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Chapter 3 CHEM

Chapter 3 chemistry Test

Law of definite Proportions Compound are made of the same elements in the Same properties regardless of size source of sample.
Law of Conservation of Mass Mass cannot be created or destroyed
Law of multiple proportions When two or more elements combine to form two compound the mass of one elements that combines with a given mass of the other is in the ration of small whole numbers
Electron A subatomic particle that has a negative electric charge
Nucleus Dense, central potion of the atom holds all the positive charge
Proton A subatomic particle with a positive charge, found in the nucleus of an atom.
Neutron A subatomic particle that his no charge and is found in the nucleus
Atomic Number the NUMBER OF PROTONS IN THE NUCLEUS OF AN ATOM, the atomic number is the same for all atoms of elements
Mass number The total number of protons and neutrons of the nucleus of an atom
Isotope Same number of protons, but different number of Neutrons
Orbital Regions around a nucleus that correspond to specific energy levels, electrons are likely to be found here.
Electromagnetic Spectrum Distance between two consecutive peaks to trough, light emissions
Ground State Lowest stare of energy
Excited State Highest state of energy
Pauli Exclusion Principle The principal that states that two particles of a certain class cannot be in the exact same energy state
Electron Configuration The atomic number represents the number of protons in an atom which also equals the number of electrons in an atom
Aufbau Principle Electrons fill orbits that have the lowest energy state
Hund's Rule Fill each orbital of an energy level with one electron before putting a second electron in the orbital.
Atomic Mass Mass of atom in measured in atomic Mass units (amu)
Created by: hackett12