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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?

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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 ionizaton enthalpy. (iii) abence of d-orbitals.
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Why the elements of the second row (first short period) show a number of difference in properties from other members of their respective families ?

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Knowledge Check

  • Oxygen differs from other member of irts family due to

    A
    its small atomic size
    B
    its high electronegativity
    C
    absence of d-orbitals
    D
    All of these

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

    A
    Both B and Al have smaller size as compared to others members of the family.
    B
    Both B and Al have high value of ionization energy
    C
    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
    D
    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 ?

    A
    Anomalous relationship
    B
    Periodic relationship
    C
    Diagonal relationship
    D
    Chemical relationship

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