Download Honors Chemistry 1st Semester Review Sheet – 2006-2007

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Honors Chemistry 1 Semester Review Sheet 2012-2013
Show all work for every problem if you want feedback from your teacher. A key will not be
provided! Items marked with an * are more challenging and require all of your skills to solve. These won’t necessarily
appear in this format on the exam but the skills needed to solve each will be needed.
Significant Figures and Metric Conversions
1) 170.4 m3
=______________ cm3 (this is a cubed conversion…careful!)
2) 58 dg
=______________ mg
3) 0.0923 km =______________ mm
4) 4.51 x 103 L =______________ mL
5) 45700 cg
=______________ kg
6) 82.4 nm
=______________ m
7) 2.00 x 10-5m =________km
8) 2.00mL/min =________L/hour
=________cm3
9) 145 ml
How many significant figures are in the following numbers?
10)
11)
12)
13)
14)
0.0090
3200
0.3004
4004
5.020 x 10
23
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Perform the following calculations using the correct number of significant figures.
15) 6.023 x 10 23 x 0.05
16) 900 + 32
17) 1.957 – 2.00/1.67
Mole Calculations
1) Determine the number of molecules contained in a 155g sample of sulfur tetrafluoride.
2) What is the mass of a sample of K2Se that contains 8.99x 1024 formula units?
3) How many moles of XeF4 are in a 35.6 kg sample of XeF4?
*4) [This problem requires many different conversions.] Lead (IV) iodate has a density of 1134
cg/cm3. How many particles are in a sample of lead (IV) iodate that has a volume of 24.2 mm3?
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Nomenclature
Name the following compounds.
1. PbCO3
_____________________________________________
2. CaBr2
_____________________________________________
3. H2SO3
_____________________________________________
4. MgO
_____________________________________________
5. SF6
_____________________________________________
6. CuI
_____________________________________________
7. K2O
_____________________________________________
8. Ni(CO3)2
_____________________________________________
9. N2O
_____________________________________________
10. Al(NO3)3
_____________________________________________
11. H2C2O4
_____________________________________________
12. PCl3
_____________________________________________
13. HBr
_____________________________________________
14. Mn2(CrO4)3_____________________________________________
15. NH4C2H3O2_____________________________________________
Write the formula of the compound.
1. dinitrogen pentoxide
__________________
2. calcium carbide
__________________
3. hydrocyanic acid
__________________
4. carbon disulfide
__________________
5. iron (III) chloride
__________________
6. chromium (VI) oxide
__________________
7. sodium selenide
__________________
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8. carbonic acid
__________________
9. tin (II) oxide
__________________
10. cadmium iodide
__________________
11. titanium (II) nitrate
__________________
12. carbon monoxide
__________________
13. hydrofluoric acid
__________________
14. barium sulfate
__________________
15. zinc chlorite
__________________
Percent Composition
Determine the percent composition by mass of Uranium hexafluoride.
Empirical and Molecular Formulas
1) A uranium and chlorine compound is composed of 0.159-g of uranium and 0.119-g of chlorine.
Determine the empirical formula of this compound and write the correct name for it.
2) Determine the empirical formula for a compound composed of 7.22-g of Nickel, 2.53-g of
phosphorus, and 5.25-g of oxygen. Determine the empirical formula of this compound and write the
correct name for it.
3) An unknown compound whose molecular mass is approximately 190g/mol has the following
elemental composition by mass: 12.14% C, 16.17% O, and 71.69% Cl. Determine the empirical and
molecular formulas.
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Chemical Reactions: Molecular and Net Ionic
1. Using the activity series table, predict whether each of the possible reactions will occur.
If the reaction will occur, write the products and balance the equation.
a. Ni (s) + CuCl2 (aq) 
b. Zn(s) + PbNO3 (aq) 
c. Cl2 (g) + KI (aq) 
d. Cu(s)s + FeSO4 (aq) 
e. Ba (s) + H2O (l) 
2. Complete and balance the equations for the following reactions and identify the type of
reaction each represents. You will need to determine if a reaction occurs or not first!
a. (NH4)2S (aq) + ZnCl2 (aq) 
b. Al (s) + Pb(NO3)2 (aq) 
c. Ba(s)+ H2O (l) 
d. Cl2 (g) + KBr (aq) 
e. H2O (l) 
f. NH4Cl(aq) + Ba(OH)2(aq) 
g. HCl(aq) + NaOH(aq) 
3. For the following reactions, write the balanced molecular equation and the net ionic
equation. Make sure to clearly slash all spectator ions and identify the precipitate formed if
the reaction forms one.
a) A solution of mercury (II) chloride reacts with potassium sulfide.
b) A solution of sodium carbonate reacts with calcium chloride
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c) A solution of copper (II) chloride reacts with ammonium phosphate.
d) Solutions of calcium carbonate and hydrofluoric acid are mixed.
Molarity Calculations
1) Determine the molarity of a solution made by dissolving 20.5g of potassium nitrate in enough
water to make 150.mL of solution.
2) What mass of potassium nitrate is used if it is dissolved into water to make a 0.588M solution
with a final volume of 125 mL?
3) How much water must be added to the previous problem to make a 0.350M solution?
4) Determine the molarity of a solution made by diluting 350. mL of a 4.50 M solution by adding 125
mL of water to it.
5) A 1.55 L solution of gold (III) chloride is originally at a concentration of 0.0443M. Determine
the concentration of a solution made by pouring 750. mL of this original solution into a container of
water with 225 mL of water in it.
6) The remainder of the original solution not used in #5 above is then placed in a beaker on a hot
plate and 550.mL of water is driven off as steam.
(a) Determine the concentration of the resulting solution.
*(b) If the rest of the water in this sample is driven off…what mass of solid gold (III) chloride will
be left in the beaker?