Give the general electronic configuration of alkali metals and provide the electronic configuration for each element of the alkali metal group.

(N/A) All alkali metals have one valence electron,$ns^{1}$,outside the noble gas core.
The loosely held $s$-electron in the outermost valence shell of these elements makes them the most electropositive metals.
They readily lose an electron to form monovalent $M^{+}$ ions. Hence,they are never found in a free state in nature.

Element	Electronic Configuration
Lithium $(Li)$	$1s^{2} 2s^{1}$
Sodium $(Na)$	$1s^{2} 2s^{2} 2p^{6} 3s^{1}$
Potassium $(K)$	$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{1}$
Rubidium $(Rb)$	$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{10} 4s^{2} 4p^{6} 5s^{1}$
Caesium $(Cs)$	$[Xe] 6s^{1}$
Francium $(Fr)$	$[Rn] 7s^{1}$