Why the element of second period shows a...

Why the element of second period shows a number of difference in properties from other members of their respective families?

Text Solution

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The differences in the properties of the first member of a group from those of the other members are due to
(i) the smaller size of the atom. (ii) high ionization enthalpy. (iii) absence of d-obritals.

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Oxygen differs from other member of irts family due to

its small atomic size

its high electronegativity

absence of d-orbitals

All of these

Both boron and aluminium show difference in properties from the remaining members of group 13. This because

Both B and Al have smaller size as compared to others members of the family.

Both B and Al have high value of ionization energy

Both B and Al have only the valence eletrons `(ns2 np1)` outside the noble gas core while the reamaining elements have filled d and `f-orbitals` in between the noble gases and the valance electrons

None of the above.

The first element of the group 1 and 2 are different from other members of the respective group.Their behaviour is more similar to the second element of the following groups,What is this relationship known as ?

Anomalous relationship

Periodic relationship

Diagonal relationship

Chemical relationship