Tag: p- block elements-ii

Chalcogens are chemical elements in group 16 of the periodic table. Germanium bonds to all natural single chalcogens except polonium.

As we move down the group the metallic character increases which impart lustrousness to the elements.

As the atomic size of the Florine is less it has more nuclear charge. So it requires more energy to remove the electron from its outer most orbit. So Florine has high ionization enthalpy and as we move down the group size increases nuclear charge decreases hence Ionization potential.

Florine is most electronegative than the other elements of that group because it has less atomic size so it attracts electrons more towards itself (Electronegativity).

The atomic number of elements are 9,17,35,53,85.
Electronic configuration of elements will be
9  = 2,7
17= 2,8,7
35= 2,8,18,7
53=2,8,18,18,7
85=2,8,18,18,32,7
The pattern shows that all elements have 7 electron in their outermost valence shell and all these elements belong to halogens.

Halogens need to lose only one electron to form an anion, and thus, their tendency to form an anion is highest. 

The general electronic configuration of chlorine is $[Ne] 3s^{2} 3p^{5}$

F does not have empty d-orbitals o it show only one oxidation state. In othens electrons can excite to empty d-orbitals and show variable oxidation state

$Br - 35$

Bond energy is inversely proportional to molecular mass as van der wall forces exist  between molecules of halogens
$\therefore$ Bond Energy order:
$Cl _2>Br _2>I _2$