CHEM 343 Quiz: chem quiz study guide ch.5 and 6

List the letter that corresponds to the reagent from the reagenttable you need to carry out the following synthesis in 5 steps orless.
Heat may not appear on the reagent table with the reagent, but youcan assume you have a hot plate and can supply neededheat.
There may be more boxes than you need. Type NA in the blank of any extra box(es).

2-ethylbut-1-ene %u2192 2-ethyl-2-methylbutanoic acid

step 1
step 2
step 3
step 4
step 5

Reagents:

A: HCl, 25o

B: Cl2, h%u03BD

C: Br2, h%u03BD, heat

O: SOCl2, pyridine

E: PBr3

X: conc. H2SO4, heat

G: KOC(CH3)3, HOC(CH3)3, heat

EE: H2, Pd

(other metals: Ni, Rh, Pt)

I: HCl, 0oC

J: 50% H2SO4, H2O

M: HBr, 0oC

F: HBr, peroxides or HBr, h%u03BD

RR: 1. B2H6, diglyme 2. H2O2, NaOH or 1. BH3-THF 2.H2O2, NaOH

P: Cl2 or Br2, CHCl3 or CCl4, dark, cool

Q: Cl2 or Br2, H2O

N: peroxyacetic acid

S: 1. O3 2. H2O, Zn or 1. O3 2. HOCH3(CH3)2S

PP: 1. O3 2. H2O

U: KOCH2CH3 HOCH2CH3

V: NaNH2, NH3

GG: 1. 3NaNH2, NH3 2. H2O

HH: H2, Lindlar

II: Na, NH3

QQ: H2SO4, HgSO4

R: NBS, benzoyl peroxide, CCl4, heat

SS: Na, NH3, HOCH3

BB: Na2Cr2O7, H2O, H2SO4, heat

NN: HNO3, H2SO4

OO: Br2, FeBr3 or Cl2, FeCl3

Z: AlCl3

Y: Zn(Hg), HCl

D: H2NNH2, KOH, triethylene glycol, heat

AA: PCC, CH2Cl2 or PDC, CH2Cl2

TT: Mg

CC: Na

DD: OsO4 (cat) (CH3)3COOH,tert-butyl alcohol,NaOH

JJ: HIO4

KK: LiAlH4

LL: NaBH4

H: NaOH, heat MM: ethylene oxide

K: NaCN

L: NaOH

T: aqueous acid

W: CO2

FF: SOCl2

Practice problems for exam 2 ______________

Useful Information:

h=6.626×10-34J·s.; c=3.0×108 m/sec; E=h ; E= hc ,  = h/mv; 1J = 1 kg-m2/s2 

mass of electron = 9.11 × 10-28 g, E= q + w ; 1 cal = 4.184 Joules Please Show all Work

1. Which of the following substances have standard heats of formation that are equal to zero by definition (circle your answers): H2(g), H(g), O3(g), H2O(s), H2O(l), Hg(l), Hg(s), Hg(g).

2. Limestone stalactites are formed in the reaction: Ca2+(aq) + HCO3-(aq) ïƒ CaCO3(s) + CO2(g) +

H2O(l)
If one mole of CaCO3 is produced at 298 K under one atmosphere of pressure, the reaction performs 590 calories of expansion work, pushing back the atmosphere as CO2 is formed. At the same time, 9310 calories of heat are absorbed from the environment. What is E in Kcal/mole for CaCO3.

3. What is the minimum wavelength of light in Å (1 Å = 10-8 cm) needed to provide enough energy per quantum to rupture the chemical bond in hydrogen iodide (HI). The bond dissociation energy of HI is 71.4 Kcal/mole.

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4. Sketch the shape and orientation of the following types of orbitals: s, px, dxy, dz2, dx2-y2

5. Give the values of (n) , (l) and (ml) for each orbital in the 4p subshell.

6. Write the complete electron configuration for the following: Ti 2+_____________________________________ Cr_______________________________________

N______________________________________

7. Calculate the standard enthalpy of formation (  Ho) for diamond from graphite [i.e. C (graphite) ïƒ C (diamond)] given that:

C (graphite) + O2 ïƒ CO2 (g) (  Ho = -393.5 KJ/mole) C (diamond)] + O2 ïƒ CO2 (g) (  Ho = -395.4 KJ/mole)

If 1.0g of graphite is converted to diamond, what is the energy change? Is this an endothermic or exothermic reaction?

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8. An 160 pound astronaut on his way to Mars is buzzing along at 10,000 miles per hour. (a) Express his weight in grams (one pound = 454 grams) so that you can calculate the astronaut’s wavelength (1mile/hour = 44.7 cm/sec)

(b) Suppose the astronaut detects outside his spacecraft a proton (m=1.7 x 10-24 g) from a “solar wind” moving at exactly the spacecraft velocity. What is the proton wavelength is in Å (1 Å = 10-8 cm.

9. What is the maximum number of electrons that can occupy each of the following subshells? a) 3d_________________ b) 1s____________________ c) 2p ____________________

10. Identify the element represented by the following electronic configuration.

a) [Ne] 3s2____________________

b) What is the electron configuration for the first excited state of this atom.______________

11. Determine the number of valence electrons for each element.
(a) Br___________ (b) Na _________ (c) Sn __________

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12. 175 g of Fe at 15.0oC is mixed with 225 g of H2O at 95.0oC. What is the final temperature of the mixture? The specific heats of iron= 0.448 J/g oC and water = 4.184 J/g oC). (keep in mind the following: heat gained + heat lost = 0 and q=mass x heat capacity x T)

13. (5 pts) Calculate values of ΔHrxn for the following reactions: CS2(g) + 3O2(g)  CO2(g) + 2SO2(g)

The heat of formation for the following substances is given in kJ/mol:

CS2 CO2 SO2 117.4 -393.51 -296.83

14. (6 pts) Use the electron configuration of Li and Be and determine which element has the greatest second ionization energy. Defend your answer.

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15. Mark beside each of the following processes either “exo” or “endo” according to whether you think the process will release heat or absorb heat.

a. Ca(g) ïƒ Ca(g)+2 + 2e-
b. I(g)+1e-ïƒ I(g)-1
c. Ca(g)+2 + S(g)-2 ïƒ CaS(s) d. I2(g)ïƒ 2I(g)

( ) ( ) ( ) ( )

16. (6 pts) In each of the following pairs, which of the two species is larger?
a) O-2 or Na+ b) Ti+4 or Ti+2 c) B or C d) N or N-3

17. Write down the Lewis dot structure for the following (a) N_______________ (b) Ne________________

18. THE BORN HABER CYCLE: I may have a problem on the Born Haber cycle. Please check my lecture notes to see how to set up the process and then calculate the lattice energy from the various thermodynamic quantities such as in the NaCl example below;

 H  f NaCl = -411KJ

Na(s)  Na(g)  H =108KJ
1⁄2 Cl2  Cl(g)  H = 122KJ Ionization Energy of Na  H = 496 KJ Electron affinity of Cl  H = -349KJ