1. Covalent Bonding Notes
Bundle 2: Periodic Table & Bonding

2. H-H = H2 Covalent Bonds SHARING OF ELECTRONS between the two elements.
The bond between TWO NON-Metals.
SHARING OF ELECTRONS between the two elements.
H-H = H2

3. 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)

4. Lewis dot structure for covalent molecules
The Lewis Dot Structure for Covalent Molecules shows how the elements share electrons.

5. 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?

6. 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.

7. 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
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 (-)

8. Covalent Bonding Practice
Using the LEWIS DOT STRUCTURE, draw CH4 (Methane) in your notebook.
Now draw the COVALENT STRUCTURE of CH4.
Draw the Water Molecule (H2O) in your notebook using the LEWIS DOT STRUCTURE.
Now draw the COVALENT STRUCTURE of H2O.

9. How to draw Lewis dot and covalent structure of Water and Methane
Water (H2O) Methane (CH4)

10. 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!

11. Naming Covalent Bonds

12. 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

13. 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

14. Practice Writing Covalent Formulas
Dinitrogen Pentoxide
Write the symbol of each element.
N O
Add the subscript as indicated by the prefixes.
N2O5

15. Practice Writing Covalent Formulas
Carbon Dioxide
Write the name of each element.
C O
Add the subscripts as indicated by the prefixes.
CO2

16. Naming Covalent Molecules
NH3
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
Name of the molecule: Nitrogen trihydride

17. Naming Covalent Molecules
P2O5
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

18. Research Assignment 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.

19. Try a few examples on your own.
Write the Chemical Formula for these names
Write the Chemical Names for these formulas
Sulfur dioxide
Sulfur monoxide
Carbon tetrachloride
Dihydrogen dioxide
Nitrogen triiodide CO
CO2
SF2
PI3
H2O

20. 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

21. Intramolecular Force – Force between Atoms to form a compound
Example: the bond between Na and Cl in a NaCl molecules
Na+
Cl-

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

23. Intramolecular Force
Intermolecular Force

24. Intermolecular Force
Intramolecular Force

25. Types of Intermolecular Forces
Hydrogen Bond – when H bonds to N, O, or F
Important in DNA (genetic material), proteins, and water molecules

26. Water