Free Printable Chemistry Midterm 1

1.

What do you fill a wash bottle that has a blue stem with?

a)

Distilled water

b)

Tap water

c)

Ethanol

d)

Hydrochloric acid

2.

What should you do with lab equipment that is still hot and you want to clean up?

a)

Leave it on the lab bench to cool before handling

b)

Immerse it immediately in cold water

c)

Return it to storage while hot

d)

Pass it to another student to speed cleanup

3.

If you obtain too much of a chemical, what should you do with it?

a)

Ask the instructor what to do

b)

Return it to the original stock container

c)

Pour it down the sink

d)

Give it to another student

4.

If you break glassware during a lab, what should you do?

a)

Notify the instructor and place broken glass in the designated container

b)

Hide the breakage to avoid losing points

c)

Pick up the shards with bare hands and throw them in regular trash

d)

Leave the area without telling anyone

5.

How do you properly heat a liquid in a test tube?

a)

Hold the test tube at an angle, move it back and forth, and keep the mouth pointed away from people

b)

Hold the test tube upright directly in the flame

c)

Cap the test tube while heating to avoid splashing

d)

Point the opening toward yourself to observe changes closely

6.

During a lab, you accidentally spill a chemical on your hand. What should you do?

a)

Immediately wash with soap and water and notify the instructor

b)

Ignore it and continue working

c)

Wipe it off with a dry paper towel only

d)

Neutralize it by adding another random chemical

7.

What piece of equipment is the most accurate way to measure volume?

a)

Graduated cylinder

b)

Beaker

c)

Erlenmeyer flask

d)

Test tube

8.

Identify the following piece of equipment.

a)

Glassware forceps

b)

Glassware tongs

c)

Beaker tongs

d)

Beaker forceps

9.

Identify the following piece of equipment.

a)

Florence flask

b)

Erlenmeyer flask

c)

Beaker flask

d)

Triangle flask

10.

Identify the following piece of equipment.

a)

Heating element

b)

Wire gauze

c)

Wire square

d)

Heating square

11.

Identify the following piece of equipment.

a)

Test tube holder

b)

Test tube clamp

c)

Test tube forceps

d)

Test tube tongs

12.

Identify the following piece of equipment.

a)

Crucible & lid

b)

Crucible & cover

c)

Evaporating dish & cover

d)

Evaporating bowl & cover

13.

Identify the following piece of equipment.

a)

Crucible

b)

Porcelain dish

c)

Evaporating dish

d)

Evaporating bowl

14.

Identify the following piece of equipment.

a)

Crucible

b)

Watch glass

c)

Glass plate

d)

Glass bowl

15.

Identify the following piece of equipment.

a)

Plastic Filter

b)

Funnel

c)

Filtrate

d)

Plastic pourer

16.

Identify the following piece of equipment.

a)

Glassware tongs

b)

Beaker forceps

c)

Beaker tongs

d)

Glassware forceps

17.

Identify the following piece of equipment.

a)

Florence flask

b)

Erlenmeyer flask

c)

Round bottom flask

d)

Beaker flask

18.

Identify the following piece of equipment.

a)

Bulbed straw

b)

Pipet

c)

Eye dropper

d)

Dropper

19.

Identify the following piece of equipment.

a)

Lighter

b)

Flint sparker

c)

Striker

d)

Fire maker

20.

Identify the following piece of equipment.

a)

Test tube holder

b)

Test tube ring

c)

Test tube clamp

d)

Test tube catcher

21.

Identify the following piece of equipment.

a)

Beaker

b)

Test tube

c)

Graduated cylinder

d)

Erlenmeyer flask

22.

Identify the following piece of equipment.

a)

Circle clamp

b)

Beaker clamp

c)

Ring clamp

d)

Stand clamp

23.

Identify the following piece of equipment.

a)

Triangle

b)

Porcelain holder

c)

Crucible stand

d)

Crucible clamp

24.

Identify the following piece of equipment.

a)

Watch glass

b)

Glass plate

c)

Glass square

d)

Watch plate

25.

Identify the following piece of equipment.

a)

Bunsen burner stand

b)

Ring stand

c)

Heating apparatus

d)

Heating stand

26.

Identify the following piece of equipment.

a)

Glassware tongs

b)

Chemical forceps

c)

Chemical tongs

d)

Tweezers

27.

Identify the following piece of equipment.

a)

Stirring rods

b)

Stirring sticks

c)

Stirrers

d)

Mixing sticks

28.

Identify the following piece of equipment.

a)

Test tube

b)

Florence flask

c)

Beaker

d)

Erlenmeyer beaker

29.

Select all indicators of a chemical reaction.

a)

Heat and/or light produced

b)

Color change

c)

A precipitate forms

d)

Gas production (bubbles or smoke)

e)

Change in state without new substance

30.

In the flow chart shown, identify the two top‑level categories used to classify matter.

a)

Pure substance and mixture

b)

Element and compound

c)

Homogeneous and heterogeneous

d)

Solid and liquid

31.

According to the flow chart, which pair correctly completes the classification under Pure Substance?

a)

Element and compound

b)

Homogeneous and heterogeneous

c)

Atom and molecule

d)

Solution and suspension

32.

According to the flow chart, which pair correctly completes the classification under Mixture?

a)

Homogeneous and heterogeneous

b)

Element and compound

c)

Solid and liquid

d)

Solute and solvent

33.

Classify the property: Flammability. Choose the correct column.

a)

Physical property

b)

Chemical property

34.

Classify the property: Density. Choose the correct column.

a)

Physical property

b)

Chemical property

35.

Classify the property: Evaporation. Choose the correct column.

a)

Physical property

b)

Chemical property

36.

Classify the property: Reacts with acid to form $\mathrm{H_2}$ . Choose the correct column.

a)

Physical property

b)

Chemical property

37.

Classify the property: Color. Choose the correct column.

a)

Physical property

b)

Chemical property

38.

Classify the type of matter: Zinc.

a)

Element

b)

Compound

c)

Homogeneous mixture

d)

Heterogeneous mixture

39.

Classify the type of matter: Trail mix.

a)

Element

b)

Compound

c)

Homogeneous mixture

d)

Heterogeneous mixture

40.

Classify the type of matter: Water.

a)

Element

b)

Compound

c)

Homogeneous mixture

d)

Heterogeneous mixture

41.

Classify the type of matter: Oil and water.

a)

Element

b)

Compound

c)

Homogeneous mixture

d)

Heterogeneous mixture

42.

Classify the type of matter: Table salt (NaCl).

a)

Element

b)

Compound

c)

Homogeneous mixture

d)

Heterogeneous mixture

43.

Identify the type of change: Burning a piece of paper.

a)

Physical change

b)

Chemical change

44.

Identify the type of change: Metal dissolving in acid.

a)

Physical change

b)

Chemical change

45.

Identify the type of change: Table salt dissolving in water.

a)

Physical change

b)

Chemical change

46.

Identify the type of change: A balloon is inflated with air.

a)

Physical change

b)

Chemical change

47.

Identify the type of change: Ice melting.

a)

Physical change

b)

Chemical change

48.

Identify the type of change: Water is heated and changed to steam.

a)

Physical change

b)

Chemical change

49.

In the reaction $\mathrm{CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O}$ , which list contains only the reactants?

a)

$\mathrm{CH_4}$ and $\mathrm{2O_2}$

b)

$\mathrm{CO_2}$ and $\mathrm{2H_2O}$

c)

$\mathrm{CH_4}$ and $\mathrm{CO_2}$

d)

$\mathrm{2O_2}$ and $\mathrm{2H_2O}$

50.

What is the difference between an endothermic and an exothermic energy change?

a)

Endothermic absorbs energy; exothermic releases energy

b)

Endothermic releases energy; exothermic absorbs energy

c)

Both absorb energy

d)

Both release energy

51.

How would you know an endothermic change took place?

a)

The surroundings feel cold to the touch

b)

The surroundings feel hot to the touch

c)

Light is produced

d)

A precipitate forms

52.

How would you know an exothermic change took place?

a)

The surroundings feel hot to the touch

b)

The surroundings feel cold to the touch

c)

No temperature change occurs

d)

A gas is absorbed

53.

Which statement correctly distinguishes qualitative from quantitative, and identifies an example of each?

a)

Qualitative is descriptive (e.g., fast); quantitative uses numbers (e.g., 3 seconds)

b)

Qualitative uses numbers (e.g., 3 seconds); quantitative is descriptive (e.g., fast)

c)

Both are descriptive only; examples: color and texture

d)

Both are numerical only; examples: mass and time

54.

How do you correctly read the volume of water in a graduated cylinder? Select all that apply.

a)

View at eye level

b)

Read the bottom of the meniscus

c)

Hold the cylinder above your head

d)

Read the top of the meniscus

55.

Which choice correctly describes accuracy and precision?

a)

Accuracy is closeness to the accepted value; precision is closeness of repeated measurements to one another

b)

Accuracy is repetition consistency; precision is closeness to the accepted value

c)

Accuracy and precision are identical concepts

d)

Accuracy is the number of significant figures; precision is the unit used

56.

What method would you use to find the volume of a penny?

a)

Water displacement

b)

Length × width × height

c)

Measure temperature change

d)

Convert mass to volume using density of air

57.

Sam measured a mass of 6.58 g for copper; the actual mass was 7.89 g. What is the percent error?

a)

$16.6\%$

b)

$1.7\%$

c)

$19.5\%$

d)

$12.3\%$

58.

A sample of iron has a mass of 19.5 g and a volume of $12.3\ \mathrm{cm^3}$ . What is its density?

a)

$1.6\ \mathrm{g/cm^3}$

b)

$12.3\ \mathrm{g/cm^3}$

c)

$0.63\ \mathrm{g/cm^3}$

d)

$19.5\ \mathrm{g/cm^3}$

59.

Graphite has a density of $2.26\ \mathrm{g/cm^3}$ . What is the mass of a $1.23\ \mathrm{cm^3}$ sample of graphite?

a)

$2.8\ \mathrm{g}$

b)

$0.54\ \mathrm{g}$

c)

$1.23\ \mathrm{g}$

d)

$2.26\ \mathrm{g}$

60.

A scientist collects 32.8 g of zinc. Given the density of zinc is $7.14\ \mathrm{g/mL}$ , what volume is this sample?

a)

$4.6\ \mathrm{mL}$

b)

$7.14\ \mathrm{mL}$

c)

$0.22\ \mathrm{mL}$

d)

$32.8\ \mathrm{mL}$

61.

How many yards are in 58,256 inches? Use $1\ \mathrm{yd}=36\ \mathrm{in}$ .

a)

$1{,}618.2\ \mathrm{yd}$

b)

$5{,}280\ \mathrm{yd}$

c)

$1{,}620\ \mathrm{yd}$

d)

$162.0\ \mathrm{yd}$

62.

How many pints are in 6.32 gal? Use $1\ \mathrm{gal}=8\ \mathrm{pt}$ .

a)

$50.56\ \mathrm{pt}$

b)

$6.32\ \mathrm{pt}$

c)

$25.28\ \mathrm{pt}$

d)

$40.0\ \mathrm{pt}$

63.

How many miles are in 789 inches? Use $12\ \mathrm{in}=1\ \mathrm{ft}$ and $5280\ \mathrm{ft}=1\ \mathrm{mi}$ .

a)

$0.012\ \mathrm{mi}$

b)

$0.12\ \mathrm{mi}$

c)

$0.0012\ \mathrm{mi}$

d)

$0.052\ \mathrm{mi}$

64.

How many ounces are in 325.94 grams? Use $453.59\ \mathrm{g}=1\ \mathrm{lb}$ and $16\ \mathrm{oz}=1\ \mathrm{lb}$ .

a)

$11.5\ \mathrm{oz}$

b)

$7.14\ \mathrm{oz}$

c)

$32.6\ \mathrm{oz}$

d)

$4.6\ \mathrm{oz}$

65.

Write 83,500 km in scientific notation.

a)

$8.35 \times 10^4$ km

b)

$8.35 \times 10^5$ km

c)

$8.350 \times 10^3$ km

d)

$8.35 \times 10^3$ km

66.

Write 0.000685 mg in scientific notation.

a)

$6.85 \times 10^{-4}$ mg

b)

$6.85 \times 10^{-5}$ mg

c)

$6.85 \times 10^{4}$ mg

d)

$6.85 \times 10^{-6}$ mg

67.

Write 732,000,000,000 kg in scientific notation.

a)

$7.32 \times 10^{11}$ kg

b)

$7.32 \times 10^{10}$ kg

c)

$7.32 \times 10^{12}$ kg

d)

$7.32 \times 10^{9}$ kg

68.

Write 0.000066757 mm in scientific notation.

a)

$6.6757 \times 10^{-5}$ mm

b)

$6.6757 \times 10^{-6}$ mm

c)

$6.6757 \times 10^{5}$ mm

d)

$6.6757 \times 10^{-4}$ mm

69.

Write each number in ordinary notation: $2.3 \times 10^8$ km.

a)

230,000,000 km

b)

23,000,000 km

c)

2,300,000 km

d)

2,300 km

70.

Write each number in ordinary notation: $8.27 \times 10^5$ mm.

a)

0.0000827 mm

b)

.82700 mm

c)

8,270 mm

d)

8,270,000 mm

71.

Write each number in ordinary notation: $6.52 \times 10^{-2}$ mL.

a)

0.0652 mL

b)

0.652 mL

c)

0.00652 mL

d)

6.52 mL

72.

Write each number in ordinary notation: $3.73 \times 10^9$ L.

a)

3,730,000,000 L

b)

373,000,000 L

c)

37,300,000 L

d)

3,730,000 L

73.

Try these conversions using the ladder method: Write out the metric prefix conversion chart in order from kilo to milli.

a)

kilo, hecto, deka, base unit, deci, centi, milli

b)

milli, centi, deci, base unit, deka, hecto, kilo

c)

base unit, kilo, hecto, deka, deci, centi, milli

d)

kilo, deka, hecto, base unit, centi, deci, milli

74.

Try these conversions using the ladder method: 255 mL = ___ dL.

a)

2.55 dL

b)

25.5 dL

c)

0.255 dL

d)

0.0255 dL

75.

Try these conversions using the ladder method: 63 mg = ___ hg.

a)

6.3 × 10^{-5} hg

b)

6.3 × 10^{-3} hg

c)

6.3 × 10^-2 hg

d)

6.3 × 10^{-1} hg

76.

Try these conversions using the ladder method: 6.7 kg = ___ dag.

a)

67 dag

b)

0.67 dag

c)

670 dag

d)

6.7 dag

77.

Try these conversions using the ladder method: 42 cm = ___ m.

a)

0.42 m

b)

4.2 m

c)

0.042 m

d)

0.0042 m

78.

Try these conversions using the ladder method: 8.3 L = ___ dL.

a)

83 dL

b)

8.3 dL

c)

0.83 dL

d)

0.083 dL

79.

Unit 3 – Atomic Structure: _____ was the first person to come up with the idea of an atom.

a)

Democritus

b)

Aristotle

c)

Niels Bohr

d)

Marie Curie

80.

Unit 3 – Atomic Structure: _____ is known as the "Father of the Modern Atomic Theory".

a)

John Dalton

b)

Ernest Rutherford

c)

J. J. Thomson

d)

Erwin Schrödinger

81.

Unit 3 – Atomic Structure: _____ discovered the neutron.

a)

James Chadwick

b)

J. J. Thomson

c)

Ernest Rutherford

d)

Robert Millikan

82.

Unit 3 – Atomic Structure: _____ discovered electrons.

a)

J. J. Thomson

b)

Ernest Rutherford

c)

Niels Bohr

d)

Henry Moseley

83.

Unit 3 – Atomic Structure: _____ discovered the nucleus.

a)

Ernest Rutherford

b)

James Chadwick

c)

J. J. Thomson

d)

John Dalton

84.

Unit 3 – Atomic Structure: What is the name of Thomson’s model of the atom?

a)

Plum pudding model

b)

Nuclear model

c)

Planetary model

d)

Quantum mechanical model

85.

Unit 3 – Atomic Structure: What is the name of Rutherford’s model of the atom?

a)

Nuclear model

b)

Plum pudding model

c)

Bohr model

d)

Thomson model

86.

Unit 3 – Atomic Structure: Identify the subatomic particle described as found in the nucleus with positive charge.

a)

Proton

b)

Neutron

c)

Electron

d)

Positron

87.

Unit 3 – Atomic Structure: Identify the subatomic particle described as found in the nucleus with neutral charge.

a)

Neutron

b)

Proton

c)

Electron

d)

Alpha particle

88.

Unit 3 – Atomic Structure: Identify the subatomic particle described as found in the electron clouds with negative charge.

a)

Electron

b)

Proton

c)

Neutron

d)

Beta particle

89.

Unit 3 – Atomic Structure: How are atoms electrically neutral?

a)

The number of protons equals the number of electrons

b)

The number of neutrons equals the number of electrons

c)

Atoms have no charged particles

d)

Protons equal neutrons

90.

Unit 3 – Atomic Structure: Atoms of the same element with different numbers of neutrons are called _____.

a)

Isotopes

b)

Ions

c)

Allotropes

d)

Isomers

91.

What are isotopes named by?

a)

Mass number

b)

Atomic number

c)

Number of electrons

d)

Charge

92.

The sum of protons and neutrons in an atom equals the _____.

a)

Mass number

b)

Atomic number

c)

Avogadro’s number

d)

Molar mass

93.

The SI unit for an amount of a substance is the _____.

a)

mole

b)

gram

c)

liter

d)

kelvin

94.

_____ is the mass of one mole of atoms or molecules and is measured in grams.

a)

Molar mass

b)

Atomic number

c)

Mass number

d)

Density

95.

What is the conversion factor between moles and grams?

a)

1 mol = molar mass (in grams)

b)

1 mol = $6.02 \times 10^{23}$ particles

c)

1 mol = 22.4 L at STP

d)

1 mol = atomic number (in grams)

96.

What is the conversion factor between moles and atoms?

a)

1 mol = $6.02 \times 10^{23}$ atoms

b)

1 mol = molar mass (in grams)

c)

1 mol = 22.4 L at STP

d)

1 mol = $6.02 \times 10^{20}$ atoms

97.

What is the mass in grams of 2.56 mol of Li?

a)

17.92 g Li

b)

25.6 g Li

c)

13.9 g Li

d)

2.56 g Li

98.

How many moles of Br are equivalent to $7.45 \times 10^{16}$ atoms?

a)

$1.24 \times 10^{-7}$ mol

b)

$7.45 \times 10^{-16}$ mol

c)

$6.02 \times 10^{-23}$ mol

d)

$2.45 \times 10^{-6}$ mol

99.

How many moles of Ag are contained in 325.8 grams of Ag?

a)

3.02 mol

b)

0.325 mol

c)

1.08 mol

d)

2.02 mol

100.

How many atoms of Ca are equivalent to 0.55 mol?

a)

$3.31 \times 10^{23}$ atoms

b)

$6.02 \times 10^{23}$ atoms

c)

$1.10 \times 10^{23}$ atoms

d)

$2.20 \times 10^{22}$ atoms

101.

Complete the following table: For 35Br with mass number 80, what is the number of neutrons?

a)

45

b)

35

c)

80

d)

55

102.

Complete the following table: For 31P (atomic number 15, mass number 31), what is the number of neutrons?

a)

16

b)

15

c)

31

d)

14

103.

Complete the following table: For 137Ba (atomic number 56, mass number 137), what is the number of electrons in a neutral atom?

a)

56

b)

81

c)

137

d)

75

104.

Unit 4 – Electrons & Notations: Who came up with the quantum mechanical model of the atom, which is the current model of the atom?

a)

Erwin Schrödinger

b)

Niels Bohr

c)

J. J. Thomson

d)

Werner Heisenberg

105.

Unit 4 – Electrons & Notations: An _____ is a three-dimensional region around the nucleus that indicates the probable location of an electron.

a)

orbital

b)

energy level

c)

nucleus

d)

quantum

106.

Unit 4 – Electrons & Notations: _____ specify the properties of the atomic orbitals and the properties of electrons in those orbitals.

a)

Quantum numbers

b)

Electron configurations

c)

Sublevels

d)

Spectral lines

107.

Unit 4 – Electrons & Notations: How many quantum numbers is each electron given?

a)

4

b)

2

c)

3

d)

5

108.

Unit 4 – Electrons & Notations: Principal quantum number indicates the main energy level.

a)

Main energy level

b)

Spatial orientation

c)

Shape of orbital

d)

Electron spin

109.

Unit 4 – Electrons & Notations: Angular momentum quantum number indicates the shape of the orbital.

a)

Shape of orbital

b)

Main energy level

c)

Spatial orientation

d)

Electron spin

110.

Unit 4 – Electrons & Notations: Magnetic quantum number indicates the spatial orientation of the orbital.

a)

Spatial orientation

b)

Main energy level

c)

Shape of orbital

d)

Electron spin

111.

Unit 4 – Electrons & Notations: Spin quantum number indicates the spin of the electron on its own axis.

a)

Electron spin

b)

Main energy level

c)

Shape of orbital

d)

Spatial orientation

112.

Unit 4 – Electrons & Notations: What is the lowest value for the principal quantum number n?

a)

1

b)

0

c)

2

d)

7

113.

Unit 4 – Electrons & Notations: What is a typical highest principal quantum number used for ground-state atoms in the periodic table?

a)

7

b)

5

c)

3

d)

2

114.

Unit 4 – Electrons & Notations: What rule states that orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin?

a)

Hund’s rule

b)

Pauli exclusion principle

c)

Aufbau principle

d)

Heisenberg uncertainty principle

115.

Unit 4 – Electrons & Notations: Identify the element with electron configuration $1s^2\,2s^2\,2p^3$ .

a)

Nitrogen (N)

b)

Oxygen (O)

c)

Carbon (C)

d)

Fluorine (F)

116.

Unit 4 – Electrons & Notations: Identify the element with electron configuration $1s^2\,2s^2\,2p^6\,3s^2\,3p^5$ .

a)

Chlorine (Cl)

b)

Sodium (Na)

c)

Phosphorus (P)

d)

Argon (Ar)

117.

Unit 4 – Electrons & Notations: Identify the element with electron configuration $1s^2\,2s^2\,2p^6\,3s^2\,3p^6\,4s^2\,3d^{10}\,4p^6\,5s^2\,4d^{10}\,5p^6$ .

a)

Xenon (Xe)

b)

Krypton (Kr)

c)

Bromine (Br)

d)

Tellurium (Te)

118.

Unit 4 – Electrons & Notations: What is the maximum number of electrons contained in an orbital?

a)

2

b)

1

c)

4

d)

6

119.

Unit 4 – Electrons & Notations: What is the maximum number of electrons contained in a p sublevel?

a)

6

b)

2

c)

4

d)

10

120.

Unit 4 – Electrons & Notations: What is the maximum number of electrons contained in an s sublevel?

a)

2

b)

6

c)

10

d)

14

121.

Unit 4 – Electrons & Notations: What is the maximum number of electrons contained in a d sublevel?

a)

10

b)

14

c)

6

d)

2

122.

Unit 4 – Electrons & Notations: True or False — An electron can be described as both a wave and a particle.

a)

True

b)

False

123.

Unit 5 – The Periodic Table of Elements: What is the difference between a group and a period? List the number of groups and periods on the periodic table.

a)

Groups are columns; periods are rows; 18 groups and 7 periods

b)

Groups are rows; periods are columns; 7 groups and 18 periods

c)

Groups are diagonal lines; periods are blocks; 8 groups and 4 periods

d)

Groups are shells; periods are families; 7 groups and 7 periods

124.

Unit 5 – The Periodic Table of Elements: Circle where you would find elements with similar properties: group or period.

a)

Group

b)

Period

c)

Diagonal across the table

d)

Random distribution

125.

Unit 5 – The Periodic Table of Elements: What is the name given to Group 1 on the periodic table?

a)

Alkali metals

b)

Alkaline earth metals

c)

Transition metals

d)

Halogens

e)

Noble gases

126.

Unit 5 – The Periodic Table of Elements: What is the name given to Group 2 on the periodic table?

a)

Alkali metals

b)

Alkaline earth metals

c)

Transition metals

d)

Halogens

e)

Noble gases

127.

Unit 5 – The Periodic Table of Elements: What is the name given to Groups 3–12 on the periodic table?

a)

Alkali metals

b)

Alkaline earth metals

c)

Transition metals

d)

Halogens

e)

Noble gases

128.

Unit 5 – The Periodic Table of Elements: What is the name given to Group 17 on the periodic table?

a)

Alkali metals

b)

Alkaline earth metals

c)

Transition metals

d)

Halogens

e)

Noble gases

129.

Unit 5 – The Periodic Table of Elements: What is the name given to Group 18 on the periodic table?

a)

Alkali metals

b)

Alkaline earth metals

c)

Transition metals

d)

Halogens

e)

Noble gases

130.

Unit 5 – The Periodic Table of Elements: How are the elements arranged on the periodic table today?

a)

Increasing atomic number

b)

Increasing atomic mass

c)

Alphabetical by element name

d)

By discovery date

131.

Unit 5 – The Periodic Table of Elements: What is the difference between anions and cations, and how are they formed?

a)

Anions are negatively charged ions formed when atoms gain electrons; cations are positively charged ions formed when atoms lose electrons

b)

Anions are positively charged ions formed when atoms gain protons; cations are negatively charged ions formed when atoms lose protons

c)

Anions are neutral atoms that share electrons; cations are atoms that share protons

d)

Anions and cations are both neutral and form by sharing electrons

132.

Unit 5 – The Periodic Table of Elements: Suppose lithium formed an ion. How many electrons and protons does a lithium ion have? (Hint: consider the typical charge of a lithium ion.)

a)

3 protons and 3 electrons

b)

3 protons and 2 electrons

c)

2 protons and 3 electrons

d)

3 protons and 4 electrons

133.

Unit 5 – The Periodic Table of Elements: Suppose nitrogen formed an ion. How many electrons and protons does a nitride ion have? (Hint: consider the typical charge of a nitride ion.)

a)

7 protons and 7 electrons

b)

7 protons and 8 electrons

c)

7 protons and 10 electrons

d)

8 protons and 10 electrons

134.

Unit 5 – The Periodic Table of Elements: Place the ionic charge for Group 1 elements on the periodic table.

a)

+1

b)

+2

c)

−1

d)

0

135.

Unit 5 – The Periodic Table of Elements: Place the ionic charge for Group 2 elements on the periodic table.

a)

+1

b)

+2

c)

−2

d)

0

136.

Unit 5 – The Periodic Table of Elements: Place the ionic charge for Group 13 elements on the periodic table.

a)

+3

b)

+4

c)

−3

d)

0

137.

Unit 5 – The Periodic Table of Elements: Place the ionic charge for Group 14 elements on the periodic table.

a)

Typically +4 or −4

b)

Always +2

c)

Always −2

d)

Always 0

138.

Unit 5 – The Periodic Table of Elements: Place the ionic charge for Group 15 elements on the periodic table.

a)

−3

b)

+3

c)

+1

d)

0

139.

Unit 5 – The Periodic Table of Elements: Place the ionic charge for Group 16 elements on the periodic table.

a)

−2

b)

+2

c)

+1

d)

0

140.

Unit 5 – The Periodic Table of Elements: Place the ionic charge for Group 17 elements on the periodic table.

a)

−1

b)

+1

c)

+2

d)

0

141.

Unit 5 – The Periodic Table of Elements: Place the ionic charge for Group 18 elements on the periodic table.

a)

0

b)

+1

c)

−1

d)

+2

142.

Arrange the following set of elements in order of DECREASING electronegativity (start with the highest and go to the lowest): Li, N, B, Be.

a)

N, B, Be, Li

b)

B, N, Li, Be

c)

Li, Be, B, N

d)

Be, B, N, Li

143.

Arrange the following set of elements in order of DECREASING electronegativity (start with the highest and go to the lowest): Te, S, O, F.

a)

F, O, S, Te

b)

O, S, F, Te

c)

S, F, O, Te

d)

Te, S, O, F

144.

Arrange the following set of elements in order of DECREASING electronegativity (start with the highest and go to the lowest): Sr, Be, Mg, C.

a)

C, Be, Mg, Sr

b)

Be, C, Mg, Sr

c)

Mg, Be, C, Sr

d)

Sr, Mg, Be, C

145.

Arrange the following set of elements in order of DECREASING first ionization energy (start with the highest and go to the lowest): F, Ga, C, N.

a)

F, N, C, Ga

b)

F, C, N, Ga

c)

N, F, C, Ga

d)

Ga, C, N, F

146.

Arrange the following set of elements in order of DECREASING first ionization energy (start with the highest and go to the lowest): K, Rb, Mg, Al.

a)

Mg, Al, K, Rb

b)

Al, Mg, K, Rb

c)

K, Rb, Mg, Al

d)

Rb, K, Al, Mg

147.

Arrange the following set of elements in order of DECREASING first ionization energy (start with the highest and go to the lowest): S, O, Se, Te.

a)

O, S, Se, Te

b)

S, O, Te, Se

c)

Se, Te, S, O

d)

Te, Se, S, O

148.

Arrange the following set of elements in order of DECREASING atomic radius (start with the highest and go to the lowest): Li, Na, K, Be.

a)

K, Na, Li, Be

b)

Na, K, Li, Be

c)

Li, Na, K, Be

d)

Be, Li, Na, K

149.

Arrange the following set of elements in order of DECREASING atomic radius (start with the highest and go to the lowest): B, C, O, F.

a)

B, C, O, F

b)

F, O, C, B

c)

O, F, C, B

d)

C, B, O, F

150.

Arrange the following set of elements in order of DECREASING atomic radius (start with the highest and go to the lowest): B, Ga, Al, In.

a)

In, Ga, Al, B

b)

In, Al, Ga, B

c)

Ga, In, Al, B

d)

B, Al, Ga, In

Chemistry Midterm 1

Total questions: 150

Worksheet time: 1hrs 15mins

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