At large interatomic separations, an alkali halide molecule MX has a lower energy as two neutral atoms, M + X ; at short separations, the ionic form ( M + ) ( X − ) has a lower energy. At a certain distance, R c , the energies of the two forms become equal, and it is near this distance that the electron will jump from the metal to the halogen atom during a collision. Because the forces between neutral atoms are weak at large distances, a reasonably good approximation can be made by ignoring any variation in potential V(R) for the neutral atoms between R c and R = ∞ . For the ions in this distance range, R c is dominated by their Coulomb attraction. (a) Express R c for the first ionization energy of the metal M and the electron affinity of the halogen X. (b) Calculate R c for LiF, KBr, and NaCl using data fromAppendix F.
At large interatomic separations, an alkali halide molecule MX has a lower energy as two neutral atoms, M + X ; at short separations, the ionic form ( M + ) ( X − ) has a lower energy. At a certain distance, R c , the energies of the two forms become equal, and it is near this distance that the electron will jump from the metal to the halogen atom during a collision. Because the forces between neutral atoms are weak at large distances, a reasonably good approximation can be made by ignoring any variation in potential V(R) for the neutral atoms between R c and R = ∞ . For the ions in this distance range, R c is dominated by their Coulomb attraction. (a) Express R c for the first ionization energy of the metal M and the electron affinity of the halogen X. (b) Calculate R c for LiF, KBr, and NaCl using data fromAppendix F.
At large interatomic separations, an alkali halide molecule MX has a lower energy as two neutral atoms,
M
+
X
; at short separations, the ionic form
(
M
+
)
(
X
−
)
has a lower energy. At a certain distance,
R
c
, the energies of the two forms become equal, and it is near this distance that the electron will jump from the metal to the halogen atom during a collision. Because the forces between neutral atoms are weak at large distances, a reasonably good approximation can be made by ignoring any variation in potential V(R) for the neutral atoms between
R
c
and
R
=
∞
. For the ions in this distance range,
R
c
is dominated by their Coulomb attraction.
(a) Express
R
c
for the first ionization energy of the metal M and the electron affinity of the halogen X.
(b) Calculate
R
c
for LiF, KBr, and NaCl using data fromAppendix F.
Formula Formula Bond dissociation energy (BDE) is the energy required to break a bond, making it an endothermic process. BDE is calculated for a particular bond and therefore consists of fragments such as radicals since it undergoes homolytic bond cleavage. For the homolysis of a X-Y molecule, the energy of bond dissociation is calculated as the difference in the total enthalpy of formation for the reactants and products. X-Y → X + Y BDE = Δ H f X + Δ H f Y – Δ H f X-Y where, ΔHf is the heat of formation.
At an electrified interface according to the Gouy-Chapman model, what types of interactions do NOT occur between the ions and the solvent according to this theory?
Please predict the products for each of the
following reactions.
Clearly show the regiochemistry (Markovnikov
vs anti-Markovnikov) and stereochemistry
(syn- vs anti- or both).
If a mixture of enantiomers is formed, please
draw all the enantiomers.
Hint: In this case you must choose the best
answer to demonstrate the stereochemistry of
H2 addition.
1.03
2. (CH3)2S
BIZ
CH₂OH
2. DMS
KMnO4, NaOH
ΖΗ
Pd or Pt (catalyst)
HBr
20 1
HBr
ROOR (peroxide)
HO
H-SO
HC
12 11 10
BH, THE
2. H2O2, NaOH
Brz
cold
HI
19
18
17
16
MCPBA
15
14
13
A
Br
H₂O
BH3⚫THF
Brz
EtOH
Pd or Ni (catalyst)
D₂ (deuterium)
1. Os04
2. H2O2
CH3CO3H
(peroxyacid)
1. MCPBA
2. H₂O*
H
B
+
H
H
H
"H
C
H
H
D
Explain how Beer’s Law can be used to determine the concentration in a selected food sample. Provide examples.
Chapter 3 Solutions
Student Solutions Manual for Oxtoby/Gillis/Butler's Principles of Modern Chemistry, 8th
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