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Unformatted text preview: Chem 14A2 Final information/Review Fall 2000 The final exam is on Friday, December 15th from 3 pm. to 6 pm. If your last name begins with "A""L“ you will take the final in Dickson 2160E
" " you will take the final in 0850 The final is comprehensive.
You may use one 5"x 8" notecard (front and back), you will need a nonprogrammable scientific calculator,
see your syllabus for standard exam rules. if you wish to have the graded final mailed to you bring 3 first class stamps
with you to the final. Otherwise you may pick up your exam next quarter in
Young Hall 4009. The final exam is comprehensive which means everything we've covered in lecture is "fair game" on this
exam. You should review all concepts and worked problems in your notes, you should rework both
midterms and the quizzes, and review the assigned homework. You will be provided with all relevant
equations, constants, MO diagrams, and a periodic table for the exam in the same manner as was done for
exams 1 and 2. Dr. Harakas will be having office hours on Monday the 11‘“ from 1 pm. to 6 pm. and
Tuesday the 12th from 11 am to 5 pm. Dr. Harakas will not have office hours on
Thursday the 14‘“. 1. Draw all the unique isomers (geometrical and optical) for the following complexes, state which pairs (if any) are
enantiomers. a) [Pt(NH3)2(CO)2]2+ (square planar geometry) b) [Co(NH3)2(H20)2(en)]2+ en=ethylenediamine .44. 2. For the molecule acetylene : HC=CH / use the above coordinate system
a) State the orbital hybridization for the carbon atoms.
b) Draw and label the orbitals that are involved in the bonding between the two carbon atoms.
Be sure to label all orbitals, indicate any orbital overlap, and designate the type of bond that they form. 3. State the bond order for each of the following species: 821', 32, 521+; also state which molecules are paramagnetic and which are diamagnetic. 4. If a mixture with mass of 100.0 grams containing both Na and Hg is reacted with an excess of water, as
shown in the reactions below, the hydrogen is isolated and found to have a total of 9.50 ml of H2 at a
temperature of 25.0°C and 1 atm. How many grams of Na was in the original mixture? Note Hg does not
react with water under these conditions. 2Na(s) + 2 5200) —> 2NaOH(aq) + Hzfg) 5. Light with a wavelength ofynm strikes the surface of cesium in a photocell, and the maximum kinetic
energy of an electron ejected is found to be 5.54 x 10'19 J. ‘ a) Calculate the work function (E) of cesium. b) Calculate the longest wavelength of light that is capable of ejecting electrons from that metal. 6. For the following quantum numbers, determine if that set of quantum numbers is allowed or is not
allowed. (circle one) a) n = 3 Z = 2 m = 1 m5 = +1/2 allowed not allowed
b) n = 6 Z = 2 m = 0 m5 = +1/2 allowed not allowed
c) n = 0 i = 4 m = 2 m5 = +1/2 allowed not allowed Chem 14A2 Final Information/Review Fall 2000 7. For the following isotopes shown below fill in the missing quantities (1 point each) o number of rotons number of neutrons 8. Given the following species circle the one you would predict to have the largest size. a) N 01+ F24
b) Fib1+ Kr Br"
c) F CI I
d) In Sn l 9. Morphine is a weak base with Kb = 8.0 x 10'7. Calculate the pH of a solution made by dissolving
4.50 x 10'2 moles of morphine in water yielding a solution with 350.0 ml of volume. 10. A gas sample with a of volume 2.50 liters at 300.0 K is heated to 1500.0 K assuming constant pressure
and no change in the amount of the gas present what is the volume at 1500.0 K? 11. Answer the following questions referring to the MO correlation diagrams a) Is Al2 diamagnetic? Yes No (circle one) b) ls 82 diamagnetic? Yes No (circle one) o) What is the bond order of B2? d) Is B2 paramagnetic or diamagnetic? (circle one) e) Can Ne2 exist? Yes No (circle one) f) Can Hez“ exist? Yes No (circle one) 12. A container is filled with Br2(g) at an initial partial pressure of 0.0500 atm and 2(g) at an initial partial
pressure of 0.0400 atm. The container is then heated to 350 Kelvin and allowed to reach equilibrium.
Calculate the partial pressures of all three gases at equilibrium. You must use the quadratic equation to
solve this problem. At 350 Kelvin, K: 322 for his reaction. 35(9) + I2(9) 2 lBr(9)
13. For the following molecules: a) Draw the best Lewis Dot structure b) Label any nonzero formal charges present in that molecule c) Name the electronic geometry d) Name the molecular geometry 9) State the orbital hybridization around the central atom t) State it the molecule is polar or nonpolar i. 302 ii. NH3 iii. 002 iv. PPS" v. XeF4 vi. I3" 14. Draw all the resonance structures that contribute to the resonance hybrid of ozone (03). 15. For the reaction N204(g)~“$‘ 2 N02(g) K = 48 , if Q = 1.0 x 10“ for this reaction will the reaction have a
tendency to form products or reactants, or is the system at equilibrium? 16. The total pressure of a mixture of sulfur dioxide and nitrogen at 25 C in a 5.00 x 102 ml vessel is 1.09 atm. The
mixture is passed over warm calcium oxide powder, which removes the sulfur dioxide ($02) by the reaction:
Ca0(s) + 802(g) —> CaS03(s) The remaining gas is then transferred to a 1.50 x 102 ml vessel,
where the pressure is 1.09 atm at 50 C. What was the mass in grams of the SO; in the initial mixture? ...
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This note was uploaded on 02/08/2012 for the course CHEM 14A 142042200 taught by Professor Lavelle during the Spring '10 term at UCLA.
 Spring '10
 Lavelle

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