Why does the first element in a group show anomalous behaviour. Give a reason 

Why does the first elements in a group show anomalous behaviour. Give a reason.

Group 13 of periodic table consists of boron or aluminium family. Boron being the first member, shows anomalous behaviour due to its small size and high nuclear charge/size ratiom high electrone gastivity and non availability of d-electrons. All the group 13 members forms hydrides, hydroxides, halides showing +3 covalency, however boron forms electron deficient species. Which one is not correct chemical change ?

Why are the elements of zero group inert?

Why are the elements of group 18 known as noble gases ?

Give two examples to show the anomalous behaviour of flurine.

Why are the elements of group 1 called alkali metals ?

How does the first element of group 14 differ from other elements of the group?

Which element of group-16 shows highest catenation ?

What elements show diagonal relationship? Give an example

The first element of a group differes from its congeners, i.e other members of the group in many ways. These difference may be due to the following i) Small size of atom and ion ii) High electronegetivity iii) Non-availability of low lying d-orbitals The first element of a group shows resemblance with the second element of the adjacent group on the right. This is known as diagonal relationship Metal (M)+ N_(2) rarr "Nitride" underset("hydroysis")overset(H_(2)O)rarr NH_(3) . Metal (M) can be