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The Atom

The Atom. REALLY early atomic theory… Democritus ~350 BC Atomos - Greek meaning indivisible Modern Definition:. My Atom Broke. Subatomic Particles. My Atom Broke. Subatomic Particles Nucleus. My Atom Broke. Subatomic Particles. Atoms vs. Ions. Atoms are !!!!!

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The Atom

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  1. The Atom • REALLY early atomic theory… • Democritus ~350 BC • Atomos - Greek meaning indivisible • Modern Definition:

  2. My Atom Broke • Subatomic Particles

  3. My Atom Broke • Subatomic Particles • Nucleus

  4. My Atom Broke • Subatomic Particles

  5. Atoms vs. Ions • Atoms are !!!!! • This means that they have

  6. Give the atom notation for the following: 1) an atom with 82 p+ and 126 no 2) an atom of iron with 28 no 3) an atom of element 29 having 34 no

  7. 209 83 74 53 24Cr 53

  8. Name that Isotope Hydrogen has 3 isotopes

  9. Information from the Periodic Table

  10. Atomic Masses • Measured in the unit amu • Stands for • Defined as • 35Cl = 34.9689 amu • 50V = 49.9472 amu • 79Br = 78.9183 amu

  11. All Isotopes are NOT Created Equal • Weighted averages

  12. All Isotopes are NOT Created Equal • Weighted averages • An equation (oh crap) • 35Cl = 34.9689 amu • Abundance = 75.77% • 37Cl = 36.9659 amu • Abundance = 24.23%

  13. All Isotopes are NOT Created Equal • 35Cl = 34.9689 amu • Abundance = 75.77% • 37Cl = 36.9659 amu • Abundance = 24.23%

  14. A Problem! What is the average atomic mass of magnesium? 78.90% of all magnesium is 24Mg  23.985 amu 10.00% of all magnesium is 25Mg  24.986 amu of all magnesium is 26Mg  25.983 amu

  15. Another Problem! Lead has 4 isotopes, the masses and abundances of which can be found in the following table. Your job? Calculate the isotope mass of lead-207.

  16. My Atom Broke • Subatomic Particles • Outside the nucleus • Electrons – e- • Carry a single negative charge • 1/1900th the size of p+ and no • Responsible for most of the chemistry that ever happens

  17. Electrons • e- are found in discreet ____________ or _______

  18. Electrons • e- are found in discreet “energy levels” or “shells” • Within these shells are ____________________ • Sub-shells are named _____________________ • _______________________

  19. Electron Sub-Shells

  20. LIGHT!!! wavelength  __________________________ frequency  _______________________________ energy speed of light  3.00x108 m/s

  21. LIGHT!!! wavelength and frequency are _________ proportional wavelength frequency

  22. LIGHT!!! wavelength and energy are ___________ proportional wavelength energy energy and frequency are ____________ proportional energy frequency

  23. 5 4 3 2 1

  24. Bohr Model of H Atoms 26

  25. Hydrogen Energy Transitions 27

  26. Examples of Spectra 28

  27. Which is a higher energy transition? 65 or 32 6 53 or 31 5 23 or 34 4 3 2 1

  28. The Beginning Mendeleev’s predictions: Property Predicted Actual color atomic mass density melting point formula of oxide density of oxide formula of chloride B.P. of chloride

  29. The Modern Periodic Table • Moseley • Set it up by ______________rather than ____________ • Periodic Law – properties occur in a repeating pattern when set up by atomic number.

  30. The Modern Periodic Table • Periods (series) • Groups (families) • 2 different labeling systems

  31. A few definitions… • Main Group Elements: • Groups ____________________ • Transition Elements: • Groups _____________________

  32. Groups of Elements • Vertical columns are called groups • Group 1 = _____________________ • Group 2 = _____________________ • Group 17 = _____________________ • Group 18 = _____________________

  33. The Modern Periodic Table • Representative elements • Also known as main group elements • Transition metals • Inner transition metals • Lanthanide series • Actinide series

  34. Diatomic Elements • Elements that exist as diatomic molecules when UNCOMBINED (meaning not in a compound with other elements).

  35. Diatomic Elements • Elements the exist as diatomic molecules when UNCOMBINED (meaning not in a compound with other elements). H2, N2, O2, F2, Cl2, Br2, I2 Examples of when these elements are NOT diatomic

  36. Periodic Trends • Atomic Radius

  37. Atomic Radius Trend • Atoms get smaller as you go bottom to top on the periodic table because there are fewer energy levels on the atom. (Na has 3 energy levels, K has 4) • Atomic radius decreases as you travel left to right across the periodic table because the number of protons in the nucleus increases.

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