Arrange the following in increasing order of property indicated:
(i) Li, Be and B (ionization energy)
(ii) F, Cl, Br, I (electron affinity)
(iii) SiO₂, P₂O₅, SO₃, Cl₂O₇ (acidic nature)
(iv) I, I⁺, I⁻ (atomic size)

Open in App

Solution

(i) Li < B < Be

Note: Explanation of this order is out of the scope of the syllabus. You will learn about this in higher classes.

(ii) I < Br < F < Cl
Electron affinity decreases on moving down a group. But fluorine has less electron affinity than chlorine because of its small size.

(iii) SiO₂ < P₂O₅ < SO₃ < Cl₂O₇
Non-metallic character increases from left to right across a period. The higher the non-metallic character of the element, the higher is the acidic character of its oxide.

(iv) I⁺ < I < I^-
Cation of the same element has smaller radius than the normal atom, while its anion has larger radius than the normal atom.

Suggest Corrections

Similar questions

(I) I < B r < F < C l increasing electron gain enthalpy

(I I) L i < N a < K < R b increasing metallic radius

(I I I) B < C < N < O increasing first ionization energy

(I V) A l^{3 +} < M g^{2 +} < N a^{+} < F^{-} increasing ionic size

Question 36
Arrange the following elements in increasing order of their atomic radii.

(a) Li, Be, F, N
(b) Cl, At, Br, I

H e, A r, N e

N a, L i, K

F, C l, B r

N a, K, L i

Arrange the following as per instructions given in the brackets.

(a) Mg. Cl, Na, S, Si (decreasing order of atomic size)

(b) Cs, Na, Li, K, Rb (increasing metallic character)

(d) Cl, F, Br, I (increasing electron affinity)

(e) Cs, Na, Li, K, Rb (decreasing electronegativity)

C l, A t, B r, I

Join BYJU'S Learning Program