Exercises

Make the pairs.

Match the followings.

If $\mathrm{n}=3,$ what are the quantum numbers $\mathrm{l}$ and ${\mathrm{m}}_{\mathrm{l}}$?

The electronic configuration of oxygen is written as $1{\mathrm{s}}^2 2{\mathrm{s}}^2 2{\mathrm{p}}_{\mathrm{x}}^2 2{\mathrm{p}}_{\mathrm{y}}^1 2{\mathrm{p}}_{\mathrm{z}}^1$ and not as $1{\mathrm{s}}^2 2{\mathrm{s}}^2 2{\mathrm{p}}_{\mathrm{x}}^2, 2{\mathrm{p}}_y^2 2{\mathrm{p}}_{\mathrm{z}}^0,$ Explain?

Write note on 'principal quantum number'.

Using concept of quantum numbers, calculate the maximum numbers of electrons present in the $\text{'}\mathrm{M}\text{'}$ shell. Give their distribution in shells, subshells and orbitals.

Indicate the number of unpaired electrons in :

$\mathrm{Si}(\mathrm{Z}=14)$and$\mathrm{Cr}(\mathrm{Z}=24)$

An atom of an element contains $29$ electrons and $35$ neutrons. Deduce the number of protons and write the electronic configuration of that element.