What You Should Know So Far

The Fundamental Laws

Conservation of Mass

Definite Composition

Multiple Proportions

Daltons Atomic Theory

The Experiments

Thomson’s Cathode Ray TubeDiscovers the electron

Rutherford’s Gold Foil ExperimentDescribes the atom as a small dense positively charges nucleus surrounded by relatively large negatively charged cloud. An atom is mostly empty space.

A wave

Amplitude

Frequency

Wavelength

What Spectrums Tell Us

Spectrum

Hydrogen Spectrum

Wave and a Particle

Planks

Duality of Nature

Electron is both a wave and a particle

The rulesAufbau principle

States that the structure of each successive element is obtained by adding one proton to the nucleus and one electron to the lowest energy orbital that is available.

Hund’s ruleFor an atom in the ground state that the number of unpaired electrons is the maximum possible and these unpaired electrons have the same spin

Pauli Exclusion PrincipleThat two particles of a certain class cannot occupy the same four quantum numbers

Pauli’s Exclusion PrincipleNo two electrons can have the same four quantum numbersorbital

Quantum Numbers

n,l,m,s n = energy level

l = suborbital s, p,d,f

m = number of electrons

s = spin

Orbital Shapes

s orbital

p obitals

d orbital

f orbital

pzpypx

s

Filling Electron Diagram

How To Write Configurations

Electron Arrow Diagram

Energy Level Diagram

EC Flow Chart

The Shortcut

Counting Atoms

Atomic MassMass of the atom in atomic mass units

1 amu has the gram equivelence of 1 gram

MoleSI unit for measuring the amount of substance

Carbon -12 is the standard

Exact number of atoms that is in 12.0 g of C-12

Avogadro's number6.022 x 1023 units/mole

Mole Map

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HUH???

Given atoms 1 mole

6.022 x 1023 atoms

= atoms

Given Moles 6.022 x 1023 atoms

1 mole

= mole

More??

Given grams 1 mole

Molar Weight

= moles

Molar Weight

= grams

1 mole

Given moles

LAST ONE

Units1 mole

6.022 x 1023 units

Molar Weight

1 mole

= grams=Units

grams 6.022 x 1023 units

Molar Weight