Arkansas State University Department of Chemistry and Physics

a)  SeO₃

b)  CrF₃•5H₂O

c)  HBr _(aq)

d)  Ac₂(SO₃)₃

e)  (NH₄)₂C₂O₄

2.  Give the formula from the name for each:

a)  ferric sulfate

b)  diphosphorus pentasulfide

c)  ruthenium(II) carbide

d)  hypochlorous acid

e)  manganic oxide

3.   State the law of multiple proportions.  State the law of definite proportions.

4.  Given the following equation:

 _____ Al₂O₃    +  _____ Fe  g    _____ Fe₃O₄    +  _____ Al

a)  balance the equation

b)  describe the type of reaction  ________________________

c)  determine the Fe:Al₂O₃ mole ratio  ___________________

5.  How would you prepare 75 mL of a 0.56 M solution of Ba(NO₃)₂ ?

6.  How would you prepare 1.2 L of a 6 M H₂SO₄ solution if you start with a 18 M H₂SO₄ solution?

7.  Write the electronic configuration for each of the following:

 a)  Ni

 b)  As

 c)  Li

 d)  Rn

 e)  Au

8.  Give the number of valence electrons in each of the following:
 

a)  Cr

b)  Al

c)  Ti

d)  B

e)  Mn

9.  Draw an energy level diagram for Cr⁺² and describe its magnetic properties.

10.  List the types of quantum numbers, what each of them represent and the possible values for each.  Be specific.

11.  Which would have the larger ionization energy, Na or P?  Why?  Define ionization energy.

12.  Which would be larger in size, C or C ^{- 4}?  Why?

13.  Of the five sets of quantum numbers listed below, 2 of them are not valid.  Circle the two incorrect sets of quantum numbers.
 

(4, 2, 0, +1/2)

(4, 4, 0, -1/2)

(5, 2, -2, -1/2)

(8, 7, -6, +1/2)

(4, 1, +2, -1/2)

14.  Draw the Lewis Dot Structure for each of the following:
 

a)  AsF5

b)  SiCl4

c)  SO32-

d)  AlH4-

15. Describe the expected angles for PF₃.

16.  Describe the bonding in each of the following:  (ionic, polar covalent or covalent)
 

a)  CO2

b)  SiI4

c)  K2S

d)  CoBr2

e)  SeO2

17.  For each of the following, give the electron arrangement (E.A.) and the molecular geometry (M.G.).

                                         E.A.                M.G.

 a)   CO₂

 b)   BrF₃

 c)   AsI₃

 d)   SO₂

 e)   BrF₄^-

18.  Describe the bonding in CO₂.  Include a diagram showing orbital overlap.

19.  Given two molecules, Br₂ and F₂, which has the higher boiling point?  Why?

20.  Write the equilibrium expression for each of the following:  Where possible, express both K_c and K_p.  (Assume each of these are equilibria equations)

 a)   2 NaN_{3 (s)}   g   2 Na _(s)   +    3 N_{2 (g)}

 b)   4 NH_{3 (g)}  +  5 O_{2 (g)}  g    4 NO _(g)  +   6 H₂O _(g)

21.  According to Le Chatelier's Principle,

 a)  what effect would the addition of Cl^- have on the equilibrium below?

   CoCl₂   +   2 Cl^-    g      CoCl₄^2-

 b)  what effect would the addition of Ag⁺ have on the equilibrium in problem 21a if the Ag⁺ precipitates as AgCl?

22. Calculate the pH of a 0.002 M NaOH solution.

23.  For each pair of acids, circle the strongest one.
 

a.	HCl	HBr
b.	HCl	H2S
c.	H2SO3	H2SO4
d.	CH4	H2O
e.	H3PO4	H3AsO4

24.  For the following salts, define the resulting solutions as either acidic, basic or neutral.

 a) NH₄Br

 b) Na₂SO₄

 c) KF

 d) sodium acetate

 e) CaCl₂

25.  Calculate the equilibrium concentrations of a 0.2 M HF solution. Ka = 7.1 x 10^-4

26.  Define a basic oxide, acidic oxide and an amphoteric oxide.

27.  Write the K_sp expression for each of the following:

 a)  AgCl _(s)  g    Ag⁺_(aq)    +    Cl^- _(aq)

 b)  Ag₂CO_{3 (s)}  g   2 Ag ⁺ _(aq)   +     CO₃^2- _(aq)

28.  Given the K_sp = 2.4 x 10^-4 for PbCl₂, determine if a precipitate will occur from mixing 0.5 L of 0.02 M NaCl solution with 0.5 L 0.02 M Pb(NO₃)₂ solution.

29.  Determine the K_sp for Ag₂SO₄ if the molar solubility is 1.5 x 10^-2 M.

30.  Fill in the blanks.

 List the Group V cations________________________________

 Reagent used to precipitate Group III cations __________

 Reagent used to precipitate Group I cations ____________

31.  Write the equation that relates DG^o with the equilibrium constant K.  Which way does the equilibrium lie if K < 1?

32.  Determine the E for the Co⁺²/Co and Pb⁺²/Pb half-cells if the [Co⁺²] = 0.50 M and the [Pb⁺²] = 0.25 M.

33.  Will I₂ react with Pb?  Explain.  If it does react, what is (are) the product(s)?  Give the balanced equation.

34.  Write the solubility rules.

35.  What are VSEPR rules and why are they important?

36.  Define an Arrhenius acid/ base, Bronsted-Lowry Acid/ base and a Lewis acid/ base.

37. What is K_sp and what information does it give?

38.  What is K_a and pK_a?  What does the magnitude of the numbers tell us?