This gives two electrons in an s subshell, six electrons in a p subshell, ten electrons in a d subshell and fourteen electrons in an f subshell.
32.
The 1s 1 electron configuration of hydrogen, while superficially similar to that of the alkali metals ( ns 1 ), is unique because there is no 1p subshell.
33.
This is because an electron in an outer subshell will have more energy than one in an inner subshell, and atoms always try to have the lowest possible energy.
34.
This is because an electron in an outer subshell will have more energy than one in an inner subshell, and atoms always try to have the lowest possible energy.
35.
However, the electrons in one " subshell " do have exactly the same level of energy, with later subshells having more energy per electron than earlier ones.
36.
Also, the electrons filling a subshell will have parallel spin before the shell starts filling up with the opposite spin electrons ( after the first orbital gains a second electron ).
37.
The farther right in each transition metal series, the lower the energy of an electron in a d subshell and the less such an electron has the properties of a valence electron.
38.
The stabilization of the 7s electrons is called the inert pair effect; the effect that separates the 7p subshell into the more-stabilized and the less-stabilized parts is called subshell splitting.
39.
The stabilization of the 7s electrons is called the inert pair effect; the effect that separates the 7p subshell into the more-stabilized and the less-stabilized parts is called subshell splitting.
40.
This group has the defining characteristic that all the component elements have 5 electrons in their outermost shell, that is 2 electrons in the s subshell and 3 unpaired electrons in the p subshell.
