2. 1 Bellringer (Friday 11/7/08) Write the question and answer. 1. Compare and Contrast the size and energy of 1S, 2S and 3S. 2. How many energy levels are there on the periodic table?

3. 2 Relative sizes of the spherical 1s, 2s, and 3s orbitals of hydrogen.

4. 3 Energy Levels n = 1 n = 2 n = 3 n = 5 n = 4 n = 6 n = 7

5. 4 Arrangement of Electrons in Atoms Electrons in atoms are arranged as LEVELS (n) SUBLEVELS (l) ORBITALS (m l )

6. 5 QUANTUM NUMBERS The shape, size, and energy of each orbital is a function of 3 quantum numbers which describe the location of an electron within an atom or ion n (principal) ---> energy level l (orbital) ---> shape of orbital m l (magnetic) ---> designates a particular suborbital The fourth quantum number is not derived from the wave function s (spin) ---> spin of the electron (clockwise or counterclockwise: ½ or – ½)

7. 6 Energy Levels Each energy level has a number called the PRINCIPAL QUANTUM NUMBER, nEach energy level has a number called the PRINCIPAL QUANTUM NUMBER, n Currently n can be 1 thru 7, because there are 7 periods on the periodic tableCurrently n can be 1 thru 7, because there are 7 periods on the periodic table

8. 7 Types of Orbitals The most probable area to find these electrons takes on a shapeThe most probable area to find these electrons takes on a shape So far, we have 4 shapes. They are named s, p, d, and f.So far, we have 4 shapes. They are named s, p, d, and f. No more than 2 e- assigned to an orbital – one spins clockwise, one spins counterclockwiseNo more than 2 e- assigned to an orbital – one spins clockwise, one spins counterclockwise

9. 8 Types of Orbitals ( l ) s orbital p orbital d orbital

10. 9 p Orbitals Sublevel p has 3 orbitals with 6 electrons.

11. 10 The shapes and labels of the five 3d orbitals. Sublevel d has 5 orbitals with 10 electrons

12. 11 f Orbitals For l = 3, ---> f sublevel with 7 orbitals and 14 electrons

13. 12 s orbitals d orbitals Number of orbitals Number of electrons p orbitals f orbitals How many electrons can be in a sublevel? Remember: A maximum of two electrons can be placed in an orbital. 1357 2 61014

14. 13 Sublevels =blocks (Types of orbitals) Quantum Number Principal Energy Level Layout p. 155 # of orbitals related to sublevel 1 2 3 4 s s 1 p s p d 1 3 1 3 5 s p d f 1 3 5 7

15. 14 Orbitals and the Periodic Table Orbitals grouped in s, p, d, and f orbitals (sharp, proximal, diffuse, and fundamental)Orbitals grouped in s, p, d, and f orbitals (sharp, proximal, diffuse, and fundamental) s orbitals p orbitals d orbitals f orbitals

16. 15 Electron Configurations Be able to explain this on a test. 2p 4 Energy Level Sublevel Number of electrons in the sublevel 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6s 2 4f 14 … etc.

17. 16 Underwater Hotel Try it out! If you are a visual learner – try this method

18. 17 Diagonal Rules s 3p 3d s 2p s 4p 4d 4f s 5p 5d 5f 5g? s 6p 6d 6f 6g? 6h? s 7p 7d 7f 7g? 7h? 7i? 1234567 Steps: 1.Write the energy levels top to bottom. 2.Write the orbitals in s, p, d, f order. Write the same number of orbitals as the energy level. 3.Draw diagonal lines from the top right to the bottom left. 4.To get the correct order, follow the arrows! By this point, we are past the current periodic table so we can stop.

19. 18 Why are d and f orbitals always in lower energy levels? d and f orbitals require LARGE amounts of energy It’s better (lower in energy) to skip a sublevel that requires a large amount of energy (d and f orbtials) for one in a higher level but lower energy This is the reason for the diagonal rule! BE SURE TO FOLLOW THE ARROWS IN ORDER!

20. 19 Let’s Try It! Write the electron configuration for the following elements: Br Sr Sb Re

21. 20 Shorthand Notation A way of abbreviating long electron configurations Since we are only concerned about the outermost electrons, we can skip to places we know are completely full (noble gases), and then finish the configuration

22. 21 Shorthand Notation Step 1: It’s the Showcase Showdown! Find the closest noble gas to the atom (or ion), WITHOUT GOING OVER the number of electrons in the atom (or ion). Write the noble gas in brackets [ ]. Step 2: Find where to resume by finding the next energy level. Step 3: Resume the configuration until it’s finished.

23. 22 Shorthand Notation Chlorine –Longhand is 1s 2 2s 2 2p 6 3s 2 3p 5 You can abbreviate the first 10 electrons with a noble gas, Neon. [Ne] replaces 1s 2 2s 2 2p 6 The next energy level after Neon is 3 So you start at level 3 on the diagonal rule (all levels start with s) and finish the configuration by adding 7 more electrons to bring the total to 17 [Ne] 3s 2 3p 5

24. 23 Bellringer Practice Shorthand Notation Write the shorthand notation for each of the following atoms: 1. Cl 2. K 3.Ca Take out electron practice and periodic table handouts.

25. 24 Orbital Diagrams Graphical representation of an electron configuration One arrow represents one electron Shows spin and which orbital within a sublevel Same rules as before (Aufbau principle, two electrons in each orbital, etc.)

26. 25 Valence Electrons Electrons are divided between core and valence electrons B 1s 2 2s 2 2p 1 Core = [He], valence = 2s 2 2p 1 Br [Ar] 3d 10 4s 2 4p 5 Core = [Ar] 3d 10, valence = 4s 2 4p 5

27. 26 Rules of the Game No. of valence electrons of a main group atom = Group number (for A groups) Atoms like to either empty or fill their outermost level. Since the outer level contains two s electrons and six p electrons (d & f are always in lower levels), the optimum number of electrons is eight. This is called the octet rule.