I was solving practice problems for electron configuration and periodic table, and I got stuck through a question:
An atom of silicon in its ground state has how many electrons with quantum number $l = 1$?
a) 14
b) 2
c) 8
d) 6
c) 28
According to the solution the answer is c: 8 electrons, but that wasn't my answer.
My analysis:
- Silicon is a chemical element with symbol $\ce{Si}$ and atomic number 14, this is its electron configuration:
$$\mathrm{1s^22s^22p^63s^23p^2}$$
- The quantum number $l = 1$ corresponds to $\mathrm{p}$ levels only. So we have:
$$\mathrm{2p^63p^2}$$
The total number of orbitals is: $6 + 2 = 8$ orbitals.
Since each orbital has 2 electrons, the total number of electrons is $8 \times 2 = 16$ electrons.
What's wrong with my answer? Maybe the question has a wrong answer?