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Quarter 2 Exam Review

Total questions: 98

Worksheet time: 1hrs 17mins

Name
Class
Date
1.

Which of the following best describes a physical change?

a)

A substance changes its chemical composition

b)

A substance maintains its chemical identity but changes in size or shape

c)

Two substances combine to form a new compound

d)

A substance undergoes irreversible transformation

2.

In the International System of Units (SI), what is the base unit for temperature?

a)

Celsius

b)

Fahrenheit

c)

Kelvin

d)

Centigrade

3.

How many significant figures are in the number 0.00304?

a)

5

b)

3

c)

2

d)

4

4.

What is the difference between accuracy and precision?

a)

Accuracy means getting consistent results, while precision means getting correct results

b)

Accuracy means getting correct results, while precision means getting consistent results

c)

Accuracy and precision mean the same thing

d)

Neither accuracy nor precision matter in scientific measurements

5.

When performing dimensional analysis, which of the following is a key principle?

a)

Always round to the nearest whole number

b)

Units must cancel out to reach the desired unit

c)

Decimals should be avoided

d)

Only metric units can be converted

6.

In the measurement 150.0 mL, how many significant figures are present?

a)

3

b)

4

c)

2

d)

1

7.

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

a)

The volume of a substance

b)

The shape of a substance

c)

The ability of a substance to react with oxygen

d)

The mass of a substance

8.

Which of the following is an example of a homogeneous mixture?

a)

Soil

b)

Salt water

c)

Granite

d)

Trail mix

9.

What is the primary purpose of significant figures?

a)

To make calculations more difficult

b)

To indicate the precision of a measurement

c)

To round numbers to whole values

d)

To eliminate decimal places

10.

Which of the following represents a chemical change?

a)

Ice melting

b)

Paper being torn

c)

Milk souring

d)

Sugar dissolving in water

11.

What type of data describes observations without numbers?

a)

Quantitative data

b)

Statistical data

c)

Qualitative data

d)

Numerical data

12.

In a scientific experiment, what is the dependent variable?

a)

The factor that the scientist changes on purpose

b)

The factor that stays constant throughout the experiment

c)

The factor that is measured as a result of the changes made

d)

The factor that isn't related to the experiment

13.

What is the primary purpose of dimensional analysis?

a)

To measure dimensions of objects

b)

To convert between different units

c)

To calculate density

d)

To determine significant figures

14.

A student's measurements are consistently close together but far from the actual value. This describes:

a)

High accuracy, low precision

b)

Low accuracy, high precision

c)

High accuracy, high precision

d)

Low accuracy, low precision

15.

Which safety equipment is essential when handling chemicals in the lab?

a)

Lab coat only

b)

Safety goggles only

c)

Gloves only

d)

All of the above

16.

What is the difference between mass and weight?

a)

They are the same thing

b)

Mass varies with gravity while weight remains constant

c)

Weight varies with gravity while mass remains constant

d)

Neither varies with gravity

17.

What is the main purpose of a control group in an experiment?

a)

To change multiple variables at once

b)

To provide a standard or base for comparing experimental groups

c)

To collect qualitative data only

d)

To speed up the experiment process

18.

What is the "sandwich rule" for significant figures?

a)

All zeros at the beginning of a number are significant

b)

All zeros between non-zero digits are significant

c)

All zeros at the end of a number are significant

d)

No zeros are ever significant

19.

According to the Law of Conservation of Mass, during a chemical change:

a)

Mass is always converted to energy

b)

The total mass of products equals the total mass of reactants

c)

Some mass is always lost to the environment

d)

The mass of products is always greater than reactants

20.

Which of the following is pure substance?

a)

Distilled Water

b)

Milk

c)

Soup with vegetables

d)

Tea with honey

21.

A student wants to investigate how different amounts of fertilizer affect plant growth. They set up an experiment with 5 tomato plants of the same species. Each plant receives different amounts of fertilizer (0g, 5g, 10g, 15g, and 20g), and the student measures the height of each plant every week for 8 weeks. All plants receive the same amount of water and sunlight, and are kept at the same temperature. Identify the independent variable in this experiment and explain why it is the independent variable.

4 lines
22.

You are going on a trip with your friends again! You want to drive 1,000 kilometers in a car that gets 10 miles per gallon. Gas costs $4.30 per gallon. There are 1.6 kilometers per mile. How much will you spend on gas? Show all your work for full credit, and circle your final answer.

4 lines
23.

What is the currently accepted model of atomic structure?

a)

Bohr's planetary model

b)

Thomson's plum pudding model

c)

Quantum mechanical model

d)

Rutherford's nuclear model

24.

What does the mass of an element represent?

a)

Protons only

b)

Electrons and protons only

c)

Protons and neutrons only

d)

Electrons only

25.

How many electrons can occupy a p sublevel?

a)

2 electrons

b)

6 electrons

c)

10 electrons

d)

14 electrons

26.

How does energy move in the electromagnetic spectrum?

a)

Waves

b)

Sounds

c)

Through solids only

d)

As a liquid

27.

What happens when an electron returns to its ground state from an excited state?

a)

It absorbs energy

b)

It emits energy

c)

Nothing happens

d)

It changes to a proton

28.

Which scientist's gold foil experiment led to the discovery of the nucleus?

a)

J.J. Thomson

b)

Ernest Rutherford

c)

Niels Bohr

d)

James Chadwick

29.

What does the atomic number of an element represent?

a)

Number of neutrons

b)

Number of protons

c)

Number of electrons

d)

Mass number

30.

In noble gas notation, which noble gas would be used for elements in period 4 for their electron configurations?

a)

Neon [Ne]

b)

Helium [He]

c)

Argon [Ar]

d)

Krypton [Kr]

31.

What is the maximum number of electrons that can occupy an s orbital?

a)

6 electrons

b)

2 electrons

c)

10 electrons

d)

14 electrons

32.

Boron and carbon have the SAME emission spectrum.

a)

True

b)

False

33.

How many electrons does Carbon (C) have?

a)

5

b)

6

c)

7

d)

12

34.

Which color of visible light has the longest wavelength?

a)

Violet

b)

Green

c)

Red

d)

Blue

35.

What happens when the number of protons in an atom changes?

a)

It becomes an isotope

b)

It becomes an ion

c)

It becomes a different element

d)

Nothing changes

36.

What happens when the number of electrons in an atom changes?

a)

It becomes an isotope

b)

It becomes an ion

c)

It becomes a different element

d)

Nothing changes

37.

Which scientist discovered the electron orbits the nucleus in levels?

a)

Ernest Rutherford

b)

J.J. Thomson

c)

Robert Millikan

d)

Niels Bohr

38.

What element is this: 1s22s22p51s^22s^22p^5

a)

Carbon

b)

Nitrogen

c)

Oxygen

d)

Flourine

39.

Which scientist discovered the electron?

a)

Ernest Rutherford

b)

J.J. Thomson

c)

Robert Millikan

d)

Niels Bohr

40.

What happens to electron energy levels as they move AWAY from the nucleus?

a)

They become more stable

b)

They decrease in energy

c)

They increase in energy

d)

They remain the same

41.

What is the electron configuration of a neutral carbon atom?

a)

1s22p31s^22p^3

b)

1s22s22p11s^22s^22p^1

c)

1s22s22p21s^22s^22p^2

d)

1s22s22p41s^22s^22p^4

42.

Which color of visible light has the highest frequency?

a)

Red

b)

Green

c)

Blue

d)

Violet

43.

When an electron absorbs energy, what happens to it?

a)

It moves to a lower energy level

b)

It moves to a higher energy level

c)

It becomes a super atom

d)

It leaves the atom completely

44.

What is the noble gas used in electron configuration for an element in period 3?

a)

[Kr]

b)

[Xe]

c)

[Ne]

d)

[He]

45.

Short Answer 1: List the three subatomic particles and their respective charges.

4 lines
46.

Short Answer 2: Tell me the number of electrons, protons, and neutrons in Cu2+Cu^{2+} . Protons → Electrons → Neutrons →

4 lines
47.

Short Answer 3: Tell me TWO key things about J.J. Thompson's Plum Pudding Model and draw a sketch of it.

4 lines
48.

Short Answer 4: Write the electron configuration for Sodium (Na) without the noble gas AND with the noble gas. Without the noble gas → With the noble gas →

4 lines
49.

Who is credited as the "Father of the Periodic Table" for arranging elements by atomic weight and leaving gaps for undiscovered elements?

a)

John Newlands

b)

Henry Moseley

c)

Dmitri Mendeleev

d)

Glenn Seaborg

50.

What is the term for a negatively charged ion formed when an atom gains electrons?

a)

Cation

b)

Proton

c)

Neutron

d)

Anion

51.

How many valence electrons do elements in Group 1 (alkali metals) have?

a)

1

b)

2

c)

3

d)

8

52.

Which trend is observed in atomic radius as you move from left to right across a period?

a)

Remains constant

b)

Increases gradually

c)

Decreases

d)

Fluctuates randomly

53.

What is the maximum number of electrons that can occupy the p sublevel?

a)

Two

b)

Ten

c)

Six

d)

Four

54.

Why are noble gases generally unreactive?

a)

They have incomplete outer shells

b)

They have a full outer shell of electrons

c)

They lack electrons

d)

They have too many protons

55.

Which group contains the most reactive nonmetals?

a)

Noble gases

b)

Alkali metals

c)

Halogens

d)

Alkaline earth metals

56.

What happens to the atomic radius as you move down a group?

a)

Decreases

b)

Stays the same

c)

Increases

d)

Alternates between increasing and decreasing

57.

What is the term for elements that have properties of both metals and nonmetals?

a)

Transition metals

b)

Noble gases

c)

Metalloids

d)

Halogens

58.

How many valence electrons do noble gases typically have?

a)

Six

b)

Four

c)

Two

d)

Eight

59.

What characteristic is shared by all transition metals?

a)

They have partially filled d orbitals

b)

They are all gases at room temperature

c)

They have eight valence electrons

d)

They are all radioactive

60.

Which block of elements contains the lanthanides and actinides?

a)

s-block

b)

p-block

c)

d-block

d)

f-block

61.

Which element would have the largest atomic radius?

a)

Lithium

b)

Carbon

c)

Fluorine

d)

Beryllium

62.

What is the maximum number of electrons that can occupy the s sublevel?

a)

Six

b)

Two

c)

Four

d)

Eight

63.

Which group of elements is known for being good conductors of heat and electricity?

a)

Nonmetals

b)

Noble gases

c)

Metals

d)

Metalloids

64.

What is the term for the measure of an atom's ability to attract electrons in a chemical bond?

a)

Ionization energy

b)

Electronegativity

c)

Nuclear charge

d)

Atomic radius

65.

Which element is the MOST electronegative?

a)

Fluorine (F)

b)

Chlorine (Cl)

c)

Bromine (Br)

d)

Iodine (I)

66.

Which statement is true about the shielding effect?

a)

It increases across a period

b)

Inner electrons shield outer electrons from nuclear charge

c)

It only affects noble gases

d)

It decreases down a group

67.

What happens to the size of an atom when it becomes a cation?

a)

Stays the same size

b)

Becomes larger

c)

Becomes smaller

d)

Changes shape but not size

68.

Which group of elements has the highest electronegativity values?

a)

Alkali metals

b)

Noble gases

c)

Halogens

d)

Alkaline earth metals

69.

What is the octet rule?

a)

Elements always share exactly eight electrons

b)

Atoms tend to gain or lose electrons to achieve eight valence electrons

c)

Only eight elements can react at once

d)

Elements must have eight protons to be stable

70.

Describe the trend for electronegativity as you move from left to right on the periodic table. Also describe the trend for atomic mass as you move left to right on the periodic table.

4 lines
71.

Label every group on the periodic table.

4 lines
72.

What is an ionic bond?

a)

Sharing of electrons between atoms

b)

Transfer of electrons from metal to non-metal

c)

Sharing of protons between atoms

d)

Transfer of neutrons from non-metal to metal

73.

Which elements are most likely to form ionic bonds?

4 lines
74.

When a metal atom loses electrons during ionic bonding, it forms a(n)…

a)

Neutral atom

b)

Cation (positive ion)

c)

Anion (negative ion)

d)

Polyatomic ion

75.

When a non-metal atom gains electrons during ionic bonding, it forms a(n)…

a)

Neutral atom

b)

Cation (positive ion)

c)

Anion (negative ion)

d)

Isotope

76.

Where are non-metals found on the periodic table?

a)

Left area

b)

Middle area

c)

Right area

d)

Bottom area

77.

In the formula NaCl, why is Na written first?

a)

Because Na has more electrons than Cl

b)

Because Na is a metal and forms a cation

c)

Because Na has a higher atomic number

d)

Because Na is more electronegative

78.

Which of the following correctly describes the "Criss-Cross-Applesauce" method?

a)

Changing the atomic numbers of the elements

b)

Flipping the charges on the opposite element

c)

Multiplying the charges to get the subscripts

d)

Adding the charges to get the subscripts

79.

What is a polyatomic ion?

a)

An ion with more than one charge

b)

An ion with two or more covalently bonded atoms

c)

An ion that can form multiple types of bonds

d)

An ion found only in transition metals

80.

When writing the formula for an ionic compound, which ion is always written first?

a)

Non-metal

b)

Metal

c)

Polyatomic ion

d)

The ion with the higher charge

81.

What is the correct formula for magnesium hydroxide? Mg has a 2+ charge ( Mg2+Mg^{2+} ) and OH has a -1 charge ( OH−1OH^{-1} ).

a)

MgOH

b)

Mg(OH)

c)

Mg(OH)2

d)

Mg2OH

82.

What is the charge typically formed by elements in Group 1 of the periodic table?

a)

+1

b)

+2

c)

-1

d)

0

83.

What is the charge typically formed by elements in Group 17 of the periodic table?

a)

+1

b)

-2

c)

-1

d)

+2

84.

Why do elements in Group 18 (noble gases) typically not form charged ions?

a)

They have too many protons

b)

They are too reactive

c)

They already have a full valence shell

d)

They have no electrons to lose

85.

Which of the following is the correct name for the compound Al2(SO4)3Al_{2}(SO_{4})_{3} ?

a)

Aluminum sulfide

b)

Aluminum sulfate

c)

Double aluminum trisulfate

d)

Aluminum sulfite

86.

What charge does iron(III) have?

a)

+1

b)

-3

c)

-1

d)

+3

87.

If the bond between sodium and chlorine is greater than 2.0, what type of bond do they form?

a)

Nonpolar covalent bond

b)

Polar covalent bond

c)

Ionic bond

d)

Metallic bond

88.

Which intermolecular force is the strongest?

a)

Dispersion forces

b)

Dipole-dipole interactions

c)

Hydrogen bonding

d)

Ionic bonding

89.

Which one is true about dispersion forces:

a)

Only occur between polar molecules

b)

Occur between all molecules

c)

Only occur between ionic compounds

d)

Only occur between hydrogen-containing compounds

90.

Hydrogen bonds form when hydrogen is bonded to which elements?

a)

Carbon (C), silicon (Si), or germanium (Ge)

b)

Oxygen (O), fluorine (F), or nitrogen (N)

c)

Sodium (Na), potassium (K) or lithium (Li)

d)

Sulfur (S), phosphorus (P), or chlorine (Cl)

91.

Which of the following correctly represents the trend in strength of intermolecular forces from weakest to strongest?

a)

Hydrogen bonding < Dipole-dipole interactions < Van der Waals forces

b)

Van der Waals forces < Dipole-dipole interactions < Hydrogen bonding

c)

Dipole-dipole interactions < Van der Waals forces < Hydrogen bonding

d)

Van der Waals forces < Hydrogen bonding < Dipole-dipole interactions

92.

Carbon (C) has an electronegativity of 2.5 while Hydrogen (H) has an electronegativity of 2.1, so what type of bond would they have when bonded together? Show your work for your answer.

4 lines
93.

How would I write this ionic compound? Include the name and the correct spelling. Show your work for your answer. Al3+O2−Al^{3+}O^{2-}

4 lines
94.

BONUS: Label which type of bond is shown. Use the word bank: Ionic bond, dipole-dipole interaction, hydrogen bond, and dispersion forces (Van der Waals).

a)

Ionic bond

b)

Dipole-dipole interaction

c)

Hydrogen bond

d)

Dispersion forces (Van der Waals)

95.

BONUS: Label which type of bond is shown. Use the word bank: Ionic bond, dipole-dipole interaction, hydrogen bond, and dispersion forces (Van der Waals).

a)

Ionic bond

b)

Dipole-dipole interaction

c)

Hydrogen bond

d)

Dispersion forces (Van der Waals)

96.

BONUS: Label which type of bond is shown. Use the word bank: Ionic bond, dipole-dipole interaction, hydrogen bond, and dispersion forces (Van der Waals).

a)

Ionic bond

b)

Dipole-dipole interaction

c)

Hydrogen bond

d)

Dispersion forces (Van der Waals)

97.

BONUS: Label which type of bond is shown. Use the word bank: Ionic bond, dipole-dipole interaction, hydrogen bond, and dispersion forces (Van der Waals).

a)

Ionic bond

b)

Dipole-dipole interaction

c)

Hydrogen bond

d)

Dispersion forces (Van der Waals)

98.

BONUS: Label which type of bond is shown. Use the word bank: Ionic bond, dipole-dipole interaction, hydrogen bond, and dispersion forces (Van der Waals).

a)

Ionic bond

b)

Dipole-dipole interaction

c)

Hydrogen bond

d)

Dispersion forces (Van der Waals)

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