Unit 3- Honors Chemistry

Ionization Energy

Energy required to remove an electron from an atom ion.
Increases across period, decreases down a group

Atomic radius

Size of a neutral atom
Decreases across period, increases down group

Electronegativity

Ability of an atom to grab/take electrons.
Increases across period, decreases down group

Electron Affinity

Energy changed when electron is added.
Increases across period, decreases down group

Schrodinger

Mathematical equation for electrons probability of location (electron cloud)

Hund's Rule

When filling up orbitals of equal energy, electrons will occupy separate orbitals with the same spin before pairing up.

Pauli's Exclusion Principle

No two electrons in a given energy level can occupy the exact same energy level with the exact same spin

Aufbau's Principle

Electrons occupy the lowest energy level first before moving up to a higher orbital

Bohr Model

Named after Niels' Bohr. Simplified representation of atomic structure

Rutherford

Gold foil experiment discovered the densely packed positive nucleus

Thomson

Discovered the electron through cathode ray tube experiment

Cations

Have lost an electron; positively charged

Anions

Have gained electrons; negatively charged

The Octet Rule

When bonding, atoms bond or try to get 8 valence electrons

Red Wavlength

Radio Characteristics: Long wavelengths, low frequences

Blue Wavelength

Gamma characteristics: Short wavelengths, high frequency, high energy

Metals

Left of the staircase, all solids except mercury (Hg), lustrous, conduct heat/electricity, malleable, ductile

Metalloids

On the staircase, tend to have both metals and non-metal properties

Non-metals

Right of staircase (+H), dull, some are solid at room temp, some are gas, Br is a liquid, poor conductors, brittle

Alkali Metals

Group 1; 1 valence electron; highly reactive with water

Alkaline Earth Metals

Group 2; 2 valence electrons; reactive; most found in earths crust

Transition Metals

Groups 3-12; valence electrons vary; have/form colored compounds

Halogens

Group 17; 7 valence electrons, most reactive non-metals

Noble Gases

Group 18; 8 valence electrons (except He, 2); non-reactive