1. Notes (on your template)
Electron Orbitals
Notes (on your template)

2. Quantum theory _____________ describe exactly the path or orbit of an electron; it can, however, describe the general area of space where the electron is likely to be found.

3. Orbital: a region of space (3D) where there is a high (90%) probability of locating an electron.
Orbital ≠ Orbit

4. Capacity of an Orbital:
Each orbital can hold a total (maximum) of ______ electrons (1 pair).

5. Types (or Shapes) of Orbitals:
s Orbital
Shape: _________
Number: ____

6. Types (or Shapes) of Orbitals:
p Orbital
Shape: _________ p
Number: ____

7. Link to px, py, pz

8. Types (or Shapes) of Orbitals:
d Orbital
Shape: _________
Number: ____

10. Types (or Shapes) of Orbitals:
Number: ____

11. Orbital Link to Periodic Table

12. Size of an Orbital
In general: the greater the energy level, the greater the energy of the electron, the farther from the nucleus, and the larger the orbital size.

13. The 1s orbital is a
sphere, centered
around the nucleus
(l = 0)

14. once the
1s orbital
is filled,

15. once the
1s orbital
is filled,

16. the 2s orbital
begins to fill
around the
1s orbital

17. once the 2s
orbital is
filled,

18. the 2p orbitals
begin to fill

19. each 2p orbital
intersects the
2s orbital and
the 1s orbital

20. each 2p orbital
gets one electron
before pairing begins

21. once each 2p orbital
is filled with a pair
of electrons, then

22. the 3s orbital
gets the next
two electrons

23. the 3s electrons
have a higher energy
than 1s, 2s, or 2p
electrons,

24. so 3s electrons are
generally found
further from the
nucleus than 1s,
2s, or 2p electrons

25. Conclusion
Remember that the shape of an orbital does NOT represent a path of the electron!
The shape is a 3D region of space in which the electron is free to move.