Among the statements (I -IV) , the correct ones are :
(I) Be has smaller atomic radius compared to Mg.
(II) Be has higher ionization enthalpy than Al.
(III) Charge/ radius ratio of Be is greater than that of Al.
(IV) Both Be and Al form mainly covalent compounds.

Why Ca has larger atomic radius than Al ?

Assertion (A) : The first ionization energy of Al is lower than Mg. Reason (R ) : Atomic radius of Al is smaller than Mg.

Among the followingstatements identify correct set of statements (a) size of Be is smaller than Mg (b) Ionisation energy of Be is greater than Al (c) Both Be and Al form covalent compounds readily (d) Both Be & Al does not react with nitrogen

Among the followingstatements identify correct set of statements (a) size of Be is smaller than Mg (b) Ionisation energy of Be is greater than Al (c) Both Be and Al form covalent compounds readily (d) Both Be & Al does not react with nitrogen

Al^(3+) has low ionic radius than Mg^(2+) because

Al^(3+) has low ionic radius than Mg^(2+) because

This question has statement I and statement II of the four choices given after the statements choose the one that best describes the two statements Statement -I:The first ionization enthalpy of Be I sgreater than that of B Statement-II:2 p orbital is lower in energy than 2s orbital

Gallium has unexpectdly less atomic radius than that of Al. Explain why ?