These are the questions that will be on your final exam (there may be a difference in the numbers or names to prevent rote memorization) All work will need to be shown to receive credit for the problems. You will be supplied a periodic table and a polyatomic ion and solubility chart with your exam.
1.) Definitions (These will be found in a multiple choice section. 15 total pts.)
a.) chemistry b.)matter c.) element d.) compound e.) solution f.) cation g.) anion
h.) the mole i.) temperature j.) pressure k.) absolute zero l.) alpha, beta, and gamma radioactivity
m.) interpreting the pH scale (acidic,basic,neutral) n.) anode o.) cathode
2.) What is the density of a piece of matter that has a volume of 24 mls and a mass of 12 grams? (2 point)
Would this piece of matter float in pure water? (1 point)
3.) Name the following compounds. (1 point each)
a.) KCl b.) Ca(NO3)2 c.) FeBr3 d.) SO2
4.) Write the formulas of the following compounds. (1 point each)
a.) magnesium fluoride b.) sodium sulfate c.) cobalt (III) nitrate d.) dinitrogen trioxide
5.) Write balanced chemical equations: (2 points each)
a.) _____ Ca(OH)2 + _____ K3PO4 b.) _____ Na + _____ AlCl3
c.) _____ C3H8 + _____ O2 d.) _____ AlCl3 (heated)
e.) _____ Na + _____ Cl2 f.) Uranium 238 undergoes alpha decay
g.) strontium-87 undergoes beta minus decay h.) sulfuric acid neutralizes a sodium hydroxide solution
6.) For each element listed: (2 points each element)
a.) give the ground-state, electron configuration, using the noble gas root
b.) predict the common oxidation numbers based on the electron configuration and stability rules.
Ca (z=20) P (z=15) Co (z=27) Eu (z=63)
7.) Draw the Lewis dot structure of a.) CaF2 b.) CO2 (2 pts. each)
8.) Calculate the empirical formula of a molecule that is 36.5% Na, 25.5% S, and 38.1 % O. (2 points)
9.) A sample of neon gas occupies 2.5 liters at 25 ^ C and 125 kPa.
a.) How many moles of neon are present in this sample? (2 points)
b.) What is the new volume if the temperature changes to 100 ^C at constant pressure? (2 points)
c.) What is the new volume if the pressure changes from 125 kPa to 100 kPa at constant temperature? (2 points)
d.) What is the new pressure if the temperature changes from 25^C to 100 ^C at constant volume? (2 points)
10.) A chemist holds a sample of 10.0 grams of Al(OH)3.
a.) Calculate the molar mass Al(OH)3. (2 points)
b.) How many moles of this compound does the chemist have? (2 points)
c.) How many molecules of this compound does the chemist have? (2 points)
d.) What is the percent composition by mass of this compound? (2 points)
e.) Calculate the molarity when this sample is dissolved in 250 mls of pure water. (2 points)
f.) Calculate the normality of hydroxide when this sample is dissolved in 250 mls of pure water. (2 points)
g.) Calculate the pH when this sample is dissolved in 250 mls of pure water. (2 points)
h.) What volume of a 0.1 M HCl is needed to completely neutralize this sample dissolved in letter “g”? (2 points)
11.) 10.0 grams of chlorine react with 10.0 grams of sodium bromide.
a.) Write a balanced chemical reaction. (2 points)
b.) Based on oxidation states of the elements, identify: (4 points)
element oxidized = element reduced = oxidizing agent = reducing agent =
c.) Using stoichiometry, show the mass of product that is generated in the reaction. (4 points)
d.) Based on (c.), identify the limiting reagent. (1 points)
e.) Calculate the enthalpy of this reaction. (2 points) Is the reaction endothermic or exothermic? (1 point)
f.) Calculate the entropy of the reaction. (2 points) Does the reaction follow the Law of Entropy? (1 point)
g.) Calculate the Gibbs’ free energy of the reaction at 300^C. (2 points) Does this reaction form products based on /\ G? (1 point)
Hf (kj/mol) / So (j/mol^K)Br2 / 0 / 153
Cl2 / 0 / 223
F2 / 0 / 203
NaCl / -411 / 72
NaF / -573 / 51
NaBr / -361 / 87