What is the full electron configuration for Cr?

Answer 1

1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d4

Answer 2

Cr Electron Configuration

Answer 3

This is one of the tricks in electron configuration. You would think that it would be (24 electrons) 1s2 2s2 2p6 3s2 3p6 4s2 3d4, but because of (a) d orbital stability or (b) the stability of having two half full orbitals rather than one full and another almost half full, we find the configuration of the last two orbitals is 4s1 3d5. This is also true for Mo which is immediately under Cr, but is not true for W which is under Mo. Sorry can't tell you why that is so.

Answer 4

atomic number of chromium is 24
expected electronic configuration is
1s2 2s2 2p6 3s2 3p6 4s2 3d4
But it was found to be
1s2 2s2 2p6 3s2 3p6 4s1 3d5
This is because of the fact that a d-sub shell with half/fully filled
(5 or 10 electrons) is more stable than the s-sub shell electrons.
this is because it takes less energy to maintain an electron in half filled d sub shell than in fully filled s-sub shell.
and also according to aufbau's rule,electrons occupy the
subshell which has least amount of energy

Answer 5

Full Electronic Configuration
Cr = 1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d4

Short Cut Electronic Configuration
Cr (Ar) = 4s2, 3d4

Answer 6

the full electronic configuration of chromium (Cr)

Z=24

1s2 2s2 2p6 3s2 3p6 4s2 3d4

and as per extra stability rule it is

1s2 2s2 2p6 3s2 3p6 4s1 3d5

Answer 7

The shapes of the orbitals at the on the spot are not round, yet diverse shapes. those shapes are so wild-searching that they extremely overlap one yet another around the atom. Electrons continually take the bottom orbital (lowest power) accessible, so if the overlapping orbital is decrease in power they're going to fill that one first. The 4s orbital is decrease in power than the hands of the 3D orbitals which extend previous the 4s factor, so the 4s fills beforehand the 3D.

Answer 8

1s2 2s2 2p6 3s2 3p6 4s2 3d4

Answer 9

2-8-13-1 (this is from the inner shell to the outer shell)