2,2-dimethylpropane has a lower boiling point of 10°C, and pentane has a higher boiling point of 30°C, even though they have the same number of carbons. Account for the validity of this statement.

The boiling point of a compound is determined by the strength of the intermolecular forces between its molecules. In the case of 2,2-dimethylpropane, the molecule is highly branched, which results in a more compact and spherical shape. This shape reduces the surface area available for intermolecular interactions, leading to weaker van der Waals forces between molecules. As a result, 2,2-dimethylpropane has a lower boiling point.

On the other hand, pentane has a linear structure, which allows for more surface area contact between molecules. This results in stronger van der Waals forces between pentane molecules, leading to a higher boiling point compared to 2,2-dimethylpropane.

Therefore, even though both compounds have the same number of carbons, their different molecular structures result in different boiling points due to variations in intermolecular forces.

The validity of this statement cannot be determined as the molecular formula of 2,2-dimethylpropane is C5H12 and not C3H8 as given in the statement.