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SDSMT Exam 1 Practice

Total questions: 100

Worksheet time: 1hrs 2mins

Name
Class
Date
1.

Which of the following is NOT a characteristic of a good scientific hypothesis?

a)

It is testable

b)

It is based on existing knowledge

c)

It is vague and general

d)

It can be used to make predictions

2.

Which of the following is NOT a requirement for a hypothesis to be considered scientific?

a)

It must be falsifiable

b)

It must be based on empirical evidence

c)

It must be a personal belief

d)

It must be able to predict outcomes

3.

Which of the following is NOT a characteristic of a scientific hypothesis?

a)

It must be testable

b)

It must be based on observable phenomena

c)

It must be a common assumption

d)

It must be able to be proven wrong

4.

Which of the following quantities is equivalent to 345 µg?

a)

0.345 mg

b)

3.45 g

c)

0.00345 kg

d)

345,000 kg

e)

0.345 g

5.

Which of the following quantities is equivalent to 500 µg?

a)

0.5 mg

b)

5 g

c)

0.005 kg

d)

500,000 kg

e)

0.5 g

6.

Which of the following quantities is equivalent to 2000 µg?

a)

2 mg

b)

20 g

c)

0.002 kg

d)

2,000,000 kg

e)

2 g

7.

You have a 200 gram sample of each of the following metals. Which sample has the smallest volume?

a)

Aluminum, d = 2.7 g/cm3

b)

Magnesium, d = 1.74 g/cm3

c)

Gold, d = 19.3 g/cm3

d)

Silver, d = 10.5 g/cm3

e)

Iron, d = 7.86 g/cm3

8.

You have a 300 gram sample of each of the following metals. Which sample has the largest volume?

a)

Lead, d = 11.34 g/cm3

b)

Copper, d = 8.96 g/cm3

c)

Platinum, d = 21.45 g/cm3

d)

Zinc, d = 7.14 g/cm3

e)

Nickel, d = 8.91 g/cm3

9.

You have a 500 gram sample of each of the following metals. Which sample has the smallest volume?

a)

Iron, d = 7.87 g/cm3

b)

Gold, d = 19.32 g/cm3

c)

Aluminium, d = 2.70 g/cm3

d)

Silver, d = 10.49 g/cm3

e)

Tin, d = 7.31 g/cm3

10.

You have a sample of each of the following five metals, with the mass and density of each sample given. Which sample has the largest volume?

a)

Al, mass = 200 g, d = 2.7 g/cm3

b)

Mg, mass = 150 g, d = 1.74 g/cm3

c)

Cu, mass = 300 g, d = 8.92 g/cm3

d)

Ag, mass = 250 g, d = 10.5 g/cm3

e)

Fe, mass = 275 g, d = 7.86 g/cm3

11.

You have a sample of each of the following five metals, with the mass and density of each sample given. Which sample has the smallest volume?

a)

Al, mass = 250 g,

d = 2.7 g/cm3

b)

Mg, mass = 200 g,

d = 1.74 g/cm3

c)

Cu, mass = 350 g,

d = 8.92 g/cm3

d)

Ag, mass = 300 g,

d = 10.5 g/cm3

e)

Fe, mass = 325 g,

d = 7.86 g/cm3

12.

Which one of the following would have approximately the same mass as 30.0 cm3 of gold (d = 19.3 g/cm3)?

a)

32.0 cm3 of silver (d = 10.5 g/cm3)

b)

10.3 cm3 of lead (d = 11.3 g/cm3)

c)

3.50 cm3 of copper (d = 8.98 g/cm3)

d)

200 cm3 of tin (5.75 g/cm3)

13.

Which one of the following would have approximately the same mass as 50.0 cm3 of silver (d = 10.5 g/cm3)?

a)

52.0 cm3 of gold (d = 19.3 g/cm3)

b)

46.5 cm3 of lead (d = 11.3 g/cm3)

c)

5.60 cm3 of copper (d = 8.98 g/cm3)

d)

300 cm3 of tin (5.75 g/cm3)

14.

A lab technician is trying to identify an unknown metal with a mass of 45.23 g. The technician fills a beaker with water and measures the volume of the water alone as 25.67 mL. The technician then immerses the metal in the water and measures the new volume as 32.00 mL. What could be the metal?

a)

Iron, d = 7.87 g/mL

b)

Copper, d = 8.96 g/mL

c)

Zinc, d = 7.14 g/mL

d)

Gold, d = 19.3 g/mL

15.

A chemist is trying to determine an unknown metal with a mass of 60.32 g.

The chemist fills a flask with water and measures the volume of the water alone as 35.45 mL.

The chemist then immerses the metal in the water and measures the new volume as 40.78 mL.

What could be the metal?

a)

Aluminium, d = 2.70 g/mL

b)

Lead, d = 11.34 g/mL

c)

Silver, d = 10.49 g/mL

d)

Platinum, d = 21.45 g/mL

16.

How many significant figures does the number 0.007600 have?

a)

2

b)

3

c)

4

d)

5

e)

6

17.

How many significant figures does the number 0.0034500 have?

a)

2

b)

3

c)

4

d)

5

e)

6

18.

How many significant figures does the number 0.7600 have?

a)

2

b)

3

c)

4

d)

5

e)

6

19.

Which of the following numbers has four significant figures?

a)

0.0001234

b)

1.2340

c)

123.40

d)

1234.0

e)

12340

20.

Which of the following numbers has five significant figures?

a)

0.0012345

b)

1.23450

c)

123.450

d)

12345.0

e)

123450

21.

The accepted value for the density of gold is 19.3 g/mL. Which of the following sets of experimental data for the density of gold is the most accurate?

a)

Group 1: 19.35 g/mL, 19.28 g/mL

b)

Group 2: 18.90 g/mL, 18.95 g/mL

c)

Group 3: 20.01 g/mL, 19.99 g/mL

d)

Group 4: 17.50 g/mL, 17.55 g/mL

e)

Group 5: 19.29 g/mL, 19.31 g/mL

22.

The accepted value for the density of silver is 10.49 g/mL. Which of the following sets of experimental data for the density of silver is the most accurate?

a)

Group 1: 10.50 g/mL, 10.48 g/mL

b)

Group 2: 9.90 g/mL, 9.95 g/mL

c)

Group 3: 11.01 g/mL, 10.99 g/mL

d)

Group 4: 9.50 g/mL, 9.55 g/mL

e)

Group 5: 10.49 g/mL, 10.51 g/mL

23.

A flask of liquid has an initial mass of 500.0 g. After being left open for a week, some of the liquid has evaporated. The new mass of the flask is found to be 468.25 g using a precise balance. Choose a value that expresses the mass of the evaporated liquid using the correct number of significant figures.

a)

31.75 g

b)

31.750 g

c)

31.8 g

d)

468.25 g

e)

32 g

24.

A beaker of solution has an initial mass of 800.0 g. After being left open for a few days, some of the solution has evaporated. The new mass of the beaker is found to be 782.50 g using a precise balance. Choose a value that expresses the mass of the evaporated solution using the correct number of significant figures.

a)

17.50 g

b)

17.500 g

c)

17.5 g

d)

782.50 g

e)

18 g

25.

A graduated cylinder contains 50.0 mL of liquid. This volume is poured into a beaker containing 125 mL of the same liquid. Choose the value that expresses the new total volume of liquid in the beaker with the correct number of significant figures.

a)

175 mL

b)

200 mL

c)

180 mL

d)

175.00 mL

e)

175.0 mL

26.

A flask contains 30.0 mL of liquid. This volume is poured into a beaker containing 70 mL of the same liquid. Choose the value that expresses the new total volume of liquid in the beaker with the correct number of significant figures.

a)

100. mL

b)

110 mL

c)

90 mL

d)

100.00 mL

e)

100.0 mL

27.

How many significant figures would this calculation have if it were completed: (8.76 + 5.321 - 14.0 + 31.2) × 3.142

a)

2

b)

3

c)

4

d)

5

e)

6

28.

How many significant figures would this calculation have if it were completed: (8.76 + 7.381 - 14.0 + 31.12) × 3.142/1.0571

a)

2

b)

3

c)

4

d)

5

e)

6

29.

Which of the following temperatures is the coldest?

a)

200 K

b)

20 oF

c)

50 oC

d)

-50 oF

e)

100 oF

30.

Which of the following temperatures is the highest?

a)

-273.15 oC

b)

0 K

c)

32 oF

d)

100 oC

e)

-459.67 oF

31.

Convert 25.0 gallons to liters. (3.7854 liters = 1 gallon)

a)

94.635 L

b)

946.35 L

c)

9.4635 L

d)

9463.5 L

e)

946.35 dL

32.

Convert 50.0 gallons to liters. (3.7854 liters = 1 gallon)

a)

189.27 L

b)

1892.7 L

c)

18.927 L

d)

18927 L

e)

1892.7 dL

33.

Which one of the following is the shortest distance?

a)

0.0001 km

b)

1 x 10-5 km

c)

0.01 m

d)

1 x 107 µm

e)

1 x 109 nm

34.

Which one of the following is the longest distance?

a)

1 x 10-9 km

b)

0.001 m

c)

1 x 105 µm

d)

0.1 km

e)

1 x 103 nm

35.

Which of the following pairs represent isotopes?

a)
Hydrogen and Helium
b)
Carbon-12 and Carbon-14
c)
Oxygen and Nitrogen
d)
Sodium and Potassium
36.

Which of the following pairs represent isotopes?

a)

14C and 14N

b)

14C and 15N

c)

14C and 13C

d)

14C and 12C

e)

14C and 16O

37.

Which of the following atoms has the same number of neutrons as 60Cu?

a)

59Co

b)

59Fe

c)

59Cu

d)

59Zn

e)

59Ni

38.

An atom of the isotope 238U contains how many protons (p), neutrons (n), and electrons (e)?

a)

92 p, 92 n, 92 e

b)

92 p, 146 n, 92 e

c)

238 p, 238 n, 238 e

d)

92 p, 238 n, 92 e

e)

238 p, 92 n, 92 e

39.

An atom of the isotope 235U contains how many protons (p), neutrons (n), and electrons (e)?

a)

92 p, 92 n, 92 e

b)

92 p, 143 n, 92 e

c)

235 p, 235 n, 235 e

d)

92 p, 235 n, 92 e

e)

235 p, 92 n, 92 e

40.

Determine the empirical formula for C8H18O3.

a)

C4H9O1.5

b)

CHO3

c)

C8H18O3

d)

C16H36O6

e)

C2H9O1.5

41.

Determine the empirical formula for C6H14O2.

a)

C3H7O

b)

CHO2

c)

C6H14O2

d)

C12H28O4

e)

C2H7O

42.

Which of the following would NOT be classified as a molecular element?

a)

N2

b)

I2

c)

CO2

d)

S2

e)

P4

43.

Which of the following is NOT a diatomic molecule?

a)

O2

b)

Cl2

c)

CO2

d)

H2

e)

N2

44.

How many H atoms are in two formula units of (NH4)2HPO4?

a)

4

b)

8

c)

24

d)

16

e)

18

45.

How many O atoms are in three formula units of (NH4)2HPO4?

a)

4

b)

12

c)

8

d)

16

e)

24

46.

How many H atoms are in three formula units of (NH4)2HPO4?

a)

27

b)

12

c)

8

d)

16

e)

24

47.

Sucrose is a common sugar found in many plants. It has the molecular formula C12H22O11.

What is its empirical formula?

a)

C12H22O11

b)

CH2O

c)

C6H12O6

d)

C3H8O3

e)

C3H6O3

48.

Glucose is a simple sugar with the molecular formula C6H12O6.

What is its empirical formula?

a)

C6H12O6

b)

CH2O

c)

C12H22O11

d)

C3H8O3

e)

C3H6O3

49.

Which of the following is most likely to form a +2 ion?

a)

Al

b)

Rb

c)

O

d)

Mg

e)

S

50.

Which of the following elements is most likely to form a -2 ion?

a)

Na

b)

Cl

c)

O

d)

Li

e)

He

51.

Which of the following elements is most likely to form a +1 ion?

a)

Ne

b)

Ar

c)

K

d)

Ca

e)

Fe

52.

Which of the following elements is most likely to form a +2 ion?

a)

Ne

b)

Ar

c)

K

d)

Ca

e)

Fe

53.

What is the formula of a compound containing Na+ and O2- ions?

a)

NaO

b)

Na2O3

c)

Na3O2

d)

Na6O6

e)

NaO2

54.

What is the formula of a compound containing K+ and S2- ions?

a)

K2S

b)

K3S

c)

K2S3

d)

K3S2

e)

KS2

55.

How many protons (p) and electrons (e) are found in a Sc3+ ion?

a)

18 p, 21 e

b)

21 p, 21 e

c)

21 p, 18 e

d)

18 p, 18 e

e)

21 p, 24 e

56.

How many protons (p) and electrons (e) are found in a Fe3+ ion?

a)

26 p, 23 e

b)

23 p, 26 e

c)

26 p, 26 e

d)

23 p, 23 e

e)

26 p, 29 e

57.

What is the number of protons (p) and electrons (e) in a O2- ion?

a)

8 p, 10 e

b)

10 p, 8 e

c)

8 p, 8 e

d)

10 p, 10 e

e)

8 p, 6 e

58.

Classify the following compounds as ionic or covalent (molecular): NaCl, SiO2, Al2O3.

a)

Covalent, covalent, covalent.

b)

Ionic, ionic, covalent.

c)

Ionic, covalent, covalent.

d)

Ionic, ionic, ionic.

e)

Covalent, ionic, covalent.

59.

Classify the following compounds as ionic or covalent (molecular): KCl, CO2, MgO.

a)

Covalent, covalent, covalent.

b)

Ionic, ionic, covalent.

c)

Ionic, covalent, ionic.

d)

Ionic, ionic, ionic.

e)

Covalent, ionic, covalent.

60.

Identify the type of bond (ionic or covalent) in the following compounds: NaCl, H2O, CaO.

a)

Covalent, covalent, covalent.

b)

Ionic, ionic, covalent.

c)

Ionic, covalent, ionic.

d)

Ionic, ionic, ionic.

e)

Covalent, ionic, covalent.

61.

Determine the type of bond (ionic or covalent) in the following compounds: KCl, CH4, MgO.

a)

Covalent, covalent, covalent.

b)

Ionic, ionic, covalent.

c)

Ionic, covalent, ionic.

d)

Ionic, ionic, ionic.

e)

Covalent, ionic, covalent.

62.

Classify the following compounds as ionic or covalent (molecular): NaCl, MgO, CO2.

a)

Covalent, Ionic, Covalent

b)

Covalent, covalent, Ionic

c)

Ionic, ionic, Covalent

d)

Ionic, ionic, ionic

e)

Covalent, ionic, ionic

63.

Identify the type of bond in the following compounds: H2O, NaBr, CH4.

a)

Covalent, Ionic, Covalent

b)

Ionic, Covalent, Ionic

c)

Covalent, Ionic, Ionic

d)

Ionic, Ionic, Covalent

e)

Ionic, Ionic, Ionic

64.

Determine the type of bond in the following compounds: NH3, KCl, CO2.

a)

Covalent, Ionic, Covalent

b)

Ionic, Covalent, Ionic

c)

Covalent, Ionic, Ionic

d)

Ionic, Ionic, Covalent

e)

Ionic, Ionic, Ionic

65.

Which of the following compounds demonstrates both ionic and covalent (molecular)

bonding characteristics?

a)

NaCl

b)

O2

c)

KOH

d)

FeS

e)

SiO2

66.

Which of the following compounds exhibits both polar and nonpolar covalent bonding?

a)

CaCO3

b)

O2

c)

CH4

d)

CO2

e)

NaCl

67.

Which of the following compounds demonstrates both ionic and covalent (molecular)

bonding characteristics?

a)

NaCl

b)

O2

c)

NaCH2COO

d)

FeS

e)

SiO2

68.

Predict the chemical formula for the ionic compound formed by Fe³+? and NO3-?

a)

FeNO3

b)

Fe2(NO3)3

c)

Fe(NO)3

d)

Fe(NO3)3

e)

Fe3NO3

69.

Predict the chemical formula for the ionic compound formed by Al³+? and SO42-?

a)

AlSO4

b)

Al2(SO4)3

c)

Al(SO)4

d)

Al(SO4)3

e)

Al3SO4

70.

Predict the chemical formula for the ionic compound formed by Ca²+? and PO43-?

a)

CaPO4

b)

Ca2(PO4)3

c)

Ca(PO)4

d)

Ca(PO4)3

e)

Ca3PO4

71.

Predict the chemical formula for the ionic compound formed by Na⁺ and SO42-?

a)

NaSO4

b)

Na2(SO4)2

c)

Na(SO)4

d)

Na(SO4)2

e)

Na2SO4

72.

Identify the correct formula for magnesium oxide.

a)

MgO

b)

Mg2O

c)

Mg3O2

d)

MgO2

e)

Mg3O

73.

Choose the correct chemical formula for calcium chloride.

a)

CaCl

b)

Ca2Cl

c)

Ca3Cl2

d)

CaCl2

e)

Ca3Cl

74.

What is the correct formula for calcium phosphate?

a)

CaPO4

b)

Ca2PO4

c)

Ca2(PO4)3

d)

Ca3(PO4)2

e)

CaPO3

75.

What is the correct formula for calcium carbonate?

a)

CaCO3

b)

Ca2CO3

c)

Ca2(CO3)3

d)

Ca3(CO3)2

e)

CaCO4

76.

What is the correct formula for sodium bicarbonate?

a)

NaHCO3

b)

Na2HCO3

c)

Na2(HCO3)3

d)

Na3(HCO3)2

e)

NaHCO4

77.

What is the chemical formula for sodium carbonate?

a)

Na2CO3

b)

Na2HCO3

c)

Na3(CO3)2

d)

Na2(CO3)3

e)

NaCO3

78.

What is the correct formula for iron(III) hydroxide?

a)

FeOH

b)

Fe(OH)3

c)

Fe3OH

d)

Fe2(OH)3

e)

Fe3(OH)2

79.

What is the correct formula for iron(II) hydroxide?

a)

FeOH

b)

Fe(OH)2

c)

Fe2OH

d)

Fe2(OH)3

e)

Fe3(OH)2

80.

Which of the following has the correct name-formula combination?

a)

Iron(II) oxide – FeO

b)

Copper(II) sulfate - CuSO4

c)

Aluminium(III) chloride – AlCl3

d)

Calcium(II) carbonate – CaCO3

e)

Lead(II) nitrate – Pb(NO3)2

81.

Which of the following is the correct formula for the given compound name?

a)

Sodium chloride – NaCl

b)

Calcium sulfate - CaSO3

c)

Potassium nitrate – KNO2

d)

Iron(III) oxide – Fe3O2

e)

Aluminium sulfate – Al2(SO3)3

82.

Which of the following is the incorrect name for the given chemical formula?

a)

NaCl – Sodium chloride

b)

CaSO4 - Calcium sulfate

c)

KNO3 – Potassium nitrite

d)

Fe2O3 – Iron(III) oxide

e)

Al2(SO4)3 – Aluminium sulfate

83.

The correct IUPAC name for FeCl3·6H2O is

a)

Iron(III) chloride hexahydrate

b)

Iron chloride hexahydrate

c)

iron trichloride hydrate

d)

iron trichloride hexahydrate

e)

iron(II) trichloride hexahydrate

84.

The correct IUPAC name for CuSO4·5H2O is

a)

Copper(II) sulfate pentahydrate

b)

Copper sulfate pentahydrate

c)

copper sulfate hydrate

d)

copper sulfate pentahydrate

e)

copper(I) sulfate pentahydrate

85.

The correct IUPAC name for FeSO4·7H2O is

a)

Iron(II) sulfate heptahydrate

b)

Iron sulfate heptahydrate

c)

Iron sulfate hydrate

d)

Iron sulfate heptahydrate

e)

Iron(I) sulfate heptahydrate

86.

The correct IUPAC name for CuSO4·5H2O is

a)

Copper(II) sulfate pentahydrate

b)

Copper sulfate pentahydrate

c)

Copper sulfate hydrate

d)

Copper(I) sulfate pentahydrate

e)

Copper sulfate

87.

Which of the following has the correct name-formula combination?

a)

Sodium sulfate - Na2SO4

b)

Calcium carbonate - Ca2(CO3)2

c)

Potassium nitrite - KNO3

d)

Barium chloride - BaCl

e)

Lithium phosphate - Li2(PO4)2

88.

Which of the following has the incorrect name-formula combination?

a)

Ammonium nitrate - NH4NO3

b)

Magnesium oxide - MgO

c)

Sodium chloride - NaCl

d)

Calcium hydroxide - Ca(OH)2

e)

Potassium sulfate - K2SO4

89.

Which of the following has the correct name-formula combination?

a)

Sodium carbonate - NaCO3

b)

Calcium carbonate - CaCO3

c)

Potassium nitrite - KNO

d)

Ammonium sulfite - (NH4)2SO4

e)

Magnesium hydroxide - MgOH

90.

Which of the following is the correct formula for the compound named 'Potassium sulfate'?

a)

KSO4

b)

K2SO4

c)

K(SO4)2

d)

KS2O4

e)

K2S2O7

91.

Which of the following is the correct formula for the given compound name?

a)

Sulfur hexafluoride - SF4

b)

Nitrogen triiodide - NI3

c)

Phosphorus pentachloride - PCl5

d)

Carbon tetrachloride - CCl4

e)

Oxygen difluoride - OF2

92.

What is the correct formula for the following compound name?

a)

Carbon tetrachloride - CCl3

b)

Nitrogen diiodide - NI3

c)

Phosphorus pentachloride - PCl5

d)

Sulfur hexafluoride - SF4

e)

Oxygen difluoride - O2F

93.

Which of the following is the correct compound name for the given formula?

a)

Carbon tetrachloride - CCl2

b)

Nitrogen triiodide - NI2

c)

Phosphorus pentachloride - PCl3

d)

Sulfur hexafluoride - SF6

e)

Oxygen trifluoride - OF2

94.

What are the coefficients in front of the Fe3O4 and the Fe2O if you balance the following unbalanced equation:

Fe3O4   +    O2     -->     Fe2O   +    O2?

a)

2, 3

b)

6, 4

c)

4, 6

d)

3, 4

e)

1, 1

95.

What are the coefficients in front of the Fe2O3 and the Fe3O if you balance the following unbalanced equation:

Fe2O3   +    O2     -->     Fe3O   +    O2?

a)

2, 3

b)

6, 4

c)

4, 6

d)

3, 4

e)

1, 1

96.

Which equation correctly represents the decomposition of solid potassium hydroxide into solid potassium oxide and water vapor?

a)

KOH (s) --> K2O (s) + H2O (g)

b)

2KOH (s) --> K2O (s) + H2O (g)

c)

4KOH (s) --> K2O (s) + 2H2O (g)

d)

2KOH (s) --> 2K2O (s) + H2O (g)

e)

4KOH (s) --> 2K2O (s) + H2O (g)

97.

Which equation correctly represents the decomposition of solid sodium hydroxide into solid sodium oxide and water vapor?

a)

NaOH (s) --> Na2O (s) + H2O (g)

b)

2NaOH (s) --> Na2O (s) + H2O (g)

c)

4NaOH (s) --> Na2O (s) + 2H2O (g)

d)

2NaOH (s) --> 2Na2O (s) + H2O (g)

e)

4NaOH (s) --> 2Na2O (s) + H2O (g)

98.

An unknown element Z has the following isotopes: 27Z (70.51% abundant), 28Z (2.27% abundant), 29Z (27.22% abundant). What is the average atomic mass in amu of Z?

a)

27.1871 amu

b)

27.187 amu

c)

27.190 amu

d)

27.19 amu

e)

27.2 amu

99.

An unknown element X has the following isotopes: 30X (60.51% abundant), 31X (5.27% abundant), 32X (34.22% abundant). What is the average atomic mass in amu of X?

a)

30.1871 amu

b)

30.187 amu

c)

30.190 amu

d)

30.19 amu

e)

30.2 amu

100.

An unknown element Y has the following isotopes: 24Y (80.51% abundant), 25Y (1.27% abundant), 26Y (18.22% abundant). What is the average atomic mass in amu of Y?

a)

24.1871 amu

b)

24.187 amu

c)

24.190 amu

d)

24.19 amu

e)

24.2 amu

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