Periodic Properties - Class 12 MCQ

Size of isoelectronic ions decreases with increasing atomic number. Order can be decided by e/p ratio, Radii decreases with decrease in ratio

Atomic size decrease along the period and increases down the group. In case of ions, anions are bigger & cations are smaller, size decreases with increases in cationic charge

The tendency to show lower ionic state increases down the group due to inert  pair effect.

Small cation has more polarizing power.

The atomic radius decreases along the period,also cations are always smaller than their parent atom and anions are always larger han their parent atom

The biggest jump in IP values exist in IP₅ and thus, element contains four electrons in its valency shell.

Cations are smaller in size than their parent atoms.

Follow bonding rules.

Electron affinity order for halogens is CI > F > Br > I.

Ionisation energy  decreases down the group and increases along the period.

First electron affinity is energy releasing process.

On moving along a period from left to right in periodic table, electrnegativity increases ( due to decrease in size). While on moving downward in a group, electronegativity decreases.
Thus, the correct order of electronegaticity is
Si > P > C > N
(1.8) (2.1) (2.5) (3.0)

The ionisation energy of elements decreases down the group, due to decrease in Z_eff

Mg²⁺ is smaller than Na⁺ thus, smaller is cation more is hydration energy.

Cations are always shorter than their parent atom, anion are always bigger.

All are isoelectronic species; more is nuclear charge, smaller is ionic size.

Electron affinty decreases down the group, but ‘O’ has small atomic size and 2p-orbital becomes very compact and already has 6 electrons, hence, there is a repulsive force among the already present and added electron, is used to reduce the  repulsion. Hence, the E.A of O is less than S, so the order is S > Se > O.

Cations are always shorter than their parent atom, anion are always bigger.

E₁ for He⁺ = E₁ for H x Z² (where Z = at.no. of He).

It is the definition of electron affinity.

Larger is anion,more is its polarizability.

All are non-metals

Both possess 1s²,2s²2p⁶,3s²3p⁶  configuration.

Removal of electron is easier in the order of shell 4 > 3 > 2 > 1

Ti⁺ has 21 electrons in it. Rest all have 10 electrons.

Both C and N⁺ have six electrons.

NaOH as well as CaO are basic in nature.

Half filled orbitals are more stable and element with 3p canfiguration is smaller then 4p.

The removal of second electron from Mg tales place from 3s-orbital whereas, the removal of second electron from Na takes place from 2p-orbital. More closer are shells to the nucleus, difficult is removal of electron.