Question

1) Which of the following atoms or ions has the highest ionization energy ?

a) Na b) Al c) Si d) P^3- e) Mg²⁺

2) Which of the following ions is expected to have the largest radius in the gas phase ?

a ) Sb^3- b) In⁺ c) Br^_ d) Te^2- e) Sn²⁺

3 ) Which of the following molecules is planar ?

a) CF₄ b)SF₄ c) PF₃ d) IF₅ e) XeF₄

_{PLEASE ANSWER THEM ALL. THEY ARE NOT LONG QUESTIONS. SIMPLE EXPLANATION IS ENOUGH ( MAYBE A SENTENCE OR SO ) THANKS A LOT IN ADVANCE.}

Answer 1

1) Mg2+ has highest ionization energy because both of its valence electrons are already taken out and it has attained the stable inert gas configuration. So further removal of electron will require very high amount of energy.

2)Sb3- will have highest ionic radius .This is because atomic radius decreases across a period and decreases down the group.Also whe electron is added radius increases and when electron is taken out atomic radius decreases. Sb 3- has three extra electrons and belongs to 5th period.

3)XeF4 is planner.Hybridization of Xenon in XeF4 is sp3d2 creating 6 hybrid orbitals which are directed along the apex of a regular octahedron.The two axial orbitals carry two lone pairs and four Fluorine atoms are in one plane.