Which two orbitals overlap to form the sigma bond between C and H in C2HF?
To determine which two orbitals overlap to form the sigma bond between carbon (C) and hydrogen (H) in C2HF, we need to examine the molecular orbital (MO) theory.
1. Start by drawing the Lewis structure of C2HF:
C - C - H
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F
There is a single bond between each carbon (C), and one hydrogen (H) is attached to one of the carbons (C). Also, there is a fluorine (F) atom connected to one of the carbons (C).
2. Identify the hybridization of the carbon atoms:
In C2HF, both carbon atoms are sp hybrids, meaning they have one s orbital and one p orbital participating in bonding. The hybridization of carbon is influenced by its surroundings. Since carbon is bonded to four other atoms (two other carbons and one hydrogen in this case), it adopts an sp hybridization.
3. Determine the individual orbitals contributing to the sigma bond between C and H:
In sp hybridization, one s and one p orbital combine to form two sp hybrid orbitals. One of these sp hybrids on each carbon overlaps with the s orbital of hydrogen to form sigma bonds. The other sp hybrids on each carbon form sigma bonds with the other carbon atoms.
Therefore, the sigma bond between the carbon (C) and hydrogen (H) in C2HF is formed by the overlap of the sp hybrid orbital on carbon with the s orbital on hydrogen.