[dolimitless]

Why are the Bond Dissociation Energies in C-H bonds higher in less substituted alkanes?. I know the the more highly substituted free radicals are more stable, but why are the BDE in the C-H bond, say in a primary carbon, harder to break than a tertiary carbon?

[Sn3]

Think about what cations are most stable (primary, secondary or tertiary carbocations) and this should lead you in the right direction.

[Schrödinger]

Think about what cations are most stable (primary, secondary or tertiary carbocations) and this should lead you in the right direction.

Isn't that reasoning valid only if you try to remove H^- or H^.?
What if you try to remove H⁺? That leaves you with a carbanion. In that case, order in the bond enthalpies will be the opposite right?