Which ion is more stable Fe3+ or Fe2+?

Fe3+ ion is more stable than Fe2+ ion. This is explained on the basis of the electronic configuration of the two ions Fe3+ on whit all the five 3d orbitals half filled, is more symmetrical than Fe2+ on in which four 3d orbitals are half filled and one is filled. Therefore, Fe3+ on is more stable than Fe2+ ion.

Which is more stable I Mn2+ or Mn3 II Fe2+ or Fe3+? Give Reason?

Mn2+ is more stable than Mn3+ due to the stable electronic configuration ofMn2+ because of half filled d-orbital. Fe3+ is more stable than Fe2+ because Fe3+ has exactly half filled d- orbitals which give the stability to Fe3+ while Fe2+ has 3d6 electronic configuration.

Why co3+ and ni3+ are unstable while Fe3+ is stable?

The Fe 3+ ion more stable than Fe 2+ ion because due to his electronic configuration i.e the electronic configuration of Fe 3+ has half filled last orbital and we know that half or fulled filled orbitals are most stable and here Fe 2+ has not half or full-filled orbital so Fe 3+ ion more stable than Fe 2+ ion.

Why Fe3+ exists more commonly than Fe2+?

The half filled orbital 3d is more stable than the same orbital filled with 6 electrons. So, Fe(III) ion is more common than Fe(II).

Why is Fe2+ more easily oxidized to Fe3+?

Fe2+ is easily oxidized to Fe3+ . so Fe3+ should be more stable than Fe2+. This is because Fe3+has a half filled stable d5 configuration . so by oxidation Fe2+ converts its electron configuration from d6 to d5(more stable).

How do you know which ion is more stable?

The larger the atom, and the further the electrons from the nucleus, the more polarizable it is. The more polarizable the atom, the more stable the anion. Within a row of the periodic table, the more electronegative an atom, the more stable the anion.

Which is more stable Mn2 or Fe2+?

Since Mn2+ has stable half filled electronic configuration, therefore Mn2+ compounds are more stable than Fe2+ towards oxidation to their +3 state.

Which is more stable Mn2+ or mn4+?

The main reason is that in Mn(II),the electronic configuration had no s electrons and have a highly stable half filled d orbital state, while in Mn (IV),2 s and d electrons are released forming a t2g configuration. Surely, Half filled state is very much stable for an ion than in t2 g and eg configurations.

Which iron ion is more stable?

Fe3+
Fe3+ is more stable than Fe2+. This is explained with the help of the electronic configuration. In Fe3+ ions, there are five 3d half-filled orbitals and is more symmetrical than Fe2+.

Why are Ni2+ compound more stable than Fe2+?

A compound has more thermodynamic stability if the ionization energy of the metal is low. Since the ionization energy of Ni2+ is less than that for Pt2+, therefore Ni2+, compounds are thermodynamically more stable than Pt2+ compounds.

Why are Fe3+ ions more stable than Fe2+ ions?

This pushes the electron inwards and reduces the size of atom which further results in decrease in energy and hence increases the stability of the ion. In Fe3+ ions, there are five 3d half-filled orbitals and is more symmetrical than Fe2+. Whereas in Fe2+ ion there are four 3d half-filled orbitals and one orbital is filled.

Why is F E 3 + more stable than F E 2+?

F e 3 + ( 3 d 5) has half filled orbitals which provide extra stability to it because of symmetrical configuration. While F e 2 + ( 3 d 6) has one electron more than the symmetrical arrangement. That is why F e 3 + is more stable than F e 2 + . The stability depends on whether you are checking it in gaseous or solution medium.

How many electrons in an ion of Fe?

Once we have the configuration for Fe, the ions are simple. When we write the configuration we’ll put all 26 electrons in orbitals around the nucleus of the Iron atom. If playback doesn’t begin shortly, try restarting your device. Videos you watch may be added to the TV’s watch history and influence TV recommendations.

How do you write the electronic configuration of Fe2+ and Fe3+?

First of all write down the electronic configuration of Fe (26). (Shown in the picture) Then write down the Fe2+ electronic configuration by removing 2 electrons from the outer most (4s) shell. Then write down the Fe3+ electronic configuration by removing 3 electrons, 2 from the outer most (4s) shell and 1 from 3d shell.