Quiz: Nov When you see a color in the flame test, what is happening? 2.Describe the behavior of an electron according to the Bohr/Rutherford model? 3.Which is more energetic, Yellow or Green light? 4.List the colors of the rainbow in order. 5.If n = 1, what energy level is the electron in? 6.Write the electron configuration for lithium Due Dates: Notebook: M 8 th Period T 5 th period W 11 th period R 10 th period F 4 th period Essay: TODAY

Answers 1.When you see a color in the flame test, what is happening? 2.Describe the behavior of an electron according to the Bohr/Rutherford model? 3.Which is more energetic, Yellow or Green light? 4.List the colors of the rainbow in order. 5.If n = 1, what energy level is the electron in? 6.Write the electron configuration for lithium (3 electrons) 1.The electron is dropping to a lower energy level. 2.The electrons revolve around the nucleus. 3.Green light is more energetic. 4.ROY G BIV Red, Orange, Yellow Green, Blue, Indigo, Violet. 5.n= 1, energy level = 1 6.1s 2 2s 1

Electron Configuration The electron configuration is used to quickly summarize the quantum numbers of electrons in the atom.. Li = 1 s 2 2 s 1 n =1 n=2 n=3 n=4 n=5 What are these? Principal Quantum Number = Energy Level What are the s’s for? This quantum number is the shape of the electron cloud. What are the superscript 2 and 1? Number of Electrons in this orbital

Electron Configurations 7s7p 6s6p6d6f 5s5p5d5f 4s4p4d4f 3s3p3d 2s2p 1s Start here #1 #8 1s 1 2 electron s 6 electron s 10 electron s 14 electrons HydrogenHelium = 1s 2

Electron Configurations 7s7p 6s6p6d6f 5s5p5d5f 4s4p4d4f 3s3p3d 2s2p 1s Start here #1 # 2 #8 1s 2 2 electron s 6 electron s 10 electrons 14 electrons 2s 1 Lithium Beryllium = 2

Electron Configurations 7s7p 6s6p6d6f 5s5p5d5f 4s4p4d4f 3s3p3d 2s2p 1s Start here #1 # 2 # 3 #8 1s 2 2 electron s 6 electrons 10 electron s 14 electrons 2s 2 2p Boron (5) = Carbon (6) = 2 Nitrogen (7)= 3

Electron Configurations 7s7p 6s6p6d6f 5s5p5d5f 4s4p4d4f 3s3p3d 2s2p 1s Start here #1 # 2 # 3 #8 1s 2 2 electron s 6 electrons 10 electron s 14 electrons 2s 2 2p Boron (5) = Oxygen (8) = 4 Fluorine (9) = 5

Electron Configurations 7s7p 6s6p6d6f 5s5p5d5f 4s4p4d4f 3s3p3d 2s2p 1s Start here #1 # 2 # 3 #8 1s 2 2 electron s 6 electron s 10 electrons 14 electrons 2s 2 2p 6 Neon (10) = 2 e- 6 e = 10 electrons TOTAL 1s 2 2 s 2 2 p 2

Write the electron configurations for Na (11), Mg (12), Al (13) 1s 2 2s 2 2p 6 3s 1 = Na 1s 2 2s 2 2p 6 3s 2 = Mg 1s 2 2s 2 2p 6 3s 2 3p 1 = Al

Electron Configurations 7s7p 6s6p6d6f 5s5p5d5f 4s4p4d4f 3s3p3d 2s2p 1s Start here #1 # 2 # 3 #4 #8 1s 2 2 electron s 6 electron s 10 electrons 14 electrons 2s 2 2p 6 3s 2 3p 3 Phosphorous

Electron Configurations 7s7p6s6p6d6f 5s5p5d5f 4s4p4d4f 3s3p3d 2s2p 1s Start here #1 # 2 # 3 #4 #5 #6 #7 #8 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 5d 10 6p 6 ….. 2 electron s 6 electron s 10 electrons 14 electrons

Write the electron Configuration for silver (47) and gold (79). 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 9 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 5s 2 4d 10 5p 6 6 s 2 4f 14 5d 9 Write the electron Configuration for iron and zinc. Fe ends in 3d 6, Zn ends in 3d 10

orbital Hund’s Rule One in each before two in any. 1s 2s 2p H = 1 He = 2 Li = 3 Be = 4 B = 5 C = 6 N = 7 O = 8 F = 9 Ne = 10 electron electron s orbitals

Homework 16: 6  13 p 118… Honors: 32  34 p e- =? n = 2 n = 2 n = 3 n = 3 n = 5 n = 5 n = 7 n = 7 7. sublevels =? n = 1 n = 1 n = 3 n = 3 n = 4 n = e- = 2(2) 2 = 8 e- e- = 2(3) 2 = 18 e- e- = 2(5) 2 = 50 e- e- = 2(7) 2 = 98 e- 7. n = 1, 1 sublevel n = 3, 3 sublevels n = 4, 4 sublevels

Homework 16: 6  13 p 118… Honors: 32  34 p orbitals/sublevel? s p d f 9. Define orbitals, list how many orbitals are in an f sublevel? 10. State Pauli’s exclusion principle. 8. s = 1 s orbital per sublevel p = 3 p orbitals per sublevel d = 5 d orbitals per sublevel f = 7 f orbitals per sublevel. 9. The space occupied by one pair of electrons is called an orbital. There are 7 f orbitals in a sublevel. 10.No two electrons in an atom can have the same set of 4 quantum numbers.

Homework 16: 6  13 p 118… Honors: 32  34 p List and explain each of the four quantum numbers. 12. If two orbitals are degenerate, what do they have in common? 13. How many sublevels will be found in level x? 11. n = the principal quantum number. It is equal to the energy level and describes the relative electron cloud size. l = shape quantum number, it describes the shape: s, p, d or f. m = the orientation in space of the electron cloud: x,y, z,… s = spin quantum number: + ½ or – ½ (clockwise or counter-clockwise) 12. Degenerate orbitals have the same amount of energy. 13. There will be x sublevels.

Homework 16: 6  13 p 118… Honors: 32  34 p Complete the chart. 33. What is an orbital, how many orbitals are possible at each sublevel. 34. Explain the factors that determine the size of an electron charge cloud. s,p,d,f44 s,p,d33 s, p 22 s11 Letter(s) # sublevels Level1 An orbital is the space that can be occupied by a maximum of two electrons; s = 1, p = 3, d = 5, f = 7 e- = 2(2)2 = 8 e- The size of the electron cloud is determined by the principal quantum number, n, repulsion of other electrons and attraction to the nucleus.

In the Bohr-Rutherford Atom The electrons revolve around the nucleus like planets around the sun. Each electron has discrete quanta of energy. The amount of energy in one photon of energy equals one quantum E = h Where h = Plank’s constant = 6.6x Joules/Hz (1Hz = 1 cycle per second) Energy is given off in quanta, not continuously. The electrons surrounding the nucleus have defined orbits. This relates to Lab 10