Respuesta :

znk

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.

adioabiola

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;

  • O²- ==> 1s² 2s² 2p⁶
  • F- ==> 1s² 2s² 2p⁶
  • Ne ==> 1s² 2s² 2p⁶
  • Na+ ==> 1s² 2s² 2p⁶

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.

Read more:

https://brainly.com/question/13308699

Otras preguntas