1 - Oregon State University



1. A polydentate ligand can:

a. Attach once to a metal ligand

b. Attach multiple times to a metal ligand

c. Bond with itself

d. Act as a Lewis Acid

2. How many unpaired d electrons are present in [Fe(H2O)6]3+ (assume water to be weak field)?

a. 0

b. 1

c. 3

d. 4

e. 5

3. The complex ion [Mn (CN)6]3- is:

a. High spin

b. Low spin

4. A transition metal complex appears orange and absorbs light of 460 nm. What is the energy splitting of the d orbitals in kJ/mol?

a. 4.32 x 10-19 kJ/mol

b. 260 kJ/mol

c. 4.32 x 10-22 kJ/mol

d. 260228 kJ/mol

e. 2.60 x 10-7 kJ/mol

5. The second law of thermodynamics states that:

a. The entropy in a system is always increasing for a spontaneous process

b. The entropy in the surrounding is always increasing for a spontaneous process

c. The entropy of the universe is always increasing for a spontaneous process

6. Determine the sign of ∆Ssurr and ∆Ssys for the following chemical reaction

C3H8 (g) + 5 O2 (g) ( 3 CO2(g) + 4 H2O (g) ∆H°rxn=-2044 kJ

a. ∆Ssurr = + ; ∆Ssys = +

b. ∆Ssurr = - ; ∆Ssys = +

c. ∆Ssurr = + ; ∆Ssys = -

d. ∆Ssurr = - ; ∆Ssys = -

7. Which of the following must be true to have a spontaneous process?

a. The system must be endothermic

b. The system must be exothermic

c. The entropy of the surrounding must increase

d. The Gibbs Free Energy must be negative

8. The oxidation number on each Ni metal ion in Na2[Ni(CN)4] is:

a. 1+

b. 2+

c. 1-

d. 2-

9. An experiment run on AgCl determined the solubility product constant at several temperatures, Ksp, for a saturated solution. The slope of a plot of ln Ksp against 1/T had a value of -15300 K. What is the value of ∆H?

a. -127 J

b. -18402 J

c. -127000 J

d. -184 J

10. The ∆G°rxn for the following reaction is -10900 J at 25 °C. What is the equilibrium constant, Kp?

I2(g) + Cl2(g) ( 2ICl (g)

a. 4.40

b. 25100

c. 81.4

d. 0.0123

11. Which element is the reducing agent in the following redox reaction?

Cr(OH)4- (aq) + ClO(aq) → CrO42-(aq) + Cl-(aq)

(A) Cr

(B) O

(C) H

(D) Cl

12. Balance the following redox reaction if it occurs in acidic solution. What are the coefficients in front of H+ and Fe3+ and water in the balanced reaction?

Fe2+(aq) + MnO4- (aq) → Fe3+(aq) + Mn2+(aq)

(A) H+ = 2, Fe3+ = 3, H2O = 2

(B) H+ = 8, Fe3+ = 5, H2O = 4

(C) H+ = 3, Fe3+ = 2, H2O = 2

(D) H+ = 5, Fe3+ = 1, H2O = 5

(E) H+ = 8, Fe3+ = 1, H2O = 4

13. Identify the location of reduction in an electrochemical cell.

(A) the anode

(B) the cathode

(C) the electrode

(D) the salt bridge

(E) the socket

13. Determine the cell notation for the redox reaction given below.

3 Cl2(g) + 2 Fe(s) → 6 Cl-(aq) + 2 Fe3+(aq)

(A) Cl2(g) | Cl-(aq) || Fe(s) | Fe3+(aq)

(B) Cl-(aq) | Cl2(g) || Fe3+(aq) | Fe(s)

(C) Fe3+(aq) | Fe(s) || Cl-(aq) | Cl2(g)

(D) Fe(s) | Cl2(g) || Fe3+(aq) | Cl-(aq)

(E) Fe(s) | Fe3+(aq) || Cl2(g) |Cl-(aq)

14. Which of the following is the weakest oxidizing agent?

(A) Sn2+(aq)

(B) Cr3+ (aq)

(C) Sn4+ (aq)

(D) Mg2+

(E) Sn(s)

15. Use the standard half-cell potentials listed below to calculate the standard cell potential for the following reaction occurring in an electrochemical cell at 25°C. (The equation is balanced.)

Sn(s) + 2 Ag+ (aq) → Sn2+ (aq) + 2 Ag(s)

Sn2+(aq) + 2 e- → Sn(s) E° = -0.14 V

Ag+ (aq) + e- → Ag(s) E° = +0.80 V

(A) +1.74 V

(B) +0.94 V

(C) +1.08 V

(D) -1.08 V

(E) -1.74 V

16. Use the tabulated half-cell potentials to calculate the equilibrium constant (K) for the following balanced redox reaction at 25°C.

Pb2+(aq) + Cu(s) → Pb(s) + Cu2+(aq)

(A) 7.9 × 10-8

(B) 8.9 × 107

(C) 7.9 × 1015

(D) 1.3 × 10-16

(E) 1.1 × 10-8

17. Identify the battery that is used as a common flashlight battery.

(A) dry-cell battery

(B) lithium ion battery

(C) lead-acid storage battery

(D) NiCad battery

(E) fuel cell

18. Nickel can be plated from aqueous solution according to the following half reaction. How long would it take (in min) to plate 29.6 g of nickel at 4.7 A?

Ni2+(aq) + 2 e- → Ni(s)

(A) 1.7 × 102 min

(B) 5.9 × 102 min

(C) 3.5 × 102 min

(D) 4.8 × 102 min

(E) 6.2 × 102 min

19. Which of the following structures is 2,2,3-trimethylheptane? C

[pic]

20. The molecular formula of

[pic]

(A) is C6H6.

(B) is C6H7.

(C) is C6H8.

(D) is C7H7.

(E) is C7H10.

21. How many isomers are there of butane, C4H10 ?

(A) 1

(B) 2

(C) 3

(D) 4

(E) 10

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