Atom video

http://www.youtube.com/watch?v=xqNSQ3OQMGI&feature=share

Basic Principle:electrons occupy

lowest energy levels available

Aufbau Principle -- “Bottom Up Rule”

Electron spin How could an orbital hold two electrons without electrostatic repulsion?

Stern-Gerlach Experiment

11s

value of energy level

sublevel

no. ofelectrons

spdf NOTATION

for H, atomic number = 1spdf Notation

Orbital Box Notation

Arrows show electron spin

(+½ or -½)

ORBITAL BOX NOTATION for He, atomic number = 2

1s

21s

2 ways to write electron configurations

Example:

Determine the electron configuration and orbital notation for the ground state neon atom.

An orbital can contain a maximum of 2 electrons,and they must have the opposite “spin.”

Pauli exclusion principle

Hund’s Rule -

Write the ground state configuration and the orbital diagram for oxygen in its ground state

Outer electron configuration for the elements

Using the periodic table to know configurations

Period1

2

3

4

5

6

7

Ne

Ar

Kr

Xe

Valence e’s for “main group” elements

Rules for Filling Orbitals

Bottom-up (Aufbau’s principle)

Fill orbitals singly before doubling up (Hund’s Rule)

Paired electrons have opposite spin (Pauli exclusion principle)

Basic Principle:electrons occupy

lowest energy levels available

Identify examples of the following principles: 1) Aufbau 2) Hund’s rule 3) Pauli exclusion

Shorthand notation practice

Examples

● Aluminum: 1s22s22p63s23p1 [Ne]3s23p1

● Calcium: 1s22s22p63s23p64s2

[Ar]4s2

● Nickel: 1s22s22p63s23p64s23d8

[Ar]4s23d8 {or [Ar]3d84s2}

● Iodine: [Kr]5s24d105p5 {or [Kr]4d105s25p5}

● Astatine (At): [Xe]6s24f145d106p5

{or [Xe]4f145d106s26p5}

[Noble Gas Core] + higher energy electrons

Electron configuration for As

Note: Not written according to Aufbau, but grouping according to n

Orbital energy ladder

s

pn = 2

s

d

p n = 3

f

s

d

pn = 4

s n = 1

Energy

PhosphorusSymbol: P

Atomic Number: 15

Full Configuration: 1s22s22p63s23p3

Valence Configuration: 3s23p3

Shorthand Configuration: [Ne]3s23p3

1s 2s 2p 3s 3p

Box Notation

Quantum numbers and orbital energies Each electron in an atom has a unique set of quantum numbers to

define it { n, l, ml, ms }

n = principal quantum number

– electron’s energy depends principally on thisl = azimuthal quantum number

– for orbitals of same n, l distinguishes different shapes (angular momentum)

ml = magnetic quantum number

– for orbitals of same n & l, ml distinguishes different orientations in space

ms = spin quantum number

– for orbitals of same n, l & ml, ms identifies the two possible spin orientations

Energy level Sublevel # of orbitals/sublevel

n = 1 1s (l = 0) 1 (ml has one value)

n = 2 2s (l = 0) 1 (ml has one value)

2p (l = 1) 3 (ml has three values)

n = 3 3s (l = 0) 1 (ml has one value) 3p (l = 1) 3 (ml has three values) 3d (l = 2) 5 (ml has five values)

n = principalquantumnumber(energy)

l = azimuthalquantumnumber(shape)

ml = magneticquantumnumber

(orientation)

Quantum numbers and orbital energies

Each atom’s electron has a unique set of quantum numbers to define it { n, l, ml, ms }

21

Concept: Each electron in an atom has a unique set of quantum numbers to define it

{ n, l, ml, ms }

Quantum numbers: unique set for each e-

s orbitals p orbitals d orbitals f orbitals

l = 0 l = 1 l = 2 l = 3

ml = 0 ml = -1, 0, 1 ml = -2, -1, 0, 1, 2 ml=-3,-2,-1,0,1,2,3

An s subshell A p subshell A d subshell An f subshell One s orbital Three p orbitals Five d orbitals Seven f orbitals

For n=1 l=0 an s subshell (with 1 orbital)For n=2 l=0,1 an s subshell and a p subshell (with 3 orbitals)For n=3 l=0,1,2 an s subshell, a p subshell, a d subshell (with 5 orbitals)For n=4 l=0,1,2,3 an s subshell, a p subshell, a d subshell, an f subshell (with 7 orbitals)

Electronic configuration of Br

1s2 2s22p6 3s23p63d10 4s24p5

[Ar] 3d104s24p5

[Ar] = “noble gas core”

[Ar]3d10 = “pseudo noble gas core”(electrons that tend not to react)

Atom’s reactivity is determined by valence electrons

valence e’s in Br: 4s24p5

highest n electrons

Valence e- shells for transition metalstransition metals v. main group elementsmain group elements

d orbitals sometimes included in valence shell

d orbitals not includedin valence shell

(pseudo noble gas cores)

Rule-of-thumb for valence electrons

Examples

● Sulfur: 1s22s22p63s23p4 or [Ne]3s23p4

valence electrons: 3s23p4

● Strontium: [Kr]5s2

valence electrons: 5s2

● Gallium: [Ar]4s23d104p1

valence electrons: 4s24p1

● Vanadium: [Ar]4s23d3

valence electrons: 4s2 or 3d34s2

Identify all electrons at the highest principal quantum number (n)

Use on exams,but recognize

limitations

Use Table 8.9for online HW

Selenium’s valence electrons

Pseudo noble gas core includes: noble gas electron core d electrons (not very reactive)

Written for increasing energy:

Core and valence electrons in Germanium

Pseudo noble gas core includes: noble gas core d electrons

Written for increasing energy:

d-block: some exceptions to the Aufbau principle

Fig. 8.9: Use this table for online homework

ParamagneticParamagnetic: atoms with unpaired electrons : atoms with unpaired electrons that are weakly attracted to a magnet.that are weakly attracted to a magnet.

DiamagneticDiamagnetic: atoms with paired electrons : atoms with paired electrons that are not attracted to a magnetthat are not attracted to a magnet..

ParamagneticParamagnetic: atoms with unpaired electrons : atoms with unpaired electrons that are weakly attracted to a magnet.that are weakly attracted to a magnet.

DiamagneticDiamagnetic: atoms with paired electrons : atoms with paired electrons that are not attracted to a magnetthat are not attracted to a magnet..

Electron spin & magnetism

For the ground state oxygen atom:

spdf configuration:

orbital box notation:

Apparatus for measuring magnetic properties