electron configuration of Cr3+?
I think is Cr: [Ar] 4s1,3d5
but how about Cr+, Cr2+, Cr3+?
Please explain?
24Cr is 1s2 2s2 2p6 3s2 3p6 3d5 4s1
For Cr^+, remove the 4s1 electron.
For Cr^+2, remove 4s1 and one 3d5
Thereafter, remove as many 3d electrons as needed.
Cr^+6 is 1s2 2s2 2p6 3s2 3p6 3d0 4s0
u stoopid
To determine the electron configuration of an ion, we need to first determine the electron configuration of the neutral atom and then remove the appropriate number of electrons to match the ion's charge. Let's break it down for Chromium (Cr) and its various ionic forms:
Neutral Chromium (Cr):
The atomic number of Chromium (Cr) is 24, meaning it has 24 electrons. The electron configuration of neutral Chromium is: 1s2 2s2 2p6 3s2 3p6 4s1 3d5.
Chromium ion with a +1 charge (Cr+):
Cr+ has lost one electron. From the electron configuration above, we'll remove one electron from the 4s orbital since it has the highest energy. Therefore, the electron configuration for Cr+ is: 1s2 2s2 2p6 3s2 3p6 3d5.
Chromium ion with a +2 charge (Cr2+):
Cr2+ has lost two electrons. Again, these electrons will be removed from the 4s orbital since it has the highest energy. So, the electron configuration for Cr2+ is: 1s2 2s2 2p6 3s2 3p6 3d4.
Chromium ion with a +3 charge (Cr3+):
Cr3+ has lost three electrons. Similar to the previous cases, the electrons will be removed from the 4s orbital. Thus, the electron configuration for Cr3+ is: 1s2 2s2 2p6 3s2 3p6 3d3.
So, the electron configurations for each of the Chromium ions are:
Cr+: 1s2 2s2 2p6 3s2 3p6 3d5
Cr2+: 1s2 2s2 2p6 3s2 3p6 3d4
Cr3+: 1s2 2s2 2p6 3s2 3p6 3d3