Are the following ions diamagnetic or paramagnetic? Cr_3^+, Ca_2^+, Na^+, Cr, Fe_3^+
1 Answer
Notice how
Anyways, we can start from the electron configuration of the neutral atoms. I'm assuming you meant
"Cr" :[Ar]3d^5 4s^1
"Ca" :[Ar]4s^2
"Na" :[Ne]3s^1
"Fe" :[Ar]3d^6 4s^2
The rightmost orbitals listed here are highest in energy, so we ionize these atoms by booting off the highest-energy electrons. Thus:
"Cr" -> "Cr"^(3+) + 3e^(-)
[Ar]3d^5 4s^1 -> color(blue)([Ar]3d^3)
Since there are
The original atom is also paramagnetic. The
That's in agreement with our expectations from Hund's Rule (generally, for the lowest-energy configuration, maximize parallel spins where possible by singly-filling all orbitals of very similar energies first and then doubling up afterwards).
"Ca" -> "Ca"^(2+) + 2e^(-)
[Ar]4s^2 -> [Ar] => color(blue)(1s^2 2s^2 2p^6 3s^2 3p^6)
This is a noble gas configuration, so no electrons are unpaired Thus, this is diamagnetic.
"Na" -> "Na"^(+) + e^(-)
[Ne]3s^1 -> [Ne] => color(blue)(1s^2 2s^2 2p^6)
This is a noble gas configuration, so no electrons are unpaired. Thus, this is diamagnetic.
"Fe" -> "Fe"^(3+) + 3e^(-)
[Ar]3d^6 4s^2 -> color(blue)([Ar]3d^5)
Since there are