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WorksheetsNCFE - Chemistry 2016
Total questions: 40
Worksheet time: 39mins
Name
Class
Date
1.
What is the chemical formula for magnesium bromate?
a)
MgBr
b)
MgBr2
c)
MgBrO3
d)
Mg(BrO3)2
2.
How are compounds with metallic bonds similar to ionic compounds?
a)
have double and triple bonds
b)
low boiling points
c)
poor conductivity
d)
high melting points
3.
Which of these elements has the greatest atomic radius?
a)
H
b)
N
c)
Cl
d)
Cs
4.
How does the amount of heat energy change as a 250-g sample of water is heated from 5.0°C to 30.0°C?
a)
The amount of heat energy increases, causing the water to sublime.
b)
The amount of heat energy increases, causing the water to evaporate.
c)
As the temperature increases, the amount of heat energy decreases.
d)
As the temperature increases, the amount of heat energy increases.
5.
Why does the temperature of the sample remain constant between point X and point Y?
a)
because the sample is transitioning from a gaseous state to a solid state
b)
because the sample is transitioning from a gaseous state to a liquid state
c)
because the sample is transitioning from a solid state to a gaseous state
d)
because the sample is transitioning from a liquid state to a solid state
6.
What occurs if the pressure of the substance at point F remains constant, and the temperature increases to point G?
a)
It will transition from a solid state to a liquid state.
b)
It will transition from a liquid state to a solid state.
c)
It will transition from a solid state to a gaseous state.
d)
It will transition from a gaseous state to a solid state.
7.
Which best describes the energy in the chemical reaction?
a)
Heat energy was released.
b)
Energy was lowered by a catalyst.
c)
8 J of energy were required to start the reaction.
d)
10 J of energy were required to start the reaction.
8.
This balanced chemical equation represents a chemical reaction:
6NO + 4NH3 → 5N2 + 6H2O
What volume of NH3 gas, at Standard Temperature and Pressure (STP), is required to react with 15.0 g of NO?
6NO + 4NH3 → 5N2 + 6H2O
What volume of NH3 gas, at Standard Temperature and Pressure (STP), is required to react with 15.0 g of NO?
a)
5.68 L
b)
7.47 L
c)
10.0 L
d)
11.2 L
9.
The equation represents a chemical reaction at equilibrium.
2HCl + Mg --> MgCl2 + H2 + heat
What happens to the system when the temperature is decreased?
2HCl + Mg --> MgCl2 + H2 + heat
What happens to the system when the temperature is decreased?
a)
The reaction shifts toward the right, and the amount of hydrogen gas increases.
b)
The reaction shifts toward the right, and the amount of hydrogen gas decreases.
c)
The reaction shifts toward the left, and the amount of hydrogen gas increases.
d)
The reaction shifts toward the left, and the amount of hydrogen gas decreases.
10.
This equation represents a chemical reaction at equilibrium:
2SO2(g)+O2(g) --> 2SO3(g)
What will happen when the concentration of SO3 is increased?
2SO2(g)+O2(g) --> 2SO3(g)
What will happen when the concentration of SO3 is increased?
a)
The reaction shifts to the right, and concentrations of SO2 (g) and O2 (g) decrease.
b)
The reaction shifts to the right, and concentrations of SO2 (g) and O2 (g) increase.
c)
The reaction shifts to the left, and concentrations of SO2 (g) and O2 (g) decrease.
d)
The reaction shifts to the left, and concentrations of SO2 (g) and O2 (g) increase.
11.
Which substance would be classified as containing the highest concentration of hydroxide ions?
a)
Ammonia
b)
Drain Cleaner
c)
Lemon Juice
d)
Vinegar
12.
A newly synthesized ionic compound is placed in water to make an aqueous solution. Which best describes the new ionic solution?
a)
The ionic solution conducts electricity.
b)
The ionic solution dissolves nonpolar solutions.
c)
The ionic solution cannot conduct electricity.
d)
The ionic solution is a neutral solution.
13.
Why is potassium chloride able to dissolve in water?
a)
because potassium ions are attracted to the partial negative charge of hydrogen
b)
because potassium ions are attracted to the partial positive charge of hydrogen
c)
because potassium ions are attracted to the partial negative charge of oxygen
d)
because potassium ions are attracted to the partial positive charge of oxygen
14.
Which occurs if an electron transitions from n = 5 to n = 2 in a hydrogen atom?
a)
Energy is absorbed, and visible light is emitted.
b)
Energy is released, and visible light is emitted.
c)
Energy is released, and visible light is not emitted.
d)
Energy is absorbed, and visible light is not emitted.
15.
When a gamma ray is emitted by an element, what happens to the atomic mass and the atomic number?
a)
The atomic mass stays the same, and the atomic number stays the same.
b)
The atomic mass changes, and the atomic number stays the same.
c)
The atomic mass stays the same, and the atomic number changes.
d)
The atomic mass changes, and the atomic number changes.
16.
How does a single covalent bond between two carbon atoms compare to a double covalent bond between two carbon atoms?
a)
A single covalent bond is stronger and has a longer bond length than a double covalent bond.
b)
A single covalent bond is stronger and has a shorter bond length than a double covalent bond.
c)
A single covalent bond is weaker and has a shorter bond length than a double covalent bond.
d)
A single covalent bond is weaker and has a longer bond length than a double covalent bond.
17.
How do the three isotopes Sn-116, Sn-118, and Sn-119 differ?
a)
Sn-116 has 166 neutrons, Sn-118 has 168 neutrons, and Sn-119 has 169 neutrons.
b)
Sn-116 has 116 neutrons, Sn-118 has 118 neutrons, and Sn-119 has 119 neutrons.
c)
Sn-116 has 66 neutrons, Sn-118 has 68 neutrons, and Sn-119 has 69 neutrons.
d)
Sn-116 has 50 neutrons, Sn-118 has 52 neutrons, and Sn-119 has 53 neutrons.
18.
Which molecule contains a triple bond?
a)
F2
b)
O2
c)
Cl2
d)
N2
19.
Which of these compounds will form a precipitate when mixed with an aqueous solution of sodium sulfate, Na2SO4?
a)
LiNO3
b)
KNO3
c)
Mg(NO3)2
d)
Ba(NO3)2
20.
Solid chromium(II) reacts with oxygen gas to form solid CrO. What is this type of reaction?
a)
decomposition
b)
synthesis
c)
single replacement
d)
double replacement
21.
Which element has 8 valence electrons?
a)
potassium
b)
oxygen
c)
helium
d)
neon
22.
How are the bonds formed in a polar covalent compound?
a)
Electrons are shared unequally.
b)
Electrons are shared equally.
c)
Electrons are gained.
d)
Electrons are lost.
23.
In a chemical reaction, how does increasing the temperature of the reactants affect the reaction process?
a)
The reactants absorb more heat, which turns them into products faster.
b)
The activation energy is decreased, which makes the reaction proceed faster .
c)
The kinetic energy of the reactants increases, causing more effective collisions.
d)
The particles break down faster, increasing the surface area and the reaction rate.
24.
Which best represents the electron configuration for an atom of iron?
a)
[Ar]4s23d6
b)
[Ar]4s2
c)
[Ar]3s23p63d8
d)
[Ar]4s24d6
25.
What is the mass number of the element represented by X?
a)
It is 88, because element X gains 2 protons.
b)
It is 218, because element X loses 2 protons and 2 neutrons.
c)
It is 220, because element X loses 2 neutrons.
d)
It is 226, because element X gains 2 protons and 2 neutrons.
26.
When aluminum and sulfur react, which compound is produced?
a)
Al2S3
b)
Al3S2
c)
AlS2
d)
AlS
27.
Which combination of elements would most likely form an ionic compound?
a)
hydrogen and oxygen
b)
carbon and chlorine
c)
sodium and fluorine
d)
silicon and sulfur
28.
Which group includes elements with the most similar properties?
a)
N, O, and F
b)
O, S, and Se
c)
Cr, Pb, and Xe
d)
Br, Ga, and Hg
29.
An atom of which element has the strongest attraction for electrons?
a)
Ba
b)
Cs
c)
O
d)
F
30.
The chemical equation below represents an unbalanced chemical reaction:
Fe + O2 --> Fe2O3
When the equation is balanced, what coefficient is needed for Fe2O3?
Fe + O2 --> Fe2O3
When the equation is balanced, what coefficient is needed for Fe2O3?
a)
1
b)
2
c)
3
d)
4
31.
How much mass is in a 3.25-mole sample of NH4OH?
a)
10.8 g
b)
34.0 g
c)
35.1 g
d)
114 g
32.
Why is KOH considered to be an Arrhenius base?
a)
It produces OH+ ions in solution.
b)
It produces H+ ions in solution.
c)
It produces H- ions in solution.
d)
It produces OH- ions in solution.
33.
At what temperature will 50 g of NH4Br produce a saturated solution when dissolved in 100 g of water?
a)
46°C
b)
54°C
c)
60°C
d)
66°C
34.
How many protons and electrons are in a Cu2+ ion?
a)
27 protons, 29 electrons
b)
27 protons, 31 electrons
c)
29 protons, 27 electrons
d)
29 protons, 31 electrons
35.
In an experiment, 2.62 g of iron react completely with 1.50 g of sulfur. What is the empirical formula for the compound produced?
a)
FeS
b)
FeS2
c)
Fe2S
d)
Fe2S3
36.
What do the ions K1+, Ca2+, and Cl1− have in common?
a)
They have the same number of protons.
b)
They will form covalent bonds with oxygen.
c)
They have the same electron configuration as argon.
d)
They are larger than their corresponding atoms.
37.
Neutralization occurs when 15.0 mL of KOH react with 25.0 mL of HNO3. If the molarity of HNO3 is 0.750 M, what is the molarity of the KOH?
a)
1.67 M
b)
1.25 M
c)
0.600 M
d)
0.450 M
38.
A gas under a pressure of 74 mmHg and at a temperature of 75°C occupies a 500.0-L container. How many moles of gas are in the container?
a)
1.7 moles
b)
7.9 moles
c)
13 moles
d)
59 moles
39.
When a piece of metal was heated and dropped into a foam cup calorimeter filled with 200mL of water at 22.5oC, the temperature of the water rose to 38.7oC. How much heat was transferred from the metal to the water?
a)
18.8 kJ
b)
13.5 kJ
c)
23.7 kJ
d)
32.3 kJ
40.
When a chemical cold pack is activated, it becomes cool to the touch. What is happening in terms of energy?
a)
An exothermic reaction is occurring, absorbing cold from its surroundings.
b)
An exothermic reaction is occurring, releasing heat to its surroundings.
c)
An endothermic reaction is occurring, releasing cold to its surroundings.
d)
An endothermic reaction is occurring, absorbing heat from its surroundings.
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