Bell Ringer (in yesterday’s notes) Bonding Atoms Type of bond More EN Atom Na & Cl Cl & Cl Types of bonds: ionic, polar covalent, nonpolar covalent

Day Topic HW Monday 10/6 -Properties of Ionic, Covalent, Metallic Compounds -Crash Course Chemistry #24 -Prelab for Bonding lab due Wed Tuesday 10/7 -Lewis Structures for Ionic & Covalent Compounds on iPads -Packet page 1 for Thursday Wednesday 10/8 -Pre-lab DUE in Lab Notebook -Lab: Ionic, Covalent, Metallic Compounds -Lab Write-Up due Friday Thursday 10/9 -VSEPR -Lab Write-Up due tomorrow -Packet page 3 for Tuesday Friday 10/10 -Short quiz on Tuesday over Lewis structures and VSEPR

Pre-Lab for tomorrow Formatting: Numbered pages Write on the fronts in pen Label each section with a section name and Roman numeral. These are found below. Heading – At the top right of each page put the lab title and the date the lab was performed. I. Pre-lab Questions – Write out all pre-lab questions and answers. II. Purpose – This is a statement of the problem to be investigated. It provides the overall direction for the laboratory investigation and must be addressed in the conclusion. III. Safety – After reading the procedure, list all safety issues that need to be kept in mind while performing the lab. This includes but is not limited to acids, bases, other dangerous chemicals, hot objects, open flames, and broken glass. Make sure to include chemical inventory information. IV. Procedure – Write out the procedure in your own words.

Lewis Dot Lewis Dot notation can be used to visualize ionic compounds and how they form.

What is the Lewis Dot Structure for calcium oxide? Use brackets to show charges of negative ions.

Practice Use Lewis Dot to predict formulas for Magnesium and Nitrogen

Lewis Dot and Covalent

Rules for drawing Lewis dot structures for covalent compounds: Step 1: Count the valence electrons in the compound. Find each element in the periodic table. The number of electrons is equal to the group number.

Rules for drawing Lewis dot structures for covalent compounds: Step 2: Put the LEAST electronegative element at the center (never hydrogen) and make single bonds from it to the other atoms. *single bond = 2 electrons ** double bond = 4 electrons *** triple bond = 6 electrons

Rules for drawing Lewis dot structures for covalent compounds: Step 3: Add remaining electrons, in pairs, to the outer atoms first to satisfy the octet rule. **Exceptions to the octet rule: Hydrogen can only hold 2. Beryllium has a maximum of 4. Boron is stable with only 6. If the central atom is from periods 3-7, it can accommodate more than 8 electrons due to the presence of d orbitals

Rules for drawing Lewis dot structures for covalent compounds: Step 4: Put any remaining pairs or single electrons around the central atom. Step 5:  If the center atom is still not satisfied, the electrons you placed on the outer atoms must be brought in and shared with the center atom in double or triple bonds until everyone is “happy”.

Draw Lewis structures for the following compounds Practice – Draw Lewis structures for the following compounds CO2

App: Lewis Dots Open “Lewis Dots” on the iPad Follow along on your lab

Exit Ticket Draw the Lewis Structures for one of the following: Barium fluoride (BaF2) H2O XeF4