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Hybrid Orbitals with Multiple Bonds
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Hybridization with Multiple Bonds
Still dealing with covalent bonds Looking more in depth at the traits of covalent bonds Chemical bonds—region of orbital overlaps
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C2H4
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Sigma(σ) Bonds All single covalent bonds
Involves ONE HYBRIDIZED orbital Formed by orbital overlap (orbitals do NOT have to be the same) Resembles an “s” orbital when looking at chemical bond σ bond framework = electron group geometry Example: Figure 10.21(a) p. 412
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Pi(π) Bonds Covalent bonds
Involves half-filled, unhybridized orbitals Resembles a “p” orbital when looking at bond Created by “parallel orbital overlap” from remaining “p” orbitals Half-filled p orbitals
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Multiple Covalent Bonds
Combination of sigma and pi bonds Double covalent bonds— 1 sigma bond 1 pi bond Triple covalent bonds— 2 pi bonds
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Again…. C2H4
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Example 1: Formic acid (HCOOH) Molecular geometry Hybridization
Bonding scheme
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Example 2: Nitric Acid (HNO3) Molecular geometry Hybridization
Bonding scheme
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Example 3: Methanol (CH3OH) Molecular geometry Hybridization
Bonding scheme
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