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Chapter 14

Chapter 14. Covalent Bonding: Orbitals. SP 3 Hybridization of methane. The 2s orbital and the three 2p orbitals are combined to form four equivalent orbitals, called sp 3 hybrids. SP 2 Hybridization of ethylene. One 2s and two 2p orbitals are used to form these hybrid orbitals.

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Chapter 14

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  1. Chapter 14 Covalent Bonding: Orbitals

  2. SP3 Hybridization of methane The 2s orbital and the three 2p orbitals are combined to form four equivalent orbitals, called sp3 hybrids.

  3. SP2 Hybridization of ethylene • One 2s and two 2p orbitals are used to form these hybrid orbitals. • Use px and py to hybridize.

  4. SP Hybridization of CO2

  5. SP Hybridization of CO2

  6. SP Hybridization of CO2

  7. SP Hybridization of CO2

  8. SP Hybridization of CO2

  9. dsp3 Hybridization

  10. dsp3 Hybridization

  11. d2sp3 Hybridization

  12. The combination of hydrogen 1s atomic orbitals to form MOs

  13. The rules of molecular orbital theory 1. The electron probability of both MOs is centered along the line passing through the two nuclei. 2. The MOs are available for occupation by electrons. The 1s atomic orbital of the hydrogen atoms no longer exist. 3. If the two electrons occupy the lower energy MO, this situation favors molecule formation. (Bonding)

  14. The rules of molecular orbital theory 4. If the two electrons were forced to occupy the higher energy MO, the separated state would be favored. (Antibonding) 5. The electrons have the greatest probability of being between the nuclei on bonding MO. 6. Bonding MO:σ1s Antibonding MO:σ1s* 7. Electrons configuration 1σ1s2

  15. Molecular Orbitals of Li2 (1s22s1)

  16. Bond Order Larger bond order indicates the greater bond strength.

  17. Molecular Orbitals of B2 (1s22s22p1)

  18. Molecular Orbitals of B2

  19. Paramagnetism and Diamagnetism • Paramagnetism causes the substance to be attracted toward the including magnetic. • Diamagnetism causes the substance to be repelled from the including magnetic. • Paramagnetism is associated with unpaired electrons, and diamagnetism is associated with paired electrons.

  20. When liquid oxygen is poured into the space between the poles of a strong magnet, it remains there until it boils away.

  21. Bond order =?

  22. The Correctly Molecular Orbitals of B2 • The σ2p orbital is changed by p-s mixing, the energies of π2p and σ2p orbitals are reverse. • The p-s mixing also changes the energies σ2p and σ2p* such that they are no longer equally spaced relative to the energy of the free 2s orbital.

  23. The Order in MOs Filling

  24. Electron Characterization in MO • Degenerate orbitals:electrons in an atomicsubshell are orbitals at identical energy levels. • Multiplicity: M=2S+1 M=1 singlet M=2 doublet M=3 triplet

  25. NO

  26. NO+ and CN-

  27. Molecular Orbital of HF

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