Answer to Question #266798 in Inorganic Chemistry for Assignment

Question

Why halogen does not form metallic bonding?

How does ionization energy influence ionic, and covalent bond formation?

Answer 1

1) We know that electronic configuration of halogens have seven valence electrons(last outer most orbit).

These atoms are so close to having a full set of eight valence electrons.

They show a chemical tendency to gain one electron by forming bonds.

That is way gain a electron and get stability.

That is elements which do not have any of the properties of metals.

2) We know that Ionic bond is much stronger than covalent bond because it involves complete transfer of elections.

And we know that Ionization energy is the energy required to remove electrons from gaseous atoms or ions.

So which bond is stronger that Ionization energy is greater then Lower bond.

And which elements are controlled his outer orbit electron tightly is higher ionization energy.

And we know that Electron gain enthalpy is defined as the amount of energy released when an electron is added to an isolated gaseous atom. During the addition of an electron, energy can either be released or absorbed.

So Ionic bond have more electron gain enthalpy due to more stronger then to covalent bond .

Outer orbital electrons is more stable then these elements have a greater ionization energy compare to less stable electron elements.