electron shells in periodic table?

Question

In the Periodic Table of the elements you note that each electron shell fills to capacity before starting to fill the next shell. At least this is the case as far as Argon. Then at Potassium, the N shell begins to fill even though the M shell contains only 8 of its possible 18 electrons. WHY IS IT SO?

Answer 1

K L M N is a primitive way of explaining electron configurations. A slightly more sophisticated way is s p d f. After potassium and calcium have filled the 4s orbitals, the 14 transition elements fill the 3d orbitals. You are entering upon a wonderful and enjoyable phase of chemistry.

Answer 2

you shall see the atomic style of the factor in periodic table and in accordance it to jot down the electron configuration understanding the utmost style of electron that must be popular by way of an orbital, for s=2, p=6, d=10, f=14 and wherein capability point which orbitals are achieveable for a million basically s, for 2 s and p, for 3 s, p and d and so on. threr is an inregularyty while that's approximately d orbitals 3-D looks after 4s, 4d after 5s and so on so for the factor with atomic style 26 the electron configuration is: 1s2 2s2 2p6 3s2 3p6 4s2 3d6 some thing like that

Answer 3

because it requires less energy to put the electrons into the N energy level