Tuesday, December 9th, 2014 HW: Agenda Questions Objective: We will be able to determine the electron configuration for an atom. Standard: IOD 402 Catalyst: F. The number of ants at each site G. The number of seed dishes placed at each site H. The mass of the elaiosome of each seed J. The type of seeds taken by the ants in each site Classroom expectations: Wear Kenwood ID. Cell phones, music players, and headphones are put away. Food is disposed of or put away. Dressed appropriately. Notebook is out and you are ready for today’s class. Answer: C ***Table of Contents 12/9 Week 15 Catalyst 84 12/9 Week 15 Agenda 85 12/9 Week 15 Textbook Reading 86 12/9 Notes: Electron Configuration 87

Tuesday, December 9th, 2014 HW: Agenda Questions Objective: We will be able to determine the electron configuration for an atom. Standard: IOD 303 Catalyst: F. 5.0 N G. 7.0 N H. 9.0 N J. 11.0 N Classroom expectations: Wear Kenwood ID. Cell phones, music players, and headphones are put away. Food is disposed of or put away. Dressed appropriately. Notebook is out and you are ready for today’s class. Answer: A ***Table of Contents 12/9 Week 15 Catalyst 78 12/9 Week 15 Agenda 79 12/9 Week 15 Textbook Reading 80 12/9 Notes: Electron Configuration 81

Announcements No tutoring today Tutoring will be Weds of this week Quiz Thursday

Catalyst/Announcements Review POGIL Notes: Electron Configuration Agenda Catalyst/Announcements Review POGIL Notes: Electron Configuration

Electron Configuration Notes 87

Electron Configuration Notes 81

Electrons are always moving around the nucleus in energy levels.

Within these energy levels, there are specific regions or sublevels where electrons are more likely to be found.

Example: Hydrogen (H): 1s1 # electrons Energy level sublevel

Energy level 1: 1 sublevel (s) Energy level 2: 2 sublevels (s, p) Energy level 3: 3 sublevels (s, p, d) Energy level 4: 4 sublevels (s, p, d, f)

TAPE!!!

Orbital Diagrams

Aufbau principle Electrons occupy the lowest energy first.

Suborbitals Each sublevel can hold a specific number of electrons. s: holds 2 electrons, 1 pair with opposite spins p: holds 6 electrons, 3 pairs with opposite spins d: holds 10 electrons, 5 pairs with opposite spins f: holds 14 electrons, 7 pairs with opposite spins

Rules for Electron Configuration Electrons fill the lowest sublevel first. Only one electron goes in an orbital at a time before doubling up. Only 2 electrons can be in an orbital and they must have opposite spins.

S-block p-block d-block f-block

Example Element: Sulfur Electron Configuration: Orbital Diagram:

Whiteboard Practice Only write when you are completing a problem. Hold up board ONLY when asked. Keep marker capped when possible.

White board practice Draw the orbital diagram for Nitrogen Draw the spdf configuration 1s22s22p3

White board practice Draw the orbital diagram for Chlorine Write the spdf notation 1s22s22p63s23p5

White board 1s22s22p63s1 1s22s1 1s22s22p63s23p64s1 1s22s22p1 Write the electron (spdf) configuration of Sodium Lithium Potassium Boron Aluminum Gallium 1s22s22p63s1 1s22s1 1s22s22p63s23p64s1 1s22s22p1 1s22s22p63s23p1 1s22s22p63s23p64s23d104p1

Noble Gas notation Electron configurations can be written in noble gas configuration The noble gas of each row becomes a placeholder for the configurations that came before. This is kind of like a checkpoint in a game you start your configuration from after each noble gas.

Practice Write the configuration of Argon 1s22s22p63s23p6 Now write the configuration of calcium 1s22s22p63s23p64s2 Now we can use the symbol [Ar] in brackets as a placeholder [Ar]4s2

Noble gas configuration You can only use noble gases for shorthand notation

White board [Kr]5s2 [He]2s2 [He]2p5 [Xe]6s1 Write short hand for the following Strontium Beryllium Fluorine Cesium Radium [Kr]5s2 [He]2s2 [He]2p5 [Xe]6s1

Whiteboard [He]2p2 [Ne]3p2 [Ar]4s2 [Ne]3s2 Write the noble gas configuration for the following Carbon Silicon Ca Mg [He]2p2 [Ne]3p2 [Ar]4s2 [Ne]3s2

Exceptions to Aufbau Principle

Exceptions to the Aufbau Principle (HONORS only) Exceptions to the Aufbau Principle d and f orbitals require LARGE amounts of energy If we can’t fill these sublevels, then the next best thing is to be HALF full (one electron in each orbital in the sublevel) There are many exceptions, but the most common ones are Copper (ends in 4s13d10) Silver (ends in 5s14d10) Gold (ends in 6s14f145d10) Chromium (ends in 4s13d5) d4 and d9

Exceptions to the Aufbau Principle (HONORS only) Exceptions to the Aufbau Principle OK, so this helps the d, but what about the poor s orbital that loses an electron? Remember, half full is good… and when an s loses 1, it too becomes half full! So… having the s half full and the d half full is usually lower in energy than having the s full and the d to have one empty orbital.

Practice 1.) Write the electron configuration for helium.

Practice 2.) Write the electron configuration for beryllium.

Practice 3.) Write the electron configuration for fluorine.

Practice 4.) Write the electron configuration for argon.

Practice 5.) Draw the aufbau diagram for boron.

Practice 6.) Draw the complateaufbau diagram for sodium.

Practice 7.) Write the electron configuration for oxygen.

Exit Ticket 8.) Draw the aufbau diagram AND write the electron cofiguration for calcium for titanium.