Wave Mechanical Model and Orbitals

1. Wave Mechanical Model and Orbitals SCH12U February 7 2012 Mr. Dvorsky

2. Schrodinger -treated electron as a wave and developed a mathematical equation to describe its wave-like behaviour. -this equation can be used to describe the location in space (x,y,z) where an electron can be found. -these regions are called orbitals

3. Heisenberg -impossible to determine the exact location of a single subatomic particle (Heisenberg’s uncertainty principle). -therefore Schrodinger’s orbitals are actually probability distributions of where an electron MAY be found.

4. Orbitals • When a planet moves around the Sun, you can plot a definite path for which it is called an orbit. • Similarly, a simple view of the atom has electrons orbiting around the nucleus. • In fact, electrons inhabit regions of space known as orbitals

5. To plot a path for something you must know where it is and where it will be an instant later. This cannot be done for electrons • Instead we use probability distributions

6. Hydrogen’s electron, the 1s orbital. Suppose you had a single hydrogen atom and at a particular instant plotted the position of the one electron. Soon afterwards, you do the same thing, and find that it is in a new position. You have no idea how it got from the first place to the second.You keep on doing this over and over again, and gradually build up a sort of 3D map of the places that the electron is likely to be found.

7. For the electron of hydrogen, it can be found anywhere in a spherical region around the nucleus. Most of the time it will be found within that region. –this region is called an orbital, it is where electrons live. –cannot say what the electron is doing in that space, just that it will have a particular energy level.

8. Each orbital has a name. • The orbital occupied by the hydrogen electron is called 1s.

10. Not all electrons inhabit s orbitals. In fact, most don’t. • At the second energy level, not only is there a 2s orbital, but also 3 2p orbitals • p orbitals resemble two balloons held together at the nucleus Why 3? At any level it is possible to have 3 identical p orbitals, just that they are pointing in different directions.

11. -there are also d and f orbitals which become available for electrons to inhabit at higher energy levels -at the third level there are 5 d orbitals, as well as the 3s orbital, and the three 3p orbitals (for a total of 9 orbitals at that level) -at the fourth level there is the 4s, plus the three 4p orbitals, plus the five 4d orbitals, and seven 4f orbitals

12. The inverted pyramid analogy • You can think of an atom as a strangely arranged house with the nucleus living o on the ground floor. There are various rooms (orbitals) on the higher floors (energy levels) occupied by the electrons. -On the first floor there is only 1 room (1s), on the second floor there are 4 rooms (2s, 2px, 2py, 2pz), on the third floor there are 9 rooms (1s, 3 3p orbitals, 5 3d orbitals). The rooms aren’t big, each can hold only two electrons.

14. The order of filling orbitals • Electrons fill low energy orbitals (closer to the nucleus) before they fill higher energy ones (Aufbau principle) • Due to electron repulsion, all orbitals of equal energy acquire one electron before any orbital accepts two electrons (Hund’s rule)

15. Diagram summarizing up to the 4p level -notice that s orbitals have lower energy than p at the same level so s orbital fills with electrons before the corresponding p orbitals Notice 3d orbitals. They are slightly higher level than the 4s and so it is the 4s which fill first followed by 3d and then 4p. -overlap causes some confusion!

16. Orbital filling and the periodic table The first period:

17. The second period:

18. The second period (continued): Make life easier. Use shortcuts! 1. You can just lump together all the various p orbitals

21. Once we get to level 4, we must recall this: -4s is at a lower energy than 3d and will therefore fill before the orbitals of 3d