Explain the difference in the bond dissociation energies for the following bonds: ( C — F , 45 0 kJ/mol ) , ( C — Cl , 33 0 kJ/mol ) , ( C — Br , 270 kJ/mol ) , ( C — I , 240 kJ/mol ) .
Explain the difference in the bond dissociation energies for the following bonds: ( C — F , 45 0 kJ/mol ) , ( C — Cl , 33 0 kJ/mol ) , ( C — Br , 270 kJ/mol ) , ( C — I , 240 kJ/mol ) .
Solution Summary: The author explains the differences in the bond dissociation energies for the given chemical bonds.
Explain the difference in the bond dissociation energies for the following bonds:
(
C
—
F
,
45
0
kJ/mol
)
,
(
C
—
Cl
,
33
0
kJ/mol
)
,
(
C
—
Br
,
270
kJ/mol
)
,
(
C
—
I
,
240 kJ/mol
)
.
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.
Is this system endothermic or exothermic, and why? *
H2 + CO2 CH202
Reactant bond energies: H-H is 432 kJ/mol, C=O is 799 kJ/mol
Product bond energies: C-H is 413 kJ/mol, C=0 is 745 kJ/mol, C-O is 358 kJ/mol, O-H is 467 kJ/mol
It is exothermic because more energy is given off by the products versus the amount
needed to break up the reactants.
It is exothermic because more energy is needed to break up the reactants versus the
amount given off by the products.
It is endothermic because more energy is needed to break up the reactants versus the
amount given off by the products.
It is endothermic because more energy is given off by the products versus the amount
needed to break up the reactants.
5.
Consider the following information:
1st ionization energy of Na(g) = 495.8 kJ/mol
Bond dissociation energy of O2(g) = 498.4 kJ/mol
1st electron affinity of O(g)=-142.5 kJ/mol
2nd electron affinity of O¹(g) = 844 kJ/mol
Lattice energy of Na2O(s) = -2608 kJ/mol
Enthalpy of formation of Na2O(s) = -416 kJ/mol
a
Draw the Born-Haber cycle for Na₂O(s).
b
Calculate the unknown. 120
C
Draw the Lewis symbol for Na₂O.
The enthalpy change for the following reaction is -148 kJ. Using bond energies, estimate the C-H bond energy in CH3CI(g).
CH3CI(g) + Cl₂(g) →→→CH₂Cl₂(g) + HCl(g)
kJ/mol
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