Atomic Theory Math Isotopes, Ions, and Average Atomic Mass.

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Presentation transcript:

Atomic Theory Math Isotopes, Ions, and Average Atomic Mass

Parts of atom as of now NameLocationActual Mass (kg) Relative Mass (amu) Actual Charge (C) Relative Charge Proton,p + nucleus1.67* * Neutron, n 0 nucleus1.67* Electron, e - Outside the nucleus in energy levels 9.1* *10 -19

Ions – electrically charged particles Positive ions – lose electrons +1 lose one electron +2 lose two electrons +3 lose three electrons Negative ions – gain electrons -1 gain one electron -2 gain two electrons -3 gain three electrons

Atomic number – number of protons, Z, id’s the element Mass Number – number of protons plus neutrons, A Why is electron NOT part of mass number Isotopes – same element different mass same atomic number different mass number same number of protons different number of neutrons same Z different A

Isotopes chart (Red text was originally blank) IsotopeAtomic Number Mass Number p+p+ n0n0 e-e- C C C H1H H2H H3H O Let’s mix it up now Mg Ne U

Average Atomic Mass Weighted average – the isotope most in abundance skews the average Mass number *abundance + Mass number *abundance = Average atomic mass total abundance