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21-22 ACP Final Exam Review

Total questions: 141

Worksheet time: 2hrs 11mins

Name
Class
Date
1.

Each vertical column in the periodic table is called a

a)

period

b)

group

c)

valence

d)

unit

2.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
3.

The elements along the stairstep are called

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

4.

Which is a halogen?

a)

Helium

b)

Chlorine

c)

Oxygen

d)

Argon

5.

Which is an alkali metal?

a)

Magnesium

b)

Iron

c)

Sodium

d)

Chlorine

6.
A horizontal row of elements in the periodic table.
a)
column
b)
group
c)
period
7.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
8.

The elements on the right of the zigzag line are:

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

9.
An element's identity is determined by the number of
a)
electrons.
b)
protons.
c)
neutrons.
d)
valence.
10.
The majority of elements on the periodic table are
a)
man made.
b)
nonmetals.
c)
metals.
d)
gases.
11.
Which elements have the most similar chemical properties?
a)
K and Na
b)
K and Ca
c)
K and Cl
d)
K and S
12.

In the modern periodic table elements are arranged by:

a)

atomic mass

b)

atomic number

c)

order of discovery

d)

number of isotopes

13.

Which element is located at Period 5, Group 2?

a)

Iodine

b)

Strontium

c)

Nitrogen

d)

Phosphorus

14.

Mendeleev arranged his PT according to repeating properties and increasing __.

a)

atomic number

b)

atomic mass

c)

number of protons

d)

order of discovery

15.

Elements in the same group have similar _______.

a)

Atomic Mass

b)

Symbol

c)

Chemical Properties

d)

Atomic Number

16.

Aluminum is a:

a)

metal

b)

nonmetal

c)

metalloid

d)

Noble Gas

17.

An element that has 6 valence electrons will be found in:

a)

Group 2 (2)

b)

Group 4 (14)

c)

Group 6 (16)

d)

Group 8 (18)

18.

Group 2 elements are known as:

a)

alkali metals

b)

alkaline earth metals

c)

transition metals

d)

inner transition metals

19.

Elements in the "d block" of the PT are known as:

a)

alkali metals

b)

alkaline earth metals

c)

transition metals

d)

inner transition metals

20.

Which of the following is NOT a metalloid?

a)

Silicon

b)

Boron

c)

Antimony

d)

Tin

21.

The Periodic Law states that when elements are arranged according to increasing ____, their properties will repeat periodically.

a)

atomic mass

b)

atomic number

c)

number of isotopes

d)

metalloids

22.

As you move DOWN a group, elements have ____ electrons/energy levels leading to a _______ shielding effect.

a)

less, weaker

b)

less, stronger

c)

more, stronger

d)

more, weaker

23.

As you move DOWN a group, the added energy levels lead to a(n) ________ attraction between the nucleus and valence electrons and a(n) ___________ ionization energy.

a)

decreased, decreased

b)

decreased, increased

c)

increased, increased

d)

increased, decreased

24.

A smaller ionization energy would mean that it requires ______ energy to remove an electron from an element's electron cloud.

a)

less

b)

more

25.

As you move left to right across a period, the number of ______ increases which leads to a(n) ________ attraction between the nucleus and valence electrons.

a)

protons, decreased

b)

protons, increased

c)

electrons, decreased

d)

electrons, increased

26.

As you move left to right across a period, there is a _______ attraction between the nucleus and valence electrons which leads to a _______ ionization energy.

a)

weaker, lower

b)

weaker, higher

c)

stronger, lower

d)

stronger, higher

27.

Which of the following elements has the SMALLEST ionization energy?

a)

Barium (Ba)

b)

Beryllium (Be)

c)

Calcium (Ca)

d)

Strontium (Sr)

28.

If an element has a HIGHER ionization energy, it is likely to be ______ reactive than an element with a lower ionization energy.

a)

more

b)

less

29.

Which of the following elements would be EASIEST to take an electron from?

a)

Sodium (Na)

b)

Magnesium (Mg)

c)

Phosphorus (P)

d)

Aluminum (Al)

30.

Which of the following elements would be HARDEST to take an electron from?

a)

Bromine (Br)

b)

Iodine (I)

c)

Fluorine (F)

d)

Astatine (At)

31.

Which of the following elements has the HIGHEST ionization energy?

a)

Potassium (K)

b)

Arsenic (As)

c)

Krypton (Kr)

d)

Gallium (Ga)

32.

Ionization energy generally increases as we move...

a)

down a group and to the right along a period

b)

down a group and to the left along a period

c)

up a group and to the right along a period

d)

up a group and to the left along a period

33.

Electronegativity refers to how strongly an atom _______ additional electrons.

a)

attracts

b)

repels

34.

Electronegativity is measured using the Pauling Scale of EN. Which of the following numbers would correspond to a HIGHLY electronegative element?

a)

1.2

b)

2.0

c)

0.8

d)

3.7

35.

Electronegativity generally increases as you move...

a)

down a group and to the right across a period.

b)

down a group and to the left across a period.

c)

up a group and to the right across a period.

d)

up a group and to the left across a period.

36.

Which of the following correctly places the elements of Group 7 in order of INCREASING electronegativity?

a)

F, Cl, Br, I

b)

Cl, F, Br, I

c)

I, Br, Cl, F

d)

Br, Cl, I, F

37.

Nitrogen (N) is ________ electronegative than Beryllium (Be).

a)

more

b)

less

38.

As you move DOWN a group, there are _______ electrons and energy levels leading to a greater shielding effect and a ________ electronegativity value.

a)

more, higher

b)

more, lower

c)

less, higher

d)

less, lower

39.

As you move to the RIGHT across a period, there are _______ protons in the nucleus leading to a ________ electronegativity value.

a)

more, higher

b)

more, lower

c)

less, higher

d)

less, lower

40.

An element with a HIGH electronegativity value will attract electrons from a neighboring atom ____________ an element with a low electronegativity value.

a)

more easily than

b)

less easily than

c)

just as easily as

41.

Which of the following has the HIGHEST electronegativity value?

a)

Sodium (Na)

b)

Lithium (Li)

c)

Cesium (Cs)

d)

Francium (Fr)

42.

Cations have a ______ charge because they have _____ electrons.

a)

negative, lost

b)

negative, gained

c)

positive, lost

d)

positive, gained

43.

Anions have a _____ charge because they have ______ electrons.

a)

negative, lost

b)

negative, gained

c)

positive, lost

d)

positive, gained

44.

If an atom GAINS electrons, it would be _______.

a)

larger

b)

smaller

c)

the same size

45.

If an atom LOSES electrons, it would be _______.

a)

larger

b)

smaller

c)

the same size

46.

Which is LARGER: O or O2- ?

a)

O

b)

O2-

c)

Neither

47.

Which is SMALLER: F or F- ?

a)

F

b)

F-

c)

Neither

48.

Which is SMALLER: Mg or Mg2+ ?

a)

Mg

b)

Mg2+

c)

Neither

49.

An anion would be _________ the neutral atom of the same element.

a)

larger than

b)

smaller than

c)

the same size as

50.

A cation would be _________ the neutral atom of the same element.

a)

larger than

b)

smaller than

c)

the same size as

51.
Which compounds contain a metal?
a)
ionic
b)
covalent
c)
both
52.
Which compounds might include a Roman numeral in the name?
a)
ionic
b)
covalent
c)
both
53.
Which type of compound does this picture represent?
a)
ionic
b)
covalent
c)
both
54.
Which type of compound does this picture represent?
a)
ionic
b)
covalent
c)
both
55.
Which type of compound will end in -ide?
a)
ionic
b)
covalent
c)
both
56.
Which compounds will include prefixes in the name?
a)
ionic
b)
covalent
c)
both
57.
Which compounds may include a polyatomic ion?
a)
ionic
b)
covalent
c)
both
58.
Which compounds include only nonmetals?
a)
ionic
b)
covalent
c)
both
59.
What kind of compound is
NaOH
a)
Ionic
b)
Covalent
60.

Which of the following represents an IONIC compound?

a)
b)
61.
What kind of compound is
P4H10
a)
Ionic
b)
Covalent
62.
What kind of compound is
MgCO3
a)
Ionic
b)
Covalent
63.
What kind of compound is
NH4NO3
a)
Ionic
b)
Covalent
64.
What kind of compound is Phosphorous Trichloride
a)
Ionic
b)
Covalent
65.
Which of these is covalent?
a)
NaCl
b)
Pb(NO3)2
c)
SO2
d)
AlCl3
66.
When preparing to write the formula for nitrogen dioxide, should you first figure out what the charges are?
a)
Yes 
b)
No
67.
When preparing to write the formula for sodium nitrate, should you first figure out what the charges are?
a)
yes
b)
no
68.
When preparing to write the formula for iron(II) carbonate, should you first figure out what the charges are?
a)
yes
b)
no
69.
When writing the name for MgCl2, should you use prefixes?
a)
yes
b)
no
70.
When writing the name for CCl4, should you use prefixes?
a)
yes
b)
no
71.
Which of these compounds is ionic? 
a)
Carbon dioxide
b)
Dinitrogen trioxide
c)
Silicon tetrachloride
d)
Lithium fluoride
72.

What is the formula for Nitrogen dioxide

a)

N5O2

b)

N2O3

c)

N6O5

d)

NO2

73.

What is the formula for Sulfur hexafluoride

a)

SF6

b)

S6F5

c)

S6F8

d)

SF9

74.

What is the name for Mg3(PO4)2?

a)

magnesium triphosphide

b)

magnesium triphosphate

c)

magnesium phosphate

d)

trimagnesium diphosphate

75.
What is the OFFICIAL name for H2O
a)
Hydrogen Oxide
b)
Oxygen Dinitride
c)
Agua
d)
Dihydrogen Monoxide
76.
What is the formula for tetraphosphorus heptaoxide
a)
P4O7
b)
P7O4
c)
P2O3
d)
P4O6
77.

What is the name for P3F4

a)

Phosphorous fluoride

b)

Triphosphorous tetrafluoride

c)

Phosphate Fluoride

d)

Trifluoride hexafluoride

78.
What is the name of P4S10
a)
phosphorous sulfide
b)
phosphorus sulfide
c)
tetraphosphorus decasulfide
d)
phosphorus (X) sulfide
79.

What is the formula for sodium nitrate?

a)

Na3NO

b)

NaNO

c)

Na3NO3

d)

NaNO3

80.

What is the formula for iron(II) carbonate?

a)

Fe2CO3

b)

FeCO3

c)

Fe2CO2

d)

FeCO4

81.
What 3D shape will this molecule have?
a)
Bent
b)
Trigonal Pyramidal
c)
Linear
d)
Trigonal Planar
82.
What 3D shape will this molecule have?
a)
Bent
b)
Trigonal Pyramidal
c)
Tetrahedral
d)
Trigonal Planar
83.
What 3D shape will this molecule have?
a)
Bent
b)
Trigonal Pyramidal
c)
Tetrahedral
d)
Trigonal Planar
84.
What 3D shape will this molecule have?
a)
Bent
b)
Trigonal Pyramidal
c)
Tetrahedral
d)
Trigonal Planar
85.
Which 3D shape is this molecule?
a)
Trigonal Planar
b)
Trigonal Pyramidal
c)
Bent
d)
Linear
86.
Which 3D shape is this molecule?
a)
Trigonal Planar
b)
Trigonal Pyramidal
c)
Bent
d)
Linear
87.

Which 3D shape has 4 atoms bonded to the center atom AND 0 pairs of unshared e-s on the center atom

a)
Tetrahedral
b)
Bent
c)
Trigonal Planar
d)
Trigonal Pyramidal
88.

Which 3D shape has 2 atoms bonded to the center atom AND either 1 or 2 pairs of unshared e-s on the center atom

a)
Linear
b)
Bent
c)
Trigonal Planar
d)
Trigonal Pyramidal
89.

What kind of bond exists between Carbon and Oxygen?

a)

NonPolar Covalent Bond

b)

Polar Covalent Bond

c)

Ionic Bond

90.

The electronegativity DIFFERENCE between a Carbon (2.5) and Hydrogen atom (2.1) is:

a)

0.4

b)

5.9

c)

-0.4

d)

1.7

91.

Carbon (EN = 2.5) and Sulfur (EN = 2.5) will

a)

share electrons evenly

b)

share electrons unevenly

c)

transfer electron from one to another

92.

Phosphorous (EN = 2.1) and Flourine (EN = 4.0) will

a)

share electrons evenly

b)

share electrons unevenly

c)

transfer electrons from one to the other

93.
Nonpolar Covalent bonds
a)
share electrons evenly
b)
share electrons unevenly
c)
transfer electrons
d)
do not share electrons
94.
Polar covalent bonds
a)
share electrons evenly
b)
share electrons unevenly
c)
transfer electrons
d)
do not share electrons
95.

A POLAR COVALENT bond has an electronegativity difference that is

a)

equal to 0

b)

between 0.1 and 2.0

c)

greater than or equal to 2

96.

Consider the EN values of each atom. Which way should the arrows point?

a)

From the middle (3.5) to the outside (3.0)

b)

From the outside (3.0) in toward the middle (3.5)

97.

Notice the arrows point to the OUTER atoms. What can you conclude about the EN value of the CENTER atom?

a)

the center must also be 3.5

b)

the center must be less than 3.5

c)

the center must be greater than 3.5

98.

The Kinetic Theory states that:

a)

atoms only move when additional heat is applied

b)

gases don’t have mass or volume, while solids and liquids do

c)

all substances are made of atoms which are constantly in motion

99.

Which has the strongest IMF?

a)

solids

b)

liquids

c)

gases

100.

Water in a freezer will...

a)

Lose energy and melt

b)

Lose energy and freeze

c)

Gain energy and melt

d)

Gain energy and freeze

101.

The electronegativity difference in each of the C-H bonds in a molecule of methane is:

a)

0.4

b)

5.9

c)

-0.4

d)

1.7

102.
All diatomic bonds are:
a)
Polar covalent
b)
Nonpolar covalent
c)
Ionic
d)
Metal
103.
In a water molecule, which atom(s) has/have a partial negative charge?
a)
Oxygen
b)
Hydrogen
c)
None of the atoms
d)
All of the atoms
104.
Hydrogen bonding occurs in molecules when ___________________.
a)
a hydrogen atom forms a covalent bond with another atom.
b)
a hydrogen atom in a molecule forms a bond with any atom.
c)
a hydrogen atoms form an ionic bond with another atom on an adjacent molecule.
d)
a hydrogen atom bonded to F, O or N is attracted to an electron pair on a F, O or N atom on an adjacent molecule.
105.
Ice has ___________ density as compared to water.
a)
higher
b)
lower
c)
the same
106.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
107.
Does H2S have hydrogen bonding?
a)
yes
b)
no
108.
Does NO2 have hydrogen bonding?
a)
yes
b)
no
109.
Does NH3 have hydrogen bonding?
a)
yes
b)
no
110.
In general, substances with stronger intermolecular forces have ___________  boiling points than those with weaker intermolecular forces
a)
higher
b)
lower
111.
What word describes when water is attracted to other substances?
a)
cohesion
b)
adhesion
c)
capillary action
d)
surface tension
112.

Water molecules are attracted to other water molecules

a)

cohesion

b)

adhesion

c)

surface tension

d)

capillary action

113.
Plant roots are able to absorb water because of ....
a)
evaporation
b)
capillary action
c)
surface tension
d)
universal solvent
114.
Paper clips are able to float on water because of ....
a)
adhesion
b)
capillary action
c)
surface tension
d)
universal solvent
115.
Water dissolves many substances so it is called the ....
a)
wonderful water
b)
capillary action
c)
water cycle
d)
universal solvent
116.
What property of water is shown in the picture?
a)
capillary action
b)
surface tension
c)
evaporation
d)
universal solvent
117.

Why are temperature variations usually not as great on Long Island as they are in central New York State?

a)

Central New York State has a higher elevation.

b)

Central New York State is more heavily wooded.

c)

Long Island has a more southerly latitude.

d)

Long Island is surrounded by a large body of water.

118.

The graph shows the average monthly temperature of cities A & B.

City A has a much greater temperature range, hotter summers and colder winters than city B. This is because city A most likely

a)

is closer to the equator

b)

is father from a large body of water

c)

is on the leeward side of a mountain

d)

at a higher elevation

119.

What is the direct cause of rising sea levels?

a)

Melting Sea Ice

b)

Melting Land Ice

c)

Climate Change

120.

Floating sea ice melts...

a)

and causes sea levels to rise because it adds water to the ocean.

b)

but does not cause sea levels to rise because the ice displaces the same amount of ocean water as the melted ice would displace.

121.
A substance with a high specific heat:
a)
Is always extremely hot.
b)
Requires a lot of energy to become hot.
c)
Is not heavy.
d)
Does not requires a lot of energy to become hot.
122.
The amount of thermal energy required to raise the temperature of one (1) kilogram of a substance by 1o C is known as:
a)
Specific heat
b)
Heat of fusion
c)
Heat of vaporization
d)
Melting point
123.
In an endothermic reaction, heat is ,,,
a)
taken in
b)
given out
124.
The number of atoms of  N (nitrogen) in 3N2O5 is
a)
5
b)
2
c)
6
d)
15
125.

What coefficient belongs on the line:

Mg + 2AgCl ------------> MgCl2 + ___Ag

a)

1

b)

2

c)

4

d)

6

126.

Which of the following reactions is balanced?

a)

2Na + Cl2-------> 2NaCl

b)

2Na + 2Cl2 ------> 2NaCl

c)

Na + 2Cl2 --------> NaCl

127.

How many Hydrogen atoms are in 4H2O?

a)

6

b)

8

c)

2

d)

4

128.

What coefficient belongs on the line?

P4 + 3O2 --> ___P2O3

a)

1

b)

2

c)

3

d)

4

129.

According to the Law of Conservation of Matter, which of the following occurs during a chemical reaction?

a)

Matter is not created or destroyed, atoms just rearrange themselves.

b)

New atoms are created as new products form.

c)

Original atoms are destroyed as new products form.

d)

Chemical bonds can never be broken.

130.
What is the definition of a catalyst?
a)
Something that speeds up a rxn
b)
Something that slows a rxn
c)
Something that makes more products
d)
Something that makes more reactants
131.

Name the part in red:


H2 + O2 -> H2O

a)

Coefficient

b)

Product

c)

Reactant

132.
Name the part in red:

H2 + O2 -> H2O
a)
Coefficient
b)
Product
c)
Yield
d)
Subscript
133.
Name the part in red:

H2 + O2 -> H2O
a)
Coefficient
b)
Product
c)
Reactant
d)
Subscript
134.

When substances react, you expect to observe

a)

change in color

b)

a release of gas or precipitate

c)

release of heat or light in the products

d)

all of the above as possibilities

135.

In a chemical equation, the symbol (aq) indicates that the substance is:

a)

water

b)

dissolved in water

c)

an acid

d)

insoluble in water

136.

The chemical symbol of an element written over the arrow in a chemical equation signifies:

a)

a byproduct

b)

the formation of a gas

c)

a catalyst for the reaction

d)

an impurity

137.

Exothermic reactions occur when additional energy is _____ as the new products form.

a)

absorbed

b)

released

138.

Which of the following is used to indicate a precipitate has formed during a chemical reaction?

a)

(aq)

b)

(p)

c)

(s)

d)

(🌨)

139.

Imagine a reaction in which water vapor is formed. How would you indicate this?

a)

H2O(g)

b)

H2O(v)

c)

W.V.(g)

d)

H2O(aq)

140.

Information about energy written on the LEFT side of a chemical equation indicates that a reaction is:

a)

exothermic

b)

endothermic

141.

If you want to produce 300.0 g of water vapor, how many grams of NH3 do you need to use in this reaction?

a)

476.5 g

b)

188.9 g

c)

24.5 g

d)

200.1 g

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