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Hnr Chem Chpt 3 Test

Chemical Reaction The transformation of a substance or substances into one or more new substances.
Law of Conservation of Mass Which states that mass is neither created nor destroyed during ordinary chemical reactions or physical changes.
Law of Definite Proportions A chemical compound contains the same elements in exactly the same proportions by mass regardless of the size of the sample or source of the compound.
Law of Multiple Proportions If two or more different compounds are composed of the same two elements, then the ration of the masses of the second element combined with a certain mass of the first element is always a ratio of small whole numbers.
Atom as the smallest particle of an element that retains the chemical properties of that element.
Nuclear Forces These short-range proton-neutron, proton-proton, and neutron-neutron forces hold the nucleus particles together.
Atomic Number Number of protons of each atom of that element.
Isotopes Different # of neutrons
Mass Number The total number of protons and neutrons that make up the nucleus of an isotope.
Hyphen Notation Name of Element - Mass of a Number
Nuclear Symbol Superscript = mass number & Subscript = atomic number
Nuclide A general term for a specific isotope of an element.
Atomic Mass Unit Exactly 1/12 the mass of a carbon-12 atom.
Average Atomic Mass The weighted average of the atomic masses of the naturally occurring isotopes of an element.
Mole Amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon-12
Avogadro's number 6.022 * 10^(23) -- the number of particles in exactly one mole of pure substance.
Molar Mass The mass of one mole of a pure substance.
Created by: MyKeilah