To draw the line bond structure of propane, we start by representing the carbon backbone. Propane has three carbon atoms connected in a straight chain. Each carbon atom is attached to enough hydrogen atoms to satisfy carbon’s tetravalency.
The line bond structure of propane can be illustrated as follows:
H H H
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H – C – C – C – H
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H H H
In reality, we can simplify the depiction to:
CH3 – CH2 – CH3
In terms of bond angles, the carbon-carbon-carbon (C-C-C) bond angle in propane is approximately 109.5 degrees. This is because propane adopts a tetrahedral geometry around each of the carbon atoms due to sp3 hybridization.
The overall shape of the propane molecule is described as a ‘trigonal planar’ arrangement around each central carbon, even though it has a linear connection making it an acyclic or straight-chain alkane. The molecule’s configuration results in its non-polar characteristic as well, since symmetrical arrangements lead to even distribution of electron density.
In summary, propane’s three carbon atoms create a linear arrangement, with bond angles close to 109.5 degrees, leading to a mostly tetrahedral geometry around each carbon, resulting in its overall shape.