Chemistry Monday, October 24, 2016

Transcription

1 Chemistry Monday, October 24, 2016 Do-Now: Quantum Number WS 1. Take out your 5.1 B Notes from Thurs/Fri (it was a WS, not Cornell) 2. Make sure you picked up the worksheet from the front 3. Complete the worksheet independently or with one partner (if working quietly) Take out your planner and ToC Announcements Complete retakes Clear missing work Current Unit: Ch. 5, 6, 8 Quiz/Lab this week J Planner: Finish WS + Read 5.2 Quiz/Lab Thurs/Fri Stamps by the end of the week Table of Contents #2: 21. Quantum Number WS CW Finish WS + Study Chemistry Tuesday, October 25 Wednesday, October 26,

2 Do-Now: 5.2 Cornell Notes 1. Write down today s do-now 2. What are our four types of orbitals? 3. How many orientations does each type of orbital have? 4. How many electrons can each orbital hold? 5. How many TOTAL electrons can the 3 rd energy level hold (n = 3) 6. Explain what 3d means. 7. How many electrons can there be in 3d? Take out your planner and ToC Announcements Must clear missing work AHend tutoring Current Unit: Ch. 5, 6, 8 Study for your quiz Have your periodic table handy for today s lesson Planner: Quiz à Monday ToC à Wednesday Lab next class J Hair ties and closed-toed shoes mandatory Finish packet and get stamped Table of Contents #2: 21. Quantum Number WS Cornell Notes 23. Ch. 5 Electron Packet FLT I will be able to express the arrangements of e - s in atoms through electron configurations by completing 5.2 Notes 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. Notes Protocol Add assignment # Copy down all bolded ideas Noise level 0 Raise hand to question/comment Be prepared to pair-share-respond 5.2: Electron Arrangement in Atoms 2

3 Quantum Model Recall Quantum Numbers Orbitals Arrangement of Electrons in Atoms Levels (n) Electron Configurations Sublevels (l ) Orbitals (m l ) 3

4 n = 1 n = 2 n = 3 n = 4 Energy Levels Arrangement of Electrons in Atoms Electron configurauon = arrangement of e - s in atoms Arrangement of Electrons in Atoms e - s assume an arrangement that gives the atom the lowest energy possible (more stable) Arrangement of Electrons in Atoms What does this look like? Electron Configurations 2p 4 Arrangement of Electrons in Atoms What does this look like? 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. 4

5 Three Principles Three Principles AuYau Principle = e - s occupy the lowest E orbital available. Use the diagonal rule 1 s Diagonal Rule 2 s 2p 3 s 3p 3d 4 s 4p 4d 4f 5 s 5p 5d 5f 5g? 6 s 6p 6d 6f 6g? 6h? 7 s 7p 7d 7f 7g? 7h? 7i? Three Principles Pauli Exclusion Principle = No more than two e - s can occupy a single orbital We note this using arrows in opposite direc<ons Three Principles Hund s Rule = Fill in single e - s in separate equal-energy orbitals before doubling up In Summary: Our Rules 5

6 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 Rules 2) Start filling orbitals in order of increasing E according to the AuYau 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 Rules 3) Hund s Rule Applies: Draw all orbitals for each type, and fill in ONE e - in each orbital before doubling up. Rules 4) Pauli Exclusion applies: Two e - s in the same orbital must have opposite spins Rules 5) Double check numbers. Make sure total # of e - s in your configura<on matches the atomic number (if your atom is neutral) Orbitals and the Periodic Table Orbitals grouped in s, p, d, and f orbitals s orbitals d orbitals p orbitals f orbitals 6

7 Examples Write the orbital notation and e - configuration for Hydrogen Write the orbital notation and e - configuration for Fluorine Write the orbital notation and e - configuration for Magnesium Write the orbital notation and e - configuration for Neon 7

8 Write the orbital notation and e - configuration for Arsenic Orbitals and the Periodic Table Orbitals grouped in s, p, d, and f orbitals s orbitals d orbitals p orbitals f orbitals Shorthand Notation Shorthand Notation We can abbreviate our long e- configura<ons by using our noble gases This is because our Noble Gases have complete full p orbitals Note: only do this when asked to Shorthand Notation 1. Find the closest noble gas to your atom with a smaller Z 2. Add/fill orbitals from where the Noble Gas leg off 8

9 Ex/Na Shorthand Notation Try: Cl Shorthand Notation Ca CW 1. Complete the electron configuration/ orbital notation worksheet 2. Check your answers with your pair-share partner(s) 3. Skip the following sections: Chemistry Thursday, October 27-Friday, October 28, 2016 Do-Now: Quantum Kahoot 1. Write down today s FLT 2. Write down the orbital notation for Calcium 3. Write down the electron configuration for Calcium 4. Write down the shorthand notation for Calcium 5. List the three rules we need to follow in order to write out electron configurations. 6. Write down your initials if you re playing with your phone, or number Take out your planner and ToC Announcements Must clear missing work AHend tutoring Current Unit: Ch. 5, 6, 8 Quiz Monday J Lab today J 9

10 Planner: Study for quiz + ToC due Wed Lab (w/ post-lab) due by Friday Schedule tutoring/retakes Table of Contents #2: 24. Quantum Kahoot Do-Now FLT I will be able to determine the identify of compounds based on their chemical properties by completing Photon Lab 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. Bunsen Burner Safety We will watch a video to review Bunsen Burner safety Failure to follow these safety rules will result in a zero and inability to parucipate in the lab Let s Recap Hair must be Ued back Goggles must be worn at all Umes Use gloves if handling the chemicals Wash hands thoroughly ager lab Photon Lab We will observe the properues of compounds by conducung a flame test. From our observauons, we will determine the idenuty of the compound. It is worth 10 lab points. You will fill out the lab packet. Then, you will ahach a wrihen report that includes the lab purpose and conclusion (results, data analysis, possible error) 10

11 Photon Lab 1. At your stauon, you will dip the splint/wire into the provided container holding the compound making sure that a few grains suck to the splint 2. Place into Bunsen burner flame and record the color that is added to the flame Photon Lab 3. Place completely used splints into the waste beaker OR rinse off wires 4. Goggles must remain on at all Umes 5. You will have two minutes at each stauon CW Complete lab packet Use complete sentences Work on post-lab report Lab Purpose (2-4 sentences) Conclusion List results Analyze data What were possible errors? ToC 11