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Ple A Typical Triple Bond Consists Of One Sigma And Two Pi Bonds

use the concept of sp hybridization to account for the formation of carbon-carbon triple bonds, and describe a carbon-carbon triple bond as consisting of one σ bond and two π bonds. list the approximate bond lengths associated with typical carbon-carbon single bonds, double bonds and triple bonds. list the approximate bond angles associated with sp3-, sp2- and sp‑hybridized carbon atoms and predict the bond angles to be expected in given organic compounds. account for the differences in bond length, bond strength and bond angles found in compounds containing sp3-, sp2- and sp‑hybridized carbon atoms, such as ethane, ethylene and acetylene.

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Key Terms

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sp hybrid orbital
Study Notes

The bond angles associated with sp3-, sp2- and sp‑hybridized carbon atoms are approximately 109.5°, 120° and 180°, respectively.

Bonding in acetylene

Finally, the hybrid orbital concept applies well to triple-bonded groups, such as alkynes and nitriles. Consider, for example, the structure of ethyne (another common name is acetylene), the simplest alkyne.

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Which Compound Is An Example Of A Network Solid ? A Network Solid: Diamond

The hybrid orbitals used (and hence the hybridization) depends on how many electron groups are around the atom in question. An electron group can mean either a bonded atom or a lone pair. Molecular geometry is also decided by the number of electron groups so it is directly linked to hybridization.

# of Electron Groups Hybrid Orbital Used Example Basic Geometry Basic Bond Angle
2 sp example of sp hybridized carbon.svg

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