Let’s Review!!!

Electronsand

ORBITALS

s orbitals are spherical and have 1 spacial orientation

s orbitals as n increases: 1s, 2s, and 3s

p orbitals are 3 dumbbell shapes or 3 spacial orientations

p orbitals

p orbitals

s and p orbitals

d orbitals are 5 complex shapes or 5 spacial orientations

d orbitals have 5 complex shapes or have 5 spacial orientations

f orbitals have 7 complex shapes or 7 spacial orientations

f orbital

The 4th shell (n=4)

An electron that is confined to a particular space around the nucleus of an atom can only move around that atom in such a way that its electron wave “fits” the size of the

atom correctly. This means that the frequencies of electron waves are quantized.

Based on the E=hν equation, the fact that only certain quantized frequencies are allowed for a given electron means that electrons can only exist in an atom at specific energies, as Bohr had previously theorized.

Remember !Heisenberg Uncertainty Principle:

states that it is impossible to determine simultaneously both the position and the velocity of a particle.

http://video.pbs.org/video/18121247/

Aufbau Principle: Electrons fill orbitals of lowest energy first.

Hund’s Rule: Electrons enter orbitals with parallel spins before pairing.

Pauli Exclusion Principle: States that a sublevel can contain up to 2 electrons and must have parallel spins.

http://www.kentchemistry.com/links/AtomicStructure/elecPT.htm

Emission Spectrum

Color of Light for some Common Elements

Metal ions & Colors

Carbon goldIronTitanium, whiteAluminum,Beryllium,Magnesium

PERIODIC TRENDSAtomic Size

Periodic TrendsElectronegativity

Periodic TrendsElectron Affinity

Periodic Trend Ionization Energy

Periodic Trend Metallic Character

Periodic TrendShielding Effect

Periodic TrendBoiling Point

Periodic Trends Reactivity in Metals

Periodic Trends Reactivity in Nonmetals