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.