List the four different sublevels and (given that only a maximum of two electrons can occupy an orbital) determine the maximum number of electrons that can exist in each sublevel. Drag the appropriate items to their respective bins. ResetHelp l = 0 l = 1 l = 2

For the quantum theory, the probability to find an electron is higher in the space region called orbital. It's impossible to determine where the electron is and his velocity at the same time (uncertainty principle). So, the theory determines four quantum numbers to characterize an electron, so it's easy to identify it:

n is the principal quantum number and identify the shell where the electron is. It varies from 1 to 7 and is represented by the letters K, L, M, N, O, P, and Q;

l is the azimuthal quantum number and identify the subshell (or sublevel) where the electron is. It varies from 0 to 3 and is represented by the letters s, p, d, and f;

ml is the magnetic quantum number, and it represents the orbital. It varies from -l to +l, passing by 0. Each orbital can have at least 2 electrons;

ms is the spin number and represents the spin of the electrons. It can be +1/2 or - 1/2.

Then, the sublevel s (l= 0) only has 1 orbital (ml = 0) so, it can have ate least 2 electrons; the sublevel p (l= 1) has 3 orbitals (ml = -1, ml= 0, ml = +1), so it can have at least 6 electrons; the sublevel d (l = 2) has 5 orbitals (ml = -2, ml = -1, ml = 0, ml = +1, ml = +2), so it can have at least 10 electrons; and the sublevel f (l = 3) has 7 orbitals (ml = -3, ml = -2, ml = -1, ml = 0, ml = +1, ml = +2, ml = +3), so it can have at least 14 electrons.