Write the electronic configurations of the following ions:

(a) $$H^–$$

(b) $$Na^+$$

(c) $$O2^–$$

(d) $$F ^–$$

Asked by Abhisek | 1 year ago |  81

##### Solution :-

(a) H  ion

The electronic configuration of the Hydrogen atom (in its ground state) 1s1. The single negative charge on this atom indicates that it has gained an electron. Thus, the electronic configuration of H = 1s2

(b) Naion

Electron configuration of Na =  1s2 2s2p6 3s1 . Here, the +ve charge indicates the loss of an electron.

∴Electronic configuration of Na+ = 1s2 2s2 2p6

(c) O2– ion

Electronic configuration of 0xygen = 1s2 2s2 2p4. The ‘-2 ‘ charge suggests that it has gained 2 electrons.

∴Electronic configuration of O2– ion = 1s2 2s2p6

(d) F – ion

Electronic configuration of Fluorine = 1s22s22p5. The species has gained one electron (accounted for by the -1 charge).

∴Electron configuration of F ion = 1s2 2s2 2p6

Answered by Pragya Singh | 1 year ago

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