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Chem Final Exam RVW

Total questions: 171

Worksheet time: 11hrs 25mins

Name
Class
Date
1.

Particles in an atom that are neutral and have no charge are 

a)

ions 

b)

electrons 

c)

neutrons 

d)

protons 

2.

If the number of protons equal the number of _____, the atom will have no charge

a)

protons

b)

neutrons

c)

electrons

d)

nucleus

3.

The subatomic particle with a negative charge is the

a)

electron

b)

proton

c)

neutron

d)

nucleus 

4.

What is the atomic number?

a)

the number of protons

b)

the number of protons and neutrons

c)

the number of neutrons

d)

the number of protons and electrons

5.

What is the mass number?

a)

the number of protons

b)

the number of protons and neutrons

c)

the number of neutrons

d)

the number of protons and electrons

6.

An atom with an unequal number of protons and electrons is said to be a(n) ___.

a)

radioactive particle

b)

isotope

c)

ion

d)

molecule

7.

Ions are: 

a)

atoms with a positive or negative charge

b)

atoms with no charge

c)

atoms with ONLY a positive charge

d)

atoms with ONLY a negative charge

8.

How many neutrons does the isotope of lithium have?

a)

8

b)

3

c)

4

d)

5

9.

How many protons does this isotope of titanium have?

a)

48

b)

22

c)

26

d)

70

10.

The state of matter with the molecules with the LOWEST amount of energy is....

a)

Gas

b)

Solid

c)

Liquid

11.

The state(s) of matter that takes the shape of its container is....(Choose the BEST answer)

a)

Gas

b)

Solid

c)

Liquid/Gas

d)

Liquid

12.

Which is the following is NOT a sign of a chemical change?

a)

Releasing a gas

b)

Change in temperature (due to breaking of bonds)

c)

Changing state of matter

d)

Production of sound/light

13.

Signs that a chemical change has occurred include

a)

a change in color

b)

the release of bubbles

c)

the production of an odor

d)

all of the above

14.

All the elements on the left side of the periodic table are called..

a)

Metals

b)

Metalloid

c)

Nonmetals

15.

A substance that is made up of one type of atom is called an:

a)

atom

b)

element

c)

compound

d)

mixture

16.

Where on the periodic table are the metalloids found?

a)

Right Side

b)

Along the Zig Zag Line

c)

Left Side

d)

Bottom

17.

Nonmetals are located in what section of this periodic table?

a)

Blue

b)

Yellow

c)

Pink

18.

CO2

a)

Element

b)

Compound

19.

H2O

a)

Element

b)

Compound

20.

Where are electrons of an atom found?

a)

Nucleus

b)

Electron Cloud

c)

Some are in the nucleus and some in the electron cloud.

d)

They are moving everywhere.

21.

How many protons does Carbon have?

a)

3

b)

4

c)

5

d)

6

22.

Density is...

a)

the amount of mass in an object

b)

the amount of space an object takes up

c)

the amount of mass in a given space

d)

the weight of an object

23.

Burning a piece of paper 

a)

Chemical Change 

b)

Physical Change 

24.

Melting Ice 

a)

Chemical Change 

b)

Physical Change 

25.

How many ATOMS are in the following compound:  C2H4O2

a)

2

b)

8

c)

1

d)

4

26.

A _________ is a substance made of two or more DIFFERENT elements chemically combined. 

a)

mixture

b)

compound

c)

substance 

27.

If the number of electrons in an element changes, a new element is formed 

a)

True 

b)

False 

28.

These are the two subatomic particles located inside the nucleus of an atom 

a)

Protons and Electrons 

b)

Protons and Neutrons 

c)

Electrons and Neutrons 

d)

Neutrons and ions 

29.

To what family of elements do the elements helium, neon, and argon belong to?

a)

Halogens

b)

Actinides

c)

Noble gases

d)

Transition metals

30.

What are the name of the atoms of the same element that have a different number of neutrons ?

a)

Allotropes

b)

Ions

c)

Anions

d)

Isotopes

31.

The substances listed on the right side of a chemical equation are the

a)

Yields

b)

Reactants

c)

Products

d)

Precipitates

32.

An ionic bond is:

a)

a metal bonded to a nonmetal

b)

a nonmetal bonded to a nonmetal

c)

a metal bonded to a metal

33.

The substances listed on the left side of a chemical equation are the

a)

Products

b)

Coefficients

c)

Precipitates

d)

Reactants

34.
In chemical reactions, what does the principle of conservation of mass mean?
a)
Matter is not created or destroyed.
b)
The total mass of the reactants is greater than the total mass of the products.
c)
The total mass of the reactants is less than the total mass of the products.
d)
Matter is not changed.
35.
How many Oxygen (O) atoms are in 2C2HO8Cl2
a)
2
b)
16
c)
8
d)
5
36.
In the following equation, what are the products?
HCl + Zn → H2 + ZnCl2
a)
HCl + Zn
b)
H2 + ZnCl2
c)
Zn → H2
d)
the stuff on the outside
37.
Which number should go in the blank?
_ H2 + O2 -> 2 H2O
a)
1
b)
2
c)
3
d)
0
38.
Which number should go in the blank?
2 Na+ _ Cl2 -> 2 NaCl
a)
1
b)
2
c)
3
d)
0
39.
H2 + O2 -> 2 H2O
Which kind of reaction is this?
a)
synthesis
b)
decomposition
c)
single displacement
d)
double displacement
40.
Mn + _ HNO3 → Mn(NO3)2 + H2
Which kind of reaction is this?
a)
synthesis
b)
decomposition
c)
single displacement
d)
double displacement
41.
FeS + HCl ---> FeCl2 + H2S
Which kind of reaction is this?
a)
synthesis
b)
decomposition
c)
single displacement
d)
double displacement
42.
H2CO3 → H2O + CO2
Which kind of reaction is this?
a)
synthesis
b)
decomposition
c)
single displacement
d)
double displacement
43.
Left of zigzag line
a)
metals
b)
nonmetals
c)
metalloid
44.
Elements with similar properties
a)
Periods
b)
Groups
45.
What is the number of protons that the element in this image contain?
a)
14
b)
7
c)
15
d)
18
46.
What is the atomic mass of "F"
a)
9
b)
18
c)
17
d)
19
47.
A "group" is a ____________ on the periodic table.
a)
column
b)
row
48.
A "period" is a ____________ on the periodic table.
a)
column
b)
row
49.
How many elements are represented in the compound?
Na2CO3
a)
1
b)
2
c)
3
d)
4
50.
How many TOTAL atoms are in this compound?
H2C3O4N5
a)
5
b)
14
c)
15
d)
19
51.
How many molecules of Carbon Dioxide?
6CO2
a)
12
b)
2
c)
6
d)
8
52.
The rings around the nucleus of an atom are called...
a)
energy levels
b)
electron circles
c)
proton levels
d)
neutron clouds
53.
What is the atomic number of Carbon-13 (C)?
a)
13
b)
12.01
c)
6
d)
26
54.
What is the mass number of Chlorine-37 (Cl)?
a)
17
b)
37
c)
7
d)
35.45
55.
Rows ⋘---⋙ on the periodic table indicate the number of...
a)
groups
b)
energy levels
c)
valence electrons
d)
total electrons
56.
An element in period 2, group 3 would have how many valence (outer) electrons?
a)
3
b)
2
c)
5
d)
8
57.
When becoming an ion, an element with 6 valence (outer) electrons would have a charge of...
a)
2-
b)
2+
c)
6-
d)
6+
58.
a)
This is an ionic bond with electrons shared
b)
This is an ionic bond with electrons transferred
c)
This is a covalent bond with electrons shared
d)
This is a covalent bond with electrons transferred
59.
a)
This molecule would be named PCl3
b)
This molecule would be named ClP3
c)
This molecule would be named PCl
d)
This molecule would be named PCl3
60.
This rule says that the amount of atoms in the reactants is equal to the amount of atoms in the products...
a)
Conservation of Energy
b)
E=MC2
c)
Conservation of Mass
d)
Rule of 8
61.
During an endothermic reaction, energy will be...
a)
released
b)
absorbed
c)
destroyed
d)
created
62.
In an _____________ reaction, the reactants will have more energy than the products. 
a)
exothermic
b)
endothermic
c)
chemical
d)
activation 
63.
Activation energy is needed during what part of a chemical reaction?
a)
to end a chemical reaction
b)
during a chemical reaction
c)
to start a chemical reation
64.
Which of these elements is a metal?
a)
argon
b)
carbon
c)
iron
d)
hydrogen
65.
When heated, oxygen reacts with copper to form copper oxide:
If this reaction occurs in a sealed container, will the mass of the container and everything in it increase, decrease, or stay the same and why?
a)
The mass will stay the same because the number of each kind of atom stays the same.
b)
The mass will increase because a new kind of molecule is formed.
c)
The mass will decrease because two substances combine to form one substance.
d)
More information is needed to tell if the mass will change.
66.
Consider the chemical equation CH4 + 2 O2 → CO2 + 2 H2O. In this equation, CH4 is a
a)
product
b)
reactant
c)
displacement
67.
 What is the mass number of this element?
a)
5
b)
27
c)
32
d)
59
68.
# neutrons + # protons = ___
a)
atomic number
b)
Atomic thing
c)
Mass Number
d)
Valence Electrons
69.
How many electrons would an atom of Krypton have?
a)
83.80
b)
36
c)
12
d)
none
70.
The group number tells us how many _________ there are in an element.
a)
groups
b)
valence electrons
c)
energy levels
d)
chemicals
71.
The ________________ tells you how many energy levels are used in an element.
a)
group number
b)
atom
c)
protons
d)
period number
72.
The element Tellurium has the atomic mass of 127.60 and its atomic number is 52. How many neutrons are in the element Tellurium?
a)
179.60
b)
127.60
c)
52
d)
76
73.
The inner energy level can only hold ______ electrons.
a)
1
b)
0
c)
2
d)
18
74.
The largest amount of electrons the 3rd energy level can hold is?
a)
18
b)
unlimited amount
c)
2
d)
8
75.
How many valence electrons do elements in group 17 have in their outer energy level?
a)
7
b)
17
c)
1
d)
0
76.
Appearance, texture, and density are classified as
a)
physical properties
b)
chemical properties
c)
magnetic properties
d)
thermal properties
77.
Mario pours three different liquids into a beaker. He notices the layers settle at different depths in the beaker.
Based on the picture, which property of the liquids is Mario most likely studying?
a)
density
b)
length
c)
mass
d)
volume
78.
The substance that is dissolved in a solution
a)
Solute
b)
Solvent
c)
Solution
d)
Solubility
79.
The temperature at which a liquid changes into a gas
a)
boiling point
b)
melting point
c)
freezing point
d)

condensing point

80.
The liquid that dissolves another substance in a solution.
a)
Solute
b)
Solvent
c)
Solution
d)
Solubility
81.
AB + CD →AD + CB
a)
Double Replacement
b)
Single Replacement
c)
Synthesis
d)
Decomposition
82.
Identify this type of reaction,
Cl2 + 2KI -->  I2 + 2KCl
a)
Synthesis
b)
Single displacement
c)
Double displacement
d)
Decomposition
83.
Which of the following is an example of synthesis?
a)
Na + Br2 --> NaBr
b)
KClO3 --> KCl + O2
c)
HgO + Cl2-->HgCl + O2
d)
Cl2 + NaBr --> NaCl + Br2
84.
Which of the following is the general formula for a decomposition reaction?
a)
A + B  → AB
b)
AB → A + B
c)
AB + C → AC + B
d)
AB + CD → AC + BD
85.
In an exothermic reaction, energy is _________.
a)
Released
b)
Absorbed
c)
Stored
d)
Doubled
86.

What type of reaction is the following:
C11H24+17O2−> 11CO2 + 12H2OC_{11}H_{24}+17O_2->\ 11CO_2\ +\ 12H_2O  

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

87.

Ionic or covalent?

CH4

a)

covalent

b)

ionic

88.

Ionic or covalent?

CaCl2

a)

ionic

b)

covalent

89.

Name this compound.

Na3N

(a)  

90.

Name this compound.

LiOH

(a)  

91.

Name this compound.

Fe(OH)3

(a)  

92.

what's the name?

SiO2

(a)  

93.

what's the name?

P2O5

(a)  

94.

what's the formula?

carbon monoxide

(a)  

95.
What is the charge on the calcium ion?
a)
1+
b)
2+
c)
2-
d)
1-
96.
Select the correct formula for sulfur hexachloride
a)
S2Cl6
b)
S6Cl
c)
SCl6
d)
SF6
97.
What is the formula for Potassium Fluoride? 
a)
KF
b)
K2F
c)
KF2
d)
none of the above
98.
What is the formula for calcium phosphide?
a)
CaP
b)
Ca2P3
c)
Ca3P2
d)
Ca2P
99.
What is the formula for calcium oxide? 
a)
Ca2O2
b)
Ca2O
c)
CaO
d)
CaO2
100.
Name the following:
Mg3P2
a)
Magnesium Phosphide
b)
Magnesium Phosphorus
c)
Magnamide Phosphide
d)
Magnamide Phosphorus
101.
What is the name of BaO?
a)
barium (II) oxide
b)
barium oxide
c)
barium oxygen
d)
barium (I) oxide
102.
If a balloon is cooled what will happen to the volume?
a)
Volume will increase
b)
Volume will decrease
c)
Volume will not change
d)
Balloon freezes to death
103.

The element Bromine (Br) has ​ (a)   Valence Electrons. The atom has ​ (b)   Energy levels (Shells)

Choose from the below words
7
4
17
14
5
104.

Match the following

a)

proton

1.

lives in the nucleus & positively charge

b)

electron

2.

lives in the cloud & negatively charge

c)

neutron

3.

lives in the nucleus & no charge

d)

valence electron

4.

lives in the last ring & negatively charge

e)

nucleus

5.

where protons & neutrons are found and largest mass

105.

The diagram shows arrangement of particles in a

a)

Solid

b)

Liquid

c)

Gas

106.

What state of matter does the picture below represent?

a)

solid

b)

liquid

c)

gas

d)

plasma

107.

Match the following

a)
1.

Solid

b)
2.

Liquid

c)
3.

Gas

108.

Match the following

a)
1.

Solid

b)
2.

Liquid

c)
3.

Gas

109.

Calcium is in Period 4, Group 2 on the Periodic Table of elements. Calcium is a ​ (a)   .

Choose from the below words
Metal
Non Metal
Metalloid
110.

match the following

a)
Metal
1.

Ag

b)
Nonmetal
2.

S

c)
Metalloid
3.

Ge

d)

noble gas

4.

Ne

111.

Match the following ion to its correct ionic charge

a)

Fluorine

1.

1-

b)

Oxygen

2.

2-

c)

Nitrogen

3.

3-

112.

Match the symbol and charge to the correct metal Cation

a)

Chromium (II)

1.

Cr2+

b)

Copper (I)

2.

Cu+

c)

Titanium(II)

3.

Ti2+

d)

Mercury (II)

4.

Hg2+

e)

Lead (IV)

5.

Pb4+

113.

How many d orbitals make up the d subshell?

a)

1

b)

5

c)

3

d)

7

114.

What orbital is shown in the picture?

a)

s orbital

b)

p orbital

c)

d orbital

d)

f orbital

115.

Heisenberg's Uncertainty Principle states that it is impossible to know both the ___________ and the __________ of a particle at the same time.

a)

velocity, position

b)

velocity, energy

c)

position, energy

d)

velocity, speed

116.

This states that no two electrons will have the same 4 quantum numbers in an atom or molecule. The two electrons of the same orbital must have opposite spin states.

a)

Pauli exclusion principle

b)

Hund's rule

c)

Aufbau principle

d)

None of the above

117.

What states that electrons fill the lowest energy orbitals/levels first before occupying higher energy levels?

a)

Pauli exclusion principle

b)

Hund's rule

c)

Aufbau Principle

d)

None of the above

118.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
119.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
120.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
121.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
122.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
123.
How many electrons can the s sublevel hold?
a)
14
b)
10
c)
2
d)
6
124.
How many electrons can the s sublevel hold?
a)
14
b)
10
c)
2
d)
6
125.

What element has the following electron configuration: 1s2 2s2 2p6 3s2?

a)

Ca+2

b)

Ca

c)

Mg

d)

Na

e)

Ar

126.

There are water droplets on the outside of a clean beaker. Two chemicals are added to the beaker. These chemicals react with each other. During the reaction, the water droplets outside the beaker freeze. Which statement BEST describes the reaction?

a)

endothermic, because energy is absorbed

b)

endothermic, because energy is released

c)

exothermic, because energy is absorbed

d)

exothermic, because energy is released

127.

__ Al + __ FeO → Al2O2 + __ Fe

a)

1, 1, 2

b)

2,1,2

c)

2, 2, 2

d)

2,4,2

128.
What is the little number after an element in a chemical equation called.
Example: H2
a)
Coefficient 
b)
Subscript
c)
Atom
d)
Equation
129.
Which problem is balanced?
a)
PbO2 + 2H2
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
130.
When balancing equations a ____ can be placed to the left of a formula of a substance to make the equations balanced
a)
charge
b)
subscript
c)
random number
d)
coefficient
131.

What does pH measure?

a)

the amount of hydrogen (H+) ions

b)

the amount of hydroxide (OH-) ions

c)

amount of water

d)

all of the above

132.
A solution has a pH of 7.0.  What would happen to the pH if H ions were added?
a)
pH would go up
b)
pH would go down
c)
pH would stay the same
d)
None of these
133.

As one moves down the pH scale from 14 to 1, what happens to the concentration of H+ in the solution?

a)

concentration of H+ decreases

b)

concentration of H+ increases

c)

concentration of H+ stays the same

134.

If pure water is added to an acid with a pH of 3, what happens to the pH of the solution?

a)

the pH increases to above 3

b)

the pH decreases to below 3

c)

the pH stays the same at 3

135.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
136.
Which type of bond has an equal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
137.
Which type of bond has an unequal sharing of electrons?
a)
Polar Covalent 
b)
Non Polar Covalent
c)
Ionic
d)
Metallic
138.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
139.
What is the number of valence electrons for Oxygen?
a)
8
b)
6
c)
2
d)
1
140.
What is the shape of this molecule?
a)
bent
b)
linear
c)
trigonal pyramidal
d)
tetrahedral
141.
What is the shape of this molecule?
a)
Linear
b)
bent
c)
tetrahedral
d)
trigonal planar
142.
What is the shape of this molecule?
a)
Linear
b)
Bent
c)
Tetrahedral
d)
Trigonal Pyramidal
143.
What is the shape of this molecule?
a)
Linear
b)
Bent
c)
Tetrahedral
d)
Trigonal Pyramidal
144.

Which Lewis Dot Model drawing correctly shows an O2 molecule?

a)
b)
c)
d)
145.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
146.
Which of the following is the correct Lewis structure for water?
a)
A
b)
B
c)
C
147.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
148.
What is the chemical formula for phosphorus triiodide?
a)
P3I
b)
PI
c)
P3I3
d)
PI3
149.

Name the following ionic compound: Cr(NO3)3

a)

chromium III nitride

b)

chromium II nitride

c)

chromium II nitrate

d)

chromium III nitrate

150.

Name the following ionic compound: MgSO4

a)

magnesium (II) sulfide

b)

magnesium sulfide

c)

magnesium sulfate

d)

magnesium (II) sulfate

151.

An atom has 12 protons and 13 neutrons in its nucleus. Which is the correct symbol?

a)
b)
c)
d)
152.

What should you not do in the lab?

a)

follow directions

b)

run

c)

prank

d)

walk

e)

push/shove

153.
Elements in the same ____________ tend to have similar properties
a)
group
b)
period
154.
Wood burning is an example of _______
a)
physical intensive property
b)
physical extensive property
c)
chemical change
d)
Physical change
155.
Physical properties of a substance include _________
a)
color and odor
b)
melting and boiling points
c)
density 
d)
all of the choices are correct
156.

The law that states that the repeating chemical and physical properties of elements relate to and depend on the elements' atomic numbers is _______.

a)
periodic
b)
period
c)
periodic table of the elements
d)
periodic law
157.
The family in the periodic table that contains the most reactive metals is the_______
a)
Alkaline Earth Metals
b)
Transition Metals 
c)
Alkali Metals
d)
Other Metals
158.
Which of the following is the most reactive in water?
a)
Lithium
b)
Sodium
c)
Potassium
159.

What happens to the reactivity of the alkali metals as you move down the group?

a)

increases

b)

decreases

160.

As you move down the group, halogens' reactivity...

a)

increases

b)

decreases

c)

doesn't change

d)

shows no trend.

161.

Which halogen is the most reactive?

a)

iodine

b)

chlorine

c)

bromine

d)

fluorine

162.

Complete this sentence: Electronegativity ____ from left to right across a period and ____ from top to bottom down a group on the periodic table.

a)

increases, decreases

b)

increases, increases

c)

decreases, decreases

d)

decreases, increases

163.

Complete this sentence: Ionization energy ____ from left to right across a period and ____ from top to bottom down a group on the periodic table.

a)

increases, decreases

b)

increases, increases

c)

decreases, decreases

d)

decreases, increases

164.

Water and methane molecules are roughly the same size and the same mass but water boils at a much higher temperature. What can we conclude about the intermolecular forces between water and methane?

a)

water has stronger intermolecular forces than methane

b)

water has weaker intermolecular forces than methane

c)

methane has stronger intermolecular forces than water

d)

methane and water have similar intermolecular forces

165.

The diagram provided here shows the reactants and the products of a common chemical reaction. The line on the graph behind them represents the energy of the system as the reaction progresses. Which of the following conclusions is best supported by the information provided?

a)

This is a fast reaction.

b)

This is a slow reaction.

c)

This reaction is endothermic.

d)

This reaction is exothermic.

166.

Atomic size generally ____

a)

decreases as you move from top to bottom within a group

b)

decreases as you move from top to bottom within a group

c)

remains constant within a period

d)

decreases as you move from left to right across a period

167.

Which of the following statements is true about ions?

a)

Cations form when an atom gains electrons.

b)

Cations form when an atom loses electrons.

c)

Anions form when an atom gains protons.

d)

Anions form when an atom loses protons

168.

What is the energy required to remove an electron from an atom in the gaseous state called?

a)

nuclear energy

b)

ionization energy

c)

shielding energy

d)

electronegative energy

169.

How many valence electrons are in an atom of phosphorus?

a)

2

b)

3

c)

4

d)

5

170.

Which of the following occurs in an ionic bond?

a)

Oppositely charged ions attract.

b)

Two atoms share two electrons

c)

Two atoms share more than two electrons

d)

Like-charged ions attract.

171.

What is the net charge of the ionic compound calcium fluoride?

a)

2-

b)

1-

c)

0

d)

1+

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