Definitions
Number of atoms or molecules in a sample of matter
Mole
6.02 x 10 to the 23
Avogadro's Number
a measure of the height of the crests or the depths of the troughs on a wave
Amplitude
any substance that cannot be broken down into simpler components
Element
Liquid to gas
Boiling point
brittle, lackluster, does not conduct
Non-metals
cells sensitive mostly to low levels of light, not very sensitive to color
Rod
diagram showing bonding between atoms of a molecule & lone pairs of electrons that may exist in the molecule
Lewis Structure
electron can occupy any space inside orbital, not out
S orbital
limits the amount of product that can be formed in the chemical reaction
limiting reactant
anything that has mass & takes up space
Matter
malleable, luster, conduct electricity
Metals
matter cannot be created or destroyed it can only change forms
Law of Mass Conservation
model created by British physicist J.J. Thompson
Plum Pudding Model
most atoms strive to attain eight valence electrons
Octet Rule
no electrons at the 1st energy level of atom, but present in second
P Orbital
no matter how large or small the # is they always include a decimal point
Scientific notation
relating the quantities of a chemical substances in a chemical reaction
Stoichiometry
shared pair of valence electrons that holds atoms together in covalent compounds
Covalent
substances that can be decomposed into elements by chemical means
Compounds
the # of wave crests that pass a given point each second
Frequency
the mass of one mole of a given compound
Molar Mass
the total # of neutrons & protons in an atom
Atomic Mass
gas to liquid
Condensing point
very complex, five different energy levels, located on 3rd energy level
D Orbital