Barron's AP Chemistry: Chapter 1

law of conservation of matter

chemical matter in a reaction is neither created not destroyed

law of constant composition

each pure chemical compound always has the same percentage composition of each element by mass.

atomic theory

-all matter is made up of tiny indivisible particles called atoms that cannot be created nor destroyed

-each element has atoms that are identical to each other in all of their properties, and these properties are different from properties of all other atoms

-chemical rxns are simple rearrangements of atoms from one combination to another in small whole-number ratios

law of multiple proportions

atoms combine in small, whole number ratios

cathode ray tube

a piece of equipment used by thomson to discover the electron.

charge to mass ratio

thomson measured this ratio for cathode rays and in doing so discovered the electron

oil drop experiment

measured the charge of an electron; the mass of an electron could then be determined

"plum pudding" model

oil drop and j.j thomsons information led to the model of the atom in which there were electrons bathed in a sea of positive charges

gold foil experiment

alpha particles were scattered by the gold foil, proving there is a nucleus

solar system model

ernest rutherford created the ______

ground state

the lowest allowable energy state of an atom

excited state

a state in which an atom has a higher potential energy than it has in its ground state

microwaves

radio waves with the shortest wavelengths and the highest frequencies

michael faraday

the english physicist and chemist who discovered electromagnetic induction (1791-1867)

j.j. thomson

discovered the electron

ernest rutherford

discovered the nucleus

balmer

visible light

niels bohr

discovered that electrons move around the nucleus in orbits called electon clouds in 1913

max planck

german physicist who developed quantum theory and was awarded the nobel prize for physics in 1918.

louis de broglie

who predicted that all matter can behave as waves as well as particles

erwin shrodinger

used a mathematical equation to describe the behavior of the electron in the hydrogen atom

werner heisenberg

uncertainty principle

wave-particle duality

the concept that all matter and energy exhibit both wave-like and particle-like properties

heisenberg uncertainty principle

it is impossible to know exactly both the velocity and the position of a particle at the same time

principal quantum number

represents the principal energy level of the atom in which the electron is located and is related to the average distance of the electron from the nucleus

azimuthal quantum number (l)

sublevel of the electron and also represents the shape of the oribitals in the sublevel

magnetic quantum number (m)

designates the orientation of an orbital in space

spin quantum number (m)

"spin" of an electron

pauli exclusion statement

can't have same spin in same quantum (cannot have two arrows both going up or down in one line, has to be one up and one down)