What is the reason for anomalous behaviour of lithium?

Lithium shows anomalous behavior due to its small size. The polarizing power of lithium ion is highest of all the alkali metal ion . Because of small size, Lithium is very hard, less reactive as compare to other alkali metals like sodium and potassium.

What is the reason for anomalous behaviour?

Reasons for Anomalous Periodic Properties The reasons for differences in periodic properties and hence in chemical behaviour are: Small size of these atoms. High electronegativity. Large charge/radius ratio.

What are the reasons for anomalous behaviour of lithium and beryllium?

Compounds of lithium are partially soluble in water whereas the alkali metals are highly soluble in water. Beryllium: The anomalous properties of beryllium is mainly due to its small size, high electronegativity, high ionization energy and high polarizing power compared to the other elements in the block.

What is anomalous behaviour of lithium Class 11?

The anomalous behaviour of lithium is as follows: Lithium is harder than other metals of the respective group. It has higher Melting and boiling point than other metals. As the polarizing power decreases with the increasing size of the ions the other alkali metal ions usually form anhydrous salts.

Why Is lithium the least reactive?

Lithium is the least reactive because it is the one with the least electrons. That means the electrons are closer to the nucleus and therefore more attracted to it.

What are the reason for the anomalous Behaviour of first element of each group in P block elements?

a) Compounds of lithium have significant covalent character. While compounds of other alkali metals are predominantly ionic. Lithium reacts with nitrogen to form lithium nitride while other alkali metals do not form nitrides.

What are the reason for the anomalous properties of the first member of a group of elements?

The main reason for showing anomalous properties of the first member of a group in s or p-block is. Tendency to form multiple bonds. Due to small size,large charge/radius ratio and high electronegativity,the first elements shows anomalous behavior.

Why lithium and beryllium form covalent compounds explain?

Lithium and beryllium are exceptionaly small in their respective groups. It’s hard to remove the electron from their last shell making formation of ions difficult. As a consequence, these elements are more prone to form covalent bonds.

What does the first member of each group show anomalous behaviour explain by taking lithium as an example?

First member of each group of representative elements (i.e, s- and p-block elements) shows anomalous behaviour due to i) small size, ii) high ionisation enthalpy, iii) high electonegartivity and (iv) absence of d-orbitals e.g. in s-block elements, lithium shows anomalous behaviour from rest of the alkali metals.

In what respects does lithium differs from other alkali?

The key difference between Lithium and other alkali metals that we can tell is that the lithium is the only alkali metal that can react with nitrogen whereas the other alkali metals cannot undergo any reaction with nitrogen. Moreover, lithium cannot form an anion while other alkali metals can form anions.

What is the anomalous behaviour of lithium in organic solvents?

Anomalous behaviour of Lithium is due to 1) very small size of lithium atom and its ions. 2) higher polarising power of Li + resulting in increased covalent character of its compounds which is responsible for their solubility in organic solvents.

What are the properties of lithium that make it unique?

1) very small size of lithium atom and its ions. 2) higher polarising power of Li+ resulting in increased covalent character of its compounds which is responsible for their solubility in organic solvents. 3) comparatively high ionization enthalpy and low electropositive character of lithium as compared to other alkali metals.

Why is there a diagonal relationship between magnesium and lithium?

Lithium is extremely electropositive in nature. This is the reason why it can form covalent bonds. The polarization behaviour of its ion somewhat in the same lines as magnesium ion. Therefore, there exists a diagonal relationship between magnesium and lithium.

What happens when lithium is burnt in air?

4) When burnt in air or nitrogen, lithium forms Lithium nitride due to its high lattice energy. The Other alkali metals do not form their corresponding nitrides because their lattice energies decreases as their size increases from Na to Cs.