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# The terminal C atom in butane is _______ hybridized.(A) \$ds{{p}^{2}}\$(B) \$sp\$ (C) \$s{{p}^{2}}\$ (D) \$s{{p}^{3}}\$

Last updated date: 06th Sep 2024
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Hint: There are 2 terminal carbons in the butane chain and both of them have the same hybridization. Both the terminal carbon atoms form 4 single bonds.

Complete step by step solution:
Butane is a member of the alkane group. It has 4 carbons. It has a straight-chain structure.
The formula of butane is \${{C}_{4}}{{H}_{8}}\$
Since it is a member of the alkane group, all the bonds in butane will be a single bond.
So the structure of butane is given below:

So, there are two terminal carbon atoms in the butane, carbon number one and four.
Both the carbon atoms are connected to three hydrogen atoms and one propyl group.
There are some steps which can help to calculate the hybridization of an atom:
First, look at the atom and count the number of atoms or molecules to which it is connected. If the atom has lone pairs, then it is also counted.