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General Chemistry Review

Total questions: 90

Worksheet time: 45mins

Name
Class
Date
1.

A 0.150 kg metallic block measures 25.0 mm in length, 43.0 mm in width, and 19.0 mm in height. What is the density of the metallic block in g/cm³?

a)

7.34 × 10⁻³ g/cm³

b)

7.34 × 10⁻⁶ g/cm³

c)

7.34 g/cm³

2.

How would you determine the density of an irregular object?

a)

D = m/v, so measure the mass of the object using a balance. Then to find volume, measure the height, width, and length using an appropriate measuring tool.

b)

D = m/v, so measure the mass of the object using a balance. Then to find volume, fill a graduated cylinder with a known amount of water and immerse the object in the water. The amount of displaced water is the volume in cm³ or mL.

c)

It would be impossible to determine the mass of the object without more information.

3.

What is the base unit for mass in the metric

a)

mg

b)

g

c)

kg

4.

What is the base unit for volume in the metric system?

a)

L

b)

dL

c)

mL

5.

Convert 18.50 ft to the SI unit for length.

a)

5.639 m

b)

0.005639 km

c)

563.9 cm

6.

Accuracy is defined as how close a measured value comes to a _____.

a)

fixed value

b)

true value

c)

core value

7.

Precision is defined as how _____ the measured values are to one another.

a)

Accurate

b)

reproducible

c)

common

8.

An experiment requires you to make several measurements. Based on the values in the table below, what would be the best statement that represents the data set if the true value is 2.73?

a)

The measurements in Trial B are precise, however, not accurate. Trial’s A and C are neither accurate nor precise.

b)

The measurements in Trial B are accurate, however, not precise. Trial’s A and C are neither accurate nor precise.

c)

The measurements in Trial’s A, B, and C are neither accurate nor precise.

9.

Which of the following would be considered a chemical change?

a)

crushing an aluminum can

b)

melting ice

c)

a rusting nail

10.

Which of the following would be considered a physical change?

a)

digesting food

b)

burning paper

c)

boiling water

11.

A salt water solution is classified as what type of matter?

a)

homogeneous mixture

b)

heterogeneous mixture

c)

pure substance

12.

How many significant figures are in 0.0000401 kg?

a)

3

b)

7

c)

2

13.

Express 1.40 × 10^-3 L in decimal notation.

a)

0.00140 L

b)

0.0014 L

c)

0.001 L

14.

What is the answer for the following calculation: (1.249 - 0.0234) × 139.37?

a)

170.8

b)

170.81

c)

170.812

15.

What is the SI unit for mass?

a)

milligram

b)

gram

c)

kilogram

16.

What is the SI unit for temperature?

a)

Fahrenheit

b)

Celsius

c)

Kelvin

17.

How many grams of iron are in 350 mg of iron?

a)

35.0 g

b)

0.350 g

c)

3.50 g

18.

The prefix milli- in the metric system represents a factor of _____.

a)

10310^3

b)

10−310^{-3}

c)

1/10−31/10^{-3}

19.

The prefix nano- in the metric system represents a factor of _____.

a)

10−610^{-6}

b)

10910^9

c)

10−910^{-9}

20.

A statement about mass always being conserved in a chemical reaction is an example of a _____.

a)

hypothesis

b)

theory

c)

law

21.

The scientific method involves various techniques which allow researchers to investigate scientific questions through _____ and _____.

a)

analysis and predictions

b)

observations and experimentation

c)

analysis and observations

22.

List the basic steps of the scientific method process in the order they must be carried out.

a)

prediction, observation, hypothesis, experimentation, and conclusion

b)

hypothesis, observation, prediction, experimentation, and conclusion

c)

observation, hypothesis, prediction, experimentation, and conclusion

23.

Which of the following is not part of the scientific method process?

a)

discussion

b)

prediction

c)

observation

24.

Which of the following would be a good example of an observation in the scientific method process?

a)

a researcher setting up a chemical reaction in a flask and allowing it to stir for 2 hours

b)

a researcher watching a chemical reaction and noting color and temperature changes

c)

a researcher watching a chemical reaction

25.

Which of the following would be good tools for making scientific observations during a chemical reaction?

a)

thermometer, your eyes, tape measures

b)

thermometer, your eyes, clock

c)

barometer, thermometer, scale

26.

What can be used to measure the mass of an object?

a)

caliper

b)

tape measure

c)

balance

27.

Once a hypothesis has been established, it can be tested by conducting an _____.

a)

experiment

b)

observation

c)

Analysis

28.

Which statement is correct about the scientific method process?

a)

after testing a hypothesis, a conclusion can be drawn on whether it will be accepted or rejected

b)

after testing an observation, a conclusion can be drawn on whether it will be accepted or rejected

c)

after testing a conclusion, it can be predicted whether a hypothesis will be accepted or rejected

29.

Why is chemistry considered a central science?

a)

because it is very important in medicine

b)

because it is a core course required for most majors in college

c)

because it is the fundamental science for many other disciplines

30.

Which of the following is an example of a physical property?

a)

an iron nail rusts

b)

carbon monoxide is poisonous

c)

water freezes at 273.15 K

31.

Which of the following is an example of a chemical property?

a)

water boils at 100 °C

b)

carbon monoxide is poisonous

c)

a copper penny weighs 3.00 g

32.

The following is an example of a chemical change.

a)

decomposing waste

b)

dissolving sugar

c)

shredding paper

33.

A website claims that there is a natural cure for all cancers; however, doctors do not want to recommend natural remedies because it would make them obsolete. Is this statement logical?

a)

yes, doctors can cure all patients

b)

yes, doctors can cure some patients with natural remedies

c)

no, doctors cannot cure all patients and regardless of treatment, some patients still remain ill and die

34.

Which of the following is not a correct element name-symbol combination?

a)

gold, Au

b)

arsenic, Ar

c)

copper, Cu

35.

Isotopes of carbon differ with respect to the number of __________.

a)

protons

b)

neutrons

c)

electrons

36.

Elements in group 17 are considered ____________.

a)

noble gases

b)

alkali Metals

c)

halogens

37.

Due to periodicity, which of the following elements has chemical behavior similar to that of Oxygen?

a)

Carbon

b)

sulfur

c)

bromine

38.

Which list of elements contains ONLY nonmetals?

a)

phosphorus, nitrogen, oxygen

b)

sodium, chromium, copper

c)

helium, carbon, gold

39.

Which of the following gases exists as a diatomic molecule?

a)

krypton

b)

hydrogen

c)

argon

40.

Which list of elements contains ONLY nonmetals?

a)

helium, carbon, gold

b)

sodium, chromium, copper

c)

phosphorus, nitrogen, oxygen

41.

Using the periodic table, what is the atomic number of argon?

a)

18

b)

13

c)

26.98

42.

The Greek philosopher Democritus phrased what word for a tiny piece of matter that cannot be divided?

a)

atom

b)

electron

c)

element

43.

Within the nucleus, the positive charge is __________.

a)

concentrated in the center of an atom

b)

spread evenly throughout an atom

c)

concentrated at multiple sites in an atom

44.

Which statement about subatomic particles is NOT true?

a)

Protons and electrons have opposite charges.

b)

Protons and neutrons have almost the same mass.

c)

Protons and neutrons have the same charge

45.

The number of protons in one atom of an element is that element’s __________.

a)

mass number

b)

atomic mass

c)

atomic number

46.

To calculate the number of neutrons in an atom, you would subtract

a)

atomic number from electron number

b)

mass number from atomic number

c)

atomic number from mass number

47.

Which of the following is not a correct element name-symbol combination?

a)

gold, Au

b)

arsenic, Ar

c)

copper, Cu

48.

Isotopes of carbon differ with respect to the number of __________.

a)

electrons

b)

neutrons

c)

protons

49.

Which of the following elements form +2 ions?

a)

strontium, magnesium, calcium

b)

lithium, sodium, potassium

c)

sodium, magnesium, aluminum

50.

How many neutrons are in chlorine-37?

a)

18

b)

20

c)

18.5

51.

Identify the chalcogen that has 18 neutrons in the nucleus.

a)

sulfur-33

b)

sulfur-32

c)

sulfur-34

52.

The chemical symbol for cobalt is _____.

a)

CO

b)

Co

c)

cO

53.

Which element is represented by the chemical symbol Th?

a)

thallium

b)

thorium

c)

Tantalum

54.

Which element is represented by the chemical symbol Tl?

a)

tantalum

b)

thallium

c)

titanium

55.

What is a cation?

a)

A cation is defined as an atom that has gained electrons and forms a negative charge

b)

A cation is defined as an atom that has gained electrons and forms a positive charge.

c)

A cation is defined as an atom that has lost electrons and forms a positive charge.

56.

Lanthanum atom is located in which block on the periodic table?

a)

p-block

b)

d-block

c)

f-block

57.

Provide the element name with a ground-state electron configuration of 1s22s22p41s^2 2s^2 2p^4

a)

Potassium

b)

carbon

c)

oxygen

58.

What is the ground-state electron configuration of calcium?

a)

1s^2 2s^2 2p^6 3s^2

b)

1s^2 2s^2 2p^6

c)

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2

59.

Due to periodicity, which element would you expect to behave most like sodium?

a)

calcium

b)

aluminum

c)

potassium

60.

Elements in group 17 are considered ____________.

a)

noble Gases

b)

alkali Metals

c)

halogens

61.

Which of the following sets of elements are the most similar to each other?

a)

H, He

b)

C, N, O, F

c)

F, Cl, Br, I

62.

As you move down a group of elements (family), the number of valence electrons

a)

increases and then decreases.

b)

stays the same.

c)

increases.

63.

What is the maximum number of electrons that can occupy the 4th energy level or shell?

a)

32

b)

16

c)

4

64.

What is the maximum number of orbitals found in the 3rd energy level or shell?

a)

9

b)

13

c)

18

65.

Based on the following electron configuration, [Xe]6s2[Xe]6s^2 , this element would most likely _____.

a)

loss 2 electrons to form a +2 cation and could form an ionic bond with a metal

b)

loss 2 electrons to form a +2 cation and could form an ionic bond with a non-metal

c)

gain 2 electrons to form a +2 cation and could form an ionic bond with a non-metal

66.

What is the electron configuration of a copper atom? (Copper doesn't follow the rules)

a)

[Ar]4s^2 3d^9

b)

[Ar]4s13d10[Ar]4s^1 3d^{10}

c)

[Ar]4s03d11[Ar]4s^0 3d^{11}

67.

What is the ground-state electron configuration of carbon?

a)

1s^2 2s^2 2p^2

b)

1s^2 2s^2 2p^1

c)

1s22s12p31s^2 2s^1 2p^3

68.

In which orbital does an electron add to in chlorine to form an octet?

a)

3d

b)

3s

c)

3p

69.

In what block, group, and period on the periodic table can the atom with a 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5 ground-state electron configuration be found?

a)

p-block, group 7A, and period 5

b)

p-block, group 7A, and period 3

c)

p-block, group 7A, and period 4

70.

How many electrons are in the most likely ion formed from an atom located in group 6A and period 3?

a)

18 electrons

b)

17 electrons

c)

16 electrons

71.

According to periodic trends, which metal has the highest ionization energy?

a)

Li

b)

Cs

c)

Rb

72.

Which nonradioactive group I metal would be the most reactive in water and why?

a)

Cesium would be the most reactive group I metal in water because it has only one valence electron.

b)

Cesium would be the most reactive group I metal in water because it’s one valence electron is the closest to the nucleus compared to the other metals.

c)

Cesium would be the most reactive group I metal in water because it’s one valence electron is the farthest from the nucleus compared to the other metals.

73.

According to the octet rule, a magnesium atom has a tendency to

a)

lose one electron.

b)

lose two electrons.

c)

gain one electron.

74.

Which one of the following elements does not exist as a diatomic molecule in nature?

a)

neon

b)

nitrogen

c)

hydrogen

75.

According to periodic trends, which element is the most electronegative?

a)

F

b)

O

c)

Ne

76.

According to the octet rule, which of the elements will have a tendency to lose 2 electrons?

a)

cesium

b)

strontium

c)

oxygen

77.

In an ionic bond, the charge on the cation (i.e. the metal) is

a)

always positive.

b)

always negative.

c)

either positive or negative.

78.

According to the octet rule, a magnesium atom has a tendency to

a)

lose two electrons.

b)

gain one electron.

c)

lose one electron.

79.

The halogens have how many valence electrons?

a)

4

b)

6

c)

7

80.

Which of the following elements are found in the p-block and can form an octet?

a)

He, Ar, Kr, Ne

b)

P, S, O, C

c)

He, P, S, As

81.

Which of the following compounds contains the largest number of atoms?

a)

1.00 mole of NH3

b)

1.00 mole of H2SO4

c)

1.00 mole of HBr

82.

What is the mass in grams of 6.022×10236.022 \times 10^{23} molecules of CO2?

a)

22 g

b)

44 g

c)

66 g

83.

What is the total number of atoms contained in 2.00 moles of iron?

a)

1.2 × 10^24

b)

6.02×10236.02 \times 10^{23}

c)

118

84.

What is the molar mass of K2CO3?

a)

99 g/mol

b)

138 g/mol

c)

106 g/mol

85.

A 44.8 g rhodium sample contains how many rhodium atoms?

a)

6.02 × 10^23 atoms

b)

2.62 × 10^23 atoms

c)

2.70 × 10^25 atoms

86.

When a salt is dissolved in water, it is represented by the following notation in a chemical reaction?

a)

(s)

b)

(aq)

c)

(l)

87.

How is a solid phase represented in a chemical reaction?

a)

(s)

b)

(g)

c)

(l)

88.

How is a gas phase represented in a chemical reaction?

a)

(l)

b)

(g)

c)

(s)

89.

What are the proper units for molar mass in chemistry?

a)

g/mol

b)

amu

c)

g/mmol

90.

How many atoms can be found in a mole of mercury?

a)

201 atoms

b)

6.02 × 10^23 atoms

c)

3.01 × 10^23 atoms

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