Allowed values for the quantum numbers of electrons are as follows:

\(n\) = 1, 2, 3, ...
\(l\) = 0, 1, 2, 3, ..., \(n\) - 1
\(m_{l}\) = 0, \(\pm\)1, \(\pm\)2, \(\pm\)3,..., \(\pm l\)
\(m_{s}\) = \( \pm {1 \over 2} \)

The relationships between n and the shell designations are noted in Table 2.1. relative to the subshells,

\(l\) = 0 corresponds to an \(s\) subshell
\(l\) = 1 corresponds to a \(p\) subshell
\(l\) = 2 corresponds to a \(d\) subshell
\(l\) = 3 corresponds to an \(f\) subshell

For the K shell, the four quantum numbers for each of the two electrons in the 1\(s\) state, in the order of \(nlm_{l}m_{s}\), are 100\(1\over 2\) and 100(-\(1\over 2\)). Write the four quantum numbers for all of the electrons in the L and M shells, and note which correspond to the s, p, and d subshells.