The subshells in the M shell are 3s, 3p, 3d, and 4s. In terms of increasing energy, the order would be 3s < 3p < 3d < 4s.
No, an electron in the 3d shell can move to the 4s shell very easily.
A break down of 2d1:2 = the quantum energy level or electron shell denoted as 'n'd = the sub-shell of the energy level (known as a degenerate level)1 = the number of electrons occupying the sub-shell.Through extensive research by scientists, no known element has a d sub-shell in the second (n=2) energy level. In fact, the d sub-shell does not appear until the fourth period (fourth row).The first d sub-shell is known to be in the third energy level (therefore the first energy level with this sub-shell is 3d, but not 2d).Transition metals are the elements known to fill the d sub-shells. The first transition metal in the periodic table is scandium (Sc) with the electron configuration of [Ar]4s23d1.The reasons for the formation of sub-shell of d is beyond my knowledge and the scope of basic chemistry.
You can tell the difference between a 2s sub-shell and 2p sub-shell from their energy levels, because a 2p sub-shell is a higher energy level than a 2s sub-shell.
they are both the same meaning
The sub-level s of energy that make the o shell is the K-shell.
M shell notation: N = 3 contains 3 sub shells s,p and d (3s,3p and 3d) *according to my chemistry book.
Atomic shorthand uses the noble gas before the element in questionAnswer: Cu: [Ar]4s[1]3d[10]Explanation: Copper Cu is an anomaly. Logically we would write 4s[2]3d[9] but for Cu, having the d sub level full is more stable than having the s sub-shell full and the d sub-shell less than full. Chromium also has this anomaly, and is written [Ar]4s[1]3d[5]
The 2d sub energy level does not exist. The first shell to contain a d sub-shell is the third shell: the 3d sub-shell contains a maximum of 10 electrons, with two electrons in each of five different d orbitals.
3d^6 Six electrons in the outer shell.
There are a maximum of 10 electrons in the 3d sub-level.
4 s , p , d , 7