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HybridizationFormal Charge | FC = (group #) - (loan pairs + bonds) | Bond Enthalpy | ΔHrxn = (sum of bonds broken) - (sum of bonds formed) | | | Weaker bonds broken provide more exothermic reactions. Weaker product bonds make for a less exothermic reaction. | Bond Order and Length | Shorter bond length = greater bond order | | | Single bonds are the longest and the weakest | | | Triple bonds are the shortest and the strongest | | | Non-integer bond order indicates resonance | Non-polar covalent bonds | ex: Cl-Cl | | | small energy difference in electronegativity | Polar Covalent Bonds | ex: H-Cl | | | medium energy difference | Ionic Bonds | ex: Li-Cl | | | large energy difference (over 1.7) | Average Bond Order | ABO = (# of bonds in the molecule) ÷ (# of resonance structures) |
MO TheoryMO diagram for F2, O2, Ne2, and all other molecules MO TheoryBond Order | (bonds-antibonds) ÷ 2 | Bonds | σ, π | Anti-Bonds | σ, π | Sigma Bond | hybridized \ | Pi Bond | unhybridized p orbital \ | Loan Pair | Spin Paired \ --> X |
| | VSEPRNumber of Electrons | Electron Geometry | Atoms + Loan Pairs | Molecular Geometry | 2 | linear | 2+0 | linear | 3 | trigonal planar | 3+0 | trigonal planar | | | | 2+1 | bent | 4 | tetrahedral | 4+0 | tetrahedral | | | | 3+1 | trigonal pyramidal | | | | 2+2 | bent | 5 | trigonal bipyramidal | 5+0 | trigonal bipyramidal | | | | 4+1 | see-saw | | | | 3+2 | T-shaped | | | | 2+3 | linear | 6 | octahedral | 6+0 | octahedral | | | | 5+1 | square pyramidal | | | | 4+2 | square planar |
PolarityRequirements for a Polar Molecule | Bonds must be polar | | | The molecule cannot have symmetry | | | A bond is polar if one side is more electronegative than the other |
MO TheoryDiagram for B2, C2, and N2 | | The Born-Haber CycleSublimation | Na (s) + 1/2 Cl2 (g) --> Na (g) + Cl (g) | +107.32 kJ | Cl-Cl bond energy | Na (g) + Cl (g) --> Na (g) + 1/2 Cl2 (g) | +121.68 kJ | ionization energy of sodium | Na (g) + 1/2 Cl2 (g) --> Na+(g) + Cl (g) + e- | +496 kJ | Electron Affinity of Cl | Na+(g) + Cl (g) + e- --> Na+ (g) + Cl- (g) | -349 kJ | Lattice Energy of NaCl | Na+ (g) + Cl- (g) --> NaCl (s) | -786 kJ |
Sigma and Pi BondsValence Bond Theory | When two atoms are in close proximity to one another, they arrange themselves at the lowest possible energy | Sigma bonds | Formed by end-on overlap of orbitals along the internuclear axis | | | the electron density is highest right between the two atoms | Pi bonds | Formed by side on overlap of orbitals | | | there is no electron density between the atoms | | | Weaker than sigma bonds | Valence electron pairs | Electron Geometry | Hybridization | 2 | linear | sp | 3 | trigonal planar | sp2 | 4 | tetrahedral | sp3 | 5 | trigonal bipyramidal | sp4 | 6 | octahedral | sp5 | Single Bonds | one sigma bond | Double Bonds | one sigma, one pi bond | Triple Bonds | one sigma, two pi bonds |
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