NEET Chemistry Classification of Elements and Periodicity in Properties MCQs

sp

sp²

sp³

sp³d

s-block

p-block

d-block

f-block

Lanthanides primarily exhibit a +3 oxidation state, while actinides show a wider range of oxidation states.

Lanthanides form less stable complexes compared to actinides.

Lanthanides are more prone to radioactivity than actinides.

The magnetic properties of actinides are more complex than those of lanthanides.

Similar radii of second and third-row transition metals

Higher densities of third-row transition metals

Difficulty in separating lanthanides

A regular increase in the basicity of Group 2 elements

$Ce^{3+} > Pr^{3+} > Nd^{3+} > Pm^{3+}$

$Pm^{3+} > Nd^{3+} > Pr^{3+} > Ce^{3+}$

$Nd^{3+} > Pm^{3+} > Ce^{3+} > Pr^{3+}$

$Pr^{3+} > Ce^{3+} > Pm^{3+} > Nd^{3+}$

Cerium (Ce)

Praseodymium (Pr)

Neodymium (Nd)

Promethium (Pm)

$\mu = \sqrt{n(n+2)}$ BM

$\mu = n\sqrt{(n+2)}$ BM

$\mu = \sqrt{n(n-2)}$ BM

$\mu = \frac{n}{\sqrt{(n+2)}}$ BM

All actinides are radioactive.

+3 is the only common oxidation state for actinides.

They are inner transition metals.

The actinide series is characterized by the filling of the 5f orbitals.

Increase in atomic radii due to increasing number of electrons.

Lanthanide contraction due to poor shielding of nuclear charge by 4f electrons.

Constant atomic radii due to similar electronic configurations.

Decrease in atomic radii due to increasing electronegativity.

$S^{2-} < Cl^- < Ar < K^+ < Ca^{2+}$

$Ca^{2+} < K^+ < Ar < Cl^- < S^{2-}$

$Ar < K^+ < Ca^{2+} < Cl^- < S^{2-}$

$K^+ < Ca^{2+} < Ar < S^{2-} < Cl^-$