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Chemistry 1A Week 1 Lecture Notes Atom · · · · · Nucleus o Protons (+), neutrons (o) o Positive charge Electrons (-) Subatomic particles (protons, neutrons, electrons) o Measured in atomic mass units (u) o Neutral atom: protons = electrons Overall mass made of protons + neutrons (mass of electrons is insignificant) Overall volume/size made of protons, neutrons & electrons Molecule · Collection of atoms chemically bonded & uncharged Element · · · Collection of one type of atom Defined by number of protons Represented by chemical symbol: Where A = Mass No, Z = Atomic No, C+/- = charge Ion · · · Atoms that have gained or lost electrons Gained electrons: Charge is negative (anion) Lost electrons: Charge is positive (cation) Isotope · · · · Atom with different number of protons and neutrons Heavier isotopes occur in natural abundances Atomic mass (u) = average mass of atoms of isotopes as the occur naturally To calculate: o Divide percentages by 100 to find natural abundances o Atomic mass = (abundance 1 x mass 1) + (abundance 2 x mass 2)