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Atomic Structure

Atomic Structure. What Is An Atom?. the smallest particle of an element that retains the chemical properties of that element Can be subdivided into electrons (e - ), protons (p + ) and neutrons (n 0 ). Diagram Of An Atom. Important Info About Subatomic Particles.

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Atomic Structure

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  1. Atomic Structure

  2. What Is An Atom? • the smallest particle of an element that retains the chemical properties of that element • Can be subdivided into electrons (e-), protons (p+) and neutrons (n0)

  3. Diagram Of An Atom

  4. Important Info About Subatomic Particles 1 amu = (1/12)(mass of C-12 isotope in kg) 1 amu = 1.660540 x 10-27 kg Amu = atomic mass units

  5. Atomic Number (Z) • Tells us the number of protons in the nucleus of an atom Z

  6. Isotopes • Some atoms of the same element will have different masses. • These atoms are called isotopes because they have the same number of protons, but differ in the number of neutrons. • Isotopes of the same element have different mass numbers. • Mass number (A) is the total number of protons and neutrons in the nucleus of an isotope

  7. How Are Isotope Symbols Denoted?

  8. Hyphen Notation of Isotopes • Isotopes can also be denoted through hyphen notation • The element symbol will be listed, following a hyphen, and then a mass number (p+ + n0) • Ex. Hydrogen has 3 isotopes (H-1, H-2, H-3)

  9. Hydrogen Isotopes AKA “Protium” 99.985% Abundant H-1 .015% Abundant H-2 Radioactive, Prepared Artifically H-3

  10. Sample Problems • How many protons, electrons, and neutrons are there in a Cl-37 atom? • How many protons, electrons, and neutrons are there in the following isotopes? -1

  11. Atomic Mass • What is the atomic mass listed on the periodic table under each element really measuring? • This mass is a weighted average of all of the naturally occurring isotopes of an element • This mass is a relative average (compared to the C-12 isotope) in atomic mass units (amu)

  12. How To Find The Atomic Mass of Hydrogen H-1 is 99.985% abundant with an atomic mass of 1.007825 amu H-2 is .015% abundant with an atomic mass of 2.016490 amu H-3 is not counted because of the fact that it is not naturally occurring To find the weighted average: (% abundance/100)(relative atomic mass of isotope 1) + (% abundance/100)(relative atomic mass of isotope 2) + (% abundance/100)(relative atomic mass of isotope 3)… *Mass # may be substituted for the relative atomic mass when given (99.985%/100)(1.007825 amu) + (.015%/100)(2.016940 amu) = 1.0079 amu

  13. Things To Remember… • If you change the number of protons, you change the type of atom itself. • If you change the number of electrons, you change the atom to an ion (charged particle). • If you change the number of neutrons, you change the isotope of that element.

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