Question

How many electrons does a Mn Mn atom have in its 3 d 3d subshell? number of electrons: 3 d electrons 3d electrons How many of those electrons are unpaired? number of unpaired electrons: unpaired electrons

Answer 1

Answer:

a Mn atom has 5 electrons in its 3d subshell

All those 5 electrons are unpaired.

Explanation:

Step 1 : Data given

Mn = manganese

Manganese has atomic number 25

Step 2: Number of electrons

Since Manganese has atomic number 25, it means it has 25 electrons

It's complete electron configuration is 1s²  2s²  2p⁶  3s²  3p⁶  4s²  3d⁵

3d⁵ = This means a Mn atom has 5 electrons in its 3d subshell.

Since there are 5 orbitals in the 3d, each electron will occupy its own orbital (this is called the Hunds rule).

Before pairing begins, the 3d orbital must be filled parallel first.

This means all those 5 electrons are unpaired.

Answer 2

Answer:

[Ar] 4s² 3d⁵ or 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁵

Explanation:

Manganese electronic configuration is [Ar] 3d⁵ 4s². Manganese has 5 electrons in its 3d shell and all five electrons and unpaired maintaining parallel spin since they must obey hund's rule.

Generally electrons first enter 4s² shell filling it first before entering the 3d shell due to the lower energy 4s orbital has compared to 3d orbital. Filling of the 3d orbital must be filled parallel first before pairing begins. However in the case of manganese, it only has five electrons in its 3d orbital which will only fill it with single spins.

Due to the fact that manganese has five electrons in its 3d orbital its highly magnetic and its classified as a "ferromagnetic" substance.

Note when manganese forms a bond, it loses electrons from its 4s orbital too first to form Mn(ii) or combined from both 4s and 3d to form Mn(iii), (iv) (vi) etc.

Attached is a diagram showing how manganese atoms are arranged in its shells