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Bohr-Diagram-lesson.ppt
- 1. Bohr's Model ofthe Atom
- 2. Bohr's Model ofthe Atom Niels Bohr (1913):
- 3. Bohr's Model ofthe Atom Niels Bohr (1913): -studied the light produced when atoms were excited by heat or electricity
- 4. Bohr's Model ofthe Atom Niels Bohr (1913): -studied the light produced when atoms were excited by heat or electricity
- 5. Bohr's Model ofthe Atom Niels Bohr (1913): -studied the light produced when atoms were excited by heat or electricity Rutherford's model couldn't explain why unique colours were obtained by atoms of different elements
- 6. Bohr's Model ofthe Atom Niels Bohr (1913): -studied the light produced when atoms were excited by heat or electricity Rutherford's model couldn't explain why unique colours were obtained by atoms of different elements Bohr proposed that electrons are in orbits & when excited jump to a higher orbit. When they fall back to the original they give off light
- 7. Bohr's Model ofthe Atom Bohr's model: -electrons orbit the nucleus like planets orbit the sun
- 8. Bohr's Model ofthe Atom Bohr's model: -electrons orbit the nucleus like planets orbit the sun -each orbit can hold a specific maximum number of electrons
- 9. Bohr's Model ofthe Atom Bohr's model: -electrons orbit the nucleus like planets orbit the sun -each orbit can hold a specific maximum number of electrons orbit maximum # electrons 1 2 2 8 3 8 4 18
- 10. Bohr's Model ofthe Atom Bohr's model: -electrons orbit the nucleus like planets orbit the sun -each orbit can hold a specific maximum number of electrons -electrons fill orbits closest to the nucleus first.
- 11. Bohr's Model ofthe Atom e.g. fluorine: #P = #e- = #N =
- 12. Bohr's Model ofthe Atom e.g. fluorine: #P = atomic # = 9 #e- = #N =
- 13. Bohr's Model ofthe Atom e.g. fluorine: #P = 9 #e- = # P = 9 #N =
- 14. Bohr's Model ofthe Atom e.g. fluorine: #P = 9 #e- = 9 #N = atomic mass - # P = 10
- 15. Bohr's Model ofthe Atom e.g. fluorine: #P = 9 #e- = 9 #N = 10 draw the nucleus with protons & neutrons 9P 10N
- 16. Bohr's Model ofthe Atom e.g. fluorine: #P = 9 #e- = 9 #N = 10 how many electrons can fit in the first orbit? 9P 10N
- 17. Bohr's Model ofthe Atom e.g. fluorine: #P = 9 #e- = 9 #N = 10 how many electrons can fit in the first orbit? 2 9P 10N
- 18. Bohr's Model ofthe Atom e.g. fluorine: #P = 9 #e- = 9 #N = 10 how many electrons are left? 9P 10N
- 19. Bohr's Model ofthe Atom e.g. fluorine: #P = 9 #e- = 9 #N = 10 how many electrons are left? 7 9P 10N
- 20. Bohr's Model ofthe Atom e.g. fluorine: #P = 9 #e- = 9 #N = 10 how many electrons are left? 7 how many electrons fit in the second orbit? 9P 10N
- 21. Bohr's Model ofthe Atom e.g. fluorine: #P = 9 #e- = 9 #N = 10 how many electrons are left? 7 how many electrons fit in the second orbit? 8 9P 10N
- 22. Bohr's Model ofthe Atom e.g. fluorine: #P = 9 #e- = 9 #N = 10 9P 10N
- 23. Bohr's Model ofthe Atom try these: hydrogen boron magnesium
- 24. Bohr's Model ofthe Atom try these: hydrogen 1P 0N
- 25. Bohr's Model ofthe Atom try these: boron 5P 6N
- 26. Bohr's Model ofthe Atom try these: magnesium 12P 12N