Question

Explain following properties and their trends in periods and groups:-
i) Metallic and non-metallic character
ii) Reducing and oxidising character
iii) Nature of oxides​

Answer 1

i ) Metallic character refers to the level of reactivity of a metal. Metals tend to lose electrons in chemical reactions, as indicated by their low ionization energies. Within a compound, metal atoms have relatively low attraction for electrons, as indicated by their low electronegativities.

The tendency to gain electrons increases on moving across a period due to an increase in the nuclear charge and decrease in the atomic size. Hence, the non-metallic character increases across a period. As we move down the group, the non-metallic character decreases due to increase in the atomic size.

ii )Oxidation is a reaction that results in the loss of an electron. Oxidation potential follows the same trends as the ionization energy. That is because the smaller the ionization energy, the easier it is to remove an electron, thus it increases along the period.

Reduction is a reaction that results in the gaining of an electron. Reduction potentials follow the same trend as the electron affinity. That is because the larger, negative electron affinity, the easier it is to give an electron and thus it decreases along the period.

iii )As electronegativity across a period increases and down the group decreases so, as we move down the group, down the group the atomic size increases.

Hence, basic character increases while as we move across a period its acidic character increases.

hope you got it the answer........

Answer 2

Answer:

Explanation:

Metallic characters decreases as move from left to right in the period table, across the group, the metallic character increases down the period.

Reducing character decreases down the period, and initially increases across the group and decreases.