1. COVALENT BONDING NOTES Bundle 2: Periodic Table & Bonding

2. WARM UP  Complete the WARM UP for September 28, 2016  Set up the next clean page for Cornell Notes.  Fill in your Table of Contents and make sure you have updated your SUMMARIES on all of your Cornell Notes.  NOTEBOOK GRADE on FRIDAY!

3. ANNOUNCEMENTS  If you need to retake or make up a quiz, I need to know TODAY so I can send it down this afternoon to TOPS.  TOPS is afterschool tutoring and make ups in the Cafeteria from 4:05pm to 5pm on Wednesdays.  Athletics cannot have practice during TOPS Wednesdays, it is school policy.

4. COVALENT BONDS ● SHARING OF ELECTRONS between the two elements. H-H = H 2 The bond between TWO NON-Metals The bond between TWO NON-Metals.

5. WHAT DOES THE LITTLE BAR MEAN?  The little bar between elements in a covalent molecule means they are SHARING TWO electrons.  What do you think 2 bars means?  Double Bond (Sharing 4 electrons)  What about 3 bars?  Triple Bond (Sharing 6 electrons)

6. LEWIS DOT STRUCTURE FOR COVALENT MOLECULES  The Lewis Dot Structure for Covalent Molecules shows how the elements share electrons.

7. CHECK FOR UNDERSTANDING  How many electrons are shared by the bar in the picture of Hydrogen Fluoride?  How many total electrons are shared between Carbon and the two Oxygen atoms in a molecule of Carbon Dioxide?

8. 2 TYPES OF COVALENT BONDS ● Polar Covalent Bond – electrons are unevenly shared; One element “pulls” more on the electrons than the other. ● Nonpolar Covalent Bond – electrons are evenly shared; each element “pulls” evenly on the electrons.

9. WATER IS A POLAR MOLECULE The O atom pulls on the shared electrons in each H causing a partial (+) charge on each H atom and partial (–) charge on the O atom The O atom pulls on the shared electrons in each H causing a partial (+) charge on each H atom and partial (–) charge on the O atom Why is O pulling the electrons towards itself? O is more attracted to the electrons it’s sharing with H – unequal sharing of electrons Why does water act like a magnet? Because the partial (+) attracts the partial (-)

10. COVALENT BONDING PRACTICE  Using the LEWIS DOT STRUCTURE, draw CH 4 (Methane) in your notebook.  Now draw the COVALENT STRUCTURE of CH 4.  Draw the Water Molecule (H 2 O) in your notebook using the LEWIS DOT STRUCTURE.  Now draw the COVALENT STRUCTURE of H 2 O.

11. HOW TO DRAW LEWIS DOT AND COVALENT STRUCTURE OF WATER AND METHANE  Water(H 2 O)Methane (CH 4 )

12. WARM UP  Complete the WARM UP for September 29, 2016  Set up the next clean page for Cornell Notes.  Fill in your Table of Contents and make sure you have updated your SUMMARIES on all of your Cornell Notes.  NOTEBOOK GRADE on FRIDAY!

13. NAMING COVALENT BONDS

14. COVALENT MOLECULE PREFIXES – EACH PREFIX TELLS YOU THE NUMBER OF ATOMS OF THAT ELEMENT IN THE MOLECULE.  Mono - 1  Di - 2  Tri - 3  Tetra - 4  Penta - 5  Hexa - 6  Hepta - 7  Octa - 8  Nona - 9  Deca - 10

15. WRITING COVALENT MOLECULE FORMULAS  Write the Chemical Symbol of the element in the first name  Look at the prefix on the first name  Put the number that matches the prefix as the subscript on the Chemical Symbol  Repeat these steps for the second element name

16. PRACTICE WRITING COVALENT FORMULAS Dinitrogen Pentoxide  Write the symbol of each element. NONONONO  Add the subscript as indicated by the prefixes. N2O5N2O5N2O5N2O5

17. PRACTICE WRITING COVALENT FORMULAS Carbon Dioxide  Write the name of each element. C O  Add the subscripts as indicated by the prefixes. CO 2 CO 2

18. NAMING COVALENT MOLECULES NH 3  Write the name of the first nonmetal using its subscript as a prefix. Nitrogen (No prefix written for the first element IF it is a one.)  Write the name of the second nonmetal using its subscript as a prefix and change the ending to -ide. Trihydride Nitrogen trihydride  Name of the molecule: Nitrogen trihydride

19. NAMING COVALENT MOLECULES P2O5P2O5  Write the name of the first nonmetal using the subscript as a prefix. Diphosphorus  Write the name of the second nonmetal using the subscript as a prefix and change the ending to -ide. Pentoxide  Name the molecule: Diphosphorus Pentoxide

20. RESEARCH ASSIGNMENT DHMO.org  Go to the website DHMO.org on your phone.  Research DHMO and write an Acrostic Poem in your notebook  Answer the question at the bottom of the Poem page and be prepared to take a stand.

21. TRY A FEW EXAMPLES ON YOUR OWN.  CO  CO 2  SF 2  PI 3 H2OH2OH2OH2O  Sulfur dioxide  Sulfur monoxide  Carbon tetrachloride  Dihydrogen dioxide  Nitrogen triiodide Write the Chemical Formula for these names Write the Chemical Names for these formulas

22. 2 TYPES OF FORCES BETWEEN ELEMENTS ● Intramolecular Force (stronger) holds elements together to make compounds ● Intermolecular Force (weaker) holds molecules together to form solids, liquids, and gases

23.  Example: the bond between Na and Cl in a NaCl molecules INTRAMOLECULAR FORCE – FORCE BETWEEN ATOMS TO FORM A COMPOUND Na + Cl -

24. Intermolecular Force – The force between different molecules  Example: an interstate highway runs between different states

25. Intermolecular Force Intramolecular Force

26. Intermolecular Force Intramolecular Force

27. TYPES OF INTERMOLECULAR FORCES ● Hydrogen Bond – when H bonds to N, O, or F o Important in DNA (genetic material), proteins, and water molecules

28. WATER