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The Atom

The Atom. Plum Pudding Model. J.J. Thomson (-) charged particles electrons Discovered using a cathode ray tube. Gold Foil Experiment Ernest Rutherford. Rutherford’s Model of the Atom. Nucleus (Center). Atomic Makeup. Electron . (-) charge Outside nucleus. Proton.

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The Atom

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  1. The Atom

  2. Plum Pudding Model • J.J. Thomson • (-) charged particles • electrons • Discovered using a • cathode ray tube

  3. Gold Foil ExperimentErnest Rutherford

  4. Rutherford’s Model of the Atom Nucleus (Center)

  5. Atomic Makeup • Electron (-) charge Outside nucleus • Proton (+) charge Inside nucleus • Neutron Chadwick (0) charger = neutral Inside nucleus

  6. Center – Nucleus Protons Neutrons Outside Nucleus Electrons

  7. Subatomic Particles Proton Neutron Electron Atomic Number (+) In nucleus Mass = 1 Neutral In nucleus Mass = 1 (-) Outside Nucleus Mass = 0 + Neutral Atom (+) = (-) Protons = electrons Mass Number (Atomic Mass)

  8. Atomic Notation Symbolic Notation Hyphen Notation Mass # (p + n) 12 C Carbon - 12 6 Mass # Atomic # (p)

  9. Isotopes • Same element (same protons) • Different mass (different neutrons) 11H 21H 31H

  10. Average Atomic Mass • Mass of all the isotopes • Based upon their naturally occurring ABUNDANCE Mass of Isotope #1 X (abundance) = #1 Mass of Isotope #2 X (abundance) = #2 Mass of Isotope #3 X (abundance) = #3 #1 + #2 + #3 = AVERAGE ATOMIC MASS

  11. Bohr Atom Electrons in specific ORBITS around nucleus

  12. Electron in the Ground State Electron Gains Energy

  13. Moves to Higher Energy Level Excited State

  14. Electron Loses Energy We see Light/Color

  15. Electron Moves Back to the Ground State

  16. What Color do we see? Determined by the energy given off • Each transition has a certain amount of energy • n=2  n=1 has a different amount of energy than n=6  n=1 E = h E = energy h = 6.626 X 10-34 J*s (Planck’s constant)  = frequency C =  c = speed of light (3.0 X 108 m/s)  = wavelength

  17. Quantum Numbers • Current model for the atom • PROBABLE location of electrons in atom • Four quantum #s to describe location nlms Energy Levels (Floors) #s (1, 2, 3, etc..) Sublevel (Rooms) S P D F Orbitals (Beds) 1 3 5 7 Spin of Electrons (Bunnies) 2 6 10 14 +1/2 -1/2

  18. Parts of Periodic Table • Groups/Families • Periods • Metals • Nonmetals • Metalloids • Solids, Liquids, Gases • Alkali Metals • Alkaline Earth Metals • Transition Elements • Halogens • Noble Gases • Lanthanides • Actinides • Rare Earth Elements/Inner Transition Metals • Columns (18) • Rows (7) • Left of Stairstep • Right of Stairstep • Elements touching stairstep • Black, Blue, Red • Group 1 • Group 2 • Groups 3 – 12 • Group 17 • Group 18 • Elements # 58-71 • Elements # 90-103 • Bottom two rows together

  19. Blocks of Perioidic Table • S block • P block • D block • F block • Groups 1 & 2 • Groups 13 – 18 • Groups 3 – 12 • Bottom two rows

  20. PeriodicityTrends within the periodic table (Across) Decreases • Atomic Radius (size of atom) • Ionization Energy • Electron Affinity • Electronegativity (Down) Increases (Across) Increases (Down) Decreases

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