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Honors Chem Ch 3

Huskychemistry Honors Ch 3

atomic mass unit (amu) the measuring unit for atomic masses, based upon the mass of carbon
atomic number the number of protons in an atom, determines the element's identity
atomic mass the mass of an atom's protons plus its neutrons
isotope atoms of the same element that have different masses due to different numbers of neutrons
molar mass the mass of one mole of a substance; for example, one mole of carbon has a mass of 12.01 grams
mole a counting unit, 6.02 x 10 23, also known as Avagadro's number
law of conservation of mass mass is neither created nor destroyed during ordinary chemical reactions
law of definite proportions compounds contain the same elements in the same proportions by mass regardless of the size of the sample
atom the smallest unit of an element that maintains the properties of that element
Democritus ancinet Greek; idea of atoms being indivisible
Aristotle ancient Greek; idea that matter was continuous and that there were no such things as atoms
Dalton 1800's; created a five part atomic theory that is still in use today
Rutherford gold foil experiment determined that the nucleus of an atom is small, dense, and has a positive charge
Thomson and Millikan conducted experiements that determined that electrons are very small, negative, and found in all atoms
proton the positive part of an atom, found in the nucleus
neutron found in the nucleus of an atom, has no charge
electron negative part of an atom, found outside the nucleus
nucleus the center part of an atom where the protons and neutrons are located
Created by: huskychemistry



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