Question

Explain Methods of writing electronic configuration.

Answer 1

Hund's rule:- It states that the pairing of the electrons does not takes place in the orbitals of a particular sub shells (s,p,d) untill all the orbitals of sub shells first singly occupied. Moreover the singly occupied orbitals must contain the electrons with the opposite spins.

Electronic configuration varies from element to element

For example the electronic configuration of aluminum is 3s23p1.

Answer 2

Step-by-step explanation:

Methods of Writing Electronic configuration;

Note that orbital sets are numbered by electron shell, but ordered in terms of energy. For instance, a filled 4s2 is lower energy (or less potentially volatile) than a partially-filled or filled 3d10, so the 4s shell is listed first. Once you know the order of orbitals, you can simply fill them according to the number of electrons in the atom. The order for filling orbitals is as follows: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p, 8s.

An electron configuration for an atom with every orbital completely filled would be written: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 7s2 5f14 6d107p6

Note that the above list, if all the shells were filled, would be the electron configuration for Og (Oganesson), 118, the highest-numbered atom on the periodic table – so this electron configuration contains every currently known electron shell for a neutrally charged atom.