Lycoming College Write name on back,
Chem 110, 2002 Exam III upper right
1. Matching: match the items in the right column by writing in the letter of a selection from the items in the left.
A. Pauli _____ h
B. Bohr’s DE _____
C. Planck's constant _____ -
D. AX5E _____ trigonal bipyramidal
E. Hund _____ 6.626 x 10-34
F. AX5 _____ octahedral
G. speed of light _____ parallel spins when possible
H. DHrxn, estimated _____ sp3
I. AX6 _____ no two e- with the same four quantum numbers
J. = _____ 2.998 x 108 m/sec
K. AX4 _____ square pyramidal
L. Planck’s quantization, E = _____ - 2.179 x 10-18 J -
2. Deduce the ground-state electron configuration (core notations acceptable) for:
a) zinc, 30Zn
b) zinc(II) ion ion, 30Zn2+
c) americium, 95Am
d) Provide an electron occupancy (orbital box) diagram for the valence shell electron configuration of phosphorus, 15P.
3. a) Calculate the energy (in joules), the frequency (in sec-1), and the wavelength (in nm) of the light associated with the transition of the electron in a hydrogen atom from state n = 2 to state n = 3.
b) For the transition from state n = 2 to state n = 3, is the light absorbed or emitted by the atom? ______
4. Name or give the symbol for the element that fits each description:
______a) [Rn] 7s2
______b) Alkali metal with a 5s valence electron configuration
______c) Of Na, Mg, Al, Si, the element whose big “jump” in successive ionization energies would occur between IE2 and IE3
______d) 1s2 2s22p6 3s23p6 4s23d104p6 5s14d5
______e) Heaviest element which has a half-filled p subshell
______f) Element with the smallest first ionization energy
______g) Element with the smallest electronegativity (noble gases excepted)
______h) A fourth-row, d-block element having only two unpaired electrons (4th row starts with K)
______i) Another fourth-period, d-block element having only two unpaired electrons
______k) Of S2-, Cl1-, Ca2+, the atom or ion having the largest radius
______l) Of Ca, Cr, and Zn, the metal which would be paramagnetic
______m) An element whose “last-filled-in” electron has quantum numbers n = 3, l = 2, ml = 2
______n) A non-metal incapable of octet expansion.
5. In each of the following bonds, on which atom would a partial negative charge (d-), if any, be located:
a) N____C b) C____S c) S____F
Electronegativies are: cC = 2.5 cN = 3.0 cS = 2.5 cF = 4.0
Which of the bonds will be the most polar? ________ Which of the bonds is essentially nonpolar? _______
6. The carbon-oxygen bond lengths in the series of molecules H3COH, H2CO , and CO are 143 pm, 123 pm, and 113 pm, respectively. Draw complete Lewis structures for each of these molecules, and then explain the observed variation in bond length. The formulas are written so as to indicate topologies.
H3COH H2CO CO
7. Use each of the following Lewis dot structures (correct for dots, but not necessarily for geometries) to predict the molecular shape, estimate the bond angle, indicate whether the species will be polar or nonpolar, and give the valence bond theory hybridization state which would best explain the central atom.
a) molec. shape __________; bond angle ______; polarity________; hybridization ___
b} molec. shape __________; bond angle ______; polarity________; hybridization _____
c) molec. shape __________; bond angle ______; polarity________; hybridization _____
d) molec. shape __________; bond angle ______; polarity________; hybridization _____
8. A satisfactory Lewis structure for carbonate ion (CO32-) looks like
a) Write in formal charges for each atom in the structure shown above.
b) What is the shape of this ion? ____________________________
c) What is the O-C-O bond angle, in degrees? __________________________
d) How many sigma () bonds, total, are represented in the structure? _____; pi () bonds? ________
d) Experiments indicate that all three carbon to oxygen distances in CO32- are equal, and intermediate between a single and double bond length. Explain this observation, using dot structures as appropriate.
9. Estimate DHrxn for the bromination of acetone reaction, using information from the bond energy table shown below.
Dot figures may help
Bond Energy, kJ/mol CH3COCH3 + Br2 ŕ CH3COCH2Br + HBr DH = ??
10. Consider the following compounds:
CH3CH=CHCl CH2=CHCH3 CHF=CHCl CH3CH=CHCH3 CH3C CCH3
How many of these five compounds can exist as cis-trans isomers? 0, 1, 2, 3, 4, all 5
For one of the compounds that you think can exist in cis and trans forms, draw and label better structural diagrams of each isomer below. Also, with arrows pointing to each carbon, indicate the hybridization state of each carbon atom in your structures.