The atomic number of iron is 56. The number of unpaired electrons in the Fe3+ ion is
1
2
3
4
5
Explanation
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iron has 3 electrons in its outermost shell, so it gives out the three to become stable. so if it gains it back it becomes unstable again
Electronic configuration Fe3+:[Ar]3d^5
Hence it has 5 unpaired electrons.
Fe is 26 and arrangements in shell is 2,8,8,8
+ losing electron
Fe3+ loses 3 electron
26-3 =23
arrangement in shell is now 2,8,8,5
so we now have 5 unpaired electron
First of all, Iron has an atomic number of 26 not 56, which may confuse a lot of people. Now the valence number of electrons in iron equals three. This implies that iron will have to forgo three in order for it to be a stable octet.
Here is an explanation:
Iron is already stable by giving out three electrons therefore Fe3+ gaining back the three electrons will have those three unpaired.
REF: Check : Chemistry Textbook under ion.
how come Fe has 4 unpaired electrons, while Fe3+ has 5 unpaired electrons. What is a proof to this statement or a reasonable explanation to this statement?
