Question

what orbitals are used to form each of CC and CH bonds in propane​

Answer 1

Answer:

Each of C-C and C-H bonds in propane​ forms sp3

Explanation:

• In the structure of propane, CH3-CH2-CH3, their area total of 10 total bonds.

• Here two carbon-carbon single bonds and eight carbon-hydrogen single bonds are present.

• Each of these single bonds is also termed as a sigma bond.

• Here every hydrogen atom in this molecule forms an s-orbital to form bonds
• The C-C bond present in the propane is formed by overlapping of two sp 3

• Here 3 orbitals and C-H bond is formed by the overlap of an sp 3

• where 3 orbital combines with 1s orbital.
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Answer 2

Answer:

The C-C bond is created when two $sp3$ orbitals overlap, and the C-H bond is created when a $sp3$ orbital overlaps with a 1s orbital.

Explanation:

• The C-C bond is created when two $sp3$ orbitals overlap, and the  CH bond is created when a $sp3$ orbital overlaps with a 1s orbital.

• Propane is a particular class of hydrocarbon known as an alkane. Single covalent bonds hold the atoms in alkane molecules together, and carbon atoms always create four covalent bonds.

• Propane  is a chain of carbon atoms containing two Carbon-Carbon single bonds.

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