Hybrid Orbitals. Sigma Bond (σ) Covalent bond which the electron density is concentrated symmetrically along the internuclear axis Line joining the two.

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Presentation transcript:

Hybrid Orbitals

Sigma Bond (σ) Covalent bond which the electron density is concentrated symmetrically along the internuclear axis Line joining the two nuclei passes through middle of overlap Could be two s orbitals overlap, two p orbitals overlap or an s and p overlap

Pi Bond (π) Overlap of orbital is perpendicular to line connecting nuclei Two p orbitals overlapping Since not a total overlap pi bonds tend to be weaker than sigma

Bond Types Single bonds are always sigma Double bonds consist of a sigma and a pi bond Triple bonds, sigma and two pi

Hybrid Orbitals Mixing of s and p orbitals creates hybrid orbitals CH 4 has four bonds coming from central atom Each bond is formed by overlap of an sp hybrid orbital

Types of Hybrids sp 3 hybrid – one s and three p orbital joined sp 2 hybrid – one s and two p orbitals sp hybrid – one s and one p orbital Hybrid orbital type accounts for observed geometry

Unshared Pairs Unshared pairs can occupy hybrid orbital NH 3 H 2 O

Predicting Hybrid Orbitals Draw structure Determine electron pair geometry Specify hybrid orbitals needed to accommodate the electron pairs

Examples What type of hybrid orbitals in –BeH 2 –BF 3 –NH 2 - –SF 4