How many unpaired electrons are present in Mn-2- ion-

Question

Toppr Admin · Accepted Answer

Atomic number of -Mn- is -Ar- 3d-5 4s-2-Therefore the electronic configuration of -Mn-2- is - -Ar- 3d-5-As there are five 3d orbitals each orbital occupied with single electron-Hence- there are 5 unpaired electrons in -Mn-2-

How many unpaired electrons are present in $$Mn^{2+}$$ ion?

Atomic number of $$Mn$$ is :
$$[Ar] 3d^5 4s^2$$
Therefore the electronic configuration of $$Mn^{2+}$$ is : $$[Ar] 3d^5$$

As there are five 3d orbitals each orbital occupied with single electron.
Hence, there are 5 unpaired electrons in $$Mn^{2+}$$

How many unpaired electrons are present in $$Mn^{2+}$$ ion?

Atomic number of $$Mn$$ is :$$[Ar] 3d^5 4s^2$$Therefore the electronic configuration of $$Mn^{2+}$$ is : $$[Ar] 3d^5$$As there are five 3d orbitals each orbital occupied with single electron.Hence, there are 5 unpaired electrons in $$Mn^{2+}$$

Atomic number of $$Mn$$ is :
$$[Ar] 3d^5 4s^2$$
Therefore the electronic configuration of $$Mn^{2+}$$ is : $$[Ar] 3d^5$$

As there are five 3d orbitals each orbital occupied with single electron.
Hence, there are 5 unpaired electrons in $$Mn^{2+}$$