1. business and industrial
2. energy
3. oil

2015 Honors Chemistry Review for the Final Exam
Each unit has practice problems. The answers are posted on the bulletin board. Please review
VIDEOS, your DILL and any other PRACTICE MATERIAL throughout the year.
Final Exam Schedule:
Thursday May 28th
1A and 3A
Monday June 1st
2A and 4A
Friday May 29th
1B and 3B
Tuesday June 2nd
2B and 4B
Unit 1: 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_____________________________________________
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Write the correct formula for the following compounds.
1. dinitrogen pentoxide
__________________
2. calcium carbide (carbide is C2-2)
__________________
3. hydrocyanic acid
__________________
4. carbon disulfide
__________________
5. iron (III) chloride
__________________
6. chromium (VI) oxide
__________________
7. sodium selenide
__________________
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
__________________
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Unit 2: Chemical Reactions
1. Using the activity series table, predict whether each of the possible single replacement reactions
will occur. If the reaction will occur, complete and balance the equation. If it will not, state the reason.
a. Ni (s) + CuCl2 (aq) 
(Ni has a 3+ oxidation state)
b. Zn(s) + PbNO3 (aq) 
c. Cl2 (g) + KI (aq) 
d. Cu(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:
a. (NH4)2S (aq) + ZnCl2 (aq) 
b. Al (s) + Pb(NO3)2 aq 
c. Mg(s)+ H2O (l) 
d. Cl2 (g) + KBr (aq) 
e. H2O (l) 
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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) Solutions of mercury (II) chloride react with potassium sulfide.
b) A solution of sodium carbonate reacts with a solution of calcium chloride.
c) Solutions of copper (II) chloride and ammonium phosphate react.
d) Solutions of acetic acid and calcium carbonate react.
e) A solution of ammonium sulfate is reacted with a solution of magnesium hydroxide
Unit 3: Metrics and Significant Figures
Convert the following to the designated unit while preserving significant figures.
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
=______________pg
6) 82.4 nm
=______________ m
7) 2.00 x 10-5m
=______________km
8) 2.00mL/min
=______________L/hour
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Determine the number of significant figures in the following numbers, then convert each to either
decimal or scientific notation.
9 ) 0.0090
________
___________
10) 3.200 x 104
________
___________
11) 0.3004
________
___________
12) 4004
________
___________
13) 5.020 x 10 23
________
___________
Perform the following calculations while observing the correct number of significant figures.
14) 6.023•10 23 x 0.052 =
15) 910 + 36 =
16) (2.957 – 2.00)/0.0165 =
__________
__________
__________
Unit 4 The Mole
1) Hydrogen and oxygen gases react under a specific set of conditions to produce liquid water.
a. How many moles of hydrogen would be required to produce 5.0 mol of water?
b. How many moles of oxygen would be required?
2) A 4.50 mole sample of the organic molecule ethane undergoes combustion.
a. How many moles of oxygen are required to consume the ethane?
b. How many moles of each product are formed?
c. Would it require more or less oxygen to combust a 4.50 mole sample of ethene? Explain?
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3) Sodium chloride is produced from its elements through a synthesis reaction. What mass of each
reactant would be required to produce 25.0 mole of sodium chloride?
4) Methanol (CH3OH) is an important industrial compound that is produced from the following
unbalanced reaction:
CO(g) + H2 (g)  CH3OH (g)
a. What mass of each reactant would be needed to produce 100.0 kg of methanol?
b. If you were given 50.0 g of carbon monoxide, how many moles of hydrogen gas would be
needed to completely react it?
5) Sulfuric acid reacts with sodium hydroxide.
a. Predict the products of this reaction and balance the equation.
b. What mass of sulfuric acid would be required to react with 0.75 moles of sodium hydroxide?
c. What mass of each product is formed by this reaction?
6) Given the reactant amounts specified in each balanced chemical equation, determine the limiting
reactant in each case.
a. HCl
+ NaOH 
2.0 mole
b. Zn
2.5 mol
6
+
NaCl + H2O
2.5 mol
2HCl
6.0 mol
 ZnCl2 + H2
7) For each reaction in #6 above (a and b), determine the moles of excess reactant that remains.
8) A 2.50 mol sample of zinc and 5.50 mol of silver nitrate are available to react by single
displacement reaction.
a. Identify the limiting reactant. Don’t forget to write the balanced chemical equation first.
b. Determine the amount of moles of each product formed.
c. Determine the mass of each product formed.
9) The percent yield for the reaction PCl3 + Cl2  PCl5 is only 83.2 %. What mass of PCl5 is expected
from the reaction of 73.7 g of PCl3 with excess chlorine given the expected yield?
10) A compound was found to contain 43.6% P and 56.36% O. The compound has a molecular mass
of 283.33 g/mol. Determine the empirical and molecular formula.
Unit 5 The Periodic Table
1) List the oxidation state(s) for the following elements: Cl, K, Ar, Mg, Ga, Mn, Fe, O, Al, Hg, Sn, Si.
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Complete the following table.
ELEMENT
LONGHAND
ORBITAL FILLING
QUANTUM
CONFIGURATION
DIAGRAM
NUMBER
Mg
3, 1, 0, +1/2
1s22s22p63s23p5
(X-2)
1s22s22p6
Mo
2) How do atomic radii change as we move…
(a) from top to bottom in a group on the periodic table?
(b) from left to right in the periodic table?
(c) Explain the theory for the size variation from top to bottom and left to right.
(d) Arrange the following atoms in order of increasing atomic radius:
(i) B, Al, Si, and Ge.
(ii) Mg, F, P, O, and Ca.
(iii) In, Ar, Rb, Ge, and He.
3) Based on their position in the periodic table, select the atom with the larger first ionization energy
from each of the following pairs and describe why: (a) B, F (b) N, P (c) Hf, Cs, (d) O, P (e) Ga, Ge
4) Identify the following elements based on the description below.
a. The noble gas isoelectronic with the alkaline-earth metal ion from period 5
b. A radioactive element from the d block whose energy level is less than 5
c. The metal in Period 6 that is a liquid at room temperature
d. The halogen with the highest ionization energy
e. The actinide which has a downspin electron in the orbital designated a zero
Unit 6 Chemical Bonding (This section should be done on separate sheets of paper!)
1) Draw the Lewis structure and identify the Shape, Polarity, and the Bond angle for the
following: NI3, SiO4-4, F2CO, and SeF6. This will help with a review of intermolecular forces.
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2) Why is fluorine a gas, but iodine a solid when they both are at room temperature? Explain
by referencing IMF’s.
3) Identify and describe the bonds within the particle and the forces between particles for:
a) two molecules of SO2 b) two molecules of CF4
c) two molecules of H2O and d) two formula units of NaCl.
4) Draw the Lewis Dot structures for the following molecules. Make sure you show the dots
representing bonds directly between the bonding atoms and show all electrons paired.
Then, describe the 3-D shape of each and note any dipole moments.
a) H2S b) PCl3
c) NCl3 d) OF2
e) CH4
f) OHg) CO2
h) NO3- i) CNj) CO3 2- k) PO4 35) Draw the resonance structures (3 total) for SCN-1 and show the formal charges on each
diagram.
Organic Chemistry – Nomenclature
1) For the following names, draw the molecule. You do not have to include the hydrogen
atoms.
a. Butane
b. 2,2-dimethyl hexane
c. Hexene
d. 2-heptyne
2) What is the difference between unsaturated and saturated hydrocarbons?
Unit 6 Gases
1) A steel cylinder contains 150. moles of oxygen gas at a temperature of 36.0 oC and a pressure
of 14.6 kPa. After some of the oxygen has been used, the pressure is 1.46 kPa at a
temperature of 24.3 oC. What mass of oxygen remains in the cylinder?
2) A bacterial culture isolate from sewage produced 59.2 mL of methane, CH4, at 105 oC and
115 mmHg. What is the volume of this methane at standard temperature and pressure?
(0.00 oC, 760. mmHg)
3) You have a steel tank of argon gas at 23.5 atm pressure at 52.6 oC. The volume of argon in
the tank is 150.0 L. Determine the volume of this gas if you allowed it to escape into a
balloon to the pressure of the surrounding air (0.974 atm)? Assume temperature remains
constant.
4) Pentane, C5H12, combusts in the presence of oxygen to form carbon dioxide and water. You
are given 274 grams of Pentane and 1109 liters of oxygen gas. Write the reaction and
calculate the (a) limiting reactant; (b) volume of carbon dioxide gas produced (assume STP);
and (c) amount, in grams, of excess reactant?
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AMHS Honors Chemistry Super Problem:
A student is synthesizing a compound of osmium metal with oxygen gas which is accomplished by
heating the metal in the presence of oxygen gas at temperatures near 400˚C. A 85.57g sample of osmium
metal is heated in a crucible (crucible mass = 254.48g and lid mass = 66.79g). The final product and the
crucible have a total mass of 435.67g. The osmium/oxygen product has a known or accepted molar mass
of 254.23 g/mol. The melting and boiling points of the product are determined to be 40.25˚C and 129.7˚C
respectively.
a) Determine both the empirical and molecular formulas for this product.
b) This is a product made from a metal and a nonmetal. However, the bonds have a more covalent
character to them than ionic. Name this product using both the ionic and covalent nomenclature
systems.
c)
What does the information in “b” above indicate to you about the elements respective
electronegativities in comparison to each other?
d) Oxygen has an electronegativity of 3.5 which is higher than that of osmium metal. What is the
minimum E.N. value for osmium if the bond can still be considered covalent and not ionic?
e) Write the full electron configuration of osmium. Identify the core and valence electrons in this
configuration. What would its oxidation number be if the product was truly an ionic compound?
f)
The shape of the “molecule” is found to be tetrahedral. Assuming this is true, what are the bond
angles in this molecule? Why aren’t the bond angles 90˚ if the central atom has four atoms around
it and no lone pairs? Explain.
g) The molecule is known to be 518 times more soluble in carbon tetrachloride than water. Does this
support or conflict with the assumption about the shape of the molecule from “f” above? Explain
your statement by clearly discussing the involved chemicals. What does this indicate about the
type of intermolecular force available to this molecule? How could the molecule be soluble at all
in water if it is so much more soluble in carbon tetrachloride? What could be added to the water
to increase the solubility of the osmium/oxygen species? Explain.
h) Consider the melting and boiling points of the product. Are the intermolecular forces less than,
equal to, or greater than that of the hydrogen bonded water molecules? Explain.
The osmium/oxygen compound synthesized above occupies a volume of 1.46 x 10 16 µm3 at a temperature
of 138.7˚C and a pressure of 110. kPa.
i)
Determine the density of this compound in g/cm3 and then g/L.
j)
Confirm the molar mass stated above by calculating the molar mass using the “Dirt Pile” gas law
equation. Calculate the percent error assuming the given molar mass is the accepted value.
k) Determine the volume that 0.588g of this gas would occupy if it were collected over water under
the conditions of 755 torr, 22.5˚C. The vapor pressure of water at this temperature is 20.5 mmHg.
Determine the volume of this sample under STP conditions.
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