentahydrate

a)

41.8

b)

3.2

c)

58.2

d)

62.8

60.

How many grams are in 2.8 moles of sodium (Na)?

a)

1.74 X 10^24 grams

b)

1.74 X 10^23 grams

c)

8.21 grams

d)

64.4 grams

61.

How many molecules are in 25 grams of K2SO4?

a)

7.23 X 10^21 molecules

b)

8.63 X 10^22 molecules

c)

8.63 X 10^23 molecules

d)

8.63 X 10^46 molecules

62.

Which of the following numbers is closest to the number of moles in 55.5 grams of CaCl2?

a)

0.500 moles

b)

0.100 moles

c)

0.050 moles

d)

2.00 moles

63.

The reason that a small number of elements have a whole number instead of a decimal as an atomic mass is because

a)

The weighted average happens to be a whole number

b)

There is only one isotope

c)

There are several isotopes with the same mass

d)

The other elements have isotopes with masses that contain a decimal (Ex: 28.4-Si)

64.

What is the percent composition of H2SO4?

H ______ S ______ O ______

a)

2% , 33% , 65%

b)

12% , 40% , 48%

c)

65% , 33% , 2%

d)

20% , 30% , 50%

65.

In the reaction 2 KClO3 → 2 KCl + 3 O2, potassium chloride is a

a)

product

b)

coefficient

c)

subscript

d)

reactant

66.

Using the reaction, H2 + ZnSO4 → Zn + H2SO4, the Zinc (Zn) is a

a)

product

b)

coefficient

c)

subscript

d)

reactant

67.

Using the reaction, H2 + ZnSO4 → Zn + H2SO4, the 4 in H2SO4 is a

a)

product

b)

coefficient

c)

subscript

d)

reactant

68.

The arrow (-->) in any reaction is best read as

a)

yields / produces

b)

forms / creates

c)

makes / synthesize

d)

arrow

69.

In the reaction 2KClO₃ → 2KCl + 3O₂, the 3 in 2 KClO₃ is a

a)

product

b)

coefficient

c)

subscript

d)

reactant

70.

The type of reaction that produces only carbon dioxide and water is called

a)

synthesis

b)

decomposition

c)

single replacement

d)

double replacement

e)

combustion

71.

Which equation is NOT balanced?

a)

2H₂ + O₂ → 2H₂O

b)

4H₂ + 2O₂ → 4H₂O

c)

H₂ + H₂ + O₂ → H₂O + H₂O

d)

2H₂ + O₂ → H₂O

72.

Which coefficients correctly balance the formula equation: ___Zn(OH)₂ + ___HC₂H₃O₂ → ___Zn(C₂H₃O₂)₂ + ___H₂O

a)

1, 2, 1, 1

b)

2, 1, 2, 1

c)

1, 2, 1, 2

d)

2, 1, 1, 2

73.

Balance the following reaction . . . . HBr + Al(OH)₃ ----> H₂O + AlBr₃

What coefficient goes with H₂O?

a)

1

b)

2

c)

3

d)

4

e)

none of these

74.

Balance the following reaction AgNO₃ + Cu → Ag + Cu(NO₃)₂

What are the coefficients?

a)

2;1;1;2

b)

1;2;1;1

c)

2;1;2;1

d)

1;1;1;2

75.

Use the following BALANCED chemical equation to determine the ratio:

2 HgO → 2Hg + O₂.

What is the ratio of HgO to O₂?

a)

1/1

b)

1/2

c)

2/1

d)

2/2

76.

Use the following chemical equation to determine the ratio: (reaction is unbalanced)

CO₂ + LiOH → Li₂CO₃ + H₂O.

What is the ratio of LiOH to H₂O?

a)

1/1

b)

1/2

c)

2/1

d)

2/2

77.

2 C₂H₆ + 7 O₂ → 4 CO₂ + 6 H₂O.

If 16 moles of carbon dioxide are formed by this reaction,

how many moles of water were also produced?

a)

28 moles

b)

6 moles

c)

24 moles

d)

96 moles

78.

Balance the reaction: __BF₃ + __Li₂SO₃ --> __B₂(SO₃)₃ + __LiF

If 8.0 moles of BF₃ are used in the reaction, how many moles of LiF are produced?

a)

2.7 moles

b)

11 moles

c)

19 moles

d)

24 moles

79.

Balance the reaction: __(NH₄)₃PO₄ + __Pb(NO₃)₄ --> __Pb₃(PO₄)₄ + __NH₄NO₃.

If 4.75 moles of lead nitrate are used in the reaction,

how many moles of ammonium nitrate are produced?

a)

19.0 moles

b)

1.19 moles

c)

4.75 moles

d)

11.1 moles

80.

Using the diagram above, which number is the coefficient?

a)

1

b)

2

c)

3

d)

4

e)

5

81.

Using the diagram, which number is the product(s)?

a)

5

b)

6

c)

7

d)

8

e)

3

82.

How many molecules of sulfur dioxide present in 1.50 moles of SO₂?

(Molar Mass of SO₂ = 64.07 g if needed)

a)

2.39E-24

b)

4.01E23

c)

33.6

d)

9.03E23

e)

none are correct

83.

How many grams are in 2.0 moles of sulfur dioxide, SO₂ gas?

(Molar Mass of SO₂ = 64.07 g if needed)

a)

1.2E24

b)

45

c)

130

d)

0.031

e)

none are correct

84.

How many moles of calcium carbonate in 50 grams of CaCO₃?

(Molar Mass of CaCO₃ = 100.09 g if needed)

a)

0.500

b)

2.23

c)

3.01E25

d)

8.30E-23

e)

none are correct

85.

How many grams are in 3.01x10²³ molecules of Sodium bromide, NaBr?

(Molar Mass of NaBr = 102.09 g if needed)

a)

51.0

b)

6.76E46

c)

204

d)

4.90E-3

e)

none are correct

86.

PCl₃ + Cl₂ ---> PCl₅ Balance the reaction if needed.

What is the mole ratio of chlorine to phosphorus pentachloride?

a)

1/1

b)

2/5

c)

3/2

d)

2/3

e)

none are correct

87.

What is the mole ratio from oxygen to water?

4 NH3 + 3 O2 ---> 2 N2 + 6 H2O

a)

4:3

b)

3:2

c)

2:6

d)

4:6

e)

1:2

88.

C2H6O + 3 O2 ---> 2 CO2 + 3 H2O

How many moles of water are made from 2.7 moles of ethanol?

a)

0.90

b)

8.1

c)

360

d)

4.88E24

e)

none are correct

89.

C (s) + SO2 (g) ---> CS2 (ℓ) + CO (g)

balance the reaction first

How many moles of carbon sulfide are produced if 3.6 moles of sulfur dioxide are used?

a)

1.8

b)

9.0

c)

7.2

d)

none are correct

90.

Pb(NO3)2 (aq) + 2 KI (aq) → PbI2 (s) + 2 KNO3 (aq)

(Molar Masses if needed Pb(NO3)2 = 331.22 g ; KI = 166 g ; PbI2 = 461 g ; KNO3 = 101.11 g)

A student reacted 0.750 g of KI according to the reaction,

how many liters of potassium nitrate are produced?

a)

0.101

b)

5.56

c)

2.02

d)

2790

91.

(Molar Masses if needed Fe = 55.85 g ; O2 = 32 g ; Fe2O3 = 159.7g)

4 Fe (s) + 3 O2 (g) → 2 Fe2O3 (s)

How many grams of iron (III) oxide (ferric oxide),

Fe2O3, are formed from the reaction of 5.00 g of iron metal?

a)

89,200

b)

2.80E-4

c)

28.6

d)

7.15

92.

How many molecules of KMnO4 are needed to carry out this reaction on 11.4 grams of KNO2?

(Molar Masses if needed KNO2 = 85.11 g ; KMnO4 = 158.04 g ; H2SO4 = 98.09 g ; KNO3 = 101.11 g ;

MnSO4 = 118.94 g ; K2SO4 = 174.27 ; H2O = 18.02 g)

5 KNO2 + 2 KMnO4 + 3 H2SO4 ---> 5 KNO3 + 2 MnSO4 + K2SO4 + 3 H2O

a)

2.02E23

b)

3.23E22

c)

2.34E26

d)

1.23E23

93.

Calculate how many grams of iodine are needed to prepare 28.6 grams of ICl by this reaction.

(Molar Masses if needed I2 = 253.8 g ; KIO3 = 214 g ; HCl = 36.46 g ; ICl = 162.35 g ; KCl = 74.55 g

H2O = 18.02 g)

2 I2 + KIO3 + 6 HCl ---> 5 ICl + KCl + 3 H2O

a)

112

b)

11.4

c)

17.9

d)

0.000278

94.

(Molar Masses if needed Pb(SO4)2 = 335.34 g ; LiNO3 = 68.95 g ; Pb(NO3)4 = 331.22 ; Li2SO4 = 109.95 g)

Pb(SO4)2 + 4 LiNO3 → Pb(NO3)4 + 2 Li2SO4

How many grams of lithium nitrate will be needed to make 250 grams of lithium sulfate,

assuming that you have an adequate amount of lead (IV) sulfate to do the reaction?

a)

310

b)

78

c)

7,600,000

d)

none are correct

95.

C2O8

a)

molecular

b)

empirical

96.

K2SO4

a)

molecular

b)

empirical

97.

Mg3O9

a)

molecular

b)

empirical

98.

What is the empirical formula for:

Mg8Si4O16

a)

MgSiO

b)

Mg2SiO4

c)

Mg4Si2O8

d)

Mg2OSi

99.

What is the empirical formula for hydrogen peroxide in the picture?

a)

H2O2

b)

H2O

c)

HO

100.

Which of the following is the molecular formula of the compound HO2?

a)

b)

c)

d)

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