1. Building Atoms Chapter 8 §1-4

2. Erwin Schrödinger Developed an equation – the wave equation – to calculate the waves created by the electron in the hydrogen atom. Developed an equation – the wave equation – to calculate the waves created by the electron in the hydrogen atom. The solutions of this equation are called wave functions, ψ. The solutions of this equation are called wave functions, ψ.

3. Erwin Schrödinger Key ideas from the Schrodinger wave equation: Key ideas from the Schrodinger wave equation: Electrons must behave as standing waves, meaning only certain wave functions are allowed. This defines the energy of the electrons as being quantized. Electrons must behave as standing waves, meaning only certain wave functions are allowed. This defines the energy of the electrons as being quantized.

4. Erwin Schrödinger Key ideas from the Schrodinger wave equation: Key ideas from the Schrodinger wave equation: The square of the wave function, ψ 2, determines the probability of the location of the electrons – the electron density. These electron densities create regions of space which are called orbitals. The square of the wave function, ψ 2, determines the probability of the location of the electrons – the electron density. These electron densities create regions of space which are called orbitals.

5. Erwin Schrödinger Key ideas from the Schrodinger wave equation: Key ideas from the Schrodinger wave equation: The solutions of the equation create the Quantum Numbers… The solutions of the equation create the Quantum Numbers… for later…

6. The Orbitals Schrodinger’s wave equation creates the modern atom, which includes energy levels, subshells, and orbitals to carry the electrons. Schrodinger’s wave equation creates the modern atom, which includes energy levels, subshells, and orbitals to carry the electrons.

7. The Orbitals Energy levels Energy levels a representation of the distance away from the nucleus of an atom The first energy level is 1. The first energy level is 1. In theory, energy levels go through infinity. In theory, energy levels go through infinity.

8. The Orbitals Subshells Subshells The energy levels are divided into subshells. The energy levels are divided into subshells. Orbital shapes Orbital shapes There are four main orbital shapes. There are four main orbital shapes.

9. The Orbitals Subshells Subshells In theory, the subshells continue after the f orbital – g, h, i, j, etc.

10. The Orbitals Orbitals Orbitals The subshells are divided into orbitals. The subshells are divided into orbitals. Orientations Orientations Each subshell has a particular set of orientations. Each subshell has a particular set of orientations.

11. The Orbitals s Orbitals s Orbitals Since the s shape is a sphere, there is only one way to position it on a x-y-z axis. Since the s shape is a sphere, there is only one way to position it on a x-y-z axis.

12. The Orbitals p Orbitals p Orbitals There are 3 orientations for the p subshell. There are 3 orientations for the p subshell.

13. The Orbitals d Orbitals d Orbitals There are 5 orientations for the p subshell. There are 5 orientations for the p subshell.

14. The Orbitals f Orbitals f Orbitals There are 7 orientations for the p subshell. There are 7 orientations for the p subshell.

15. The Orbitals Putting it all together… Putting it all together… Energy Level Subshell Orientations 1s1 2spsp 1313 3spdspd 135135

16. The Filling Order Putting it all together Putting it all together 1s 2s2p 3s3p3d 4s4p4d4f 5s5p5d5f5g 6s6p6d6f6g6h 7s7p7d7f7g7h7i etc

17. Filling Order Rules Fill in order of energy – lowest E should be filled first

18. Filling Order Rules no 2 e – can have the same 4 quantum numbers, meaning that no orbital can contain more than 2 e – Pauli Exclusion Principle

19. Filling Order Rules 1 electron per spin in an orbital – any electrons that share an orbital must have opposite spins

20. Filling Order Rules when e – occupy orbitals of equal energy (the same subshell), each orbital must obtain one e – in parallel spins before any orbital can obtain a second e – spread out the e – Hund’s Rule of Maximum Multiplicity

21. Let’s Practice Write the electron configuration of N. Start by finding the number of electrons in N. Look at the filling order: 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p Place electrons into the subshells according to how many electrons can be held in each subshell. 223

22. Let’s Practice Write the electron configuration of Ga. Start by finding the number of electrons in Ga. Look at the filling order: 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p Place electrons into the subshells according to how many electrons can be held in each subshell. 226262 101

23. Fill with the Periodic Table The filling order is on the periodic table, too.

24. Let’s Practice Write the electron configuration for Ge. Start by finding Ge on the periodic table.Now follow the periodic table as you fill in e -. 1s 1 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 4p 2 3d 10

25. Let’s Practice Write the Noble gas configuration for Ge. Substitute a noble gas for a section of electrons. Ar 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 4p 2 3d 10