Question

The H⁻ ion can be formed in ordinary chemical reaction under proper conditions, but the H⁺ ion cannot. The best explanation for this difference is due to
(a) the radius of the H nucleus
(b) the electronegativity of H atom.
(c) the ionisation energy of the H-atom
(d) the bond dissociation energyof H–H bond

Answer 1

this is because it has to complete its duplet so gorm h+ion not h- which has no electron so no valency since no electrons

Answer 2

Answer:

Because of the difference in radius,$H^{+}$ can't exist, while $H^{-}$can. As a result, A is the proper response.

Explanation:

Because hydrogen only has one electron, it has the configuration $1s^{1}$

When an electron loses a hydrogen atom, the nucleus (H+) shrinks to        $1.5$×$10^{-3}$pm in size, which is very tiny in comparison to typical atomic or ionic sizes. As a result, H+ ions are no longer free to exist.

A hydrogen ion cannot exist independently because when a hydrogen atom loses electrons, all that has been left is a proton. It transforms into the positively charged hydrogen ion known $H^{+}$, which is  unstable to exist in ordinary condition