Knierim – Semester 2 Final Study Guide
Unit 5: Bonding
1.
a. Where are valance electrons found? _______________________________
b. On the picture below, label where valance electrons are found.
1. Why are valance electrons important?
2. How many valance electrons does each atom want to have?
____________
2. Draw the Lewis Dot structure for each of the following molecules:
P2
NF3
3. The best Lewis dot structure of phosphorus is
A.
P
B.
P
C.
4. Which element is more electronegative?
5. Which element is less electronegative?
6.
Molecule
H2S
Lewis Structure
Central
Atom
(C.A.)
P
D.
Cl
Li
or
or
Atoms
attached to
C.A.
Lone Pairs
on C.A.
P
Ca
Cs
VSEPR
Shape
Unit 5 & 6: NOMENCLATURE
7.
An ionic bond is formed by
A. sharing electrons equally.
B. sharing electrons unequally.
C. transferring electrons to the non-metal.
D. transferring electrons to the metal.
8. Which is the number of hydrogen atoms in one molecule of ammonium sulfide, (NH4)2S?
A. 1
B. 2
C. 4
D. 8
9.
What is the name of Fe2O3?
A. iron oxide
B. diiron trioxide
C. iron(II) oxide
D. iron(III) oxide
10. What is the name of N2O?
A. nitrogen oxide
B. dinitrogen monoxide
C. nitrogen monoxide
D. nitrogen dioxide
11. What is the name of CaCl2?
A. calcium dichloride
B. calcium (II) chloride
C. calcium chlorate
D. calcium chloride
12. What is the name of Na2CO3?
A. disodium carbon trioxide
B. sodium carbonate
C. sodium carbide
D. sodium(I) carbonate
13. What is the formula for calcium nitrate?
A. CaNO3
B. CNO3
C. Ca2NO3
D. Ca(NO3)2
14. What is the formula for tin(IV) sulfate?
A. TiSO4
B. SnSO4
C. Sn2(SO4)4
D. Sn(SO4)2
15. What is the formula for aluminum phosphide?
A. AlP
B. Al2PO4
C. AlP2
D. Al2P3
16. What is the correct formula dinitrogen tetraoxide?
A. HNO2
B. H2O
C. N2O4
D. OH
17. What is the correct formula for magnesium hydroxide?
A. MgOH
B. MgOH2
C. Mg(OH)2
D. MgO
18. Does an anion have a positive or negative charge?
______________________
19. Do the metals have a positive or negative charge?
______________________
20. In an ionic bond, are electrons shared or stolen?
______________________
21. Barium has a charge of +2, did it gain or lose electrons?
______________________
Unit 7: REACTIONS
22. If an equation is balanced properly, both sides of the equation must have the same number of
A. atoms
B. coefficients
C. molecules
D. moles of molecules
23. What is the correct order of coefficients for the following unbalanced equation?
___ AlCl3 + ___ H2O  ___ HCl + ___ Al2O3
A.
B.
C.
D.
3, 2, 1, 6
2, 3, 6, 1
4, 2, 1, 1
1, 3, 1, 2
24. What is the correct order of coefficients for the following unbalanced equation?
__ CO2 + __H2O  __C2H6 + __O2
A.
B.
C.
D.
2, 3, 1, 7
4, 6, 2, 7
2, 3, 1, 3
3, 2, 1, 2
25. What is the correct order of coefficients for the following unbalanced equation?
____ Cu(OH)2 + ____ Al  ____ Al(OH)3 + ____ Cu
A. 2 , 3, 1, 2
B. 3, 4, 3, 3
C. 2, 1, 3, 1
D. 3, 2, 2, 3
26. Which of the following reactions best describes a double replacement reaction?
A. 3 O2 + S  2 SO3
B. Pb(NO3)2 + 2 K  2 KNO3 + Pb
C. CuCl2 + 2 AgNO3  2 AgCl + Cu(NO3)2
D. C12H20 + 17 O2  12 CO2 + 10 H2O
27. A reaction in which a hydrocarbon reacts with oxygen and a large amount of heat and light are produced is
called:
A. single replacement
B. synthesis
C. combustion
D. decomposition
28. Which type of reaction best describes the following reaction: (NH4)2CO3  NH3 + H2O + CO2
A. single replacement
B. double replacement
C. decomposition
D. hydrocarbon combustion
29. Given the reactants on the right, identify all products that will be formed:
A. LiCl
B. LiCl + Zn
C. Li2Zn + Cl
D. Cl2Li + Zn
30. Given the reactants on the right, predict the products in the chemical reaction.
A. NaCl + CaCO3
B. Na2Cl2 + CaCO3
C. Na2Ca + Cl2CO3
D. Na + Ca + CO3 + Cl2
Li + ZnCl2 
Na2CO3 + CaCl2 
31. When aluminum and bromine gas combine, what will be produced?
A. AlBr
B. AlBr2
C. AlBr3
D. Al + Br2
Directions: Place a checkmark by the statements that describe evidence of a chemical reaction.
32.________ An icicle melted into liquid water.
33.________ When copper wire was added to H2SO4, the clear liquid turned blue.
34.________ A piece of aluminum foil was ripped into two pieces.
35.________ When baking soda and vinegar are combined, gas bubbles are produced.
36.________ Aluminum foil was placed in a solution and red clumps formed.
Unit 8: Kinetics
37. Raising the temperature of reactants speeds up the rate of a chemical reaction by increasing
A. only the energy of the collisions.
B. only the frequency of the collisions.
C. neither the energy nor the frequency of the collisions.
D. both the energy and the frequency of the collisions.
38. Increasing the concentration of aqueous reactants speeds up the rate of a chemical reaction by increasing
A. only the energy of the collisions.
B. only the frequency of the collisions.
C. both the energy and the frequency of the collisions.
D. neither the energy nor the frequency of the collisions.
39. All of the following statements about the effect of a catalyst on a reaction are true EXCEPT?
A. A catalyst provides a new pathway for the reaction to occur more rapidly.
B. The catalyst lowers the heat of reaction, ΔH.
C. The catalyst lowers the activation energy, Ea, for a reaction.
D. The catalyst increases the reaction rate.
40. When a cube of zinc is added to hydrochloric acid, the reaction is slow. Which procedure would increase
the rate of reaction if the reaction were repeated?
A. Using powdered zinc
B. Using hydrochloric acid with a lower molarity
C. Decreasing the temperature
D. Increasing the atmospheric pressure.
Consider the diagram shown to the right and the following reaction for questions 58-60.
A(g) + B(g) ↔ C(g) + D(g)
41. What is the heat of reaction (ΔH) for the forward
reaction?
A. -20 kJ/mole
B. +20 kJ/mole
C. +40 kJ/mole
D. +60 kJ/mole
42. What is the activation energy, Ea, for the forward
reaction?
A. 20 kJ/mol
B. 40 kJ/mol
C. 60 kJ/mol
D. 80 kJ/mol
43. What is the energy of the activated complex for this reaction?
A. 20 kJ/mol
B. 40 kJ/mol
C. 80 kJ/mol
D. 100 kJ/mol
Unit 8: Nuclear Reactions;
44. Describe the difference between fusion and fission.
45. How are nuclear and chemical reactions similar?
46. How are nuclear and chemical reactions different?
47. Write the nuclear equation for the following alpha decay.

Create a diagram to demonstrate the nuclear reaction from start to finish, illustrating what is happening to the nucleus.
(Creating 6 pts).
14
6𝐶

Directions: Predict the products for the nuclear equation for the following beta decay. (Understanding 2pts)
48.
237
93𝑁𝑝

49. What is the difference between an ion and an isotope?
Unit 9: MOLES
50. Avogadro’s number, 6.02 x 1023, is
B. the mass of molecules in 1 mole of pure substance
C. the number of molecules in 1 mole of pure substance
D. the number of atoms in a chemical formula
E. the number of molecules in exactly 1 g of pure substance
51. The molar mass of aluminum nitrate, Al(NO3)3 , is
A. 57.0 g/mole
B. 89.0 g/mole
C. 185.0 g/mole
D. 213.0 g/mole
52. If a student measured 15 grams of lead on a balance, which of the following would describe how a student
could convert that mass to moles?
A. multiply 15 by the molar mass
B. divide 15 by the molar mass
C. divide the molar mass by 15
D. multiply by 6.022 x 1023
53. Calculate the mass of 0.461 moles of NiSO4.
A. 2.77 x 1023 grams NiSO4
B. 71.4 grams NiSO4
C. 0.00298 grams NiSO4
D. 7.66 x 10-25 grams NiSO4
54. How many grams of carbon dioxide are present in 0.0578 moles?
A. 2.54 grams
B. 0.0013 grams
C. 3.48 x 1022 grams
D. 9.60 x 10-26 grams
55. Calculate the number of moles given 2.49 x 1023 molecules of H2O.
A. 0.414 moles H2O
B. 1.50 x 1047 moles H2O
C. 1.38 x 1022 moles H2O
D. 4.48 x 1024 moles H2O
56. How many molecules of H2O2 are present in 2.00 moles?
A. 6.02 x 1023 molecules
B. 1.20 x 1024 molecules
C. 3.32 x 10-24 molecules
D. 2.00 molecules
57. The amount of molecules in 150 g of potassium chloride (KCl) is
A. 1.8 x 1026 molecules
B. 1.2 x 1024 molecules
C. 2.0 molecules
D. 3.3 x 10-22 molecules
58. How many grams of H2O are present in 5.44 x 1024 molecules of H2O?
A. 298 grams
B. 9.04 grams
C. 1.63 x 1048 grams
D. 163 grams
STOICHIOMETRY
59. The purpose of stoichiometry is to
A. Calculate moles
B. Balance equations
C. Predict amounts
D. Determine the density
Use the following reaction to answer the next three questions:
2AgNO3 + Mg  Mg(NO3)2 + 2 Ag
60. How many moles of silver are produced when two moles of silver nitrate react with one mole of
magnesium?
A. 1
B. 2
C. 3
D. 4
61. How many moles of magnesium are needed to completely react with 4 moles of silver nitrate?
A. 1
B. 2
C. 3
D. 4
62. If four moles of magnesium nitrate are produced, how many moles of magnesium are needed?
A. 1
B. 2
C. 3
D. 4
Use the following equation for the next three questions:
2Fe + 3H2SO4  3H2 + Fe2(SO4)3
63. When the reaction occurs, what is the mole ratio between Fe and H2?
A. 1 mole Fe to 1 mole H2
B. 1 mole Fe to 3 mole H2
C. 2 mole Fe to 1 mole H2
D. 2 mole Fe to 3 mole H2
64. If the reaction began with 6 moles of H2SO4, how many moles of H2 would be produced?
A. 1 mole
B. 2 moles
C. 3 moles
D. 6 moles
65. If 10.5 moles of iron(III) sulfate is produced, how many moles of iron would have reacted?
A. 10.5 mole
B. 21.0 moles
C. 5.25 moles
D. 2.00 moles
Unit 10: Gases
66. When a sample of CO2 gas is heated, the CO2 molecules will
A. get larger.
B. get smaller.
C. move faster.
D. move slower.
67. If a sample of gas is subjected to a higher pressure with no change in temperature, then
A. the number of gas molecules will decrease.
B. the number of gas molecules will increase.
C. the volume of the gas sample will decrease.
D. the volume of the gas sample will increase.
68. The amount of force per unit area exerted by a gas on the walls of its container is called the gas
A. volume.
B. energy.
C. temperature.
D. pressure.
69. The temperature of a substance is best described as a measurement of its particles’
A. heat energy.
B. average kinetic energy.
C. molecular velocity.
D. pressure.
70. A sample of ammonia gas is released from a flask in an open classroom. Its odor is detected after a
short time all over the classroom. This is because the ammonia molecules
A. move randomly in all directions.
B. bond with air molecules.
C. have a high pressure compared to the atmosphere
D. have a higher kinetic energy than air.
71. Consider a sample of air trapped in a syringe at a constant temperature. Which of the following is true?
A. When more pressure is applied to the plunger on the syringe, the volume of the trapped air decreases.
B. When more pressure is applied to the plunger on the syringe, the volume of the trapped air increases.
C. When more pressure is applied to the plunger on the syringe, trapped air molecules move farther apart.
D. When more pressure is applied to the plunger on the syringe, the trapped air molecules move slower.
72. Suppose a balloon filled with helium gas is carried from inside a warm building, outside into a cold
winter
day. Which of the following is true?
A. When the temperature of the balloon decreases, its volume also decreases.
B. When the temperature of the balloon decreases, its volume increases.
C. When the temperature of the balloon decreases, the helium atoms inside of it hit the balloon harder.
D. When the temperature of the balloon decreases, the helium atoms inside the balloon leak out of it faster.
73. Which of the following describes the reason the gas pressure in a container (of fixed size and at constant
temperature) increases when more particles of a gas are added?
A. The gas particles in the container collide with one another with a greater impact force.
B. The gas particles in the container collide with one another more frequently.
C. The gas particles in the container hit the sides of the container with a greater impact force.
D. The gas particles in the container hit the walls of the container more frequently.
74. Which of the graphs below shows the relationship between volume and pressure for a fixed number of
moles of gas at constant temperature?
Pressure
D.
Pressure
Volume
Volume
C.
Volume
B.
Volume
A.
Pressure
Pressure
75. A sample of gas with a constant volume is at 283 K and 1.00 atm. What will the gas pressure be if its
temperature is increased to 373 K?
A. 0.759 atm
B. 1.32 atm
C. 2.39 atm
D. 7.59atm
76. Suppose a 100 mL sample of a gas is measured at a temperature of 100 K and a pressure of 400 mmHg. If
the gas is heated to a temperature of 400 K and the pressure changes to 800 mm Hg, what is the
resulting volume of the gas?
A. 100 mL
B. 200 mL
C. 300 mL
D. 400 mL
77. A balloon containing helium gas has a volume of 3.0 L at 1.5 atm. What will be the volume of the balloon
if the pressure is increased to 4.5 atm?
A. 1.0 Liters
B. 1.5 Liters
C. 3.0 Liters
D. 9.0 Liters
78. If a 200. L container is filled with nitrogen at a pressure of 1.00 atm, how many moles of nitrogen are
present at 298K? (R = 0.0821atmL/molK)
A. 0.122 moles
B. 8.17 moles
C. 19.3 moles
D. 97.5 moles
Refer to the following phase diagram for a pure substance in order to answer questions
34-36.
79. As the temperature increases from point C to point D what happens to the substance?
A. The solid state gets warmer, melts, and then the liquid state gets warmer.
B. The liquid state gets warmer, boils, and then the gas state gets warmer.
C. The gas state gets cooler, condenses, and then the liquid state freezes.
D. The solid state gets warmer, sublimes, and then the gas state gets warmer.
80. The point labeled “A” on the diagram is known as the______ of the substance.
A. critical point
B. triple point
C. boiling point
D. origin
81. At a high pressure and a low temperature, the state of matter most likely to exist is the _____ state.
A. solid
B. liquid
C. gas
D. ionic