Chemistry. Monday, October 9 th Tuesday, October 10 th, 2017

Transcription

1 Chemistry Monday, October 9 th Tuesday, October 10 th, 2017

2 Do-Now: Unit 1 Test Day Do-Now 1. Write down today s FLT Copy & Complete 2. Write down one question you have about the test (topic-wise or format-wise). 3. The change from a solid to a is called. 4. When doing calculations, I need to always include. 5. Dalton thought that atoms of the same element were identical. Correct Dalton by completing the sentence frame: While I agree that atoms of the same element, I disagree that because atoms of the same element can. Take out your planner and ToC

3 Planner: Get stamps through #10 Read Ch. 11 Table of Contents #2: 9. Unit 1 Test Day Do-Now 10. Basic Atomic Structure WS

4 FLT I will be able to demonstrate my mastery of atomic chemistry by completing the Unit 1 Test Standard HS-PS1-8: Develop models to illustrate the changes in the composi;on of the nucleus of the atom and the energy released during the processes of fission, fusion, and radioac;ve decay

5 CW Complete the Basic Atomic Structure WS à you will need to know the atomic theory from Ch. 3 to follow along with Ch. 11 (Modern Atomic Theory) You may also read Ch. 11 quietly

6 Chemistry Wednesday, October 11 th Thursday, October 12 th, 2017

7 Do-Now: Ch. 11 Demo 1. Write down today s FLT 2. Distinguish between subatomic particles and nucleons 3. What do protons and neutrons have in common? 4. What do electrons and protons have in common? 5. Use a pro-talk sentence frame to explain something about subatomic particles. 6. We will do our demo notes under this do-now Take out your planner and ToC

8 Demo I have a plasma ball and two types of lights/bulbs. Underneath your do-now Use your pro-talk sentence frame In my opinion because to make a predic?on about what you THINK will happen.

9 Demo Now, write down three ques?ons you have about the demo.

10 Demo Discuss your ques?ons with your group. Decide as a group which ques?on is the best or the most interes?ng, and everyone should write it on their paper. What do you think we saw?

11 Demo Now, we will watch a video. During the video, write down one or two pieces of evidence that can help you explain what s happening.

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13 Demo Use the informa?on from the video and the demo to answer your ques?on. Use one of the following pro-talk sentence frames: First I considered, then... Proves my claim because If we look at both. and. We can see that. Based on the evidence, we can conclude that.

14 Planner: Guided Reading WS Last day for Ch. 19 Quiz retakes is tomorrow Schedule Unit 1 Retakes à complete by the end of next week. Fleming ASAP. Table of Contents #2: 11. Ch. 11 Inquiry Demo CN Part A 13. Ch. 11 Guided Reading WS

15 FLT I will be able to describe modern atomic theory by completing Ch. 11 Notes A Standard HS-PS1-8: Develop models to illustrate the changes in the composi;on of the nucleus of the atom and the energy released during the processes of fission, fusion, and radioac;ve decay

16 Notes Protocol Title your notes & add assignment # Complete Cornell-style Copy down all bolded ideas Noise level 0 Raise hand to question/comment Be prepared to pair-share-respond

17 Ch. 11 A: Bohr s Atomic Model

18 Draw 5 circles on your notes

19 Recall Atomic models so far: Dalton Thomson Rutherford

20 Atomic Models:

21 Atomic Models:

22 Atomic Models:

23 Rutherford s Atomic Model What was inadequate about Rutherford s atomic model?

24 Rutherford s Atomic Model It could not explain the behavior of e - s or the chemical proper?es of elements The behavior of electrons is important to understanding the physical proper;es of elements, such as why objects change color when heated.

25 Bohr Atomic Model

26 Electron Cloud/Quantum Model

27 The Bohr Model What was the new proposal in the Bohr model of the atom?

28 The Bohr Model Bohr tried to explain the behavior of electrons Why didn t electrons crash into the nucleus?

29 The Bohr Model An e - is found only in specific circular paths (energy levels) around the nucleus.

30 The Bohr Model Energy Levels = e - s have fixed energies for each orbit

31 The Bohr Model Quantum of energy = The amount of energy required to move an e - from one E level to another

32 The Bohr Model e - s absorb energy when they move to a higher E level

33 The Bohr Model e - s emit E when they move to a lower E level

34 Bohr Model

35 The Bohr Model Like the rungs of the strange ladder, the energy levels in an atom are not equally spaced. Higher energy levels require less energy for an e - to move up

36 Pair-Share-Respond 1. What are the four models of the atom that we have learned about so far? 2. What was an issue with Rutherford s model? 3. Describe Bohr s model of the atom 4. When do electrons absorb energy, and when do they emit energy? 5. How are higher energy levels different than lower energy levels?

37 CW 1. Guided Reading WS (finish for HW) 2. Finished? Work on your stamps or begin reading Don t forget Finish your Ch. 19 Quiz Retakes Schedule your Unit Test retake through Make sure you have cleared your missing work before you schedule

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

39 Do-Now: Ch. 11 Demo 1. Write down today s FLT 2. List our three subatomic particles 3. What do protons and neutrons have in common? 4. What do electrons and protons have in common? 5. Use a pro-talk sentence frame to explain something about subatomic particles. Take out your planner and ToC

40 Demo I have a plasma ball and two types of lights/bulbs. Underneath your do-now Use your pro-talk sentence frame In my opinion because to make a predic?on about what you THINK will happen.

41 Demo Now, write down three ques?ons you have about the demo.

42 Demo Discuss your ques?ons with your group. Decide as a group which ques?on is the best or the most interes?ng, and everyone should write it on their paper. What do you think we saw?

43 Demo Now, we will watch a video. During the video, write down one or two pieces of evidence that can help you explain what s happening.

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45 Demo Use the informa?on from the video and the demo to answer your ques?on. Use one of the following pro-talk sentence frames: First I considered, then... Proves my claim because If we look at both. and. We can see that. Based on the evidence, we can conclude that.

46 Announcements Unit 1 Test Retakes 1 week lew! Clear missing work & schedule with Ms. Fleming ASAP No study guides on retake

47 Planner: Study Ch. 11! Quiz next week J 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)

48 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 rela;ve proper;es of elements based on the pa\erns of electrons in the outermost energy level of atoms.

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

50 Ch. 11 B: Quantum Atomic Model

51 Atomic Models

52 Need for a New Model

53 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

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

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56 Quantum Mechanical Model

57 Quantum Model

58 The Quantum Mechanical Model The quantum mechanical model is based on quantum theory Scien;sts, such as Schrödinger, noted that ma\er can behave like waves, and developed complex mathema;cal equa;ons that could describe the behavior of e - s

59 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

60 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 loca;ons around the nucleus

61 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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63 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 some;mes called e - clouds

64 Atomic Orbital Shapes

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67 Quantum Model

68 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

69 Quantum Numbers

70 Quantum Numbers Four numbers, called quantum numbers, describe the characteris;cs of electrons and their orbitals

71 Quantum Numbers n = Principal Quantum Number l = Angular Momentum Quantum Number m l = Magne?c Quantum Number m s = Spin Quantum Number

72 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?

73 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?

74 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

75 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

76 Quantum Numbers

77 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

78 Quantum Numbers m l = Magne;c 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?

79 Quantum Numbers m l = Magne;c Quantum Number Just remember: s subshell has one orbitals p subshell has three orbitals d subshell has five orbitals f subshell has seven orbitals

80 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

81 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.

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

83 Atomic Orbitals Four of the five d orbitals have the same shape but different orienta;ons in space.

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

85 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?

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