Chemistry

Law of Definite Proportions

Atoms can combine with each other in simple whole number ratios to form compounds.

Law of Multiple Proportions

Atoms can combine in 2 or more ways to form compounds

Thomson Atomic Model

Electrons and Positive Charges were dispersed throughout the atom.

Rutherford Model

Atoms comprised of mostly empty space

Positively Charged Nucleus with Protons and Neutrons, Electrons Orbit around it.

Excited State

The state an electron enters when it absorbs energy and move to a higher Principle Energy Level and/or Orbital.

Ground State

Electrons destabilize in excited state and fall back down to the lowest available principle energy level.

Photon Release

When an electron returns to ground state, it releases the energy it held in the form of a photon/light energy.

Principle Energy Level Formula

2n²

Protons

Exist inside the nucleus

1 Atomic amass Unit

+1 Positive Charge

Neutrons

Exists inside the nucleus

1 Atomic Mass Unit

Neutral Charge

Electron

Exists outside the nucleus, orbiting it in the PELs

0 Atomic Mass Unit

-1 Negative Charge

Superposition

Non Newtonian property saying that a particle can exist at all of its possible locations at the same time.

Schrödinger

Proposed that electrons don’t orbit in circles around the nucleus but move in regions called orbitals.

Orbitals

A region in which an electron is most likely to be located

Wave Mechanical Model

The Modern Atomic Model where electrons do not orbit in circles around the nucleus but instead move in spaces called orbitals where they are most likely to be located.

Atomic Charge

Total charge of an atom or ion.

Valence electrons

Electrons in the outermost energy level

Kernel Electrons

Everything but valence electrons.

Anion

Negatively charged ion

Cation

Positively charged ion