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Hybridization: Localized Electron Model

Hybridization: Localized Electron Model. Why Hybridization Occurs. Example: Methane (CH 4 ) 4 hydrogens bonded to the central carbon atom The 4 electrons involved in bonding on the C atom are: 2s 2 2p 2 Which of these electrons have higher energy levels?

raven-simmons
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Hybridization: Localized Electron Model

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  1. Hybridization: Localized Electron Model

  2. Why Hybridization Occurs • Example: Methane (CH4) • 4 hydrogens bonded to the central carbon atom • The 4 electrons involved in bonding on the C atom are: • 2s2 • 2p2 • Which of these electrons have higher energy levels? • But all 4 bonds have the SAME energy level.

  3. Why Hybridization Occurs (continued) • To accomplish this “same energy level bonds” arrangement, the 4 electron orbitals “hybridize” to a combined s and p orbital, with energy somewhere between the two original s and p orbitals.

  4. Carbon Hybridization

  5. Hybridization Generalizations • Hybridizations refer to effective pairs! • A double bond is how many effective pairs? • A triple bond is how many effective pairs? • 4 effective pairs = sp3 orbitals • 3 effective pairs = sp2 orbitals • 2 effective pairs = ????? • 5 effective pairs = ?????

  6. sp2 Hybridization • Example: H2CO • Central atom? • How many effective pairs around the central atom? • What electrons on the C atom are involved in bonding? • This time, the 2s2 and 2p2 electrons only need to hybridizes to form 3 orbitals. • You will have 3 sp2 hybrid orbitals and a lone original p orbital.

  7. H2CO Carbon Hybridized Orbitals

  8. H2CO Oxygen Orbitals • How many effective pairs exist around the oxygen atom in H2CO? • What type of hybridization is this? • In the molecule, how may of each of the following exist? • Lone pairs • Single bonds • Double bonds • Hybrid orbitals on the C atom • Hybrid orbitals on the O atom • Regular (unhybridized) orbitals on C/O atoms

  9. sp2 Hybridization and Double Bonds • σ (“sigma”) bonds join the atoms together in single OR multiple bonds. • In a multiple bond, π bonds are composed of overlapping regular p orbitals parallel to the main σ bond.

  10. H2CO Orbital Diagram What is missing from this orbital diagram???

  11. sp Hybridization How many effective pairs would be on the atom? If we are still examining C, which electrons (and orbitals) are involved in bonding? So what would the new orbitals be AFTER hybridization? Example: acetylene (ethyne) C2H2

  12. dsp3 Hybridization • How many effective pairs on the atom? • Why can’t we use C as an example? • Give me an element we CAN use. • Example 1: (using element provided) • Example 2: I3-1 • Determine the BEST Lewis structure based on formal charges. • Examine the bond types on each I atom.

  13. 6 Effective Pairs What would the hybridization be? Give an example of a molecule you have “seen” that has 6 effective pairs.

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