erwin schrodinger proved - ms. phornvoranunt...

• Erwin Schrodinger proved

the idea of the “Planetary

Atom” wrong

• He said the e- does not move

around in fixed orbits

• He proved that the e- moves

in 3D areas around the

nucleus

• He made a complicated

math equation describing

the area of an e-

• BUT…its just a probability of

where an e- may be in the

atom

• We do not know exactly

where an e- is in an atom

• e- have different energy

levels called principal

quantum numbers (n)

• Within the energy levels

are sublevels that have their

own significant shape

• 3D non-circular areas where

e- can be

• Inside sublevels there are

orbitals, where e- are

arranged

• s is the first and

simplest sublevel

• Has only 1 orbital that

holds 2 electrons

• p is the second sublevel

• 3 orbitals

each holds 2 electrons

• A total of 6 electrons

• d is the third sublevel

• 5 orbitals

each holds 2 electrons

• A total of 10 electrons

• f is the last sublevel

• 7 orbitals

each holds 2 electrons

• A total of 14 electrons

Sublevel Orbitals Electrons

s 1 2

p 3 6

d 5 10

f 7 14

All electrons follow three

rules when filling energy

levels and sublevels. They

are:

• Aufbau Principle

• Pauli Exclusion Principle

• Hund’s Rule

• Each electron occupies

the lowest energy

orbital available

Here’s how to remember…

• Principal quantum numbers are like floors of a hotel

• e- enters the lowest level first

The Hotel Californium

1st floor

2nd floor

5th floor

n = 1

n =2

n = 5

= electron

• A maximum of two

electrons may occupy a

single orbital, but only

if the electrons have

opposite spins

Here’s how to remember…

Spin one index finger away

from your

Spin the other index finger

toward you

• Single electrons with

the same spin must

occupy each equal-

energy orbital before

additional electrons

with opposite spins can

occupy the same

orbital.

Here’s how to remember…

“Strangers on a bus”

• Do you sit next to a stranger or pick an empty seat?

• Pick an empty seat…unless there isn’t one, then you sit with the stranger

• Includes a box for each

of the atom’s orbitals

• Boxes are filled with

arrows representing

electrons

Up and down facing

arrows to show opposite

spins

Orbital Diagrams

1s

2s 2p

3s 3p 3d

4s 4p 4d 4f

5s 5p 5d 5f

6s 6p 6d 6f

7s 7p 7d 7f • Start from bottom of

Aufbau diagram.

• Remember orbital table

for the sublevels

1s2s2p3s3p4s3d

Incr

easi

ng e

ner

gy

• Remember the rules

electrons follow when

filling energy levels,

sublevels and orbitals

Aufbau Principle

Pauli Exclusion Principle

Hund’s Rule

• Let’s determine the

orbital diagram for

Phosphorus

15 electrons

Filling in Orbital Diagrams:

• The first 2 e- go into 1s

orbital (line )

• only 13 more to go...

• Next e- go into 2s orbital

• only 11 more…

• Next e- go into 2p orbital

• only 5 more…

• Next e- go into 3s orbital

• only 3 more…

• Last e- go into 3p orbital

• e- by themselves before

being paired

• 3 unpaired e-

1s2s2p3s3p4s3d

Notice the opposite

spins (one ↑, one ↓)

• Determine the orbital

diagram for the

following:

Cobalt (Co)

Germanium (Ge)

1s2s2p3s3p4s3d

Cobalt – 27 e- Germanium – 32 e-

1s2s2p3s3p4s3d

4p

Electron

Configurations• 1s2 2e-

• 1s22s2 4e-

• 1s22s22p63s2 12e-

• 1s22s22p63s23p64s2 20e-

• 1s22s22p63s23p64s23d10

4p65s2 38e-

• 1s22s22p63s23p64s23d10

4p65s24d105p66s2 56e-1s

2s 2p

3s 3p 3d

4s 4p 4d 4f

5s 5p 5d 5f

6s 6p 6d 6f

7s 7p 7d 7f

Example: Oxygen

1s

2s 2p

3s 3p 3d

4s 4p 4d 4f

5s 5p 5d 5f

6s 6p 6d 6f

7s 7p 7d 7f• 1s2

• 2 electrons

• 4 electrons

• Total 8 electrons

• Stop once the # e- = the

atomic number

• Last sublevel doesn’t have

to be completely filled

8

16O

8 electrons2s2 2p4

• Use your periodic

tables to find the

atomic numbers and

the electron

configurations of the

following elements:

Silicon

Uranium

• Silicon

1s22s22p63s23p2

• Uranium

1s22s22p63s23p64s23d10

4p65s24d105p66s24f14

5d106p67s25f4