La³⁺ < Ce³⁺ < Pm³⁺ < Yb³⁺

Yb³⁺ < Pm³⁺ < Ce³⁺ >La³⁺

La³⁺ = Ce³⁺ < Pm³⁺ < Yb³⁺

Yb³⁺ < Pm³⁺ < La³⁺ < Ce³⁺

their sizes are same

Cl^- ion is bigger than K⁺ ion

K⁺ ion is relatively bigger

their sizes depend on other cation and anion

Electron affinity

Ionisation enthalpy

Hydration enthalpy

Bond dissociation energy

Mg <Al< Na⁺ < F ^-

Na⁺ < Al < Mg < F ^-

Na⁺ < F ^- < Al < Mg

Na⁺ < F ^-  < Mg < Al

the properties of the elements are the periodic function of their atomic number

non-metallic elements are lesser in number than metallic elements

the first ionisation energies of elements along a period do not vary in a regular manner with increase in atomic number

for transition elements, the d-subshells are filled with electrons monotonically with increase in atomic numbers

2.80 : 1

1.80 : 1

2.40 : 1

4.20 : 1

1s²

1s²,2s² 2p²

1s²,2s² 2p⁶

1s²,2s² 2p⁶,3s¹

Li < Na < K < Rb : increasing metallic radius

I < Br < F < Cl : increasing electron gain enthalpy (with negative sign)

B < C < N < O : increasing first ionisation enthalpy

Al³⁺ < Mg²⁺ < Na⁺ < F ^- : increasing ionic size

Li⁺ > Be²⁺ > Na⁺ > Mg²⁺

Na⁺ > Li⁺ > Mg²⁺ > Be²⁺

Li²⁺ > Na⁺ > Mg²⁺ > Be²⁺

Mg²⁺ > Be²⁺ > Li⁺ > Na⁺

2.09 : 1

0.09 : 1

3.09 : 1

1.09 : 1