Chemistry Day 20 Monday, October 15 th Tuesday, October 16 th, 2018
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
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 relative properties of elements based on the patterns of electrons in the outermost energy level of atoms.
Ch. 11: Electron Arrangement in Atoms
Recall
Quantum Model
Quantum Numbers
Orbitals
Electron Configurations
Arrangement of Electrons in Atoms Levels (n) Sublevels (l ) Orbitals (m l )
Energy Levels n = 1 n = 2 n = 3 n = 4
Arrangement of Electrons in Atoms Electron configuration = 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 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.
Arrangement of Electrons in Atoms What does this look like?
Three Principles
Aufbau Principle = e - s occupy the lowest E orbital available. Use the diagonal rule Three Principles
1 s Diagonal Rule 2 s 2p 3 4 5 6 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?
Three Principles Pauli Exclusion Principle = No more than two e - s can occupy a single orbital We note this using arrows in opposite directions
Three Principles Hund s Rule = Fill in single e - s in separate equal-e orbitals before doubling up
In Summary: Our Rules
Rules 1) Determine the # of e - s by looking up Z (atomic number) Assume the atom is neutral unless stated otherwise (more on this later). Draw orbitals first to help you. Ex/ Nitrogen
Rules 2) Start filling orbitals in order of increasing E according to the Aufbau 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
5) Write e - config Rules Make sure total # of e - s in your configuration 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
Examples
Write the orbital notation and e - Fluorine configuration for
Write the orbital notation and e - configuration for Magnesium
Write the orbital notation and e - Titanium configuration for
Write the orbital notation and e - Arsenic configuration for
Orbitals and the Periodic Table Orbitals grouped in s, p, d, and f orbitals s orbitals d orbitals p orbitals f orbitals
Shorthand Electron Notation
Shorthand Electron Notation We can abbreviate our long e- configurations by using our noble gases This is because our Noble Gases have complete full p orbitals Note: only use shorthand when asked to
Shorthand e - 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 left off Ex/Na
Try: Ca Shorthand Notation
Chemistry Day 21 Wednesday, October 17 th Thursday, October 18 th, 2018
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) 6. How many TOTAL electrons can there be if n = 3 and l = 2? 7. What four quantum numbers describe an electron in the 4s orbital spinning clockwise? Take out your planner and ToC
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 relative properties of elements based on the patterns of electrons in the outermost energy level of atoms.
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
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
Chemistry Day 22 Friday, October 19 th Monday, October 22 nd, 2018
Do-Now: Lab Day Do-Now Have long hair? Tie your hair back 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 configuration for Calcium 5. List the three principles/rules we need to follow in order to write out electron configurations. Take out your planner and ToC
FLT I will be able to investigate the relationship between electrons and energy by completing Quantum Lab Standard HS-PS1-1: Use the periodic table as a model to predict the relative properties of elements based on the patterns 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 participate in the lab
Let s Recap Hair must be tied back Goggles must be worn at all times Use gloves if handling the chemicals Wash hands thoroughly after lab
Photon Lab We will observe the properties of compounds by conducting a flame test. From our observations, we will determine the identity of the compound. The packet itself is worth 10 lab points. Be specific and detailed to get your points There will be a written report that will be submitted in addition to your packet worth 10 points as well