1. Ch. 9: Chemical Bonding I: Lewis Theory (cont’d)
Dr. Namphol Sinkaset
Chem 200: General Chemistry I

2. I. Chapter Outline Introduction Energy of Ionic Bond Formation
Energy of Covalent Bond Formation

3. I. Energies of Bond Formation
Previously in this chapter, we talked about how ionic and covalent bonds form.
Now we look at the energies involved.
For ionics, we apply Hess’s Law.
For covalents, we use bond energies (enthalpies).

4. II. Ionic Bond Formation
Recall that we envision the creation of ionic bond as an e- transfer from the metal to the nonmetal.
However, if we look at the energies involved in these two steps, we see something puzzling.

5. II. Ion Formation for NaCl
We break up the e- transfer process into two steps and add up the energies.
Na(g)  Na+(g) + e IE1 = 496 kJ/mole
Cl(g) + e-  Cl-(g) EA = -349 kJ/mole
Na(g) + Cl(g)  Na+(g) + Cl-(g) IE1 + EA = 147 kJ/mole

6. II. Other Energies
For most ionics, this is typical; ion formation is an endothermic process.
So why do ionics form at all?
There must be a huge exothermic process to offset these endothermic processes.
The strong +/- attractions that are formed are the source of this exo step.

7. II. Lattice Energy
lattice energy: the energy associated with forming a crystalline lattice of alternating cations and anions from gaseous ions.

8. II. Born-Haber Cycle
Although lattice energy is a critical component of ionic bond formation, it cannot be measured directly.
We use Hess’s Law in the Born-Haber Cycle.

9. II. Born-Haber Cycle for NaCl

10. II. Calculating Lattice Energy
Since enthalpy is independent of path, the following equation applies.
ΔH˚f = ΔH˚atom + ΔH˚BE + ΔH˚IE + ΔH˚EA + ΔH˚lattice

11. II. Sample Problem
Calculate the lattice energy for CaCl2 given the following enthalpy values: heat of sublimation for Ca = kJ/mole, Cl2 bond energy = 243 kJ/mole, 1st ionization energy Ca = kJ/mole, 2nd ionization energy Ca = kJ/mole, 3rd ionization energy Ca = kJ/mole, electron affinity Cl = -349 kJ/mole, heat of formation CaCl2 = kJ/mole.

12. III. Covalent Bond Strength
The strength of a covalent bond depends on how strongly the e- are held by both nuclei.
The bond energy or bond enthalpy (BE) is the energy needed to overcome this attraction. It is defined as the energy needed to break 1 mole bonds in the gas phase
Another way to envision it…

13. III. Formation of H2

14. III. Bond Energies Breaking bonds require energy…
A-B(g)  A(g) + B(g) ΔH˚break = BEA-B
Forming bonds releases energy...
A(g) + B(g)  A-B(g) ΔH˚form = -BEA-B
Different bonds have different levels of attraction (have different depths to their wells) and thus different BE’s.

15. III. BE’s and Chemical Change
In a reaction, bonds are broken and new bonds are formed.
Relative strengths of bonds determine whether rxn is exo or endo.
The energy released or absorbed in a reaction is due to the difference between reactant and product bond energies.

16. III. Estimating Rxn Enthalpies

17. III. Calculating w/ BE’s
A reaction can be considered a two-step process:
Heat absorbed to break bonds
Heat absorbed to make bonds
We can sum these to get the heat of reaction.

18. III. Sample Problem
Calculate ΔH˚rxn for the reaction shown below. Use the indicated bond enthalpies.