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Chemistry Semester 2 Final exam 2023-203-24

Total questions: 151

Worksheet time: 8hrs 44mins

Name
Class
Date
1.

A teacher asks her students to examine titles of four scientific articles. Which titled article is specifically about a chemical change?

a)

How Baking Soda Reacts with Vinegar

b)

How Rust Can Be Scraped off of Metal

c)

How Metals Respond to Electrical Currents

d)

How Elements Can Change Phase When Heated

2.

Identify ALL of the chemical changes

a)

Boiling water

b)

Burning a marshmallow

c)

Fireworks going off

d)

Cutting your hair

e)

Dying your hair

3.

If you cut a wooden block in half, each half would have:

a)

Half the density of the original piece

b)

Twice the density of the original piece

c)

The same density as the original piece

4.

Which best represents a balanced equation?

a)

120 grams of carbon plus 20 grams of oxygen → 200 grams of carbon dioxide

b)

120 grams of carbon plus 50 grams of oxygen → 200 grams of carbon dioxide

c)

120 grams of carbon plus 80 grams of oxygen → 200 grams of carbon dioxide

5.

The following chemical reaction occurs.


2H2O2 → 2H2O + O2

How many atoms of hydrogen are involved in the reaction?

a)

1

b)

2

c)

4

d)

8

6.

The compound ammonia is composed of nitrogen and hydrogen atoms. If two atoms of nitrogen completely react with six atoms of hydrogen to form two molecules of ammonia, which best describes the number of hydrogen atoms present in the two molecules of ammonia?

a)

2

b)

4

c)

6

7.

Which is best represented by the equation?

2Mg + O2 2MgO

a)

Law of Conservation of Energy

b)

Law of Conservation of Mass

c)

Law of Superposition

8.

When chemicals react in a closed container, which must be true?

a)

The mass both before and after the reaction is the same.

b)

The mass both before and after the reaction is variable.

c)

The same number of compounds is present both before and after the reaction.

9.

A chemistry teacher combines 20 grams of lemon juice with 25 grams of baking soda in a flask covered with a balloon. The flask and balloon have a combined mass of 105 grams. What is the mass of the entire setup after a reaction has occurred?

a)

45 g

b)

150 g

c)

605 g

10.

The equation below shows a reaction between sodium (Na) and water (H2O).

2Na (s) + H2O (l) → 2NaOH (aq) + H2 (g)

Which best explains why the equation is not balanced?

a)

There is too much sodium in the reactants.

b)

There is not enough water in the reactants.

c)

There is too much hydrogen gas in the products.

d)

There is not enough sodium hydroxide in the products.

11.

What coefficient for O2 demonstrates the law of conservation of mass?


CH4(g) + __O2(g) → CO2(g) + 2H2O(g)

a)

1

b)

2

c)

3

d)

4

12.

Which best describes how to balance the chemical equation shown below to support the law of conservation of mass?

Mg + O2 → MgO

a)

Add the coefficient 2 before the Mg on both sides of the equation.

b)

Add the coefficient 2 before the O2 on the left side of the equation.

c)

Add the coefficient 2 before the Mg on the left side of the equation.

d)

Add the coefficient 2 before the MgO on the right side of the equation.

13.

In the equation below, suppose 11 grams of zinc react with 12 grams of hydrogen chloride to form 16 grams of zinc chloride and an unknown amount of hydrogen gas.

Zn + 2HCl → ZnCl2 + H2

Based on the Law of Conservation of Mass, how many grams of hydrogen gas will form?

a)

1 g

b)

7 g

c)

19 g

14.

Which best explains why the total mass of the product(s) would be less than the total weight of the reactant(s) after a chemical reaction?

a)

A physical change occurred.

b)

Atoms involved in the reaction lost mass

c)

Precipitates were created in the new solution

d)

Gases were released into the atmosphere.

15.

If 100 grams of vinegar and 5 grams of baking soda are poured in a container, a small amount of gas will be produced. What will the final mass of the products be if the gas is trapped in the container?

a)

100 g

b)

104 g

c)

105 g

d)

110 g

16.

Which of the following is a correctly written chemical equation that demonstrates the conservation of mass?

a)

Mg + HCl --> H2 + MgCl2

b)

H2O + CO2 --> H2CO3

c)

KClO3 --> KCl + O2

d)

H2 + O2 --> H2O

17.

What is the total number of oxygen atoms on the reactant side of the equation shown below?


CH3COOH + NaHCO3 → CH3COONa + H2O + CO2

a)

2

b)

3

c)

5

d)

7

18.

An ice cube is put into a heated pan. What will most likely happen to the molecules in the ice as the ice is heated?

a)

The molecules will begin to move slower.

b)

The molecules will begin to move faster.

c)

The molecules will begin to increase in density.

d)

The molecules will begin to condense in air.

19.

Two clear solutions are mixed together in a beaker. Which result would indicate a chemical reaction had occurred between these solutions?

a)

increase of volume in the beaker

b)

decrease of volume in the beaker

c)

increase in temperature of the beaker

20.

John and Lisa collected a sample of ocean water and placed it in a jar. Within a couple of days, the water had evaporated and salt was visible at the bottom of the jar. This is an example of a

a)

physical change

b)

chemical change

c)

new substance being formed

21.

What does the Law of Conservation of Mass state?

a)

Matter is created and destroyed in a chemical reaction.

b)

Matter is neither created nor destroyed, just transferred.

c)

Matter is only destroyed in a chemical reaction.

d)

Matter can be transformed into energy.

22.

When balancing chemical equations, what is the first step?

a)

Balance the most complex molecule.

b)

Sum all the atoms and make a chart.

c)

Guess and check the coefficients.

d)

Balance the hydrogen atoms first.

23.

What does balancing a chemical equation involve?

a)

Changing the chemical formulas of the reactants and products.

b)

Adding coefficients to ensure the number of atoms of each element is equal on both sides.

c)

Removing elements to simplify the equation.

d)

Increasing the temperature of the reaction.

24.

What should be true for all elements in a balanced chemical equation?

a)

They should all be gases.

b)

They should react with each other.

c)

They should be equal and as simplified as possible.

d)

They should be in their elemental form.

25.

What is the purpose of making a chart when balancing chemical equations?

a)

To list the physical properties of each element.

b)

To track the number of atoms of each element.

c)

To determine the temperature of the reaction.

d)

To identify the catalysts in the reaction.

26.

What is meant by ‘balancing’ in the context of chemical equations?

a)

Ensuring the equation is symmetrical.

b)

Making sure the physical states of all reactants and products are mentioned.

c)

Ensuring the number of atoms for each element is the same on both sides of the equation.

d)

Confirming that the reaction is exothermic.

27.

What role do coefficients play in balancing chemical equations?

a)

They indicate the temperature at which the reaction occurs.

b)

They change the chemical properties of the substances involved.

c)

They represent the number of molecules of each substance.

d)

They show the speed of the chemical reaction.

28.

What is typically the first element balanced in a chemical equation?

a)

The element with the least atoms.

b)

The element with the most complex structure.

c)

Any random element.

d)

An element chosen based on its position in the periodic table.

29.

Why might balancing chemical equations involve some trial and error?

a)

Because the exact composition of substances is unknown.

b)

Due to the unpredictability of chemical reactions.

c)

Because finding the correct coefficients may require adjustment.

d)

Because the laws of chemistry are not always consistent.

30.

In a balanced chemical equation, what happens to atoms from the beginning to the end of the reaction?

a)

They change into different atoms.

b)

They are destroyed and then recreated.

c)

They remain the same, just rearranged.

d)

They are converted into energy.

31.

How many oxygen atoms are in the products for the chemical reaction below?
4Fe + 3O2 → 2Fe2O34Fe\ +\ 3O_{2\ }\rightarrow\ 2Fe_2O_3  

a)

2

b)

3

c)

5

d)

6

32.

What do we call the chemicals that result from a chemical reaction?

a)

reactants

b)

products

c)

subscripts

d)

coefficients

33.

The Law of Conservation of Mass says that matter can neither be __________ or __________.

a)

created; destroyed

b)

recycled; renewed

c)

subtracted; added

d)

joined; separated

34.

How many atoms are in the products below?
4Fe +3O2 → 2Fe2O34Fe\ +3O_{2\ }\rightarrow\ 2Fe_2O_3  

a)

7

b)

10

c)

17

d)

20

35.

According to the Law of Conservation of Mass, what happens to the wood and oxygen when it is burned?

a)

The wood disappears.

b)

It stays the same chemically.

c)

The atoms in the wood and oxygen rearrange and form smoke and ash.

d)

Nothing.

36.
Substances present at the start of a chemical reaction
a)
subscripts
b)
coefficients
c)
reactants
d)
products
37.
A 55-gram egg is placed in a pot. After the egg is boiled, which is most likely the mass of the egg?
a)
50 
b)
55 
38.
What does the principle of conservation of mass mean?
a)
The total mass of the reactants is more than the products
b)
Matter is not created or destroyed
c)
The total mass of the reactants is less than the products
39.
In a reaction A + B ----> C,  reactant A has 5g and product  C has 9g. How many grams does reactant B should have? 
a)
4g
b)
5g
c)
9g
d)
14g
40.
Is this equation balanced or unbalanced? 
H2 + O2 --> H2O
a)
balanced
b)
unbalanced
41.
12g of Carbon react with 16g of Oxygen, how much carbon monoxide (CO) is formed? 
a)
28 g
b)
4g
c)
30g
d)
12g
42.

When sodium and chlorine combine to form sodium chloride, sodium chloride is the:

a)

Originator

b)

Reactant

c)

Product

d)

Produce

43.
Is melting butter for popcorn a chemical or physical change?
a)
chemical
b)
physical
44.
Which of the following is a sign that a chemical reaction has occurred?
a)
change in shape
b)
melting
c)
formation of a gas
d)
dissolving
45.

How many Hydrogen atoms are in 4H2O?

a)

6

b)

8

c)

2

d)

4

46.

What does the subscript in a chemical formula tell you? (a)  

Choose from the below words
How many molecules are present
How many atoms are present
How many elements are present
How many neutrons are present
47.

How many elements are in this chemical formula?

H2SO4H_2SO_4  

a)

1

b)

2

c)

3

d)

4

48.

How many atoms of Carbon are in this formula? C6 H12O6C_{6\ }H_{12}O_6  

a)

6

b)

1

c)

12

49.

What elements are represented in this chemical formula? Fe2O3Fe_2O_3  

a)

Iron, Oxygen

b)

Francium, Europium, Oxygen

c)

Ferrium, Oxygen

d)

Berylium, Oxygen

50.

What is the total number of atoms in this formula? H2O2H_2O_2  

a)

2

b)

4

c)

3

51.

How many more atoms of Oxygen than than Magnesium are in this formula? (subtraction) MgSO4MgSO_4  

a)

4

b)

3

c)

2

d)

6

52.

Which of the following elements is least likely to form a compound?

a)

Hydrogen

b)

Sodium

c)

Argon

d)

Potassium

53.

Which of the following is a molecule of a compound?

a)

H2H_2

b)

Cl2Cl_2

c)

H2OH_2O

d)

F2F_2

54.

Which does not belong in the group?

a)

Sodium

b)

Glucose

c)

carbon

d)

Element

55.

Is this an element or a compound? CaSO4CaSO_4  

a)

Element

b)

Compound

56.

Which chemical formula correctly displays 1 atom of nickel and 2 atoms of Fluorine?

a)

niF2

b)

NIF2

c)

Ni1F2

d)

NiF2

57.

What is the total number of atoms in this chemical formula? C8H3NaBr12C_8H_3NaBr_{12}  

a)

18

b)

12

c)

25

d)

24

58.

Which element has the greatest number of atoms? AgNO3AgNO_3  

a)

Silver

b)

Gold

c)

Nitrogen

d)

Oxygen

59.

Molecules that are made of more than one type of atom are called?

a)

Molecules

b)

Elements

c)

Mixtures

d)

Compounds

60.

How many elements are in this chemical formula? NaHCO3NaHCO_3  

a)

1

b)

2

c)

3

d)

4

61.
Number of C's in 2Na₂CO₃
a)
1
b)
2
c)
3
d)
5
62.
How many Elements are in the compound C2H8O ?
a)
2
b)
1
c)
3
d)
0
63.
How many total atoms are in the compound C2H8O ?
a)
11
b)
2
c)
8
d)
1
64.
How many Sodium (Na) are in 6NaCl?
a)
1
b)
12
c)
6
65.
How many Chlorine are in MgCl2?
a)
2
b)
1
c)
3
66.
How many Magnesium are in 10MgCl2?
a)
10
b)
5
c)
20
67.
How many elements are in C6H12O6?
a)
1
b)
2
c)
3
d)
4
68.
Number of H in 3(NH₄)₂CrO₄
a)
4
b)
2
c)
8
d)
24
69.
How many atoms are there TOTAL in:
H2SO4
a)
6
b)
5
c)
7
d)
3
70.
Number of N in (NH₄)₂CrO₄
a)
1
b)
2
c)
8
d)
16
71.
How many valence electrons does nitrogen have?
a)
3
b)
2
c)
5
d)
1
72.
What can be generalized about covalent bonds?
a)
Electrons will be exchanged.
b)
Electrons will be transferred.
c)
Electrons will be given and taken.
d)
Electrons will be shared.
73.

What is it called if there are three-pairs of electrons being shared?

a)

Triple Bond

b)

Three Single Bonds

c)

Tribond

d)

Double and Single Bond Combo

74.

Which of the following is the best representation of a molecule of fluorine (F2)?

a)

A

b)

B

c)

C

d)

D

75.

Carbon is in 4A, so how many bonds can it form based on electrons needed to fill its outer shell?

a)

1

b)

3

c)

4

d)

5

76.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal & 1 Metal
c)
2 Metals
d)
2 Noble Gases
77.
What is a diatomic element?
a)
a metal bonded with a nonmetal
b)
2 or more nonmetals bonded together
c)
2 or more metals bonded together
d)
2 atoms of the same element bonded together
78.
How many electrons are shared in a double bond?
a)
2
b)
4
c)
6
d)
8
79.

What bond is formed between a metal and a nonmetal?

a)

Covalent bond

b)

Ionic bond

c)

Hydrogen bond

d)

Metallic bond

80.

When two nonmetals do not share electrons evenly, the resulting covalent bond will be

a)

nonpolar

b)

polar

c)

ionic

d)

metallic

81.

Since covalent compounds do not have free charges, they are

a)

good conductors

b)

poor conductors

c)

ionic

d)

metallic

82.
Most covalent compounds are do not exist in which state?
a)
solid
b)
liquid
c)
gas
83.
The number of bonds an element will form in a covalent compound will be equal to
a)
the number of valence electrons
b)
eight electrons
c)
the number of electrons needed to reach an octet
d)
the group number
84.

Which would be the only situation where valence electrons would be shared evenly?

a)

metals and nonmetals

b)

different nonmetals

c)

nonmetals of the same element

d)

metalloids of the same element

85.

Which formula is for phosphorus trichloride?

a)

KCl3

b)

PCl3

c)

K3Cl

d)

P3Cl

86.

Silicon dioxide is the compound in sand. What is its formula?

a)

SO2

b)

NaO2

c)

SiO2

d)

SiO

87.
The chemical formula of sulfur hexabromide is
a)
SBr₆
b)
S₆Br
c)
S(VI)Br
d)
S6Br
88.

What is the formula for diphosphorus pentoxide?

a)

P2O5

b)

PO5

c)

P5O2

d)

P2O6

89.
What is the correct name for NO?
a)
Mononitrogen Monoxide
b)
Nitrogen Monoxide
c)
Mononitrogen Dioxide
d)
Nitrogen Oxide
90.
Which of the following is NOT an ionic compound:
a)
CaO
b)
NaOH
c)
BaCl2
d)
Br2
91.
What is the name of N2O3
a)
Nitrogen trioxide
b)
Dinitrogen oxide
c)
Dinitrogen trioxide
d)
Nitrogen oxide
92.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
93.
What is the name of C3Cl8 ?
a)
Carbon octachloride
b)
Tricarbon octachloride
c)
Carbon trichloride
d)
Octacarbon trichloride
94.
What is the chemical formula for Nitrogen triiodide?
a)
NI
b)
N3I
c)
NI3
d)
None of these
95.
What is the name of Br6F10 ?
a)
Bromium fluoride
b)
Hexabromine fluoride
c)
Bromium decafluoride
d)
none of the above
96.
What is the name of CO
a)
Carbon oxide
b)
Carbon dioxide
c)
Carbon monoxide
d)
Carbon II oxide
97.
What is the chemical formula for CP ?
a)
Carbon phosphide
b)
Monocarbon phosphide
c)
Carbon monophosphide
d)
none of the above
98.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
99.
The chemical formula of sulfur hexabromide is
a)
SBr₆
b)
S₆Br
c)
S(VI)Br
d)
S6Br
100.
The chemical formula of dinitrogen textroxide is
a)
Ni₂O₄
b)
NiO
c)
N₂O₄
d)
NiO₂
101.
The chemical formula of tetraphosphorus heptaoxide is
a)
F₄O₁₀
b)
P₄O7
c)
PO
d)
P₁₀O₄
102.
What's the formula for chlorine dioxide
a)
ClO2
b)
CLO
c)
ClO3
d)
HClO2
103.
What is the formula for Hexaboron Monosilicide
a)
B6Si
b)
BSi
c)
BSi6
d)
B6Si6
104.
What is the OFFICIAL name for H2O
a)
Hydrogen Oxide
b)
Oxygen Dinitride
c)
Agua
d)
Dihydrogen Monoxide
105.
BrO3
a)
bromine oxide
b)
monobromine trioxide
c)
bromine trioxide
d)
bromine (III) oxide
106.
What is the formula for Tricarbon Octahydride?
a)
Ca3O
b)
C2H8
c)
C3H8
d)
Ca3H8
107.
A binary covalent bond exists between
a)
2 metals
b)
1 metal and 1 nonmetal
c)
2 nonmetals
d)
Any 2 elements
108.
Which of the following is NOT an ionic compound:
a)
CaO
b)
NaOH
c)
BaCl2
d)
Br2
109.
Which following is a molecular compound?
a)
SO2
b)
K2O
c)
CaO
d)
BeO
110.
Which of the following is NOT an ionic compound:
a)
CaO
b)
NaOH
c)
BaCl2
d)
CH4
111.

What is a positive ion called?

a)

anion

b)

cation

c)

isotope

d)

covalent

112.

What is a negative ion called?

a)

anion

b)

cation

c)

covalent

d)

isotope

113.

Which types of elements from cations?

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

114.

Which types of elements from anions?

a)

metals

b)

nonmetals

c)

metalloids

d)

noble gases

115.

Why do elements form bonds?

a)

to get a charge

b)

so they can make friends

c)

to become stable by getting a full valence shell

d)

to become stable by increasing their mass

116.

How many electrons would a Nitrogen ion gain/lose?

a)

lose 5

b)

gain 5

c)

lose 3

d)

gain 3

117.

How many electrons would a Calcium ion gain/lose?

a)

lose 1

b)

gain 1

c)

lose 2

d)

gain 2

118.

What is the ion formed from Sulfur?

a)

S+2

b)

S-2

c)

S+6

d)

S-6

119.

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

a)

true

b)

false

120.

A Bromine ion gains 1 electron, which of the following is the correct symbol for a Bromine ion?

a)

Br-1

b)

Br+1

c)

Br+7

d)

Br-7

121.

This image shows the bonding between Lithium and Fluorine. What does the red arrow show?

a)

electrons being shared

b)

electrons being transferred to Fluorine

c)

electrons being transferred to Lithium

d)

electrons being destroyed

122.

Which of the following is NOT a step in forming an ionic bond?

a)

One atom shares its electrons with another one

b)

Opposite charged ions form due to the transfer of electrons

c)

One atom gives electrons to another one

d)

Oppositely charged ions attract

123.

An ionic bond is the attraction between: (Select ALL that apply)

a)

oppositely charged ions

b)

similarly charged ions

c)

metals and nonmetals

d)

neutral atoms

e)

cations and anions

124.

Which of the following is the correct formula for these two ions: Al+3 & S-2

a)

AlS3

b)

Al2S3

c)

Al3S2

d)

Al3S

125.

If I had a cation with a charge of 2+ how would you describe the formation of that ion?

a)

gained 2 electrons

b)

lost 2 electrons

c)

gained 4 electrons

d)

lost 4 electrons

126.

If I had an anion with a charge of 3- how would you describe the formation of that ion?

a)

gained 2 electrons

b)

lost 2 electrons

c)

gained 3 electrons

d)

lost 3 electrons

127.

Looking at the periodic table, when the alkali metals form an ion what charge do they have?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

128.

Looking at the periodic table, when the alkaline earth metals form an ion what charge do they have?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

129.

Looking at the periodic table, when the halogens form an ion what charge do they have?

a)

1-

b)

1+

c)

2-

d)

2+

e)

3-

130.

Nitrogen, N, will form which of the following ions?

a)

N

b)

N-3

c)

N-5

d)

N+5

131.

In the compound aluminum oxide, which is the cation?

a)

[ Al ] +3

b)

Al

c)

[ O ] -2

d)

O

132.

When ionic compounds form what is the overall charge?

a)

neutral

b)

positive

c)

negative

133.

What is responsible for bringing cations and anions together?

a)

the size of the ions

b)

the opposite charges are attracted to one another

c)

the similar charges are attracted to one another

d)

depends on what period they're in

134.

What is another name of an ionic compound

a)

salt

b)

cation

c)

anion

d)

polyatomic ion

135.

Which is the correct name for CaBr2?

a)

Calcium Bromine

b)

Bromine Calcium

c)

Calcium Bromide

d)

Bromine Chloride

e)

Calcium Bromate

136.

What is the name for CsBr?

a)

Cesium Bromide

b)

Calcium Bromine

c)

Calcium Bromide

d)

Cesium Bromine

e)

Bromine Ceside

137.

Which of the following is the correct formula for Sodium Nitride ( [ Na ] + & [ N ] 3- )

a)

NaN3

b)

Na3N

c)

Na2N3

d)

Na3N2

138.

Which of the following is the correct formula for Potassium Sulfide

a)

K2S

b)

KS2

c)

K3S

d)

K2S3

139.

When assigning ionic charge it is always written as a...

a)

superscript

b)

subscript

c)

coefficient

d)

script

140.

When assigning the number of individual atoms in a chemical formula it is written as a...

a)

superscript

b)

subscript

c)

coefficient

d)

script

141.
Which of the following is an ionic compound:
a)
CH4
b)
I2
c)
LiBr2
d)
CO
142.
Name the following ionic compound: BeCl2
a)
beryllium chlorine
b)
beryllium II chloride
c)
beryllium chloride
d)
beryllium dichloride
143.
name the following ionic compound: NaF
a)
nitrogen fluorine
b)
sodium fluoride
c)
nitrogen fluoride
d)
sodium fluorine
144.
Which of these combinations is an ionic compound made of?
a)
Metal and Metal
b)
Nonmetal and Nonmetal
c)
Metal and Nonmetal
d)
Cation and Cation
145.
Name this compound: 
KF
a)
Potassium fluoride
b)
Potassium fluorite
c)
Fluorine potasside 
d)
Potassium fluorate
146.
What would be the proper chemical formula for combining Al3+ and Cl- :
a)
AlCl3
b)
Al3Cl
c)
AlCl
d)
Al3Cl3
147.
What formula results when Ca+2  and  Br- ions bond?
a)
Ca2Br2
b)
CaBr
c)
Ca(br)2
d)
CaBr2
148.

NaCl

a)

Sodium monochlorine

b)

Sodium chloride

c)

Sodium monochloride

d)

Sodium chlorine

149.

MgI2

a)

Magnesium Iodine

b)

Monomagnesium di-iodide

c)

Magnesium iodide

d)

Magnesium tetraiodide

150.

N2O

a)

Nitrogen Oxide

b)

Dinotrogen dioxide

c)

Nitrous dioxide

d)

Nitrogen Oxygen

151.

AlCl3

a)

Aluminum dichlorine

b)

Aluminum trichlorine

c)

Monoaluminum chloride

d)

Aluminum chloride

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