WorksheetsChemistry NCFE Review
Total questions: 30
Worksheet time: 40mins
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)
Both tend to have double and triple bonds
b)
Both tend to have low melting points
c)
Both tend to have poor conductivity
d)
Both tend to have high melting points
3.
Which element has the greatest atomic radius?
a)
H
b)
Na
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.
This graph represents data collected when a sample of a gas is uniformly cooled from 155°C. 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.
The phases of a substance under various pressure and temperature combinations are shown on this phase diagram. 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.
The potential energy diagram of a chemical reaction is shown below. 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 STP), is required to react with 15.0 g of NO?
6NO + 4NH3 5N2 + 6H2O
What volume of NH3 gas, (at 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.
This equation represents a chemical reaction at equilibrium.
HCl (aq) + Mg (s) <--> MgCl2 (aq) + H2 (g) + heat What happens to the system when the temperature is decreased?
HCl (aq) + Mg (s) <--> MgCl2 (aq) + H2 (g) + 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?
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.
A student conducts an experiment to identify the pH of some common household substances. The data is recorded in this table. 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.
Which is the electronic configuration of calcium?
a)
1s2 2s2 2p6 3s2 3p8
b)
1s2 2s2 2p6 3s2 3p6 4s2
c)
1s2 2s2 2p6 3s2 3p6 3d2
d)
1s2 2s2 2p8 3s2 3p6
18.
The half-life of a radioactive isotope is 20 minutes. What is the total amount of 1.00 g of sample of this isotope remaining after 1 hour?
a)
0.500 g
b)
0.333 g
c)
0.250 g
d)
0.125 g
19.
An unknown substance is tested in the laboratory. The physical test results are:
Nonconductor of electricity
Insoluble in water
Soluble in oil
Low melting point
Based on these results, what is the unknown substance?
Nonconductor of electricity
Insoluble in water
Soluble in oil
Low melting point
Based on these results, what is the unknown substance?
a)
ionic and polar
b)
ionic and nonpolar
c)
covalent and polar
d)
covalent and nonpolar
20.
Arrange the following elements in order of increasing electronegativity, from lowest to highest: F, K, Si, and S.
a)
F < K < S < Si
b)
K < Si < S < F
c)
Si < F < K < S
d)
S < Si < F < K
21.
1000 J of heat is added to 2 g of the following substances. Which one will experience the biggest change in temperature?
a)
aluminum
b)
copper
c)
iron
d)
lead
22.
A student mixes two chemicals in a test tube. The test tube turns hot and bubbles appear. What indicators of chemical reaction is the student observing?
a)
Change in color and formation of precipitate.
b)
Change in color and formation of gas.
c)
Change in temperature and formation of precipitate
d)
Change in temperature and formation of gas.
23.
Consider this combustion reaction equation: C4H10 + O2 --> CO2 +H2O When the equation is balanced, what will be the coefficient of O2?
a)
1
b)
7
c)
10
d)
13
24.
How many grams of KCl are required to make a saturated solution in 50.0 g of water at 80oC?
a)
25.0 g
b)
50.0 g
c)
100.0 g
d)
150.0 g
25.
A compound consisting of 56.38% phosphorus and 43.62% oxygen has a molecular mass of 220 g/mole. What is the molecular formula of this compound?
a)
PO
b)
PO2
c)
P2O3
d)
P4O6
26.
When a set amount of marble chips (CaCO3) is added to a small amount of dilute hydrochloric acid, a reaction occurs. What should be done to decrease the rate of reaction the next time the experiment is performed?
a)
Use more acid
b)
Stir
c)
Use larger marble chips
d)
Add heat
27.
What volume of 0.200M HCl will neutralize 10.0mL of 0.400M KOH?
a)
20.0 mL
b)
40.0 mL
c)
8.00 mL
d)
5.00 mL
28.
Given the balanced chemical equation the reaction, P4 + 5O2 --> P4O10 What mass of oxygen is needed to completely react with 7.75 g P4 ?
a)
2.00 g
b)
5.00 g
c)
10.00 g
d)
40.00g
29.
What causes an inflated balloon to shrink when it is cooled?
a)
because cooling the balloon causes gas to escape from the ball
b)
because cooling the balloon causes the gas molecules to collide more frequently
c)
because cooling the balloon causes gas molecules to become smaller
d)
because cooling the balloon causes the average kinetic energy of the gas molecules to decrease
30.
What causes the process of perspiration to be cooling for human skin?
a)
It involves condensation and is exothermic.
b)
It involves evaporation and is exothermic
c)
It involves condensation and is endothermic
d)
It involves evaporation and is endothermic.
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