Question

The charge/size ratio of a cation determines its polarizing
power. Which one of the following sequences represents
the increasing order of the polarizing power of the cationic
species, K⁺, Ca²⁺, Mg²⁺, Be²⁺ ?
(a) Ca²⁺ < Mg²+ < Be²+ < K⁺
(b) Mg²⁺ < Be²⁺ < K⁺ < Ca²⁺
(c) Be²⁺ < K⁺ < Ca²⁺ < Mg²⁺
(d) K⁺ < Ca²⁺ < Mg²⁺ < Be²⁺

Answer 1

Answer:

The charge/size ratio of a cation determines its polarizing

power. Which one of the following sequences represents

the increasing order of the polarizing power of the cationic

species, K⁺, Ca²⁺, Mg²⁺, Be²⁺ ?

(a) Ca²⁺ < Mg²+ < Be²+ < K⁺

(b) Mg²⁺ < Be²⁺ < K⁺ < Ca²⁺

(c) Be²⁺ < K⁺ < Ca²⁺ < Mg²⁺

(d) K⁺ < Ca²⁺ < Mg²⁺ < Be²⁺

Answer 2

K⁺ < Ca²⁺ < Mg²⁺ < Be²⁺ is the trend of polarizing power.

Explanation:

• The polarizing power of a cation depends on two factors

• A. The charge of the cation.

• B. The size of the cation.

• The polarizing power varies directly with the charge of cation and varies inversely with the size of the cation.

• Here potassium has charge of +1, so has least polarising power.

• Among beryllium, magnesium and calcium, beryllium belongs to 2nd period, magnesium to 3rd period and calcium to 4th period.

• So size varies as Be < Mg < Ca due to addition of new shell of electrons.

• Thus, the polarizing power of the ions varies as K⁺ < Ca²⁺ < Mg²⁺ < Be²⁺.

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