Answer:
(b) O²⁻,F⁻ ,Ne, Na⁺
Explanation:
An isoelectronic series is a sequence of atoms/ions with the same electron configuration.
(a) F⁻, Cl⁻, Br⁻, I⁻
F⁻: [He] 2s²2p⁵
Cl⁻: [Ne] 3s²3p⁵
Br⁻: [Ar] 4s²4p⁵
I⁻: [Kr] 5s²5p⁵
The ions all have different electron configurations. Not isoelectronic.
(b) O²⁻,F⁻ ,Ne, Na⁺
O²⁻: [Ne]
F⁻ : [Ne]
Ne: [Ne]
Na⁺: [Ne]
The species all have the same electron configuration. Isoelectronic.
(c) S, Cl, Ar, K
S: [Ne] 3s²3p⁴
Cl: [Ne] 3s²3p⁵
Ar: [Ar]
K: [Ar] 4s
The atoms all have different electron configurations. Not isoelectronic.
(d) Si²⁻ ,P²⁻, S²⁻-, Cl²⁻
Si²⁻: [Ne] 3s²3p⁴
P²⁻: [Ne] 3s²3p⁵
S²⁻: [Ar]
Cl²⁻: [Ar] 4s
The ions all have different electron configurations. Not isoelectronic.
The group of atoms which constitute an isoelectronic series are: O2- ,F- ,Ne, Na+
Definition:
An isoelectronic series refers to a group of atoms/ions with the same electron configuration.
The electron configuration of the atoms/ions in the isoelectronic series are as follows;
It is evident from above that the electron configuration of atoms/ions in the isoelectronic series are equal.
This is not the case in other group of atoms; As such, they are not isoelectronic.
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