Question

*Which of the following is not a reason for anomalous behaviour of an element?*

1️⃣ Small size
2️⃣ High ionisation enthalpy
3️⃣ Absence of vacant d orbital
4️⃣ Poor shielding effect by low lying electrons​

Answer 1

Answer:

Anomalous behavior of lithium is due to extremely small size of lithium. Its cation on account of small size and high nuclear charge, lithium exerts the greatest polarizing effect out of all alkali metals on the negative ion. Consequently, lithium ion possesses a remarkable tendency towards solvation and develops a covalent character in its compounds.

But lithium like other metals of the same group is a strong reducing agent. In fact, Lithium is the strongest reducing agent in aqueous solution.

Explanation:

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Answer 2

Answer:

1️⃣ Small size

Explanation:

Anamaolous behaviour is the different behaviour shown by an element of a group. It has anamolous properties i.e., properties different from its group.

An element's anomalous behaviour makes it distinct from other elements in the same group, and its unique properties show a deviation from the usual properties of the group. An element's abnormal behaviour is defined as its distinct behaviour in comparison to other elements in the same group. It has anomalous properties due to its one-of-a-kind characteristics.

The anomalous behaviour of first element of s and p block elements of each group as compared to other group members is due to following reasons: Small size of atom, large charge/radius ratio, high electronegativity and non availability of d-orbitals in their valence shell. Second period elements show anomalous behavior due to small size, high electronegativity and absence of d-orbitals and fluorine is a second period element.
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