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The Atom

The Atom. Part 2. Review of the Atom. So far we have discussed: P rotons , E lectrons and N eutrons. Protons and neutrons are located in the n ucleus and adding them together will give you the Mass Number . Atoms , which are normally electrically n eutral and

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The Atom

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  1. The Atom Part 2

  2. Review of the Atom So far we have discussed: Protons, Electrons and Neutrons. Protons and neutrons are located in the nucleus and adding them together will give you theMass Number. Atoms, which are normally electrically neutral and Ions, which carry an electrical charge.

  3. Isotopes • While the number of protons is always constant in any atom of a given element, the number of electrons can vary (Ions) • The number of neutrons in an atom can also vary. • Two atoms of the same element that contain different numbers of neutrons are called isotopes.

  4. An Example of an Isotope Hydrogen has 3 isotopes – There are 3 different “versions” of a hydrogen atom • 1 proton and 0 neutrons (mass number = 1) • 1 proton and 1 neutron (mass number = 2) • 1 proton and 2 neutrons (mass number = 3) Notice that the # of protons stays the same!

  5. Ever wonder why the masses of atoms are such weird numbers? • Example • Carbon has a mass of 12.011 amu (atomic mass unit)

  6. Why All the Decimal Places? There are a few important things to know!!! • Atomic mass= “weighted” average of all the different isotopes of that element • This is the “weird” number on the periodic table that usually has a bunch of places past the decimal point • Mass Number = the sum of protons + neutrons • This one kind of makes sense because remember we said the electrons essentially don’t have any mass • This HAS to be a whole number!!!!! – It has to be, because you can’t have part of a proton or neutron • Mass number is NOT given on the periodic table

  7. APE MAN • AtomicNumber = Protons = Electrons • Mass Number = AtomicNumber + Neutrons

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