• Each shell can be divided further into?subshells,?labelled?s, p, d and f
• Each subshell can hold a specific number of orbitals:
  • s subshell : 1 orbital
  • p subshell : 3 orbitals labelled p_x, p_y?and p_z
  • d subshell : 5 orbitals
  • f subshell : 7 orbitals

• Each orbital can hold a maximum number of 2 electrons so the maximum number of electrons in each subshell are as follows:
  • s : 1 x 2 = total of 2 electrons
  • p : 3 x 2 = total of 6 electrons
  • d : 5 x 2 = total of 10 electrons
  • f : 7 x 2 = total of 14 electrons
• In the ground state, orbitals in the same subshell have the same energy and are said to be degenerate, so the energy of a p_x?orbital is the same as a p_y?orbital

Shells are divided into subshells which are further divided into orbitals

Summary of the Arrangement of Electrons in Atoms Table

s orbitals

• The s orbitals are?spherical?in shape
• The?size?of the s orbitals increases with increasing shell number
  • E.g. the s orbital of the?third?quantum shell (n?= 3) is bigger than the s orbital of the?first?quantum shell (n?= 1)

The s orbitals become larger with increasing principal quantum number

p orbitals

• The p orbitals are?dumbbell-shaped
• Every shell has three p orbitals except for the first one (n?= 1)
• The p orbitals occupy the x, y and z axes and point at right angles to each other, so are oriented?perpendicular?to one another
• The lobes of the p orbitals become?larger?and?longer?with increasing shell number

The p orbitals become larger and longer with increasing principal quantum number