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Bohr and Quantum Models: A Beginner's Guide

Dive into the Bohr and Quantum Mechanical models of the atom! Learn about energy levels, electron orbits, and how to draw Bohr models step by step. Discover the transition from Bohr's model to the Quantum Mechanical model, including electron clouds and orbital shapes. Get excited about the fascinating world of atomic structure with helpful examples and practice exercises.

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Bohr and Quantum Models: A Beginner's Guide

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  1. A Whirlwind Introduction to Bohr Model and Quantum Mechanical Model We’ve got a lot to do, so let’s get going!!

  2. Remember Niels Bohr? • What was Bohr’s main contribution? • Planetary model of the atom • Electrons orbit the nucleus. • Each orbit (also called shells) has a specific amount of energy. • Each orbit also has a maximum number of electrons it can hold. • Electrons must be in an orbit; they cannot be inbetween.

  3. How About Those Energy Levels? • Orbits labeled with whole numbers, n=1, n=2, n=3, etc. • Closer to the Nucleus = Less Energy.

  4. How Much Can an Orbit Hold? Must fill up the lower-energy shells before moving outward.

  5. How to Draw Bohr Models • Find number of electrons. • For a neutral (no charge) atom, atomic # = # protons = # electrons • Draw a nucleus (big dot) in the middle. • Draw circles for electron shells. • Place littledots on shells to represent electrons.

  6. What Would be the Bohr Model for Al? 13 13 • Atomic # = ? • # protons = ? • # electrons = ? • Maximum numbers to fill up shells • Maximum # electrons in 1st shell? • Do you have that many to put in there? • Do you have more than that and have to keep going? • Maximum # electrons in 2nd shell? • Do you have that many to put in there? • Do you have more than that and have to keep going? • Maximum # electrons in 3rd shell? • Do you have that many to put in there? • Can you leave the very outer one partly empty? • So how many total will you put in the 3rd level? • Then draw it! 13 2 yes yes 8 yes yes 18 no yes 3

  7. Isn’t It Pretty? Notice e- are in pairs except for n=1. Not necessary, but would be good to start practicing. Al

  8. You Do One! • You knew that was coming, didn’t you? • Do Chlorine, Cl!

  9. Check It! • Cl: atomic number = 17 = 17p+ = 17e- • 1st shell holds 2 (must keep going) • 2nd shell holds 8 (must keep going) • 3rd shell holds 18 (only have 7 to put there; it’s OK) Cl

  10. Now Homework…Yay! • More practice with Bohr models!! • Don’t get excited; we’re not done!

  11. I’ve Had Enough of Bohr… • Bohr’s model worked great for H, but not so great for the rest of the elements. • Quantum Mechanical Model was established and in use today! • https://www.youtube.com/watch?v=1StzvGFX4_c

  12. Quantum Mechanical Model • Like Bohr’s model, electrons exist in energylevels (and not in between). • Like Bohr, the levels are labeled as whole numbers, from the inside to the outside. • Like Bohr, the lower n, the lower energy. • Unlike Bohr, QMM has electron clouds (also called orbitals) instead of orbits which show where an electron is likely to be.

  13. Sounds Fascinating, Right?! • It is!! • The different electron clouds have different shapes, and there is a letter associated with each! • Get excited!!

  14. Spherical shape Can hold up to 2 e- Lowest energy s orbital

  15. Color in s-block Helium belongs with the s-block! 1s

  16. Dumb-bell shaped Can hold up to 6 e- More energy than s orbital p orbital

  17. Color in p-block Helium belongs with the s-block! 1s 1s

  18. Different shapes. Can hold up to 10 e- More energy than p orbital. d orbital **Draw these 2

  19. Color in d-block 1s 1s

  20. Oribitals • https://www.youtube.com/watch?v=K-jNgq16jEY

  21. Very odd shapes Can hold up to 14 e- Highest energy f orbital **Draw these 2

  22. Color in f-block: 1s 1s Make them the same color…

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