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NAME ______________________
CHEMISTRY FINAL REVIEW
Puskas/Oberto - Career
1.
What is matter?
2.
What are the two forms of matter?
3.
What is the difference between the two types of mixtures?
4.
Give examples of the two types of mixtures.
5.
What is the difference between the two types of Pure Substances?
6.
What are the two types of Pure Substances. __________ _________
a. What is an atom?
b. What is a molecule?
7.
What is a chemical property? Give an example.
8.
What is a physical property? Give an example.
9.
What is the formula for calculating density?
10.
What is the density of a liquid that has a mass of 50 g and a volume of 300 mL?
11.
What is the difference between an intensive and extensive property? Give an
example of each regarding your pencil/pen.
12.
What are the three subatomic particles and their charges that make up an atom?
13.
Where are they located in an atom?
14.
What is the atomic number of an atom?
15.
16.
What is the mass number of an atom?
What is an ion?
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17.
How does an atom become an ion?
18.
What does the electron configuration tell you about an atom?
19.
Label the Periodic Table according to charges. Then label valence electrons.
20.
Write the electron configuration for the following elements. (1s2, 2s2, 2p6…)
a. Cl
b. Mn
c. Fr
21.
What are valence electrons?
22.
How many valence electrons do the following elements have?
a. Na
b. O
c. Kr
23.
What makes an atom stable (regarding electrons)? What rule tells us this?
24.
What type of ion forms if an atom gains electrons?
25.
What type of ion forms if an atom loses electrons?
26.
What is the common ion charge for the elements below?
a. Li
b. N
c. F
d. Al
27.
What are the two main differences between an ionic and covalent compound?
28.
Which ion is written in the formula first?
29.
30.
List 4 polyatomic ions.
List the prefixes for numbers 1-5.
13-
52
231.
32.
4-
Determine the formula of the following compounds. (Remember, you must first
determine if the compound is molecular or ionic!)
a. Magnesium Chloride
m. Hydrogen Nitride
b. Iron Sulfide
n. Beryllium Chloride
c. Dihydrogen Monoxide
p. Lead Sulfide
d. Sodium Sulfate
q. Tetracarbon Hexaiodide
Write the name of the following compounds. (Remember, you must first determine if
the compound is molecular or ionic.)
a. PBr5
o. NaF
b. Ba(NO3)2
p. CrSe
c. Mg3(PO4)2
q. FeCO3
d. NH4Cl
w. PbS2
33.
What is a reaction? What actually occurs in a reaction?
34.
What are the two parts in a reaction (before + after arrow)?
35.
What is the name of the number that is used to balance chemical equations?
36.
What are the five types of reactions?
37.
Label the type of reaction and then balance the following chemical equations.
a. ________________________
Al +
b. ________________________
CaBr2 + H3PO4
c. ________________________
C4H8 +
O2 
d. ________________________
KHCO3
→
H2O
Fe(C2H3O2)3
→
Cu(C2H3O2)2
e. ________
38.
CuSO4
+
→
O2
Al2O3

HBr + Ca3(PO4)2
CO2
+
+ H2O
CO2
+
K2CO3
+ Fe2(SO4)3
What does the word “mole” mean?
** The “mole” can also be called “Avogadro’s number” **
3
39.
What is molar mass (also called formula mass and Molecular weight)?
40.
Determine the number of moles that is equal to the following masses given.
a. 100g of BaCl2
b. 35g of (NH4)3PO4
c. 0.821g of BF3
d. 68g of Al2(SO4)3
41.
Determine the mass that is equal to the following number of moles given.
a. 2.16 moles of SrF2
b. 0.91 moles of C6H12O6
c. 5.00 moles of Fe(MnO4)3
d. 0.075 moles of LiOH
42.
What is stoichiometry?
43.
Determine the number of moles of ALL the other reactants and products in the
following chemical reactions using the number of moles of the one substance given in
the equation. (These are 1-step “mole-step” problems!)
a. 1.5 moles of HBr
3 CaBr2
+
2 H3PO4

6 HBr
+
Ca3(PO4)2
b. 2.2 moles CO2
4
C4H8
44.
+
6 O2

4 CO2
+
4 H2O
Determine the masses of ALL the other reactants and products in the following
chemical reactions using the mass of the one substance given in the equation. (These
are 3-step problems!)
a. 200 g C3H6
2 C3H6
+
9 O2
→
6 H2O
+
6 CO2
b. 45.9 g Cu(C2H3O2)2
3 CuSO4
45.
+
2 Fe(C2H3O2)3
→
3 Cu(C2H3O2)2
+
Fe2(SO4)3
What is:
a. Boyle’s Law?
b. Charles Law?
46.
What does the “inverse” relationship in Boyle’s law tell us?
47.
What does the “direct” relationship in Charles’ Law tell us?
48.
What is the formula for the Combined Gas Law?
49.
What unit does temperature have to be measured in to solve any gas law problem?
50.
How do you convert degrees Celsius into the unit from #73?
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52.
Solve the following problems using the best Gas Law. Remember that standard
temperature is 0C and standard pressure is 1 atm, 101 kPa, 760 mm Hg or 760 torr.
a. Oxygen gas kept at 45C has a pressure of 105 kPa. The pressure is decreased to
90 kPa. What temperature will allow this to happen?
c. What was the original volume of Hydrogen gas at 15C if it is now at 23C and in
a 2000 mL container?
d. What is the original pressure of a gas in a 1.1 L container if its new volume is
1.35 L with a pressure of 1.05 atm?
e. What is the new volume of Chlorine gas at STP when it was in a 2.5 L container
with a pressure of 720 torr at 33C?
f. Neon gas that was at 1.08 atm is now at 1.19 atm and 25C. What was its original
temperature?
53. What is a solution?
54. What are the 2 parts to a solution?
55.
What is the difference between the 2 parts in #54?
56.
What is solubility?
57.
What is a solution called if water is the solvent? ______________
58.
What are the three levels of saturation?
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59.
What are the differences between the three?
60.
What is molarity?
61.
What is the formula for molarity?
62.
What is the difference between dilute and concentrated?
63.
What is the molarity of a 5 L solution that contains 2 moles of K2CO3?
63.
How many moles of solute are there in 0.5 L of a 1.28 M NaNO3 solution?
64.
How many liters of a 2.75 M Cu(ClO3)2 solution do you need to obtain 0.25 moles of
Cu(ClO3)2?
65.
Label the following as ACID, BASE, BOTH, or NEITHER.
a. ____________
A substance with a pH value of 7.
b. ____________
A substance that turns phenolphthalein pink.
c. ____________
A substance that has a pH value of 2.
d. ____________
A substance whose formula is Mg(OH)2.
e. ____________
A substance that turns litmus paper blue.
f. ____________
A substance whose formula is HBr.
i. ____________
A substance that feels slippery.
l. ____________
A substance that has a pH value of 11.
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