LECTURE 9- Quantum Numbers, Shells, and Subshells of Orbitals

orbitals with the same value of n form a

spherical shell

size of each shell gets bigger as

n increases

orbitals within a shell are further divided into subshells based on

values of l

there are n diff values of l in all

and n subshells in a shell with a value of n

one subshell (l=0) for shell n=1

two subshells (l=0 and 1) for shell n=2 (etc)

letters (s,p,d,f) correspond to

l values

shape of atomic orbitals

describes the space within which there is a likelihood of finding the electron in the atom

1) electron density map

denser regions of dots show locations with high probability of finding an electron

2) radial probability

• y= (4πr²) y²

• x= distance from the nucleus, r

3) 3D boundary surface

90% probability that the electron will be found (hypothetical sharp boundary around the circle)

shape of s orbitals

l=0

shape of p orbitals

l=1

shape of d orbitals

l=2

shape of f orbitals

l=3

nodes

empty space

where x & y join

• nucleus

• low probability of finding the electron

degenerate

identical energies (same shape)

different shades

opposite signs of wave function

same color

same sign og wave function

ml values

could be assigned to any graph ONCE