Aufbau Principle

An electron occupies the lowest energy orbital that can receive it.

Pauli Exclusion Principle

No two electrons in the same atom can have the same set of four quantum numbers.

Hund’s Rule

Orbitals of equal energy are each occupied by 1 electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin.

Heisenberg Uncertainty Principle

It is impossible to determine simultaneously both the position and the velocity of an electron or any other particle.

Bohr Model of Hydrogen

http://science.sbcc.edu/physics/solar/sciencesegment/bohratom.swf

Quantum Numbers

Principle Quantum NumberSymbolized by n

Indicates the energy level

Values are all positive integers

# of orbitals in energy level = n2

Angular MomentumQuantum Number

Symbolized by l

Indicates the shape of the orbital

Values of l: 0 and all integers ≤ n-1

Magnetic Quantum Number

Symbolized by m

Indicates the orientation of an orbital around the nucleus

Spin Quantum Number

Has only two possible values +1/2, -1/2

Indicates the two fundamental spin states of an electron in an orbital

Chapter 4 Things to Review

VocabularyElectron ConfigurationOrbital NotationNoble Gas ConfigurationBohr’s Model of HydrogenWave: crest, trough, amplitude, wavelengthCalculations: Energy, Wavelength, Frequency

Chapter 4 Review page 118

1, 3, 4, 6, 8, 9,11,12, 13, 14a&b, 16, 17,18a, 19a, 20, 21, 22, 23, 24,25, 36, 27, 28. 29, 30, 32, 36, 37, 39, 40, 41, 42, 43, 44, 44, 45

1, 3, 4, 6, 8, 9, 11-13, 14a&b, 16, 17,18a, 19a, 20-30, 32, 36, 37, 39- 45