- A. 1
- B. 2
- C. 3
- D. 4
- E. 5 ✓
The answer to the question is: E. 5
To determine the number of unpaired electrons in the Fe3+ ion, we need to understand the electronic configuration of iron (Fe) and how it forms the Fe3+ ion.
Electronic Configuration of Iron (Fe)
Iron has an atomic number of 26, which means a neutral iron atom has 26 electrons. The electronic configuration of a neutral iron atom is: 1s2 2s2 2p6 3s2 3p6 4s2 3d6.
Formation of Fe3+ Ion
When iron loses three electrons to form the Fe3+ ion, it loses these electrons from its outermost shell. The electronic configuration of Fe3+ can be determined by removing three electrons from the neutral iron atom’s configuration. This results in the Fe3+ ion having the electronic configuration: 1s2 2s2 2p6 3s2 3p6 3d5.
Number of Unpaired Electrons in Fe3+ Ion
In the electronic configuration of Fe3+, there are five unpaired electrons in the 3d subshell. Unpaired electrons are those that have their spins aligned in the same direction, making them available for bonding with other atoms to form chemical bonds.
