The correct order of the increasing ionic character is

Question

The correct order of the increasing ionic character is (A) BeCl 2< MgCl 2< BaCl 2< CaCl 2 (B) BeCl 2< MgCl 2< CaCl 2< BaCl 2 (C) BeCl 2< BaCl 2< MgCl 2< CaCl 2 (D) BaCl 2 < CaCl 2 < MgCl 2 < BeCl 2

Tardigrade Admin · Accepted Answer

In the alkaline earth metal group, down the group as the size increases the ability to lose electrons i.e. ionic character increases. The smaller metal require more ionisation potential for cation formation.

Q. The correct order of the increasing ionic character is

$B e C l_{2} < M g C l_{2} < B a C l_{2} < C a C l_{2}$

$B e C l_{2} < M g C l_{2} < C a C l_{2} < B a C l_{2}$

$B e C l_{2} < B a C l_{2} < M g C l_{2} < C a C l_{2}$

$B a C l_{2} < C a C l_{2} < M g C l_{2} < B e C l_{2}$

In the alkaline earth metal group, down the group as the size increases the ability to lose electrons i.e. ionic character increases. The smaller metal require more ionisation potential for cation formation.

Q. The correct order of the increasing ionic character is

BeCl2​<MgCl2​<BaCl2​<CaCl2​

BeCl2​<MgCl2​<CaCl2​<BaCl2​

BeCl2​<BaCl2​<MgCl2​<CaCl2​

BaCl2​<CaCl2​<MgCl2​<BeCl2​

In the alkaline earth metal group, down the group as the size increases the ability to lose electrons i.e. ionic character increases. The smaller metal require more ionisation potential for cation formation.

$B e C l_{2} < M g C l_{2} < B a C l_{2} < C a C l_{2}$

$B e C l_{2} < M g C l_{2} < C a C l_{2} < B a C l_{2}$

$B e C l_{2} < B a C l_{2} < M g C l_{2} < C a C l_{2}$

$B a C l_{2} < C a C l_{2} < M g C l_{2} < B e C l_{2}$