1s2 2s2 2p3 or otherwise denoted [He]2s2 2p3
K=2, L=5
1s2 2s2 2p3
Nitrogen is 1s22s22p3
these elements have 5 electron in the valence shells and have configuration of ns np5
This is because in nitrogen the 2p subshells are filled by 3 electrons which is half filled electronic configuration. But oxygen has to lose an electron to attain the half filled electronic electronic configuration. Hence nitrogen is more stable than oxygen.
because of ammonia electronic configuration, pair of electrons on the central atom,Nitrogen.
Electronic configuration of scandium: [Ar]3d1.4s2
what is the electronic configuration of the atomC6
The electronic configuration of tin is: [Kr]D10.5s2.5p2.
The electronic configuration of Bromine is [Ar] 3d10 4s2 4p5.
The electronic configuration of magnesium is [Ne]3s2.
Nitrogen's symbol is N. Its electron configuration is 2s, 3p.
As Nitrogen (N) have atomic number 7, and electronic configuration is 2,5. therefore N required 3 elecrons to complete their outermost shell or orbital.
Electronic configuration means the arrangement of electrons in shells in atoms. Eg:Electronic configuration of Sodium is 1s2,2s2,2p6,3s1.