Download 2009-10 Chemistry 1st Semester Final Exam Topics and Review

2012-13 Chemistry 1st Semester Final Exam Topics and Review: Chapters 1 - 8
Major Topics Covered:
1.
2.
3.
4.
5.
6.
7.
8.
9.
Scientific Method
Scientific notation
Metric system
Significant Figures
Dimensional Analysis
Density
Physical and Chemical properties, Physical and chemical changes
Matter- elements and compounds, mixtures and pure substances
Elements, atoms, atomic structure- parts, location, charges, and masses. For any atom, ion, or isotope be
able to identify: atomic number, mass number (atomic mass), # protons, # electrons, # neutrons
10. Periodic Table: what is found where? What information is in the table?
11. What is meant by the average atomic mass of an element? How is it calculated?
12. Ions -- cations and anions
13. Polyatomic ions
14. Naming binary compounds
15. Writing formulas from names and names from formulas
16. Evidence that a chemical reaction has occurred
17. Balancing equations
18. Writing and balancing from names of compounds
19. Predicting products
20. Types of chemical reactions
21. Molecular, complete ionic, and net ionic equations
22. Labeling states of matter in equations
23. Solubility rules and how to use them
24. Mole conversions
25. Percent composition
26. Empirical and molecular formulas of compounds
Review:
1. a. Convert 0.00012 to sci notation
b. convert 5.63 x 10-2 to regular notation
2. Rules for determining significant figures. Be sure to understand how zeros are treated.
3. Round this measurement to 3 sig. figs: 3.41236 cm
4. a. convert 5.72g to Kg
b. Convert 275.6mL to L
5. What is the volume of an object with a density of 8.03g/cm3 and a mass of 6.00 x 102g?
6.
13
C How many protons, electrons, neutrons, atomic number, mass number
7. Given the ion Na+1. How many protons, electrons, and neutrons? atomic number? mass number?
8. a. write a formula for aluminum bromide
b. name the compound As2O5
9. Write the products and balance, what kind of reaction: NaOH + HCl 
10. Express each in sci notation: a. 9367958
b. 0.7728 c. .000037001 d. 19873460000
11. Write each in conventional notation: a. 8.2001112 x 105
12. Convert to Celsius: a. 57 oF
b. -24.7 oF
13. Convert to Fahrenheit: a. -31 oC
c. 1.09857 x 101
c. 212 K
b. 78.22 oC
14. Convert to Kelvin: a. 8.23 oC
b. 3.23876 x 10-4
c. 237 K
b. 91 oF
15. Solve with answer in sci notation with correct sig figs:
a. 149.0 Kg + 3388.228 Kg + 2.98 Kg
b. 1.092 x 103m – 4.33 x 106m
c.
(4.932 x109 )(5.43x107 )
(4.32 x104 )(9 x102 )
16. a. The density of an item is 0.933Kg/L. find the volume of a 4.9909g sample.
b. The mass of an item is 4234g and the volume is 893cm3. What is the density in Kg/L?
17. Define the following: heterogeneous, homogeneous, mixture, compound, element, distillation, filtration,
chemical property, physical property, isotope, metal, nonmetal, metalloid, ductile, malleable.
18. Fill in the following chart:
Element
Symbol
Atomic #
Oxygen
Cl-1
Cobalt
Zirconium
34
Mass #
Protons
neutrons
electrons
10
charge?
+2
53
54
19. How many protons and neutrons are in the following isotopes:
a.
244
Pu
b.
133
Cs
c.
277
Ac
d.
57
Fe
20. Name the following:
a. SeO
b. B2O3
c. AsBr3
d. SnO2
g. NH4NO2 h. AgNO3
i. Ba(OH)2
j. KC2H3O2
m. HBr
n. HC2H3O2
o. HNO2
e. CuS
k. Li2CO3
f. Ca3N2
l. Fe2(SO4)3
21. Give the formulas for the following:
a. barium nitride
b. silver iodide
c. sulfur hexafluoride
d. carbon tetrachloride
e. magnesium acetate
f. iron (II) sulfate
g. zinc chromate
h. cobalt (II) carbonate
i. calcium bromide
j. lithium sulfite
k. nitric acid
l. sulfurous acid
m. copper (II) permanganate
n. phosphoric acid
o. iron (III) oxide
22. Complete, balance and identify the type of reaction for each of the following:
a. sodium carbonate and potassium chloride
b. tricarbon octohydride and oxygen
c. aluminum and sulfuric acid
d. barium chloride and sodium sulfate
23. An unknown metal sample whose mass is 14.58 g is heated from 22.3 oC to 54.6 oC. If 234 J is added to
make this change, what is the specific heat of the metal?
24. Write a complete balanced molecular equation, a complete ionic equation, and a net ionic equation for the
following:
a. barium nitrate and sodium sulfate
b. copper (II) chloride and lead (II) nitrate
25. Rubidium has two common isotopes: 85Rb and 87Rb. If the abundance of 85Rb is 72.2% and the abundance
of 87Rb is 27.8%, what is the average atomic mass of rubidium?
26. Dimensional analysis: Show all work. Make sure that your answer has the correct number of significant
figs and is in sci notation. Convert
a.
b.
c.
d.
e.
f.
g.
h.
i.
j.
111109 g to lbs
5400 in to mi
19 cm to ft
36 cm to miles
16 weeks to seconds
54 yds to mm
7500000 μL to km3
15673.35 dL/hour to L/week
1.56 x 10-4 GL to quarts
(G = giga-)
89751236 lbs to mg (milligrams)
27. Sig figs: Do the following calculations making sure that the answer has the correct number of sig figs.
a. (649.23)(750)
453
b.
9865
(65)(54319)
c. 956.75 – 654.1 + 25
28. Temperature Conversions- Show all work for the following temperature conversions.
a. 37.95 ºF  K
b. 95 ºC  oF
29. Density Problems:
a. What is the density of an object that measures 5.60cm by 3.3cm by 1.456cm and has a mass of 2.34 g?
b. An irregularly shaped object with a density of 3.556 g/mL is dropped into a graduated cylinder filled
with 22.56 mL of water. If the water level rises to 44.5mL, what is the mass of the object.
30. Write the complete chemical symbol for the ion with 84 protons, 125 neutrons, and 80 electrons.
31. Write the complete chemical symbol for the ion with 27 protons, 32 neutrons, and 25 electrons.
32. Write the complete chemical symbol for the ion with 73 protons, 108 neutrons, and 68 electrons.
33. Write the complete chemical symbol for the ion with 31 protons, 39 neutrons, and 28 electrons.
34. Name the following:
a. H3PO4
f. Fe2O3
k. Al(OH)3
p. CO
u. HClO3
b. CsOH
g. H2SO4
l. NaC2H3O2
q. MgBr2
v. K2O
c. Li2O
h. FeCO3
m. Na2SO3
r. SnBr2
d.
i.
n.
s.
Ca(OH)2
SO3
H2CO3
N2O
e.
j.
o.
t.
CaBr2
BaCO3
LiH
NH4F
35. Write and balance the chemical equations for the following reactions. Include the physical states (aq, s, l, g)
of the reactants and products.
a. When zinc metal and sulfur powder are heated, they form solid zinc sulfide.
b. When sodium metal is placed in a beaker of water, hydrogen gas and sodium hydroxide solution are
formed.
c. Aqueous iron (III) chloride will react with aqueous sodium hydroxide to produce aqueous iron (III)
hydroxide and aqueous sodium chloride.
d. Hydrogen gas reacts with nitrogen gas to form ammonia. Write and balance a chemical equation for this
reaction.
e. One of the problems with space travel is the building up of carbon dioxide produced by the astronauts.
The typical procedure is to react the carbon dioxide with lithium hydroxide to form lithium carbonate and liquid
water.
36. Write and balance a chemical equation for this reaction.
a. Aluminum metal burns in pure oxygen to produce solid aluminum oxide.
b. Hydrogen sulfide gas reacts with oxygen gas to form water vapor and solid sulfur.
c. Hydrogen gas and iron (III) oxide powder react to form liquid water and solid iron powder.
37. Write balanced molecular equations for the following: if they are double replacement or acid base then also
show phases of all parts of reaction.
a.
b.
c.
d.
e.
f.
g.
magnesium plus nitric acid
tricarbon dihydride plus oxygen
calcium chloride plus nitric acid
zinc plus copper (II) sulfate
ammonium sulfate plus lead (II) nitrate
iron (III) chloride plus potassium sulfate
sodium plus oxygen
38. Complete the following table: Be able to show work for each problem.
mass of sample
moles of sample
particles (atoms or molecules) of
sample
4.24 g hexacarbon hexahydride
0.224 mol water
2.71 x 1022 molecules carbon dioxide
0.297 g nitric acid
1.26 mol hydrochloric acid
4.21 x 1024 molecules magnesium acetate
1478 mg ammonium carbonate
1.40000 x 103 mol beryllium
permanganate
9.97654 x 1023 molecules hypochlorous
acid