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Fall Physical Science Semester Test Review 2025

Total questions: 60

Worksheet time: 30mins

Name
Class
Date
1.

In a Lewis diagram, the dots represent—

a)

Protons

b)

Valence electrons

c)

Atomic mass

d)

Bond energy

2.

A correct Lewis diagram shows—

a)

All electrons paired

b)

Only valence electrons

c)

All electrons in the atom

d)

Charges on every atom

3.

Which mistake would make a Lewis diagram invalid?

a)

Showing lone pairs

b)

Drawing straight lines

c)

Having too many electrons around an atom

4.

Lines between atoms in a Lewis model represent—

a)

Energy levels

b)

Shared electron pairs

c)

Ionic transfer

d)

Neutron clusters

5.

A triple bond contains—

a)

One shared pair

b)

Two shared pairs

c)

Three shared pairs

d)

No shared pairs

6.

Which element usually forms four bonds in covalent structures?

a)

Oxygen

b)

Fluorine

c)

Carbon

d)

Nitrogen

7.

Why would Ca form a 2+ charge in a Lewis diagram?

a)

To show sharing

b)

Ca must give two electrons to O

c)

To form double bonds

d)

Because both are gases

8.

Arrows in a Lewis diagram indicate—

a)

Covalent bonds

b)

Electron transfer

c)

Plasma formation

d)

Metallic bonding

9.

Diatomic molecules such as F₂ require—

a)

No electrons

b)

A triple bond

c)

Two ionic bonds

d)

One shared pair

10.

Lone pairs represent—

a)

Protons

b)

Unshared electrons

c)

Covalent bonds

d)

Ionic charges

11.

Which atom has only two valence electrons?

a)

Carbon

b)

Helium

c)

Nitrogen

d)

Chlorine

12.

The starting materials in a reaction are—

a)

Reactants

b)

Products

c)

Catalysts

d)

Enzymes

13.

Which is a sign of chemical change?

a)

Melting

b)

Formation of gas

c)

Cutting metal

d)

Dissolving salt

14.

During a chemical reaction, mass—

a)

Is created

b)

Is destroyed

c)

Stays the same

d)

Doubles

15.

A reaction forming one product from two reactants is—

a)

Decomposition

b)

Combustion

c)

Synthesis

d)

Displacement

16.

Which process absorbs energy?

a)

Burning wood

b)

Ice melting

c)

Metal rusting

d)

Fireworks

17.

An exothermic reaction—

a)

Absorbs heat

b)

Releases heat

c)

Does not involve energy

d)

Forms colder products

18.

If heat appears on the product side, the reaction is—

a)

Endothermic

b)

Exothermic

c)

Slow

d)

Neutral

19.

In a balanced equation, atoms—

a)

Must be equal on both sides

b)

Can differ

c)

Must double

d)

Don’t matter

20.

Combustion reactions always involve—

a)

Oxygen

b)

Metals

c)

Lithium

d)

Plasma

21.

A precipitate forms when—

a)

A solid melts

b)

A solid forms from two solutions

c)

A gas cools

d)

A mixture separates

22.

Which result supports conservation of mass?

a)

30 g reactants, 30 g products

b)

Products > reactants

c)

Mass decreases

d)

Mass doubles

23.

Burning methane is what type of reaction?

a)

Synthesis

b)

Decomposition

c)

Combustion

24.

The image represents what type of reaction.

a)

Synthesis

b)

Combustion

c)

Single replacement

d)

Double replacement

25.

Which is NOT a sign of chemical change?

a)

Color change

b)

Temperature change

c)

Gas formation

d)

Freezing

26.

Breaking chemical bonds—

a)

Releases heat

b)

Requires absorbing energy

c)

Releases releasing heat

d)

Requires no energy

27.

If 12 g react and 12 g result, this shows—

a)

Conservation of mass

b)

A physical change

c)

An ionic bond

d)

A decomposition reaction

28.

Coefficients show—

a)

Temperature

b)

Number of molecules

c)

Charge

d)

State of matter

29.

Subscripts show—

a)

Temperature

b)

Number of atoms

c)

Charge

d)

State of matter

30.

Which equation is balanced?

a)

N₂+H₂→NH₃

b)

N₂+3H₂→NH₃

c)

N₂+3H₂→2NH₃

d)

2N₂+H₂→NH₃

31.

Rows on the periodic table are—

a)

Groups

b)

Periods

c)

Levels

d)

Blocks

32.

Columns on the periodic table show—

a)

Groups

b)

Periods

c)

Levels

d)

Blocks

33.

Valence electrons determine—

a)

Mass

b)

Reactivity

c)

Temperature

d)

Electron speed

34.

Which are metalloids?

a)

O, S, Se

b)

B, Si, Ge

c)

Fe, Ni, Co

d)

He, Ne, Ar

35.

Electronegativity is highest among—

a)

Bottom left

b)

Top right

c)

Group 18

d)

Transition metals

36.

Elements with full outer shells are—

a)

Reactive

b)

Metals

c)

Noble gases

d)

Liquids

37.

Which is a chemical property?

a)

Color

b)

Density

c)

Reactivity

d)

Volume

38.

Which is a physical property?

a)

Flammability

b)

Reactivity

c)

Density

d)

Rusting

39.

Isotopes differ because they have different—

a)

Electrons

b)

Protons

c)

Neutrons

d)

Charges

40.

A neutral atom becomes negative by—

a)

Losing electrons

b)

Gaining electrons

c)

Losing neutrons

d)

Gaining protons

41.

A family on the periodic table is a—

a)

Period

b)

Group

c)

Block

d)

Row

42.

Most reactive metals are in—

a)

Group 17

b)

Group 1

c)

Group 18

43.

Atomic number equals number of—

a)

Neutrons

b)

Protons

c)

Valence electrons

d)

Energy levels

44.

Group 18 elements are—

a)

Highly reactive

b)

Not reactive

c)

Usually charged

d)

Black solids

45.

Across a period, atomic radius—

a)

Increases

b)

Decreases

46.

Down a group, atomic radius—

a)

Increases

b)

Decreases

c)

Stays the same

d)

Becomes zero

47.

Metals tend to—

a)

Lose electrons

b)

Gain electrons

c)

Share electrons

d)

Form gases

48.

Density equals—

a)

Mass ÷ volume

b)

Mass × volume

c)

Volume ÷ mass

d)

Volume × mass

49.

What is the formula for density?

a)

Mass ÷ volume

b)

Volume ÷ mass

c)

Weight × height

d)

Mass × height

50.

An object less dense than water will—

a)

Sink

b)

Float

c)

Boil

d)

Dissolve

51.

What is the most dense state of matter?

a)

Gas

b)

Solid

c)

Plasma

d)

Vapor

52.

Where are electrons located?

a)

In the nucleus

b)

In the electron shells/rings

c)

In the proton shell

d)

In the neutron field

53.

Variable changed on purpose is the—

a)

Dependent variable

b)

Independent variable

c)

Constant

d)

Conclusion

54.

Factor measured is the—

a)

Control

b)

Dependent variable

c)

Constant

d)

Hypothesis

55.

Control group is used as—

a)

Control

b)

Dependent variable

c)

Constant

d)

Hypothesis

56.

What is a good hypothesis written as?

a)

Because... therefore...

b)

If... then...

c)

Who... what...

d)

Fact statement

57.

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

a)

Rusting

b)

Melting

c)

Burning

d)

Gas production

58.

Largest atomic radius is found

a)

Bottom left

b)

Top right

c)

Group 18

d)

Transition metals

59.

Which name for CaBr₂ is correct? (8th only)

a)

Calcium dibromide

b)

Calcium dibromine

c)

Calcium bromide

d)

Calcium bromine

60.

What is the correct name for PCl₅ (8th only)

a)

Phosphorus chlorine

b)

Phosphorus chloride

c)

Phosphorus pentachloride

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