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Worksheets

7th grade comp

Total questions: 94

Worksheet time: 52mins

Name
Class
Date
1.

Which is the SI unit of mass?

a)

Milligram (mg)

b)

Centigram (cg)

c)

Kilogram (kg)

d)

Gram (g)

2.

Which is a unit of volume?

a)

Millimeter (mm)

b)

Centimeter (cm)

c)

Millimeters cubed (mm³)

d)

Mile (mi)

3.

Which is the SI unit of length?

a)

Kilometer (km)

b)

Millimeter (mm)

c)

Centimeter (cm)

d)

Meter (m)

4.

Which is the SI unit of temperature?

a)

Celsius

b)

Fahrenheit

c)

Kelvin

d)

Millimeters of Mercury

5.

Which is the SI unit of time?

a)

Seconds

b)

Minutes

c)

Hours

d)

Nanoseconds

6.

McLellan measured 145.89 g of iron. How many kilograms of iron is this?

a)

0.14589 kg

b)

1.4589 kg

c)

145.890 kg

d)

0.014589 kg

7.

Luke had 91.300 mL of Bromine in a volumetric flask. Sky removed 5.25 mL of Bromine. What volume of Bromine does Luke now have to correct significant figures?

a)

86 mL

b)

86.1 mL

c)

86.05 mL

d)

86.050 mL

8.

What is the smallest unit of an element that still retains the element’s properties?

a)

Electron

b)

Atom

c)

Proton

d)

Compound

9.

Which of the following is made up of only one type of atom?

a)

NaF

b)

N₂

c)

SiF₄

d)

MgI₂

10.

Which of the following substances can’t be broken down by ordinary chemical means?

a)

Water (H₂O)

b)

Copper (Cu)

c)

Isopropyl Alcohol (C₃H₈O)

d)

Glucose (C₆H₁₂O₆)

11.

Substances that are combined physically and can be physically separated are called:

4 lines
12.

Substances composed of atoms of 2 or more different elements that are bonded are called:

a)

Diatomic elements

b)

Compounds

c)

Homogenous Mixtures

d)

Heterogeneous Mixtures

13.

Which of the following substances is a suspension?

a)

Fog

b)

Tomato juice

c)

Salt water

d)

Air

14.

Which of the following substances is dissolved in water?

a)

HNO₃ (s)

b)

HNO₃ (l)

c)

HNO₃ (g)

d)

HNO₃ (aq)

15.

A pure substance made up of only one type of atom is called a(n) (a)   .

16.

Which of the following is not found as a diatomic element in nature?

a)

B₂

b)

O₂

c)

H₂

d)

F₂

17.

In which phase does a substance have very fast moving, compressible particles?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

18.

In which phase does a substance have particles that are very tightly packed?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

19.

In which phase does a substance have a definite volume but no definite shape?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

20.

Changes that result in a change in the identity of a substance are called:

a)

Physical changes

b)

Chemical changes

c)

Identical changes

d)

Phase changes

21.

Which of the following is not a physical property?

a)

Density

b)

Melting Point

c)

Flammable

d)

Odor

22.

A teacher pours sulfuric acid on sugar in a beaker. The sugar turns yellow and then black. Smoke rises, and a strong smell is released. This is an example of what kind of change?

a)

Physical

b)

Chemical

c)

Electrical

d)

Magnetic

23.

Which of the following is the change from a liquid to a gas?

a)

Boiling

b)

Melting

c)

Condensation

d)

Freezing

24.

Which of the following is the change from a gas to a liquid?

a)

Boiling

b)

Melting

c)

Condensation

d)

Freezing

25.

Which of the following is the change from a liquid to a solid?

a)

Boiling

b)

Melting

c)

Condensation

d)

Freezing

26.

When a substance is melted, what happens to the particles in the substance?

a)

They make new bonds

b)

They get further from each other

c)

They break bonds

d)

They get closer together

27.

The ability of a substance to allow the flow of either heat or electricity is called:

a)

Ductility

b)

Malleability

c)

Conductivity

d)

Luster

28.

The ability of a substance to be beaten into a thin sheet is called:

a)

Ductility

b)

Malleability

c)

Conductivity

d)

Luster

29.

Which of the following is not an example of a chemical reaction?

a)

Combustion of methane gas

b)

Sublimation of carbon dioxide

c)

Rusting of copper metal

d)

Tarnishing of silver

30.

Which types of matter are pure substances?

a)

Elements

b)

Homogeneous Mixtures

c)

Compounds

d)

Both a and b

31.

Which of the following diagrams depicts a mixture?

4 lines
32.

Salt completely dissolved in water. In this mixture, water is the ____________.

a)

Solute

b)

Solution

c)

Solvent

d)

Suspension

33.

Suspensions are which of the following?

a)

Have large particles (>1000nm)

b)

A and B

c)

Particles settle out.

d)

Are uniform.

34.

Compounds have __________ composition and mixtures have __________ composition.

(a)  

35.

Distillation is a separation technique that takes advantage of the difference in __________ of the components in the mixture.

a)

Affinity for the mobile phase

b)

Density

c)

Particle size

d)

Boiling point

36.

What would be the best method for separating solid tea leaves from a pot of liquid tea?

a)

Distillation

b)

Chromatography

c)

Filtration

d)

Decanting

37.

Liquid Isopropyl Alcohol (boiling point of 82.6 °C) and liquid water (boiling point of 100 °C) are mixed to form a homogenous mixture. What is the best technique for separating this mixture?

a)

Chromatography

b)

Filtration

c)

Distillation

d)

Decantation

38.

Which technique involves pouring a less dense substance out of a container, leaving the more dense substance behind?

a)

Distillation

b)

Using a magnet

c)

Chromatography

d)

Decantation

39.

Decantation and Filtration are separation techniques used to separate what substances?

a)

Elements

b)

Heterogeneous mixtures

c)

Compounds

d)

Homogeneous mixtures

40.

All of the following are physical properties of matter except __________.

a)

Luster

b)

Density

c)

Acidity

d)

Malleability

41.

(a)   is the ability of a substance to be drawn into wires without breaking.

42.

As pressure increases, the boiling point of a substance will ____________ while the melting point of a substance will ____________.

a)

Increase, Increase

b)

Increase, Decrease

c)

Decrease, Decrease

d)

Decrease, Increase

43.

The following properties of matter can be observed without changing the identity of the substance, except for ______________.

a)

Boiling Point

b)

Ductility

c)

Solubility

d)

Reactivity

44.

What is the name of the phase change from solid to liquid?

a)

Freezing

b)

Melting

c)

Condensation

d)

Evaporation

45.

Which phase of matter has fixed volume but takes the shape of its container?

a)

Solid

b)

Gas

c)

Liquid

d)

Plasma

46.

Which phase of matter has particles that are tightly packed together and vibrating?

a)

Solid

b)

Gas

c)

Liquid

d)

Plasma

47.

What is the name of the phase change from a gas to a solid?

a)

Evaporation

b)

Deposition

c)

Sublimation

d)

Condensation

48.

What is the mass of an atom with 14 protons, 11 neutrons, and 10 electrons?

a)

21 amu

b)

27 amu

c)

24 amu

d)

25 amu

49.

Where are the sub-atomic particles found?

a)

Protons, Electrons, and neutrons are in the nucleus.

b)

Protons are in the nucleus, electrons and neutrons are in the electron cloud.

c)

Protons, neutrons, and electrons are in the electron cloud.

d)

Protons and neutrons in the nucleus, and electrons are in the electron cloud.

50.

A neutron has a charge of ________, and a mass of ________.

(a)  

51.

Which element has 80 protons?

a)

Mercury

b)

Nickel

c)

Bismuth

d)

Bromine

52.

Which subatomic particles contribute to the mass of an atom and are in the nucleus?

a)

Protons and electrons

b)

Protons

c)

Electrons and neutrons

d)

Protons and Neutrons

53.

In an isotope, two atoms of the same element have different.

a)

Charges

b)

Numbers of protons

c)

Numbers of electrons

d)

Numbers of neutrons

54.

In an atom of Carbon-14, which of the following is an accurate description of its sub-atomic particles?

a)

Protons: 14, Neutrons: 12, Electrons: 14

b)

Protons: 6, Neutrons: 6, Electrons: 6

c)

Protons: 6, Neutrons: 8, Electrons: 6

d)

Protons: 14, Neutrons: 6, Electrons: 14

55.

Using hyphen notation, we can write an isotope of Carbon with two extra neutrons as:

a)

13th-Carbon

b)

Carbon-14

c)

Carbon-13

d)

14th-Carbon

56.

When a neutral atom loses electrons, it becomes:

a)

An anion.

b)

An isotope.

c)

A cation.

d)

A different element

57.

When a neutral atom gains electrons, it becomes:

a)

An anion.

b)

An isotope

c)

A cation

d)

A different element

58.

Atoms that have a different number of protons and electrons are called

(a)  

59.

Nitrogen gains 3 electrons. Which of the following is a correct description of it?

a)

Neutral

b)

Cation

c)

Anion

d)

Metal

60.

When calcium becomes a cation, it becomes Ca²⁺. How many TOTAL electrons will it have?

a)

2

b)

18

c)

8

d)

20

61.

What is the formula for Nitrate?

(a)  

62.

What is the formula for Ammonium?

(a)  

63.

Carbonate and Sulfate all have a charge of:

a)

+2

b)

+1

c)

-2

d)

-1

64.

Hydroxide, Cyanide, and acetate all have a charge of:

a)

+2

b)

+1

c)

-2

d)

-1

65.

Selenium is in which period?

a)

6

b)

6A

c)

4

d)

4A

66.

How many electron shells does Iodine have?

a)

5

b)

7

c)

53

d)

17

67.

Which element has 4 electron clouds and 3 valence electrons?

a)

Si

b)

Ga

c)

Sc

d)

Ti

68.

Which of the following is a property of nonmetals?

a)

Lustrous

b)

Dull

c)

Semi-conductors

d)

Malleable

69.

The correct electron configuration for Cl is

a)

1s²2s²2p⁶3s²3p⁴

b)

1s²2s²2p⁶3s²3p⁵

c)

1s²2s²2p⁶3s²3p³

d)

1s²2s²2p⁶3s²3p¹

70.

Of the following elements, which one would have the smallest radius?

a)

Fluorine (F)

b)

Oxygen (O)

c)

Nitrogen (N)

d)

Carbon (C)

71.

The least electronegative elements are the…

a)

Halogens

b)

Noble gases

c)

Metalloids

d)

Alkali metals

72.

Of the elements below, which element has the largest ionization energy?

a)

Li

b)

Na

c)

K

d)

Rb

73.

The Lewis dot structure of NH₃ depicts __________ number of lone pairs on the central atom.

a)

There are no lone pairs of electrons

b)

There is one lone pair of electrons

c)

There are two lone pairs of electrons

d)

There are three lone pairs of electrons

74.

If the metal in an ionic compound is not in group 1A or 2A or in the “Triangle Metals”, then the compound is a _______________ ionic compound.

a)

Metallic

b)

Binary I

c)

Binary II

d)

Binary III

75.

Which of the following metals would form a binary II ionic compound with oxygen?

a)

Zirconium

b)

Fluorine

c)

Cesium

d)

Gallium

76.

Which of the following charges is not a possible charge for the metal in a Binary II Ionic Compound?

a)

+1

b)

-2

c)

+4

d)

+2

77.

What do the Roman Numerals in the name of a Binary II ionic compound represent?

a)

Charge on the compound

b)

Charge on the nonmetal

c)

Charge on the metal

d)

Subscript on the metal

78.

What kind of bonding is involved in sodium cyanide?

a)

Metallic

b)

Covalent

c)

Ionic

d)

Both b and c

79.

What is the chemical formula for rubidium selenide?

a)

RbSe

b)

RbSe2

c)

Rb2Se

d)

Rb2Se

80.

What is the chemical formula for scandium (III) chloride?

a)

ScCl

b)

ScCl3

c)

Sc2Cl3

d)

Sc3Cl

81.

What is the chemical formula for the carbonate ion?

a)

CO3+2

b)

CO3-2

c)

CO2+3

d)

CO2-3

82.

What is the chemical formula for the acetate ion?

a)

C₂H₃O₂⁺

b)

C₂H₃O₂⁺

c)

C₂H₃O₂⁻

d)

C₂H₃O₂⁻

83.

What is the chemical formula for magnesium hydroxide?

a)

MgHO

b)

Mg₂OH

c)

MgOH

d)

Mg(OH)₂

84.

What is the chemical formula for lithium oxide?

a)

LiO

b)

LiO₂

c)

Li₂O

d)

Li₂O₂

85.

What is the chemical formula for barium sulfate?

a)

BaSO₃

b)

Ba(SO₃)₂

c)

BaSO₄

d)

BaS

86.

What type of bond would Carbon and Fluorine form?

a)

Ionic

b)

Metallic

c)

Covalent

d)

They wouldn’t bond

87.

An ionic bond is between ____________.

a)

Two metals

b)

Two nonmetals

c)

One metal and one nonmetal

d)

One nonmetal and one metalloid

88.

Subscripts in a chemical formula represent the __________.

a)

Charge

b)

Neutrons

c)

Protons

d)

Number of atoms

89.

Ionic compounds have ________ melting points and ________ boiling points.

a)

High, high

b)

Low, high

c)

High, low

d)

Low, low

90.

Binary I ionic compounds include:

a)

A metal with variable charge and a nonmetal

b)

A metal with fixed charge and a nonmetal

c)

Two nonmetals

d)

Two metals

91.

The correct name of Cu(OH)₂ is:

a)

Copper Hydroxide

b)

Copper (II) Hydroxide

c)

Copper Dihydroxide

d)

Copper (I) Dihydroxide

92.

What is the formula for carbon tetrafluoride?

a)

C₄F

b)

C₄Fl

c)

CF₄

d)

CFl₄

93.

How many electrons are shared in a single covalent bond?

a)

1

b)

4

c)

2

d)

8

94.

Which of these compounds would NOT have covalent bonds?

a)

PCl₃

b)

C₂H₆

c)

K₂O

d)

H₂O₂

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