Analyse and asses the electronic configuration of the following ions a)H- b)Na+ c)O2- d)F-

Sure, let's analyze and assess the electronic configuration of the following ions:

a) H-: The hydrogen atom usually has 1 electron. However, H- is a hydride ion, meaning it has gained an extra electron. Therefore, its electronic configuration is 1s2, similar to Helium.

b) Na+: Sodium (Na) normally has 11 electrons with the configuration 1s2 2s2 2p6 3s1. However, Na+ means it has lost one electron. Therefore, its electronic configuration is 1s2 2s2 2p6, similar to Neon.

c) O2-: Oxygen (O) normally has 8 electrons with the configuration 1s2 2s2 2p4. O2- means it has gained two extra electrons. Therefore, its electronic configuration is 1s2 2s2 2p6, similar to Neon.

d) F-: Fluorine (F) normally has 9 electrons with the configuration 1s2 2s2 2p5. F- means it has gained one extra electron. Therefore, its electronic configuration is 1s2 2s2 2p6, similar to Neon.

In summary, ions often have electronic configurations similar to noble gases. This is due to the stability of noble gases' electron configurations.