Free Printable Study Guide (8th Grade Science Winter Exam)

1.

Physical science is the study of (nonliving/living) things.

a)

Nonliving things

b)

Living things

2.

What is the goal of science?

a)

To explain and understand the natural world using evidence

b)

To prove personal opinions are correct

c)

To keep traditions unchanged

d)

To collect facts without drawing conclusions

3.

What accumulates over time in order for science to progress?

a)

Knowledge built from evidence

b)

Random guesses

c)

Unchanging rules

d)

Personal beliefs

4.

What are the two branches of physical science?

a)

Physics and chemistry

b)

Biology and geology

c)

Astronomy and zoology

d)

Ecology and botany

5.

Does physical science follow a strict sequence of unchangeable steps?

a)

No, the process can vary

b)

Yes, the steps never change

6.

What gives matter the ability to change?

a)

Energy

b)

Mass

c)

Shape

d)

Volume

7.

The study of matter and energy at the scale of atoms and molecules is called ________.

a)

Chemistry

b)

Geology

c)

Meteorology

d)

Astronomy

8.

What are the forms energy can take?

a)

Kinetic and potential

b)

Solid and liquid

c)

Hot and cold

d)

Mass and volume

9.

Give an example of a problem that is most likely to be investigated by a physical scientist.

a)

How the mass of a ball affects its acceleration down a ramp

b)

How leaves make food in a plant

c)

Why a species of bird migrates earlier in the spring

d)

How a vaccine triggers an immune response

10.

Place the following steps of the scientific method in the correct order: Experiment – Observation – Hypothesis – Conclusion.

a)

Observation → Hypothesis → Experiment → Conclusion

b)

Hypothesis → Observation → Experiment → Conclusion

c)

Experiment → Observation → Hypothesis → Conclusion

d)

Observation → Experiment → Hypothesis → Conclusion

11.

What should a scientist do after forming a hypothesis?

a)

Design and conduct an experiment to test it

b)

Write the final report immediately

c)

Change the hypothesis until results fit

d)

Ignore evidence that disagrees

12.

Label the sentence: "The increased amount of CO2 in the air is because of pollution." Choose hypothesis, question, or observation.

a)

Hypothesis

b)

Question

c)

Observation

13.

Label the sentence: "Why is there so much CO2 in the air?" Choose hypothesis, question, or observation.

a)

Hypothesis

b)

Question

c)

Observation

14.

Label the sentence: "I wonder if the CO2 in the air is causing pollution." Choose hypothesis, question, or observation.

a)

Hypothesis

b)

Question

c)

Observation

15.

Place the 5 steps of the scientific method in order.

a)

Ask a question → Form a hypothesis → Conduct an experiment → Analyze data → Draw a conclusion

b)

Make an observation → Draw a conclusion → Form a hypothesis → Analyze data → Conduct an experiment

c)

Ask a question → Conduct an experiment → Form a hypothesis → Analyze data → Draw a conclusion

d)

Form a hypothesis → Analyze data → Conduct an experiment → Ask a question → Draw a conclusion

16.

Fill in the unit conversion stairs.

a)

kilo → hecto → deka → base (meter/liter/gram) → deci → centi → milli

b)

kilo → deci → centi → milli → base → hecto → deka

c)

milli → centi → deci → base → deka → hecto → kilo

d)

base → kilo → hecto → deka → deci → centi → milli

17.

How many grams are in $1$ kilogram?

a)

$1{,}000$ g

b)

$100$ g

c)

$100{,}000$ g

d)

$10$ g

18.

What prefix multiplies a basic SI unit by $0.001$ ?

a)

Milli-

b)

Centi-

c)

Deci-

d)

Micro-

19.

What prefix multiplies a basic SI unit by $0.01$ ?

a)

Centi-

b)

Milli-

c)

Deci-

d)

Micro-

20.

Complete the conversion: $2{,}000\ \text{m} =$ ______.

a)

$2$ km

b)

$0.2$ km

c)

$20$ km

d)

$200$ km

21.

Complete the conversion: $5{,}000\ \text{m} =$ ______.

a)

$5$ km

b)

$0.5$ km

c)

$50$ km

d)

$500$ km

22.

Complete the conversion: $3\ \text{kg} =$ ______.

a)

$3{,}000$ g

b)

$300$ g

c)

$30$ g

d)

$3$ g

23.

What SI base unit is used to measure length?

a)

Meter (m)

b)

Gram (g)

c)

Liter (L)

d)

Second (s)

24.

In the USA, what unit is used to measure length?

a)

Inches, feet, and miles (customary units)

b)

Meters and kilometers only

c)

Liters and grams

d)

Newtons

25.

What piece of lab equipment measures the volume of a liquid?

a)

Graduated cylinder

b)

Triple-beam balance

c)

Thermometer

d)

Meterstick

26.

The amount of matter in a substance is called what?

a)

Mass

b)

Volume

c)

Density

d)

Weight

27.

What is the measure of how closely packed together the particles of matter are in a specific substance or object called?

a)

Density

b)

Volume

c)

Mass

d)

Buoyancy

28.

How do we find the volume of an irregularly shaped object?

a)

By using water displacement in a graduated cylinder

b)

By measuring its length, width, and height and multiplying

c)

By weighing it and dividing by density

d)

By measuring with a ruler and protractor

29.

Which has the greater density: Helium with density $0.167\ \text{kg/m}^3$ or air with density $1.225\ \text{kg/m}^3$ ?

a)

Helium

b)

Air

30.

If an object has a mass of $60\ \text{g}$ and a volume of $30\ \text{cm}^3$ , what is the object's density?

a)

$0.5\ \text{g/cm}^3$

b)

$2\ \text{g/cm}^3$

c)

$30\ \text{g/cm}^3$

d)

$1\ \text{g/cm}^3$

31.

At $4^{\circ}\text{C}$ , water has a density of $1000\ \text{kg/m}^3$ and ice has a density of $917\ \text{kg/m}^3$ . Why does ice float in water?

a)

Ice is less dense than water

b)

Ice is more massive than water

c)

Water repels solid ice

d)

Ice has a larger volume than water

32.

A graduated cylinder contains $10\ \text{mL}$ of water. After an irregular solid is added, the level rises to $25\ \text{mL}$ . What is the volume of the irregular solid?

a)

$10\ \text{mL}$

b)

$15\ \text{mL}$

c)

$25\ \text{mL}$

d)

$35\ \text{mL}$

33.

Given mass $=60\ \text{g}$ and volume $=30\ \text{mL}$ , what is the density of the substance?

a)

$0.5\ \text{g/mL}$

b)

$1.5\ \text{g/mL}$

c)

$2.0\ \text{g/mL}$

d)

$3.0\ \text{g/mL}$

34.

Given volume $=10.4\ \text{mL}$ and density $=7.75\ \text{g/mL}$ , what is the mass?

a)

$72.2\ \text{g}$

b)

$80.6\ \text{g}$

c)

$88.0\ \text{g}$

d)

$104.0\ \text{g}$

35.

Given mass $=598\ \text{g}$ and density $=1.04\ \text{g/mL}$ , what is the volume?

a)

$556\ \text{mL}$

b)

$570\ \text{mL}$

c)

$575\ \text{mL}$

d)

$598\ \text{mL}$

36.

A property that can be measured or observed without matter changing to an entirely different substance is called what?

a)

A physical property

b)

A chemical property

c)

A mixture

d)

A reaction

37.

Which of the following are physical properties of matter? Select all that apply.

a)

Density

b)

Color

c)

Volume

d)

Reactivity

e)

Flammability

38.

To see if a substance is sugar or salt, we can dissolve it in alcohol. The ability of a substance to dissolve is known as what?

a)

Solubility

b)

Electrical conductivity

c)

Density

d)

Malleability

39.

What is a characteristic of matter that can be observed as it changes to a different type of matter?

a)

A chemical property

b)

A physical property

c)

An extensive property

d)

A mixture

40.

Which of the following are chemical properties of matter? Select all that apply.

a)

Flammability

b)

Reactivity with acids

c)

Ability to rust

d)

Density

e)

Color

41.

Rust forms when iron is exposed to water and oxygen during what process?

a)

Oxidation

b)

Melting

c)

Evaporation

d)

Condensation

42.

What is the ability of matter to combine chemically with other substances known as?

a)

Reactivity

b)

Conductivity

c)

Solubility

d)

Malleability

43.

What are the building blocks of matter?

a)

atoms

b)

molecules

c)

compounds

d)

elements

44.

All atoms of the same element can have different numbers of what?

a)

protons

b)

neutrons

c)

electrons

d)

nuclei

45.

Which subatomic particles make up an atom? Select all that apply.

a)

protons

b)

neutrons

c)

electrons

d)

photons

46.

Which subatomic particles are in the nucleus of an atom? Select all that apply.

a)

protons

b)

neutrons

c)

electrons

d)

positrons

47.

What charge does a proton have?

a)

positive

b)

negative

c)

neutral

48.

What charge does a neutron have?

a)

positive

b)

negative

c)

neutral

49.

What charge does an electron have?

a)

positive

b)

negative

c)

neutral

50.

What does the atomic number tell us?

a)

number of protons

b)

number of neutrons

c)

total electrons

d)

number of valence electrons

51.

What does the atomic mass tell us?

a)

number of protons

b)

number of neutrons

c)

total of protons and neutrons

d)

electrons plus protons

52.

How many neutrons are in Carbon-14? (14 is the atomic mass. 6 is the atomic number.)

a)

6

b)

8

c)

14

d)

20

53.

What is an atom that has a positive or negative charge because it has unequal numbers of protons and electrons?

a)

isotope

b)

ion

c)

molecule

d)

element

54.

What are atoms of the same element that differ in their numbers of neutrons called?

a)

ions

b)

isotopes

c)

molecules

d)

allotropes

55.

What do we call a negatively charged ion?

a)

cation

b)

anion

c)

isotope

d)

neutral atom

56.

What is a pure substance that cannot be separated into any other substances?

a)

mixture

b)

compound

c)

element

d)

solution

57.

An element is represented by how many capital letter(s)?

a)

one capital letter

b)

multiple capital letters

c)

lowercase letters only

d)

a symbol with a number but no letters

58.

A compound is represented by how many capital letter(s)?

a)

one capital letter

b)

multiple capital letters

c)

a single lowercase letter

d)

a single number

59.

Which of the following are examples of elements? Select all that apply.

a)

oxygen

b)

water

c)

sodium

d)

iron

e)

carbon dioxide

60.

What is the most common element in the universe?

a)

oxygen

b)

hydrogen

c)

carbon

d)

helium

61.

Which are properties of metals? Select all that apply.

a)

good conductors of heat and electricity

b)

typically malleable and ductile

c)

tend to be brittle

d)

often have luster

62.

Which are properties of metalloids? Select all that apply.

a)

have properties of both metals and nonmetals

b)

act as semiconductors

c)

generally very reactive metals

d)

usually gases at room temperature

63.

Which are properties of nonmetals? Select all that apply.

a)

poor conductors of heat and electricity

b)

brittle when solid

c)

dull appearance

d)

malleable and ductile

64.

What are unique substances that form when two or more elements combine chemically?

a)

mixtures

b)

solutions

c)

compounds

d)

alloys

65.

The properties of a compound can be which of the following compared to the properties of the elements that form them?

a)

different from

b)

the same as

c)

identical and unchanged

d)

unpredictable only

66.

What elements make up the compound $H_2O$ ?

a)

hydrogen and oxygen

b)

hydrogen and nitrogen

c)

oxygen and carbon

d)

carbon and hydrogen

67.

How much carbon, hydrogen, and oxygen are in the compound $C_6H_{12}O_6$ ?

a)

6 carbon, 12 hydrogen, 6 oxygen

b)

1 carbon, 2 hydrogen, 1 oxygen

c)

12 carbon, 6 hydrogen, 6 oxygen

d)

6 carbon, 6 hydrogen, 12 oxygen

68.

Label A in the atom diagram: Identify what the label A points to in the pictured atom.

a)

Electron

b)

Proton

c)

Neutron

d)

Nucleus

69.

Label B in the atom diagram: Identify what the label B points to in the pictured atom.

a)

Energy level (electron shell)

b)

Electron

c)

Proton

d)

Neutron

70.

Label C in the atom diagram: Identify what the label C points to in the pictured atom.

a)

Neutron

b)

Electron

c)

Proton

d)

Nucleus

71.

Label D in the atom diagram: Identify what the label D points to in the pictured atom.

a)

Proton

b)

Electron

c)

Neutron

d)

Energy level (shell)

72.

Label E in the atom diagram: Identify what the bracket E represents in the pictured atom.

a)

Electron cloud (all energy levels)

b)

Single proton

c)

Single energy level only

d)

Nucleus only

73.

What are the electrons in the outermost energy level of an atom known as?

a)

Valence electrons

b)

Core electrons

c)

Protons

d)

Nuclear electrons

74.

Which rule states that atoms tend to want 8 valence electrons in their outer shell to be stable?

a)

Octet rule

b)

Pauli exclusion principle

c)

Law of conservation of mass

d)

Heisenberg uncertainty principle

75.

What determines the chemical behaviors of atoms?

a)

Protons

b)

Neutrons

c)

Valence electrons

d)

Atomic mass

76.

Why are noble gases in group 18 of the periodic table very unreactive?

a)

They have full outer electron shells

b)

They contain no protons

c)

They have unstable nuclei

d)

They share electrons easily

77.

Which element in group 18 only has 2 valence electrons?

a)

Helium

b)

Neon

c)

Argon

d)

Krypton

78.

For oxygen (O), how many valence electrons should be shown in its electron dot diagram?

a)

6

b)

2

c)

4

d)

8

79.

For boron (B), how many valence electrons should be shown in its electron dot diagram?

a)

3

b)

2

c)

5

d)

7

80.

For chlorine (Cl), how many valence electrons should be shown in its electron dot diagram?

a)

7

b)

5

c)

6

d)

8

81.

For argon (Ar), how many valence electrons should be shown in its electron dot diagram?

a)

8

b)

6

c)

4

d)

2

82.

For beryllium (Be), how many valence electrons should be shown in its electron dot diagram?

a)

2

b)

3

c)

4

d)

6

83.

Rubidium (Rb) contains 1 valence electron.

a)

True

b)

False

84.

Tin (Sn) contains 4 valence electrons.

a)

True

b)

False

85.

Xenon (Xe) contains 8 valence electrons.

a)

True

b)

False

86.

Helium (He) has 8 valence electrons.

a)

True

b)

False

87.

All elements in the same group (column) have the same number of what?

a)

Valence electrons

b)

Protons

c)

Neutrons

d)

Energy levels

88.

What is a force of attraction between atoms or ions called?

a)

Chemical bond

b)

Electric field

c)

Magnetic force

d)

Nuclear force

89.

What is the bond between metals and nonmetals that holds together oppositely charged ions called?

a)

Ionic bond

b)

Covalent bond

c)

Metallic bond

d)

Hydrogen bond

90.

How many electrons typically make a full outer shell for most atoms?

a)

8

b)

2

c)

10

d)

12

91.

Classify the bonding in NaCl.

a)

Ionic

b)

Covalent

c)

Metallic

d)

Hydrogen

92.

Classify the bonding in FeAu.

a)

Metallic

b)

Ionic

c)

Covalent

d)

Hydrogen

93.

Classify the bonding in CO.

a)

Covalent

b)

Ionic

c)

Metallic

d)

Hydrogen

94.

In ionic compounds, which types of elements become cations?

a)

Metals

b)

Nonmetals

c)

Metalloids

d)

Noble gases

95.

Why do metals tend to lose valence electrons?

a)

To achieve a stable full outer shell

b)

Because electrons repel the nucleus completely

c)

To decrease their number of protons

d)

To become nonmetals

96.

In ionic compounds, which types of elements become anions?

a)

Nonmetals

b)

Metals

c)

Noble gases

d)

Metalloids

97.

Why do nonmetals tend to gain valence electrons?

a)

To achieve a stable full outer shell

b)

To increase atomic mass

c)

To lose energy levels

d)

To become metals

98.

Complete the statement about ionic bonds: Ionic bonds ______ electrons.

a)

transfer

b)

share

c)

split evenly

d)

create new protons from

99.

Complete the statement about covalent bonds: Covalent bonds ______ electrons.

a)

share

b)

transfer

c)

destroy

d)

repel

100.

What is the term for a covalent bond where electrons are not shared equally between two atoms?

a)

Polar covalent bond

b)

Nonpolar covalent bond

c)

Ionic bond

d)

Metallic bond

101.

What is the term for a covalent bond where valence electrons are shared equally between two atoms?

a)

Nonpolar covalent bond

b)

Polar covalent bond

c)

Ionic bond

d)

Metallic bond

102.

Up to how many covalent bonds can nitrogen form?

a)

3

b)

2

c)

4

d)

1

103.

Identify the properties of covalent compounds.

a)

Low melting and boiling points

b)

Poor electrical conductivity

c)

Often gases or liquids at room temperature

d)

Form molecules with definite shapes

e)

Conduct electricity when dissolved in water

104.

Identify the properties of ionic compounds.

a)

High melting and boiling points

b)

Conduct electricity when molten or dissolved

c)

Form crystal lattices

d)

Often gases at room temperature

e)

Do not conduct electricity in any state

Study Guide (8th Grade Science Winter Exam) — Unit 1 and Unit 2

Total questions: 104

Worksheet time: 52mins

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