quantum mechanics

Line spectrum

Individual colored lines will appear only at specific wavelengths

Wavelength range nm

400-750nm

Energy levels are denoted

N

Spacing between energy levels is

Not uniform

Blue line in hydrogen spectrum

434 nm

Requires atom to absorb most energy

n=1—>n=2

Rydberg constant Rh

E=-2.18×10^-18(1/n2 -1/n2)

Heisenberg uncertainty principle

Impossible to know the exact location and directional speed of an electron

Erwin schondinger

Only predict general location within an atom

Areas of high electron density

Electron clouds

Orbitals

Every numerical value of l is assigned

A specific letter

Orbital

Three dimensional region where there is a high probability of electron density ( finding an electron)

Every orbital regardless of type can accommodate a total of

2 electrons

Spin quantum number ms

Describes an individual electron as opposed to the entire orbital

Independent of the tree quantum numbers

Spin up

Ms= +1/2

Spin down

Ms=-1-2

Node

No density of electrons

Nodal surfaces can be classified as

Planar(flat) spherical(radial)

relationship between planar nodes to l

l=#planar nodes

relationship between total number of nodes to n

N-1=total number of planar nodes

In orbital is a probability distribution map showing

Where the electron is likely to be found

S orbital looks like a

Sphere

P orbital looks like a

Peanut

D orbital looks like a four leaf

Clover

Possible values for quantum number (n)

Integer values of 1,2,3 etc

The principal quantum number determines

Overall energy and size of an orbital

Possibly values for angular momentum quantum number

Non negative integers 0 1 2 3 etc

The angular momentum number determines

Shape of orbital

Possible values for magnetic quantum number

Integer values of -l to +l

The magnetic quantum number determines

The orientation of an orbital

If n=1 then

l=0

If n=2 then

l=0,1

If n=3 then

l=0,1,2

If n=4

l=0,1,2,3

If l=0

Ml=0

If l=1

Ml= -1,0,1

If l=2

Ml= -2,-1,0,1,2

Equation to determine possible values of Ml from the value of l

Ml= 2l +1

Which of these orbits do not exist?

4s 3D 3s 2d

2d