There are 11 atomic orbitals in the #h# subshell, and they can hold a total of 22 electrons.

The hydrogenic (one-electron) orbitals are each associated with a principal quantum number (#n#) and an orbital angular momentum quantum number (#l#). The different values of #l# are denoted by letters instead of numbers.

For example, orbitals having #l=0# are called #s# orbitals, those with #l=1# are called #p# orbitals, then #d, f, g, h, # and so on.

(excluding j)

Following the lettering system, we see that #h# orbitals are associated with #l=5#.

Finally, the number of orbitals in each sub-shell is equal to #2l+1#, so there is only 1 #s# orbital, but there are 3 #p# orbitals, and 5 #d# orbitals in each sub-shell. Following this trend, we see that the number of #h# orbitals is equal to #2times5+1=11#.

(Each orbital can hold up to 2 electrons if they have opposite spin angular momentum quantum numbers, so the #h# shell can hold a maximum of 22 electrons.)