There will be 6 electrons in the full second orbital, being that-
s=2
p=6
d=10
f=14
8
A total number of 8 electrons. Two in the 2s orbital and six in the 2p orbital
it takes 8 electrons for the second shell to be considered full
8 electrons. The second energy level (n=2) has 4 orbitals. One s orbital and three p orbitals. Each orbital can hold 2 electrons of opposite spin.
An atom with the first two electron orbitals completed would have 10 total electrons. The first electron orbital can hold up to 2 electrons (2 in the s subshell), and the second electron orbital can hold up to 8 electrons (2 in the s subshell and 6 in the p subshell).
The S orbital contains a maximum of two electrons
A single orbital can hold up to two electrons.
Each orbital can hold a maximum of 2 electrons.
6 electrons can ocupy the 2p, 3p, 4p, and so on. each p subshell has 3 orbitals, and each orbital can hold up to 2 electrons, so each p subshell can hold up to 6 electrons total.
There are two electrons at most in an orbital, further, they have spins in opposed directions.
Zinc has a full outer electron shell with 2 electrons in the S orbital and 10 electrons in the D orbital, so it has a total of 12 rings or energy levels.
The second energy level contains eight valance electrons when it's full.