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Chemistry Review Packet 2nd 9Wks 2025

Total questions: 105

Worksheet time: 3600secs

Name
Class
Date
1.

Identify how many valence electrons Br has.

a)

5

b)

7

c)

6

d)

8

2.

Select the atom with 2 valence electrons:

a)

Mg

b)

N

c)

Na

d)

Cl

3.

Write the electron configuration for Ca.

a)

1s2 2s2 2p6 3s2 3p6 4s2

b)

1s2 2s2 2p6 3s2 3p6 3d2

c)

1s2 2s2 2p6 3s2 3p6 4p2

d)

1s2 2s2 2p6 3s2 3p6 3d10

4.

Write the electron configuration for S.

a)

1s2 2s2 2p6 3s2 3p4

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p6 3s2 3p2

d)

1s2 2s2 2p6 3s2 3p3

5.

Write the electron configuration for Mn (do not use shorthand).

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d5

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d6

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d4

d)

1s2 2s2 2p6 3s2 3p6 4s1 3d6

6.

Which element has a full outer shell?

a)

Ne

b)

O

c)

Na

d)

F

7.

Identify the group number of the halogens.

a)

Group 17

b)

Group 2

c)

Group 7

d)

Group 18

8.

Identify the group number for the noble gases.

a)

Group 18

b)

Group 1

c)

Group 7

d)

Group 2

9.

Which atom is larger?

a)

K (Potassium)

b)

Ca (Calcium)

10.

Which atom is smaller?

a)

O

b)

S

11.

Which element has the highest electronegativity?

a)

F

b)

N

c)

C

d)

Li

12.

Noble gases have low electronegativity because:

a)

They have a complete valence electron shell and do not need to attract more electrons.

b)

They have a high tendency to lose electrons.

c)

They have a strong attraction for electrons.

d)

They have an incomplete valence shell.

13.

An isotope is defined as:

a)

Atoms of the same element with different numbers of neutrons.

b)

Atoms of different elements with the same number of protons.

c)

Atoms of the same element with the same number of neutrons.

d)

Atoms of different elements with different numbers of electrons.

14.

Which particle changes when an isotope is formed?

a)

proton

b)

neutron

c)

electron

15.

Which particle determines the identity of an atom?

a)

Proton

b)

Neutron

c)

Electron

d)

Photon

16.

Name the compound: CoCl2.

a)

Cobalt(II) chloride

b)

Cobalt(I) chloride

c)

Cobalt(III) chloride

d)

Copper(II) chloride

17.

Name the compound: Fe2O3.

a)

Iron(III) oxide

b)

Iron(II) oxide

c)

Ferric chloride

d)

Iron(III) sulfate

18.

Name the compound: NaClO3.

a)

Sodium chlorate

b)

Sodium chloride

c)

Sodium chlorite

d)

Sodium hypochlorite

19.

Name the compound: NaClO2.

a)

Sodium chlorite

b)

Sodium hypochlorite

c)

Sodium chloride

d)

Sodium chlorate

20.

Write the formula for magnesium phosphate.

a)

Mg₃(PO₄)₂

b)

MgPO₄

c)

Mg₂(PO₄)₃

d)

Mg₃PO₄

21.

Write the formula for calcium hydroxide.

a)

Ca(OH)2

b)

CaO

c)

CaCO3

d)

CaSO4

22.

26. Select the correct Lewis structure for CO₂.

a)

O=C=O with no lone pairs on carbon and two lone pairs on each oxygen atom

b)

O–C≡O with one lone pair on carbon and three lone pairs on each oxygen atom

c)

O≡C–O with two lone pairs on carbon and two lone pairs on each oxygen atom

d)

O–C–O with three lone pairs on each oxygen atom and one lone pair on carbon

23.

Identify whether CO₂ is polar or nonpolar.

a)

Nonpolar

b)

Polar

c)

Ionic

d)

Amphiprotic

24.

Identify whether H₂O is polar or nonpolar.

a)

Polar

b)

Nonpolar

c)

Ionic

d)

Metallic

25.

Identify whether CH₄ is polar or nonpolar.

a)

Nonpolar

b)

Polar

c)

Ionic

d)

Amphiprotic

26.

Identify whether NH₃ is polar or nonpolar.

a)

Polar

b)

Nonpolar

c)

Ionic

d)

Metallic

27.

Which of the following molecules is tetrahedral?

a)

CH₄

b)

H₂O

c)

NH₃

d)

CO₂

28.

Which of the following molecules is bent?

a)

CH₄

b)

CO₂

c)

H₂O

d)

NH₃

29.

Which molecule has a trigonal pyramidal shape?

a)

NH₃

b)

CO₂

c)

BF₃

d)

CH₄

30.

35. Metals conduct electricity well because ______.

a)

they have free-moving electrons

b)

they have tightly bound electrons

c)

they have a high melting point

d)

they are shiny

31.

36. Ionic compounds conduct electricity when ______.

a)

dissolved in water or molten

b)

in solid state

c)

kept dry

d)

mixed with oil

32.

Covalent compounds generally have ______ melting points.

a)

low

b)

high

c)

variable

d)

extremely high

33.

Which set of elements has similar chemical properties?

a)

Li–Na–K

b)

C–N–O

34.

What pattern did Mendeleev use to organize the elements?

a)

Increasing atomic mass

b)

Decreasing atomic number

c)

Alphabetical order

d)

Increasing density

35.

Determine whether the bond in HCl is ionic or covalent.

a)

Covalent

b)

Ionic

c)

Metallic

d)

Hydrogen

36.

How many valence electrons does Al have?

a)

3 valence electrons.

b)

1 valence electron.

c)

5 valence electrons.

d)

7 valence electrons.

37.

How many valence electrons does Cl have?

a)

7 valence electrons.

b)

5 valence electrons.

c)

8 valence electrons.

d)

6 valence electrons.

38.

How many valence electrons does S have?

a)

6 valence electrons.

b)

4 valence electrons.

c)

2 valence electrons.

d)

8 valence electrons.

39.

How many valence electrons does Br have?

a)

7 valence electrons.

b)

5 valence electrons.

c)

2 valence electrons.

d)

8 valence electrons.

40.

What is the symbol for magnesium?

a)

Mg

b)

Mn

c)

Ma

d)

MgO

41.

What is the electron configuration of Ca?

a)

1s² 2s² 2p⁶ 3s² 3p⁶ 4s²

b)

1s² 2s² 2p⁶ 3s² 3p⁶ 3d²

c)

1s² 2s² 2p⁶ 3s² 3p⁶ 4p²

d)

1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹ 4s¹

42.

What is the electron configuration of S?

a)

1s² 2s² 2p⁶ 3s² 3p⁴.

b)

1s² 2s² 2p⁶ 3s² 3p⁶.

c)

1s² 2s² 2p⁶ 3s² 3p².

d)

1s² 2s² 2p⁶ 3s² 3p⁵.

43.

What is the electron configuration of Mn?

a)

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁵.

b)

1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁶ 4s¹.

c)

1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁶.

d)

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁶.

44.

What is the symbol for neon?

a)

Ne

b)

No

c)

Na

d)

Ni

45.

To which group does chlorine belong?

a)

Group 17.

b)

Group 1.

c)

Group 2.

d)

Group 18.

46.

To which group does argon belong?

a)

Group 18.

b)

Group 1.

c)

Group 2.

d)

Group 17.

47.

Which is larger: K or Na?

a)

K is larger.

b)

Na is larger.

c)

Both are the same size.

d)

Neither is larger.

48.

Which is smaller: O or S?

a)

O is smaller.

b)

S is smaller.

c)

Both are the same size.

d)

Cannot be determined.

49.

True or False:

a)

F.

b)

T.

c)

Maybe.

d)

Not sure.

50.

Why are noble gases unreactive?

a)

Their valence shell is full.

b)

They have a high melting point.

c)

They are metals.

d)

They have unstable nuclei.

51.

What are isotopes?

a)

Isotopes are atoms of the same element with different numbers of neutrons.

b)

Isotopes are atoms of different elements with the same number of neutrons.

c)

Isotopes are molecules with different numbers of electrons.

d)

Isotopes are atoms of the same element with different numbers of protons.

52.

Which subatomic particles differ in isotopes of the same element?

a)

Neutrons.

b)

Protons.

c)

Electrons.

d)

Quarks.

53.

Which subatomic particles determine the atomic number?

a)

Protons.

b)

Neutrons.

c)

Electrons.

d)

Quarks.

54.

What is the name of CoCl₂?

a)

Cobalt(II) chloride.

b)

Copper(II) chloride.

c)

Cobalt(I) chloride.

d)

Calcium chloride.

55.

What is the name of Fe₂O₃?

a)

Iron(III) oxide.

b)

Iron(II) oxide.

c)

Ferric chloride.

d)

Ferrous sulfate.

56.

What is the name of NaClO₂?

a)

Sodium chlorite.

b)

Sodium hypochlorite.

c)

Sodium chloride.

d)

Sodium chlorate.

57.

Fill in the blank: The chemical compound for sodium perchlorate is _______.

a)

NaClO4

b)

NaCl

c)

Na2SO4

d)

NaNO3

58.

Fill in the blank: The chemical formula for magnesium phosphate is _______.

a)

Mg₃(PO₄)₂.

b)

MgPO₄

c)

Mg₂(PO₄)₃

d)

Mg₃PO₄

59.

Fill in the blank: The chemical formula for calcium hydroxide is _______.

a)

Ca(OH)₂.

b)

CaCO₃.

c)

CaO.

d)

CaSO₄.

60.

Fill in the blank: The Lewis structure for carbon dioxide is _______.

a)

O = C = O (two lone pairs on each O).

b)

O - C ≡ O (three lone pairs on each O).

c)

O ≡ C - O (one lone pair on each O).

d)

O = C = O (no lone pairs on O atoms).

61.

Fill in the blank: The number of hydrogen bonds and lone pairs in NH₃ is _______.

a)

3 H bonds + 1 lone pair.

b)

2 H bonds + 2 lone pairs.

c)

4 H bonds + 0 lone pairs.

d)

1 H bond + 3 lone pairs.

62.

Fill in the blank: The polarity of CO₂ is _______.

a)

nonpolar.

b)

polar.

c)

ionic.

d)

amphiprotic.

63.

Fill in the blank: The polarity of H₂O is _______.

a)

polar.

b)

nonpolar.

c)

ionic.

d)

metallic.

64.

Fill in the blank: The polarity of CH₄ is _______.

a)

nonpolar.

b)

polar.

c)

ionic.

d)

amphiprotic.

65.

Fill in the blank: The polarity of NH₃ is _______.

a)

polar.

b)

nonpolar.

c)

ionic.

d)

neutral.

66.

Fill in the blank: The chemical formula for methane is _______.

a)

CH₄.

b)

C₂H₆.

c)

CO₂.

d)

CH₃OH.

67.

Fill in the blank: The chemical formula for water is _______.

a)

H₂O.

b)

CO₂.

c)

O₂.

d)

H₂SO₄.

68.

Fill in the blank: The chemical formula for ammonia is _______.

a)

NH₃.

b)

NH₂.

c)

NO₂.

d)

CH₄.

69.

Fill in the blank: Metals conduct electricity because _______.

a)

electrons move freely.

b)

protons are stationary.

c)

atoms are tightly packed.

d)

metals are shiny.

70.

Fill in the blank: Ionic compounds conduct electricity _______.

a)

when melted or dissolved in water.

b)

when in solid state.

c)

when exposed to air.

d)

when mixed with oil.

71.

Fill in the blank: Covalent compounds have _______ melting points.

a)

low melting points.

b)

high melting points.

c)

variable melting points.

d)

no melting points.

72.

Fill in the blank: The alkali metals in order are _______.

a)

Li–Na–K.

b)

Na–K–Li.

c)

K–Li–Na.

d)

Na–Li–K.

73.

Fill in the blank: The periodic table shows _______.

a)

patterns in properties/valence electrons.

b)

the number of neutrons in each atom.

c)

the melting points of all elements.

d)

the atomic mass of compounds.

74.

Fill in the blank: The type of bond formed by sharing electrons is _______.

a)

covalent.

b)

ionic.

c)

metallic.

d)

hydrogen.

75.

Select the correct Lewis dot structure for Al.

a)

Al with three dots around it

b)

Al with one dot around it

c)

Al with five dots around it

d)

Al with seven dots around it

76.

2. Select the correct Lewis dot structure for Cl.

a)

Cl with 7 dots around it

b)

Cl with 8 dots around it

c)

Cl with 6 dots around it

d)

Cl with 5 dots around it

77.

3. Select the correct Lewis dot structure for S.

a)

S: ••••••

b)

S: •••••

c)

S: •••••••

d)

S: ••••

78.

Identify how many valence electrons Br has.

a)

5

b)

7

c)

6

d)

8

79.

Select the atom with 2 valence electrons:

a)

Mg

b)

N

c)

Na

d)

Cl

80.

6. Write the electron configuration for Ca.

a)

1s2 2s2 2p6 3s2 3p6 4s2

b)

1s2 2s2 2p6 3s2 3p6 3d2

c)

1s2 2s2 2p6 3s2 3p6 4p2

d)

1s2 2s2 2p6 3s2 3p6 3d10

81.

Write the electron configuration for S.

a)

1s2 2s2 2p6 3s2 3p4

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p6 3s2 3p2

d)

1s2 2s2 2p6 3s2 3p3

82.

8. Write the electron configuration for Mn (do not use shorthand).

a)

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁵

b)

1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁶

c)

1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁶

d)

1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁵

83.

Which element has a full outer shell?

a)

Ne

b)

O

c)

Na

d)

F

84.

10. Identify the group number of the halogens.

a)

Group 17

b)

Group 7

c)

Group 2

d)

Group 18

85.

11. Identify the group number of the noble gases.

a)

Group 18

b)

Group 1

c)

Group 7

d)

Group 2

86.

Which atom is larger?

a)

K (Potassium)

b)

Ca (Calcium)

87.

Which atom is smaller: O or S?

a)

O

b)

S

88.

Which element has the highest electronegativity?

a)

F

b)

N

c)

C

d)

Li

89.

15. Noble gases have low electronegativity because:

a)

they have a complete valence shell and do not need to attract more electrons

b)

they have a high tendency to lose electrons

c)

they have a small atomic radius

d)

they are highly reactive

90.

An isotope is defined as:

a)

Atoms of the same element with different numbers of neutrons.

b)

Atoms of different elements with the same number of protons.

c)

Atoms of the same element with identical atomic masses.

d)

Atoms of different elements with different numbers of electrons.

91.

Set up the average atomic mass problem for two isotopes with masses 20 amu (75%) and 22 amu (25%).

a)

Average atomic mass = (0.75 × 20 amu) + (0.25 × 22 amu)

b)

Average atomic mass = (0.25 × 20 amu) + (0.75 × 22 amu)

c)

Average atomic mass = (0.50 × 20 amu) + (0.50 × 22 amu)

d)

Average atomic mass = (0.75 × 22 amu) + (0.25 × 20 amu)

92.

Which particle changes when you form an isotope?

a)

proton

b)

neutron

c)

electron

93.

19. Which particle determines the identity of an atom?

a)

Proton

b)

Neutron

c)

Electron

d)

Photon

94.

Name the compound: CoCl₂.

a)

Cobalt(II) chloride

b)

Cobalt(I) chloride

c)

Cobalt(III) chloride

d)

Copper(II) chloride

95.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the there should only be 1 orbital in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
96.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
97.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
98.
This is the correct dot diagram for nitrogen (N)
a)
true
b)
false
99.
This could be the dot diagram of
a)
Mg
b)
Cl
c)
C
d)
O
100.
This could be the dot diagram of
a)
O
b)
B
c)
Li
d)
Ne
101.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
102.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
103.

What is the orbital notation for oxygen?

a)

↑↓|↑↓|↑_↑_|_

b)

↑↓|↑↓|↑↑|_

c)

↑↓|↑_|↑_|↑_

d)

↑↓|↑↓|↑↓|_

104.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
105.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon

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