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Chemistry Fall Final Review

Total questions: 104

Worksheet time: 3hrs 52mins

Name
Class
Date
1.

where are the metaloids found

a)

far left, vertical

b)

stair step/diagonal

c)

far right horizontal

d)

at the bottom

2.

What group number are the halogens found?

a)

18 (8A)

b)

1

c)

2

d)

17 (7A)

3.

What is the name of group number 1?

a)

halogens

b)

noble gases

c)

alkali metals

d)

alkaline earth metals

4.

A grouping of elements based on similar chemical properties, arranged by columns in the periodic table; also known as a group

a)

family

b)

period

c)

row

d)

isotope

5.

A row on the Periodic Table of Elements

a)

family

b)

period

c)

row

d)

isotope

6.
___________ is the only metal that is a liquid at room temperature.
a)
Platinum
b)
Water
c)
Tin
d)
Mercury
7.
__________ would have some characteristics of metals and some characteristics of nonmetals.
a)
Gold
b)
Sodium
c)
Arsenic
d)
Bismuth
8.

Metals (select all that apply)

a)

are found on the right side of the periodic table.

b)

are found on the left side of the periodic table.

c)

are good conductors of heat and electricity.

d)

are brittle.

e)

are malleable and ductile.

9.

Nonmetals (select all that apply)

a)

are found on the right side of the periodic table.

b)

are found on the left side of the periodic table.

c)

are good conductors of heat and electricity.

d)

are brittle.

e)

can be solid, liquids, or gases at room temperature.

10.

Which element is found in group 2, period 6?

a)

Oxygen (O)

b)

Barium (Ba)

c)

Selenium (Se)

d)

Carbon (C)

11.

Which halogen is found in period 4?

a)

Krypton (Kr)

b)

Xenon (Xe)

c)

Bromine (Br)

d)

Iodine (I)

12.

Isotopes of an element have a different number of...

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

13.

Potassium-39 has how many neutrons?

a)

19

b)

18

c)

20

d)

21

14.

Nickel-59 has how many neutrons?

a)

30

b)

31

c)

32

d)

33

15.

76 protons and 114 neutrons

a)

Osmium-114

b)

Osmium-76

c)

Osmium-190

d)

Osmium-190.23

16.

12 protons and 13 neutrons

a)

Mg-12

b)

Mg-13

c)

Mg-25

d)

Mg-24.305

17.

Rubidium has two common isotopes, 85Rb and 87Rb. If the abundance of 85Rb is 72.2% and the abundance of 87Rb is 27.8%, what is the average atomic mass of rubidium?

a)

85.468 amu

b)

37 amu

c)

85.6 amu

d)

86.4 amu

18.

There are two primary isotopes found in any sample of copper: copper-63 and copper-65. The isotope 65Cu composes 69.2% of the sample and 63Cu comprises the other 30.8%. Based on this data, what is the atomic mass of copper?

a)

29 amu

b)

63.546 amu

c)

64.4 amu

d)

63.6 amu

19.

How do you calculate mass number?

a)

Mass x percent

b)

Protons + Electrons

c)

Protons + Neutrons

d)

Neutrons + Protons + Electrons

20.

What is the difference between Neon-20 and Neon-22?

a)

They have different numbers of electrons.

b)

They have different numbers of neutrons.

c)

Only 1 is radioactive.

d)

No difference.

21.

How many neutrons are in this isotope?

a)

20

b)

41

c)

61

d)

21

22.

What is a positive ion called?

a)

anion

b)

cation

c)

isotope

d)

covalent

23.

What is a negative ion called?

a)

anion

b)

cation

c)

covalent

d)

isotope

24.

How many electrons would a Nitrogen ion gain/lose? If it has 5 valence electrons.

a)

lose 5

b)

gain 5

c)

lose 3

d)

gain 3

25.

What is the ion formed from Sulfur? If it has 6 valence electrons.

a)

S+2

b)

S-2

c)

S+6

d)

S-6

26.

How many electrons would a Calcium ion gain/lose? If it has 2 valence electrons.

a)

lose 1

b)

gain 1

c)

lose 2

d)

gain 2

27.

If an atom loses electrons, the charge will be positive.

a)

true

b)

false

28.

An atom with 2 protons, 3 neutrons, and 4 electrons has a charge of ____.

a)

+2

b)

-2

c)

+3

d)

0

29.

Match the following

a)

gain electrons

1.

anions

b)

lose electrons

2.

cations

c)

cations are

3.

positively charged

d)

anions are

4.

negatively charged

e)

atoms are

5.

neutral

30.
Which of the following is chromate?
a)
CrO42-
b)
CrO32-
c)
CrO22-
d)
CrO2-
31.
Identify Cessium Nitrate
a)
CsNO3
b)
Cs2(NO3)3
c)
Cs2NO3
d)
Cs3NO3
32.
Identify chromic acid
a)
Li2CrO4
b)
Na2CrO4
c)
H2CrO4
d)
K2CrO4
33.
What is the name of Al(NO3)3?
a)
Aluminum trinitrate
b)
Monoaluminum nitrate
c)
Aluminum (III) nitrate
d)
Aluminum Nitrate
34.
What is the name of Mg(OH)2?
a)
Magnesium Hydride
b)
Magnesium Dihydride
c)
Magnesium Dihydroxide
d)
Magnesium Hydroxide
35.
What is the name of H3PO4? (This molecule makes the slightly tangy taste in sodas)
a)
Hydrogen Phosphate
b)
Trihydrogen Phosphate
c)
Phosphoric Acid
d)
Triple Hydrogen PhosphoOxoPlutonide!!!
36.

The formula for Copper (1) Sulfide is...

a)

Cu1S2

b)

CuS

c)

Cu1S

d)

Cu2S

37.

The formula for Chromium (III) Selenide is...

a)

Cr2Se3

b)

Cr3Se2

c)

Cr3S

d)

CrS

38.

The formula for Nickel (II) Oxide is...

a)

Ni2O2

b)

NiO2

c)

NiO

d)

Ni2O

39.

The charge on Tin (II) Oxide is...

a)

2+

b)

2-

c)

0

d)

1+

40.

We would name FeF2...

a)

Iron Fluoride

b)

Iron (I) Fluoride

c)

Iron (II) Fluorine

d)

Iron (II) Fluoride

41.

We would name FeSO4...

a)

Iron Sulfate

b)

Iron Sulfite

c)

Iron (II) Sulfate

d)

Iron (II) Sulfite

42.
What is a transition metal?
a)
They are elements that charges vary and are represented by roman numerals during nomenclature.
b)
A type of squirrel.
c)
Elements that are not defined as metals or nonmetals.
d)
A metal with no charge.
43.

What is the name of this ion?

a)

Magnesium (II)

b)

Magnesium (2)

c)

Manganese (II)

d)

Magnesium (+2)

44.

What electron configuration matches an oxygen atom?

a)

1s22s22p63s2, 3p64s23d104p5

b)

1s22s22p4

c)

1s22s22p6

d)

1s22s22p63s23p64s23d1

45.

Identify the Electron Configuration for Aluminum (Al)

a)

1s2 2s2 2p6 3s2 3p1

b)

1s2 2s2 2p6 3s2 3p3

c)

1s2 2s2 2p6 3s2 4p1

46.

An electron orbital is _______

a)

A 3-dimensional space around the nucleus of an atom where electrons and protons exist

b)

A 3-dimensional space around the nucleus of an atom where an electron is most likely exist

c)

An orbit which electrons circle the nucleus like planet circle the Sun

d)

A 3-dimension space where nuclear reactions take place

47.

Chemical reactions involve ________

a)

electrons

b)

protons

c)

neutrons

d)

beta particles

e)

heat

48.

How many electrons are in Radium-226

a)

88

b)

138

c)

226

d)

314

49.

Choose the correct electron configuration for Terbium (Tb).

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d19 5p6 6s2

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f9

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f5

50.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
51.

What does Pauli exclusion principle state ?

a)

states that each electron occupies the lowest energy orbital available

b)

states that -no two electrons in the same orbital can have the same spin

c)

states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals

52.

What is the maximum number of electrons that an S orbital can have?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

53.

How many electrons can the d sublevel(orbital) hold?

a)

8

b)

10

c)

2

d)

4

54.

What is this element?

1s22s22p63s23p64s23d104p6

a)

Argon

b)

Krypton

c)

Selenium

d)

Bromide

55.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
56.

What is the maximum number of electrons that an f orbital can have?

a)

11 electrons

b)

14 electrons

c)

13 electrons

d)

12 electrons

57.

What is the correct electron configuration of silver (Ag)?

a)

[Kr]5s24d9

b)

[Kr]5s14d10

c)

[Kr]5s245d10

d)

[Kr]5s24d10

58.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
59.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
60.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
61.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
62.

What does electronegativity mean?

a)

ability to increase energy levels

b)

ability to react with elements

c)

ability to attract electrons

63.

In the alkali metals, which element has a larger atomic radius?

a)

lithium, Li

b)

sodium, Na

c)

potassium, K

d)

cesium, Cs

64.

In the halogen family, which element is the most electronegative?

a)

iodine, I

b)

fluorine, F

c)

chlorine, Cl

d)

helium, He

65.

Which of the following elements is the most electronegative?

a)

Hydrogen, H

b)

Aluminum, Al

c)

Oxygen, O

d)

Cesium, Cs

66.

What is the correct name for Al2O3?

a)

Aluminum (III) Oxide

b)

Aluminum Oxide

c)

DiAluminum Trioxide

d)

None of the above

67.

Single bonded carbons are called _________.

a)

Alkanes

b)

Alkynes

c)

Alkenes

d)

Arenes

68.

what is the name of CCl4?

a)

carbon tetrachloride

b)

monocarbon tetrachloride

c)

tetracarbon monochloride

d)

carbon chloride

69.

What is the name of the compound P2O5

a)

Pentaphosphorus dioxide

b)

Phoshphide dioxide

c)

Diphosphorus pentoxide

70.
Name the following ionic compound: LiNO3
a)
lithium nitrate
b)
lithium III nitrate
c)
lithium nitride
d)
lithium oxide
71.

Name the compound NH4OH

a)

ammonium hydroxide

b)

ammonia oxyhydride

c)

mononitrogen tetraoxihydride

d)

hydrogen nitrate

72.
The chemical formula for an ionic compound of potassium and oxygen is
a)
KO.
b)
K2O.
c)
K2O2.
d)
KO2.
73.
As4O10
a)
arsenic oxide
b)
quadarsenic decoxide
c)
tetraarsenic decoxide
d)
arsenic decoxide
74.
hydrochloric acid
a)
H(ClO3)
b)
H(ClO2)
c)
HClO
d)
HCl
75.
HI
a)
iodic acid
b)
hydroiodic acid
c)
iodous acid
d)
hypoiodous acid
76.
HC2H3O2
a)
acetate
b)
hydrogen acetate
c)
acetic acid
d)
hydroacetic acid
77.
chromiun(III) chloride
a)
CrCl
b)
CrCl3
c)
Cr3Cl
d)
ClCr3
78.

Which coefficient must go in the missing spot to balance the chemical equation?


___Cu + O2 --> 2Cu2O

a)

4

b)

1

c)

5

d)

3

79.

What type of reaction is below?

CH4 + O2 --> CO2 + H2O

a)

Combination/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

80.

What type of reaction is below?

Cu2O + K --> K2O + Cu

a)

Combination/Synthesis

b)

Decomposition

c)

Double Replacement

d)

Combustion

e)

Single Replacement

81.

What type of reaction is below?

H2O --> H2 + O2

a)

Combination/Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

82.

What type of reaction is below?

Mg(NO3)2 + Na2O --> NaNO3 + MgO

a)

Combination/Synthesis

b)

Single Replacement

c)

Double Replacement

d)

Combustion

83.

Predict the products of this reaction: MgO + Li --> ?

a)

LiO + Mg

b)

MgO + Li

c)

Li2O + Mg

d)

LiMg + O

e)

MgLi + O

84.

Balance the following reaction: ___Na + ___O2 --> ___Na2O

a)

4Na, 2O2, 3Na2O

b)

2Na, 2O2, 3Na2O

c)

4Na, O2, 2Na2O

d)

1Na, O2, 2Na2O

85.
All of the following are physical properties of matter EXCEPT
a)
mass
b)
color
c)
melting point
d)
ability to rust
86.
Which of the following is a chemical property?
a)
color
b)
hardness
c)
freezing point
d)
ability to react with oxygen
87.
What happens to matter during a chemical reaction?
a)
matter is neither destroyed or created
b)
some matter is destroyed
c)
some matter is created
d)
some matter is destroyed and some is created
88.
Potassium hydroxide (KOH)
a)
Soluble 
b)
Insoluble
89.

Identify the precipitate in the reaction:

Pb(NO3)2 + 2NaCl → 2NaNO3 + PbCl2

a)

Pb(NO3)2

b)

NaCl

c)

NaNO3

d)

PbCl2

90.

Identify the precipitate in the reaction:

CdSO4 + K2S → CdS + K2SO4

a)

CdSO4

b)

K2S

c)

CdS

d)

K2SO4

91.

Acetates (CH3COO-) (CH3CO2)

a)

Soluble

b)

Insoluble

92.
What is the VSEPR theory used to predict?
a)
Bond Strength
b)
Polarity
c)
Molecular Shape
d)
Electronegativity
93.
According to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?
a)
Pairs of valence electrons
b)
Inner shell electrons
c)
Mobile Electrons
d)
Electrons closest to the nucleus
94.
What is the measure of a tetrahedral bond angle?
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
95.
Which of the following shapes has unshared pairs of electrons on the central atom? 
a)
Bipyramidal
b)
Bent
c)
Trigonal Planar
d)
Tetrahedral
96.
Which molecule would have this shape?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
97.
What molecule could this be? 
a)
BF3
b)
CH4
c)
H2O
d)
CO2
98.
The bond angle for a trigonal planar molecule is 
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
99.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
100.
Who could this be?
a)
H2O
b)
NH3
c)
CO2
d)
CH4
101.
Will this molecule be polar or nonpolar? PH3
a)
polar
b)
nonpolar
102.
Will this molecule be polar or nonpolar? CS2
a)
polar
b)
nonpolar
103.

Match the following shapes to their Names

a)
1.

Trigonal Planar

b)
2.

Tetrahedral

c)
3.

Trigonal Pyrimidal

d)
4.

Linear

e)
5.

Bent

104.

Which Lewis Structure would be linear? Mark all that apply

a)
b)
c)
d)

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