Chemistry
1. Name the following compounds:
a. Ca3N2
b. NO2
c. H3PO4
d. HBr
e. N5O10
Final Exam Study Guide
2015
f.
g.
h.
i.
j.
Br2
HNO3
CuO2
Li2SO4
PCl3
2. Write formulas for the following:
a. sodium oxide
f. chlorine gas
b. sulfur trioxide
g. chloric acid
c. phosphorous acid
h. iron(II) oxide
d. hydrochloric acid
i. calcium sulfate
e. disulfur decaoxide
j. carbon tetrachloride
3. Write the formulas for the diatomic elements.
a. hydrogen
e. chlorine
b. nitrogen
f. bromine
c. oxygen
g. iodine
d. fluorine
4. Identify the prefixes for the following:
a. 1
f. 6
b. 2
g. 7
c. 3
h. 8
d. 4
i. 9
e. 5
j. 10
5. When substances undergo chemical changes, ________________________ differences usually occur.
6. List five evidences of chemical change:
a. ________________________________ (a banana turns yellow as it ripens)
b. ________________________________ (mixing two liquids results in the formation of a solid)
c. ________________________________ (temperature rises 12◦C)
d. ________________________________ (rotten eggs stink)
e. ________________________________ (bubbles form)
7. Chemists use statements called _____________________ to represent chemical reactions.
8. A substance that undergoes a reaction is called a _________________________.
9. When reactants undergo a chemical change, each new substance formed is called a _______________________.
10. To express chemical reactions, scientists use _______________ equations, _______________ equations, and
__________________ to indicate the physical state of the substances.
11. In _______________ equations, acetic acid + sodium hydrogen carbonate → sodium acetate + water + carbon
dioxide reads as “acetic acid and sodium hydrogen carbonate react to produce sodium acetate, water, and
carbon dioxide”.
12. ____________________ equations use symbols and formulas to represent the reactants and products.
13. (aq)
_________________________________
14. (s)
_________________________________
15. (l)
_________________________________
16. (g)
_________________________________
17. The law of _________________________________ of atoms: The number and kinds of atoms present in the
reactants of a chemical reaction are the same as those present in the product.
18. A ________________________ is a number, which is always positive, that is placed in front of the parts of a
chemical reaction to indicate how many units are involved.
19. Whenever two or more substances combine to form a single product, the reaction is called a
_____________________________ reaction.
20. A _________________________________ reaction is one in which a compound breaks down into two or more
simpler substances.
21. A _________________________________ reaction is one in which one element takes the place of another in a
compound.
22. A _________________________________ reaction is one in which the positive ions of two ionic compounds are
interchanged.
23. A _________________________________ reaction is one in which a substance rapidly combines with oxygen to
form one more oxides.
24. The amount of energy the particles must have when they collide is called the
__________________________________________ of the reaction.
25. Most reactions go faster at ________________________ temperatures.
26. Raising the ________________________________, or amount of the substance present in a certain volume, will
speed up a reaction because there are more particles per volume.
27. When the __________________________________, or the reactant in limited supply, is used up, the reaction
stops and no new product is formed.
28. A _____________________________ is a substance that speeds up the rate of a reaction without being
permanently changed or used up itself.
29. Danish physicist ________________________________ suggested that electrons revolve around the nucleus
like planets revolve around the Sun.
30. Bohr’s model explained _____________________________’s emission spectrum, but failed to explain any other
element’s emission spectrum.
31. The current atomic model explains electron behavior by interpreting the
__________________________________________ of all the elements.
32. Closely spaced lines in a spectrum suggest that _________________________—divisions within a level—exist
within an energy level.
33. The energy sublevels are indicated as __________________________________.
34. s orbitals are ___________________________ in shape.
35. p orbitals are ____________________________-shaped.
36. d orbitals are ____________________________-shaped.
37. f orbitals are ____________________________.
38. The _____________________________ states that each electron occupies the lowest energy sublevel available.
39. Each energy level has a specific number of sublevels, which is the same number of the ____________________.
40. The ________________________________________________ states that it is fundamentally impossible to
know precisely both the velocity and position of a particle at the same time.
41. The only quantity that can be known is the __________________________ for an electron to occupy a certain
region around the nucleus.
42. The space in which there is a high probability of finding an electron is called an _______________________.
43. Each energy level relates to orbitals of different __________________ and ____________________.
44. The most stable arrangement of electrons in sublevels and orbitals is called an __________________________.
45. Because orbitals are mostly ________________________, this space can be used by another pair of electrons
and the orbitals can _______________________.
46. The shape of the modern periodic table is a direct result of the order in which ____________________ fill
energy sublevels and their orbitals.
47. Chemical properties _____________________ when elements are arranged by atomic number because electron
configurations repeat in a certain pattern.
48. __________________________________ uses symbols in brackets to shorten inner electron configurations of
other elements.
49. The stable electron configurations explain the lack of ________________________ of the noble gases.
50. The lanthanides and actinides are called the ______________________________________ because their last
electron occupies a 5f orbital in the seventh period.
51. The higher the energy, the _________________________ the outermost electrons are from the nucleus.
52. As the valence electron gets _________________ from the nucleus, the s orbital it occupies gets larger and
larger.
53. Identify the type of reaction:
a. A + X
b. AX
c. A + BX
AX
A+X
AX + B
d. AX + BY
AY + BX
e. CxHy + O2  CO2 + H2O
54. Which of the following shows evidence of a chemical reaction?
a. Ice melting
e. A precipitate forming
b. Magnesium metal burning brightly
f. Bubbles forming
c. Carbon dioxide gas forming
g. Leaves turning color in the fall
d. Glass breaking
h. Temperature changing
55. Another name for a solid formed during a chemical reaction is a ________________________.
56. The term used to indicate something is dissolved in water is ________________________.
57. Balance the following equations:
a. ___ F2 + ___ KCl  ___ KF + ___ Cl2
b. ___ Hg + ___ O2  ___ HgO
c. ___ MgSO4 + ___ KNO3  ___ Mg(NO3)2 + ___ K2SO4
d. ___ CH4 + ___ O2  ___ CO2 + ___ H2O
e. ___ FeCl3 + ___ NaOH  ___ Fe(OH)3 + ___ NaCl
f.
___ KClO3  ___ KCl + ___ O2
58. When balancing a chemical equation, only the ______________________ can be changed.
59. Write the electron configuration and orbital notation for the following elements.
a. H
i. F
b. He
j.
c. Li
k. Na
d. Be
l.
e. B
m. Fe
f.
C
n. Sn
g. N
o. Ba
h. O
p. Xe
60. How many molecules are in 4.0 moles of CO2?
61. How many moles of Au contain 4.49 x1023 atoms of Au?
62. What is the molar mass of Ca3(PO4)2?
63. How many grams are in 1.933 moles of KCl?
64. How many moles are in 452 grams of Mg?
Ne
P
65. How many formula units are in 3.6 grams of NaBr?
66. What is the mass of 8.50 x 1022 atoms of helium?
67. What is the percent composition of sodium in sodium oxide, Na2O?
68. What is the percent composition of Ca3(PO4)2?
69. An unknown compound is analyzed and found to be composed of 34.53% zinc, 14.79% nitrogen, and 50.68%
oxygen. What is the empirical formula for the compound?
70. A compound of phosphorus and sulfur contains 27.87% phosphorus and 72.13% sulfur. The molar mass of the
compound is 222.30 g/mol. What is the molecular formula for the compound?
71. Balance the following equation:
___ CO2(g) + ___ LiOH(s) → ___ Li2CO3(s) + ___ H2O(l)
a. How many moles of lithium carbonate can be produced from 3.50 moles of carbon dioxide?
b. How many grams of lithium hydroxide are needed to produce 100.0 grams of lithium carbonate?
c. If 20 grams of carbon dioxide react with 20 grams of lithium hydroxide, which reactant is limiting?
d. How many grams of lithium carbonate are produced from the reaction in part c?
e. If 26.99 grams of lithium carbonate are yielded from the reaction, what is the percent yield?