SHS Chemistry

LEARNING TARGET I will record detailed observations about a lab procedure. WARM UP Construct the following table on a clean sheet of paper. Be sure to leave enough space to record detailed observations for each procedure. ProcedureObservations Sugar Solution Salt Solution Melting of Sugar Melting of Salt

 What questions could this lab answer? Brainstorm at least 2 per group that could have been used as a guiding question  What would your conclusions be at this point of the experiment?  What were your dependent variables? What were your independent variables? What are your controls?

LEARNING TARGET I will record detailed observations about a lab procedure. WARM UP Have your observation sheet from yesterday out and ready for Part 2 of the lab. Each person in your group needs goggles.

Take two minutes and independently list 3 questions that were raised by the lab. Use the data you collected. This must be done independently

 In your group – verbally share your questions (3 minutes)  The group will determine if the questions are closed or open. Closed questions will have a “C” next to them, Open with an “O” (3 minutes)  As a group, rewrite any closed questions to be open in the rewritten questions box

 Find pieces in 12.1 that might support or answer the questions that you have – this is a class set of the reading, so do not write or highlight on the paper. You can take notes on your observation sheet when you find items that support or answer your questions (5 minutes)  In your groups, share what evidence you found in the reading (5 minutes)

1. What questions do you have that are still un- answered? 2. Why do you think you weren’t able to answer all the questions? 3. How did this text impact your thinking? 4. What new questions do you have after discussing and reading?

 Write what you would do next, as a scientist, to further investigate and answer your questions  Reflect on what you got out of today’s class

LEARNING TARGET I will be able to: 1. Identify properties of ionic and covalent compounds WARM UP Have your lab observations and any notes from the reading out

 Individually write down at least one property of an ionic compound and at least one property of a covalent compound.  Write each property on its own post-it note.  It can be from the lab or the reading.

 As a group…  Go around the table in a circle  Read one of your properties out loud to your group, and place it in the proper column of the chart. Discuss any disagreements as they occur.  Continue until you have shared all of the properties your group came up with.

 When called on, the spokesperson at your table will share one of your group’s properties. Do not tell the class whether it is ionic or covalent.  I will give you a few seconds to discuss, then call on the manager from another table to say what compound the property represents.

Ionic CompoundsCovalent Compounds Transfer ElectronsShare Electrons Metal and NonmetalOnly Nonmetals Soluble in waterSometimes soluble in water Conducts electricity when dissolved in water Does not conduct electricity Extremely high melting point and boiling point Low melting and boiling point

LEARNING TARGET I will be able to: 1. Draw Lewis Structures for compounds with single bonds 2. Draw Lewis Structures for compounds with double & triple bonds 3. Predict type of bonds that will form based on total number of valence electrons. WARM UP (on your white board) What is one property of an ionic compound?

 Use the kit at your table to construct a diagram of Carbon’s valence electrons.  Use the kit at your table to construct a diagram of Hydrogen’s valence electron with a different disc color  Now build the covalent compound CH 4

Lewis Structure Bonding Pair

Non-Bonding Pair

Show non-bonding pairs

 Center Atom – Carbon is always a center atom in a compound  Hydrogen is always on the outside  Draw valence electrons for all atoms  Start with the center atom  Then move to the other atoms and place them around looking for single electrons to bond to  When you satisfy the octet rule on all atoms you are done.

 Take out your periodic table and a highlighter or colored pencil.  Diatomic elements are elements that exist naturally as two atoms of the same element covalently bonded together into a molecule.

 Covalent and Ionic Compound Properties  Lewis Structures  Octet Rule  Valence electrons on an atom from the Periodic Table  Draw Lewis structures for single bond compounds  Identify bonding and non-bonding electron pairs  Diatomic Elements

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 electrons  elements can form single, double, or triple bonds

C CHH

LEARNING TARGET I will be able to: 1. describe resonance structures 2. draw resonance structures for polyatomic ions WARM UP  Make one pile of homework, and a separate pile of everyone’s notes.

Independent Practice Activity Suggested Date to Complete (after class) Learning Target D: Lewis Structures for Polyatomic Ions Learning Target E: VSEPR

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

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

LEARNING TARGET I will practice creating Lewis Structures on paper. WARM UP Be sure you have back your quiz and your independent practice paper.

 Use the whiteboards to practice drawing your Lewis Dot Diagrams before copying your final answer onto your paper. Use the models too if you want to!  Finish independent practice first, and turn it in.  Then work on the Lewis Structure Practice handout  Quiz Monday!