How numerous electrons does a Mn Mn atom have in that is 3 d 3d subshell? variety of electrons: 3 d electrons 3d electron How numerous of those electrons room unpaired? number of unpaired electrons: unpaired electrons

4s² 3d⁵ or 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁵


Manganese electronic configuration is 3d⁵ 4s². Manganese has 5 electron in that 3d shell and also all five electrons and unpaired maintaining parallel spin due to the fact that they should obey hund"s rule.

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Generally electrons an initial enter 4s² shell filling it an initial before entering the 3d shell as result of the lower energy 4s orbit has compared to 3d orbital. Filling of the 3d orbital should be to fill parallel very first before pairing begins. However in the case of manganese, it just has 5 electrons in that is 3d orbital which will just fill that with solitary spins.

Due come the reality that manganese has 5 electrons in that 3d orbit its highly magnetic and its classified together a "ferromagnetic" substance.

Note when manganese develops a bond, it loser electrons from its 4s orbit too very first to kind Mn(ii) or combined from both 4s and 3d to type Mn(iii), (iv) (vi) etc.

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


a Mn atom has 5 electron in that 3d subshell

All those 5 electrons are unpaired.


Step 1 : Data given

Mn = manganese

Manganese has atomic number 25

Step 2: number of electrons

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

It"s finish electron configuration is 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁵

3d⁵ = This way a Mn atom has actually 5 electrons in that is 3d subshell.

Since there space 5 orbitals in the 3d, each electron will occupy its very own orbital (this is referred to as the Hunds rule).

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

This means all those 5 electrons space unpaired.

B) The he atom has actually two electron that have actually parallel spin in the 1s orbital.

C) Electrons normally occupy the lowest energy orbital first.

D) The plan of the orbitals is the very same in a multielectron atom and a single-electron atom

E) The C atom has actually two unpaired electrons.


In writing sublevel notations details rules are followed:

The maximum variety of electrons in the orbitals of sublevels are:

two for s-sublevel v one orbital

six for p-sublevel with 3 orbitals

ten because that d-sublevel with 5 orbitals

fourteen for f-sublevel with 7 orbitals

Aufbau"s principle states that sublevels with lower energies are filled before those with greater energies.

1s 2s 2p 3s 3p 4s 3d 4p 5s boosting order of filling

Pauli exclusion principle states that no two electrons can have the same set of the four quantum numbers i.e electrons in the exact same orbital cannot spin in the exact same direction. Hund"s dominion states the electrons go into degenerate orbitals singly an initial before pairing up.

Based on this principles and the animation, the following alternatives are correct:

B) The that atom has actually two electron that have actually parallel spin in its 1s orbital.

Helium has two electron in the 1s orbital. Native Pauli"s exemption principle, we see that the two electrons can not spin in the exact same way. Therefore, they have actually parallel spin

C) Electrons normally occupy the lowest power orbital first.

From Aufbau"s principle, electrons go into orbitals with reduced energies first before those with greater energies.

D) The arrangement of the orbitals is the very same in a multi-electron atom and also a single-electron atom

1s 2s 2p 3s 3p 4s 3d 4p 5s

Orbitals space arranged in the bespeak of their energies indigenous the lowest to the highest.

E) The C atom has two unpaired electrons.

Configuration because that carbon atom is displayed below:

1s² 2s² 2p²

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The answer would be B.

As paramagnetic through 3 unpaired electrons. Since there are 6 ligands approximately the Co+2 ion it isoctahedral and these ligands are neutral. This provides the all at once charge ~ above the complicated +2 and also therefore originates from the configuration for Co+2 i beg your pardon is 3d7. Since it is in high rotate you should fill every the orbitals with at the very least one electron and then pair up any kind of that remain. If you perform this, 3 unpaired electron remain. Para magnetism occurs in substances through unpaired electrons.

Phosphorus atoms will be paramagnetic. Iodine atoms will certainly be paramagnetic. Germanium atom will likewise be paramagnetic.


Phosphorus has actually 3 unpaired electrons. Iodine has actually 1 unpaired electron. And Germanium has 2 unpaired electrons. But all these simple compound will be diamagnetic because they pair your electrons on molecule orbitals.

See explanation


Fe(H20)6>2+ is a high rotate octahedral facility because water is weak ar ligand. A high spin facility has a maximum variety of unpaired d electrons.

The spin state that Fe(H20)6>2+ is S=2. The last electron goes into an zb orbital. If the steel is oxidized come Fe^3+, the link lengths decreases. For an oxidation that M2+ facility to M3+, the M3+L bonds will certainly be much shorter due come the greater charge thickness on the metal. Because the occupation the the zb orbitals in both complexes is the same it then adheres to that that the difference in the link lengths should be because of the fee alone.


I have the right to only answer 2 that the problems because the direction that the rest are confusing/unclear. A) Magnesium (Mg) B) Ruthenium (Ru)
The following statements space correct : B,C,D,EFurther explanation

In an atom there space levels of energy in the shell and sub shell

This power level is to express in the kind of electron configurations.

Writing electron configuration starts from the shortest to the highest sub-shell energy level. There room 4 sub shell in the shell of an atom, specific s, p, d and also f. The maximum number of electrons because that each sub shell is

•s: 2 electrons

•p: 6 electrons

•d: 10 electron and

•f: 14 electrons

Charging electron in the sub shell offers the complying with sequence:

1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶, 5s², 4d¹⁰, 5p⁶, 6s², etc.

Determination of electron configurations based upon principles:

•1. Aufbau: Electrons occupy orbitals the the lowest energy level

•2 Hund: electrons fill orbitals through the same energy level

•3. Pauli: no electrons have actually the very same 4 quantum numbers

Let watch the prize choices

A) In the Li atom, the 3s, 3p, and also 3d orbitals have different energies

electron configurations Li : 1s², 2s¹

So the facet Li does not have 3s, 3p, and also 3d orbitals

The statement is false

B) The that atom has actually two electrons that have parallel spin in that 1s orbital

electron configurations that : 1s²

so He has actually 2 pararel rotate : +1/2 and also -1/2

The explain is true

C) Electrons generally occupy the lowest energy orbital first.

in accordance through the rule of Aufbau

The explain is true

D) The arrangement of the orbitals is the very same in a multielectron atom and a single-electron atom.

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a single-electron atom choose H : 1s¹ and also multielectron atom prefer C : 1s², 2s², 2p² is the same : The arrangement from the shortest to the highest sub-shell energy level.