1. SHS Chemistry 2014-2015

2. LEARNING TARGET Polyatomic Ion Lewis Structures Resonance WARM UP Have your notebook out for a quick review on lewis structures IP #2 Due Thursday Quiz 2 Thursday

5.  When you are done with the quiz, pick up Independent Practice #2  Independent Practice #2 is due Thursday 1/14  Quiz #2 is Thursday 1/14

6. THE RULES  all atoms except hydrogen should have 8 valence electrons  you must include all valence electrons that each atom brings into the bond  you cannot add extra electrons (unless there is a charge)  elements can form single, double, or triple bonds  Lewis structures for charged particles are placed in brackets, with the charge as a superscript on the outside

10. LEARNING TARGET I will be able to: 1. describe resonance structures 2. draw resonance structures for polyatomic ions

11. LEARNING TARGET VSEPR WARM UP On your white board, draw the Lewis Structure for CO 2

12.  Be sure that you are fully completing your role for the activity.  Do not rush. We will be working on this today and tomorrow, stopping periodically to check in as a whole class.  Work as a group!

14.  Pairs of electrons will (attract/repel) each other.  Two bonds on the same atom will try to get as (close to/far apart from) each other as possible.  A lone pair of electrons and a bonded pair of electrons will (push away from/move toward) each other.

16. How do lone pairs of electrons affect the bond angle differently than electrons shared in a bond?

17. LEARNING TARGET I will be able to predict polarity based on molecular shape. WARM UP Divide the following compounds among your group members. Draw a Lewis Structure on a post it note (one per molecule). Build each molecule COMPOUNDS HOCl H 2 O CO 2 HCN CF 4 CH 3 Cl NH 3 PCl 3 COH 2 COCl 2

18.  Working as a group, sort the models/Lewis structures by molecular geometry.  Use your POGIL activity from yesterday’s class as a reference.  Check in when you are done.

19.  Guiding Question: How can we use molecular geometry and Lewis structures to predict molecular polarity?  What does it mean for something to be polar?  Discuss with your group and now divide your models into those that are polar and those that are nonpolar.  Check in when done.

22. LEARNING TARGET Polarity WARM UP Prepare for the Quiz! IP #3 Due Tuesday Quiz #3 Tuesday

25.  Polarity occurs when there is an unequal sharing of electrons around the atoms in a covalently bonded molecule.

26.  Hydrogen bonding occurs between the hydrogen atom of one molecule and the Fluorine, Oxygen, or Nitrogen of another molecule. It is a weak attraction between molecules.

27.  What does it mean for a molecule to be polar?  Define hydrogen bonding in your own words.

28.  Use your knowledge of Lewis Structures and sketches of molecular geometry to predict the polarity of each compound (polar or nonpolar).  When your group is done, send a representative to the board to add your predictions to the chart provided.

29. Chemical Formula Group 1 Group 2 Group 3 Group 4 Group 5 Group 6 Group 7 Group 8 H2H2 CO 2 H2OH2O H2SH2S COH 2 BCl 3 NH 3 PCl 3 CCl 4 CF 4

30. LEARNING TARGET Electronegativity WARM UP

31.  Work through this activity together

32.  When calculating differences, you use the electronegativity of the element, but do not account for number of atoms  Electronegativity differences can give us a better estimate of bond polarity  Bond Polarity IONIC POLAR COVALENT NONPOLAR COVALENT LESS THAN 0.5 1.6-0.51.7 OR GREATER