Name __________________________
Chemistry Final Exam: Practice Problems
Per. __________
1. Key Vocabulary/Terms:
atm
empirical formula
atomic number
torr
balanced equation
element
Combined
Gas
law
heat
compound
Ideal Gas Law
temperature
kinetic theory
kPa
specific heat
acid
ion
heat capacity
base salt
ionic bond
Joule
vaporization
covalent bond
Calorie
condensation
Kelvin
calorie
evaporation
Celsius
Conservation of mass
boiling
mole
Conservation of energy
sublimation
Avogadro’s number
diffusion
energy level
endothermic
effusion
valence electron
exothermic
isotope(s)
metal
octet
rule
representative elements
nonmetal
solid
transition elements (metals)
metalloid
liquid
(Lewis) electron dot diagrams
Charles’ law
gas
catalyst
Boyle’s Law
molar mass
Gay-Lussac’s law
Problems/Concepts: Know (memorize) and be able to apply the following equivalents, relationships, formulas, etc.:
P × V = P × V (Boyle’s)
V
V
--- = ---- (Charles’)
T
T
Moles
=
mass
(g)
/ molar mass
P
P
----- = ----- (Gay-Lussac)
T
T
P xV
P xV
---------- = ----------- (Combined)
T
T
PV = nRT or… n = PV/RT (remember R = 8.31) (Ideal)
P = P + P + P + … (partial pressure)
4.184 J = 1 cal
1 J = 0.2390 cal
q (heat in joules or calories)
C = -------------
m· T
q = C·m· T
q = s·m· T
moles of solute
Molarity
= ------------------------liters of solvent
Moles of solute = Molarity (M) x Liters of solution
Dilution:
MV =MV
or N V = N V
D = m/v
1. Find the following temperatures in Kevin:
a. 0 °C = _______
b. 23 °C = _______
c. 100 °C = _______ d. -273°C = _______
temperatures in °C:
2. Finda.the0 Kfollowing
= _______
b. 100 K = _______
c. 373 K = _______
d. 273 K = ________
STP in…
3. Define
K and mmHg
_______________________
K and kPa
_______________________
K and atm
_______________________
K and torr
_______________________
°C and kPa
_______________________
°C and mmHg
_______________________
°C and torr
_______________________
°C and atm
_______________________
________________________
4. Which of the above is the SI unit for pressure?
________________________
5. How many atoms are in a mole of any element?
6. Which of the above have the same numerical value?
________________________
7. Fill in the blanks: 1 atm = _____ mmHg = ______ torr = ______ kPa
8. What kinds of atoms form covalent bonds? _________________________________________________
9. What kinds of atoms form ionic bonds? _________________________________________________
1
1
1
2
2
1
2
1
2
1
2
1
2
1
1
2
1
total
1
2
2
2
3
1
1
2
2
1
1
2
2
Name __________________________
Chemistry Final Exam: Practice Problems
Per. __________
10. Which of the following would form covalent (C), which would form ionic (I) bonds and which would not bond (N)?
a. Ca & Cl ______
b. S & O ______
c. Mg & Fe ______
d. C & H _____
11. What is meant by an atom’s the ground state and atoms that have ‘excited electrons?
_______________________________________________________________________________
12.
How
can you identify atoms that have the same number of electrons in their highest occupied energy (valence )
levels?
_______________________________________________________________________________
13. How can you identify atoms that have similar chemical properties?
_______________________________________________________________________________
_____________________________________________
14. Where are the metals located in the periodic table?
_____________________________________________
15. Where are the nonmetals located in the periodic table?
_____________________________________________
16. Where are the metalloids located in the periodic table?
Describe each of the following types of chemical reactions:
17. Combination/Synthesis:
________________________________________________________________________
18. Decomposition:
________________________________________________________________________
19. Single replacement:
________________________________________________________________________
20. Double replacement:
________________________________________________________________________
21. Combustion:
________________________________________________________________________
22. In any period of the periodic table, what kind of changes occur as you go from left to right?
a. ______________________________ (atomic radius)
b. ______________________________ (ionization energy)
c. ______________________________ (electronegativity)
d. ______________________________ (metallic character)
23. What happens to atomic size (radius) as you go down a column (group) and why?
________________ / _______________________________________________________________________
24. What happens to atomic size (radius) as you go across a period and why?
________________ / _______________________________________________________________________
25. Which of the following elements would have the greatest atomic radius?
a. P
b. F
c. Cl
26. Which
of the following elements would have the greatest ionization energy?
a. P
b. F
c. Cl
27. What do all acids contain?
______________________________________________
28. What do all bases contain?
______________________________________________
29. What is a salt?
______________________________________________________________
30. Neutralization reaction result in what kinds of products? _______________ & _______________
31. What term is used when a substance like CO2 turns directly from a solid to a gas? ____________________
32. __________________________ A 47.7-g piece of copper increases from 25.0°C to 48.0°C when it absorbs 425 J
of heat. What is the specific heat of copper? (show your work)
33. Circle which units can be used to measure heat flow: Joules moles degrees calories(c)
kilocalories (C)
34. What is the octet rule? ______________________________________________________________________
35. If a compound’s name ends with “-ate” or “-ite” it must contain ____________________.
2
Chemistry Final Exam: Practice Problems
In a graph below …
36. Where is the substance only a solid?
___________
37. Where is the substance only a liquid?
___________
38. Where is the substance only a gas?
___________
39. Where is the substance turning from liquid to gas?
___________
40. Where is the substance solid to liquid?
___________
Name __________________________
Per. __________
E
D
C
B
A
41. How do cations form and what type of element(s) form(s) them? _______________________________________
42. How do anions form and what type of element(s) form(s) them? _______________________________________
43. At STP what is the volume of 1 mole of any gas?
_____________________
44. What is the relationship between the size of a gas molecule and diffusion and effusion?
_________________
_______________________________________________________________________________________
45. At the same temperature and pressure, which gas will move fastest (and therefore diffuse or effuse faster)?
a. H2
b. O2
c. N2
d. Ar
0___1___2___4___5___6___7___8___9__10__11__12__13__14
46. On a pH scale like the one above…
a. … where would bases fall?
b. … where would neutral substances fall?
c. … where would bases fall?
__________
__________
__________
47. If you decrease the volume of a container holding a gas without changing temperature of the gas what happens to its
pressure. ___________________________________________________
48. At what temperature will water boil when the external pressure is 115.5 mmHg? (Initial conditions are at STP)
_______________________________
49. If you triple the temperature of a gas in a rigid inflexible container, what happens to its pressure?
___________________________________________________
50. In terms of arrangement and movement of particles what is the difference between a solid, a liquid and a gas?
__________________________________________________________________________________________________
__________________________________________________________________________________________________
__________________________________________________________________________________________________
51. In terms of volume and shape what is the difference between a solid, a liquid and a gas?
__________________________________________________________________________________________________
__________________________________________________________________________________________________
__________________________________________________________________________________________________
52.
The formation of aluminum oxide is expressed in the following reaction:
Balance the equation:
______ Al + ______ O2
How many moles of aluminum are needed to form 3.7 moles of Al2O3?
3
______ Al2O3
______________________
Chemistry Final Exam: Practice Problems
Name __________________________
Per. __________
53. Acetylene gas (C2H2) is produced by adding water to calcium carbide (CaC2).
CaC2 + 2H2O
C2H2 + Ca(OH)2
54. How many grams of acetylene are produced by adding water to 5.00 g CaC2?
55. What is molar mass?
______________________
__________________________________________________________________
56. What is and how do you calculate the molar mass of CuSO4?
______________________
_____________________________________________________________________________________________
57. How can molar mass of a compound be determined? ______________________________________________
_______________________________________________________________________________________
58. What is the molar mass of C6H12O6 (glucose)?
_______________________________
59. What is the empirical formula for glucose in then above question?
_______________________________
60. Balance the following chemical equations:
a. ____ Mg (s) + ____ HCI (aq)
b.
____ Al
c. ____ Fe
+
____ MgCl2 (aq) + ____ H2 (g)
____ H SO
2
____ Al (SO )
4
2
+ ____ O
4 3
+
____ H
2
____ Fe2O3
2
61. How many moles are present in 34 g of Cu(OH)2?
_________________________________
62. How many moles of hydrogen molecules (H2) are there in 2.45 x 1023 molecules of CH4?
___________
63. How many moles of aluminum are needed to react completely with 1.2 mol of FeO below?
(Show your work)
2Al + 3FeO
3Fe + Al2 O3
__________
64. How much heat is required to raise the temperature of 68.0 g of iron from 30.0 °C to 55.0 °C?
(Show your work)
(Specific heat of iron = 0.44 J/g °C)
65. Given the reaction at STP: 2KClO3 (s)
2KCl (s) + 3O2 (g)
What is the total number of liters of O2 (g) produced from the complete decomposition of 0.500 mole of KClO3(s)?
(Show your work)
4
Chemistry Final Exam: Practice Problems
Given the reaction:
2Al2O3
Name __________________________
Per. __________
4Al + 3O2
66. What is the total volume of oxygen released when 1.00 mole of Al2O3 decomposes?
(Show your work)
67. What is the electron configuration for a phosphorus atom?
______________________________
68. What is the correct e- configuration for an argon atom?
______________________________
69. How many covalent bonds formed in the compound CO2?
______________________________
70. A gas has a volume of 50 L at a temperature of 200 °C. What will the new volume of the gas be if the temperature is
reduced to 100 °C?
______________________________
71. Draw Lewis Dot Structure for the following atoms:
a.
Ca
b.
Xe
c.
Ga
d.
Al
72. How many milliliters of 0.50 M HCI are needed to exactly neutralize 20 milliliters of 1.0 M KOH?
73. How many moles of a gas will a 1000 ml flask hold at 65.0 °C and a pressure of 56 kPa?
74. What is the correct formula for the following acids? a. sulfuric acid _______
75. Given the reaction: 4Al + 3O2
(Show your work)
2Al2O3
b. nitric acid ______
How many moles of aluminum are needed to form 3.7 mol Al2O3?
76. The energy absorbed when a substance dissolves in water and the surroundings cool down may be expressed as?
a. Degrees
b. Kilocalories
c. Moles
d. Grams per mole
77. If 148 grams of calcium hydroxide [Ca(OH)2] are used to prepare a 4.00 M solution, what volume in mL of solution
can be made?
______________________
5
Chemistry Final Exam: Practice Problems
Name __________________________
Per. __________
The reaction of fluorine with ammonia produces dinitrogen tetrafluoride and hydrogen fluoride.
5F2 (g) + 2NH3 (g)
N2F4 (g) + 6HF(g)
78. If you have 66.6 g NH3, how many grams of F2 are required for complete reaction? (Show your work)
79. A solution with a pH between 7 and 14 would be a(n) _______________.
80. A solution with a pH between 0 and 7 would be a(n) _______________.
81. A solution with a pH of exactly 7.0 would be
_______________.
82. What is the molarity of a 500 ml solution that contains 150.0 grams of NaCl?
83. A 2.4 g sample of a metal requires 6 J of energy to change its temperature from 18 °C to 30 °C. What is the specific
heat of the sample?
84. Define a base: __________________________________________________________________________________
85. Define an acid: __________________________________________________________________________________
86. Define a salt: __________________________________________________________________________________
87. What are the names for the following groups?
IA
_______________
IIA
VIIA _______________
_______________
1B - 7B _______________
VIIIA _______________
88. What is the pH of a solution with a hydrogen ion concentration of 0.1 moles per liter?
_________________
89. What is the pH of a solution with a hydrogen ion concentration of 0.05 moles per liter?
_________________
--
90. ______________ Given the structural formula for ethyne: H–C
shared between the two carbon atoms?
C–H, What is the total number of electrons
91. List at least 5 properties of acids and 5 properties of bases.
Acid
Base
a. ________________________________________
_________________________________________
b. ________________________________________
_________________________________________
c. ________________________________________
_________________________________________
d. ________________________________________
_________________________________________
e. ________________________________________
_________________________________________
92. Make a sketch below of the following orbitals (see chapter 5.1)
s
p
d
93. Aluminum and hydrochloric acid are mixed resulting in the formation of aluminum chloride and hydrogen gas.
Write the balanced equation for this reaction below:
6
Chemistry Final Exam: Practice Problems
Name __________________________
Per. __________
At STP, what is the total number of liters of hydrogen gas produced when 6.00 moles of hydrochloric acid
solution is completely consumed?
94. The temperature of a piece of lead with a mass of 110 g changes from 28.0°C to 48.0°C when the metal absorbs
283J of heat. What is the specific heat of the lead?
95. How many milliliters of 2 M HCI are needed to exactly neutralize 40 milliliters of 6 M Ca(OH)2?
96. What is the pOH of a solution if the [H+] = 1 x 10-6 moles /L?
97. Hydrogen peroxide (H2O2) decomposes into water and oxygen gas. Write a balanced equation of this reaction
below:
If 3.0 moles of hydrogen peroxide decomposes, what volume of oxygen gas is produced?
98. Balance the following equation:
___ C2H6 (g) + ____ O2 (g)
___ CO2 (g) + ___ H2O (g)
How many grams of O2 (g) are needed to react completely with 2 moles of C2H6 (g)?
99. What are the principle contributions of each of the following scientists to the creation of the modern model of the
atom? (You may use pictures in as well as words in your answer.)
JJ Thomson
Ernest Rutherford
Niels Bohr
Modern Quantum (wave) Model
7