Chemistry. Friday, October 13 th Monday, October 16 th, 2017

Transcription

1 Chemistry Friday, October 13 th Monday, October 16 th, 2017

2 Do-Now: Atomic Orbital WS 1. Write down today s FLT 2. What was wrong with Rutherford s atomic model? 3. Sketch a diagram of Bohr s model. Label it. 4. Summarize Bohr s model in 1-2 sentences. 5. Explain what happens when electrons move up or down an energy level. We will use this paper for our classwork after our notes, so keep it accessible Take out your planner and ToC

3 Planner: Study Ch. 11! Quiz this week Recommendation: Use flashcards and study notes and examples carefully Table of Contents #2: 14. Ch. 11 Notes B WS 15. Orbital WS (on separate paper)

4 FLT I will be able to describe the quantum atomic model by completing Ch. 11 Notes B Standard HS-PS1-1: Use the periodic table as a model to predict the rela7ve proper7es of elements based on the pa;erns of electrons in the outermost energy level of atoms.

5 Notes Protocol Add assignment # Copy down all bolded ideas Noise level 0 Raise hand to question/comment Be prepared to pair-share-respond

6 Ch. 11 B: Quantum Atomic Model

7 Atomic Models

8 Need for a New Model

9 Bohr Model Shortcomings of the Bohr Model: e - s can t orbit the nucleus Did not explain the proper<es of large atoms à only explained the behavior of hydrogen atoms

10 The Quantum Mechanical Model A new model needed to be developed to explain the forces and behavior of atoms

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12 Quantum Mechanical Model

13 Quantum Model

14 The Quantum Mechanical Model The quantum mechanical model is based on quantum theory Scien7sts, such as Schrödinger, noted that ma;er can behave like waves, and developed complex mathema7cal equa7ons that could describe the behavior of e - s

15 The Quantum Mechanical Model Quantum Theory: Uncertainty Principle = it s impossible to know both the exact posi<on & momentum of an e - at the same <me

16 The Quantum Mechanical Model Quantum Mechanical Model Determines the allowed energies an e - can have and how likely it is to find the e - in various loca7ons around the nucleus

17 The Quantum Mechanical Model In the quantum mechanical model, the probability of finding an electron within a certain volume of space surrounding the nucleus can be represented as a fuzzy cloud The cloud is more dense where the probability of finding the electron is high.

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19 The Quantum Mechanical Model Instead of orbits, the model uses orbitals Atomic Orbitals = regions of space in which there is a high probability of finding an e - Orbitals are some7mes called e - clouds

20 Atomic Orbital Shapes Each type can hold up to TWO electrons

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23 Quantum Model

24 Pair-Share-Respond 1. What was wrong with Bohr s atomic model? 2. State the uncertainty principle. 3. What does the quantum model use instead of orbits? 4. Define the term atomic orbital

25 Quantum Numbers

26 Quantum Numbers Four numbers, called quantum numbers, describe the characteris7cs of electrons and their orbitals

27 Quantum Numbers n = Principal Quantum Number l = Angular Momentum Quantum Number m l = Magne<c Quantum Number m s = Spin Quantum Number

28 Quantum Numbers n = Principal Quantum Number This is the size of the orbital and the specific energy level n = 1, 2, 3, Ex/ n=2 means electrons in the 2 nd energy level/shell n=3 means? n=5 means?

29 Quantum Numbers n = Principal Quantum Number The total number of e - s that an energy level can hold is 2n 2 Ex/ n=2 is the 2 nd energy level. It can hold 2(2) 2 electrons à 8 electrons total How many electrons can be on the 3 rd energy level?

30 Quantum Numbers l = Angular Momentum Quantum Number This specifies the shape of the orbital: s, p, d, or f l = 0,, n-1 Ex/ if n=1, then l = 0 à s orbitals Ex/ If n = 3? l = 0 l = 1 l = 2 l = 3 s p d f

31 Quantum Numbers l = Angular Momentum Quantum Number If n = 2, l can be 0 or 1 (up to n-1) If n = 3, l can be 0, 1, or 2 If n = 4? l = 0 l = 1 l = 2 l = 3 s p d f

32 Quantum Numbers

33 Quantum Numbers Ex/ If n = 3 and l = 0, then it is the 3s subshell This means the s orbital on the 3 rd energy level Ex/ If n = 2 and l = 1, then It is the 2p subshell Ex/ If n = 4 and l = 2, then It is the 4d subshell

34 Quantum Numbers m l = Magne7c Quantum Number Describes the orienta<on of the orbitals May be l, 0, +l Ex/ n = 2 and l = 1 à so m l = -1, 0, +1 (3 orbitals) What if n = 3 and l = 2?

35 Quantum Numbers m l = Magne7c Quantum Number Just remember: s subshell has one orbitals p subshell has three orbitals d subshell has five orbitals f subshell has seven orbitals

36 Quantum Numbers m s = Spin Quantum Number This describes the direc<on of the electron either clockwise or counterclockwise Only two values: +1/2 or -1/2 Therefore, there are only two e - s in each subshell with opposite spins

37 Note: The fewer the quantum numbers, the less we know about the electrons. Ex/ If n = 3, I could be talking about 2n 2 or 18 electrons on the 3 rd energy level The MORE quantum numbers we have, the more we know about the electrons. Ex/ If n = 3 and l = 2, I could be talking about any electrons in the d orbitals. Since there are 5 d orbitals, this means I could be talking about 10 electrons. Ex/ If n = 3, l = 2, and m l = 0, then I am talking about one specific d orbital, and therefore 2 electrons. Ex/ If n = 3, l = 2, m l = 0, and m s = + ½, then I am only talking about one electron.

38 Atomic Orbitals Different atomic orbitals are denoted by le;ers. The s orbitals are spherical, and p orbitals are dumbbell-shaped.

39 Atomic Orbitals Four of the five d orbitals have the same shape but different orienta7ons in space.

40 Atomic Orbitals The numbers and kinds of atomic orbitals depend on the energy sublevel.

41 Pair-Share-Respond 1. List the names and symbols of the four quantum numbers 2. What are the possible m s values? 3. Explain the meaning of n =3 and l = 2 4. If n = 3 and l = 2, How many total orbitals will there be? 5. If n=3, How many total electrons can there be?

42 CW Complete the Orbital WS questions on your do-now paper Finished? Read Ch. 11 Complete ToC work I HIGHLY recommend making flashcards for this chapter feel free to spend class time making some!

43 Chemistry Tuesday, October 17 th Wednesday, October 18 th, 2017

44 Do-Now: Quantum Number WS 1. Take out your Ch. 11 B Notes (WS) 2. Make sure you picked up the worksheet from the front 3. Complete at least the first side of the worksheet independently or with one partner (if working quietly). Take out your planner and ToC

45 Planner: Finish all CW Get stamps through #17 Study for quiz! Table of Contents #2: 16. Quantum Number WS 17. Ch. 11 CN Part C 18. Electron Config/Notation Packet

46 FLT I will be able to express the arrangements of e - s in atoms using orbital notation and electron configurations by completing Ch. 11 Notes C Standard HS-PS1-1: Use the periodic table as a model to predict the rela7ve proper7es of elements based on the pa;erns of electrons in the outermost energy level of atoms.

47 Notes Protocol Add assignment # Copy down all bolded ideas Noise level 0 Raise hand to question/comment Be prepared to pair-share-respond

48 Ch. 11: Electron Arrangement in Atoms

49 Recall

50 Quantum Model

51 Quantum Numbers

52 Orbitals

53 Electron Configurations

54 Arrangement of Electrons in Atoms Levels (n) Sublevels (l ) Orbitals (m l )

55 Energy Levels n = 1 n = 2 n = 3 n = 4

56 Arrangement of Electrons in Atoms Electron configura<on = arrangement of e - s in atoms

57 Arrangement of Electrons in Atoms e - s assume an arrangement that gives the atom the lowest energy possible (more stable)

58 Arrangement of Electrons in Atoms What does this look like?

59 Electron Configurations 2p 4 Energy Level Number of electrons in the sublevel 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.

60 Arrangement of Electrons in Atoms What does this look like?

61 Three Principles

62 AuXau Principle = e - s occupy the lowest E orbital available. Use the diagonal rule Three Principles

63 1 s Diagonal Rule 2 s 2p s 3p 3d s 4p 4d 4f s 5p 5d 5f 5g? s 6p 6d 6f 6g? 6h? 7 s 7p 7d 7f 7g? 7h? 7i?

64 Three Principles Pauli Exclusion Principle = No more than two e - s can occupy a single orbital We note this using arrows in opposite direc7ons

65 Three Principles Hund s Rule = Fill in single e - s in separate equal-e orbitals before doubling up

66 In Summary: Our Rules

67 Rules 1) Determine the # of e - s by looking up Z (atomic number) Assume the atom is neutral unless stated otherwise. Draw orbitals first to help you. Ex/ Nitrogen

68 Rules 2) Start filling orbitals in order of increasing E according to the AuXau Principle. A single orbital can hold a max of 2 e - s Orbital Type Number of Orbitals s 1 p 3 d 5 f 7

69 Rules 3) Hund s Rule Applies: Draw all orbitals for each type, and fill in ONE e - in each orbital before doubling up.

70 Rules 4) Pauli Exclusion applies: Two e - s in the same orbital must have opposite spins

71 5) Write e - config Rules Make sure total # of e - s in your configura7on matches the atomic number (if your atom is neutral)

72 Orbitals and the Periodic Table Orbitals grouped in s, p, d, and f orbitals s orbitals d orbitals p orbitals f orbitals

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74 Examples

75 Write the orbital notation and e - Fluorine configuration for

76 Write the orbital notation and e - configuration for Magnesium

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78 Write the orbital notation and e - Titanium configuration for

79 Write the orbital notation and e - Arsenic configuration for

80 Orbitals and the Periodic Table Orbitals grouped in s, p, d, and f orbitals s orbitals d orbitals p orbitals f orbitals

81 Shorthand Notation

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83 Shorthand Notation We can abbreviate our long e- configura7ons by using our noble gases This is because our Noble Gases have complete full p orbitals Note: only use shorthand when asked to

84 Shorthand Notation 1. Find the closest noble gas to your atom with a smaller Z and put in [ ] 2. Fill orbitals from where the Noble Gas leg off Ex/Na

85 Try: Ca Shorthand Notation

86 CW 1. Complete the electron configuration/ orbital notation worksheet 2. Check your answers with your pair-share partner(s)

87 Chemistry Thursday, October 19 th Friday, October 20 th, 2017

88 Do-Now: Ch. 11 Quiz Day Do-Now 1. Write down today s FLT 2. What are our four types of orbitals? 3. How many orientations does each type of orbital have? 4. How many electrons can one orbital hold? 5. How many TOTAL electrons can the 5 th energy level hold (n = 5) Take out your planner and ToC

89 Announcements Use dojo points by next Fri! Lab next week This lab will also have a wri;en report MUST have closed-toed shoes and 7ed-back hair No dangling clothes/jewelry Contact lenses not recommended

90 Planner: Get stamps through #20 Lab next class! Close-toed shoes and hair ties are a must Table of Contents #2: 19. Ch. 11 Quiz Day Do-Now 20. Ch. 11 Quiz Review Packet

91 FLT I will be able to demonstrate my understanding of modern atomic models and electron configurations by completing Ch. 11 Quiz Standard HS-PS1-1: Use the periodic table as a model to predict the rela7ve proper7es of elements based on the pa;erns of electrons in the outermost energy level of atoms.

92 1. Review packet Complete together CW Make sure you can EXPLAIN your answers resist the urge to skip over problems you don t understand Ask questions 2. Study for quiz by reviewing your notes and worksheets We will take a KAHOOT before the quiz

93 Quiz/Test Protocol You may use your reference sheet Noise level 0 Eyes on own paper Mark answers clearly Do your best J Flip over when done