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Chemistry Ch 3

Ch 3 Notes/Definitions/Vocab Etc

Law of conservation of mass mass is neither created not destroyed during ordinary chemical reactions or physical changes.
Law of definite proportions the fact a chemical compound contains the same elements in exactly the same proportions by mass regardless of the size, sample, or source of the compound.
Law of multiple proportions If 2 or more different compounds are composed of the same 2 elements, then the ratio of the masses of the second element combined with a certain mass of the first element is always the ratio of small whole numbers.
Atom smallest particle of an element that retains the chemical properties of that element
Nuclear forces short-range proton-neutron, proton-proton, neutron-neutron, forces hold the nuclear particles together
Atomic Number the # of protons of each atom of that element
Isotopes atoms of the same element that have different masses
Mass number total # of protons and neutrons that make up the nucleus of an isotope
Nuclide general term for a specific isotope of an element
Atomic mass unit 1amu is exactly 1/12 the mass of a carbon-12atom
Average atomic mass the weighed 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
Avagrado's Number 6.022 x 10^23. The # of particles in exactly one mole of a pure substance
Molar Mass mass of one mole of a pure substance
Created by: ArrowForever