1. Bond Order, Length, and Energy

2. Bond Order
The number of bonding electron pairs shared by two atoms in a molecule.
Can be whole numbers as well as fractional numbers.
Draw H2, NH3, and CH4.
Each have a bond order of 1
Draw CO2 and C2H4
The C=O bond in CO2 has a bond order of 2, as does the C=C bond in C2H4.
Draw N2 and CO
Bond orders of 3

3. Bond Order
Draw O3
It has 2 resonance structures, so how do I calculate the bond order?
Bond Order = _[Number of shared pairs in all X-Y bonds]_
[Number of X-Y links in the molecule or ion]
Bond Order = _[Number of bonds]_
[Number of structures]
Each O-O bond has a total of 3 shared pairs/2 structures
Bond Order = 1.5

4. Bond Order Draw C2O4-2 … Draw OCN- …
How many resonance structures are there?
What’s the bond order between Carbon and Oxygen?
Draw OCN- …
What’s the bond order between C and O? C and N?

5. Bond Length Is the distance between the nuclei of two bonded atoms.
Related to 2 things:
Size of the atom
The larger the atom, the longer the bond
H-F < H-Cl < H-Br < H-I
Bond Order
When comparing bonds between the same two atoms, the larger the bond order, the shorter the bond
C-O > C= O > C= O
Single bonds are longer than double bonds, which are longer than triple bonds

6. Bond Length
Compare the bond lengths between carbon monoxide, carbon dioxide, and carbonate ion. Arrange them in order of increasing bond length.
Carbon Monoxide < Carbon Dioxide < Carbonate Ion
Bond order:

7. Bond Enthalpy Bond Dissociation Enthalpy
the enthalpy change for breaking a bond in a molecule with the reactant and products in the gas phase
Enthalpy (ΔH)
The process of breaking bonds in a molecule is always endothermic
ΔH is positive. Energy must be put in to break a bond.
The process of forming bonds in a molecules is always exothermic
ΔH is negative. Energy is released when a bond is formed

8. Bond Enthalpy
ΔHrxn = [∑(Bond enthalpies bonds broken)] – [∑(Bond enthalpies bonds formed)] or ΔHrxn = [∑ ΔHbonds broken ] – [ ∑ ΔHbonds formed]

9. Practice Problems
Compare the nitrogen-nitrogen bond in hydrazine, H2NNH2, with that in “laughing gas”, N2O. In which molecule is the nitrogen-nitrogen bond shorter? In which is the bond stronger?

10. Practice Problems
The compound oxygen difluoride is quite reactive, giving oxygen and HF when treated with water.
OF2(g) + H2O(g)  O2(g) + 2HF(g)
ΔHrxn = -318kJ/mol●rxn
Using bond dissociation enthalpies, calculate the bond dissociation energy of the O-F bond OF2.
H-O = 463 kJ/mol
O=O = 498 kJ/mol
H-F = 565 kJ/mol