1. You need: Chemical Bonding Article Yellow Chemical Bonding paper Is your spiral turned in??? Do it NOW! Unit 6

2. Fold your yellow paper like a letter… HURRY!

3. You have 15 minutes to read the Chemical Bonding article and transfer the info learned into the right section of the brochure And go….

4. Time’s Up! Now check to see if you got the same thing I got… Include my drawings if you didn’t have time to draw any from the article Take good notes –> assignment will be easy!

5. A chemical bond is: An attraction between the nuclei and valence electrons of different atoms that holds the atoms together (the hook up!!!)

6. Why do atoms bond? (outer flap) Most elements (besides noble gases) are very unstable When they bond they become more stable (like a noble gas) Everybody has their 8!!! They had to share to help each other out.

7. How do atoms bond? atoms bond by gaining, losing, or sharing e- Most Group A elements (s and p - block) want to attain an octet (8 valence e-) Octet Rule – most elements want to have 8 valence electrons to achieve stability

8. Types of bonding (open flaps) 1. Ionic Bonds Transfer e - from a metal to a nonmetal Smallest ratio is called a formula unit Example  (metal) CaCl 2 (nonmetal)

9. Ionic Bond (draw & label this!) Notice the pair of electrons is all the over on the right. Higher electronegativity More attractive! + + Metal  nonmetal e-e- e-e- e-e- e-e-

10. 2. Covalent sharing of e- between 2 nonmetals Smallest ratio of a covalent compound is called a molecule Examples: H 2 H 2 O & C 6 H 12 O 6

11. 2 types of covalent bonds: (draw pics too) Nonpolar covalent Equal sharing of e - Example: H 2 Polar covalent Unequal sharing of e - Notice right is pulling harder Example: HCl + + = + +

12. Polar Covalent Bond electrons shared unequally Chlorine has higher electronegativity (EN) so it pulls harder HCl Hydrochloric acid

13. 3. Metallic Bonding  All involved atoms are metals (duh!)  Electrons are shared in a “sea of free flowing or mobile electrons” by all atoms  This flow is responsible for ductility, malleability, luster and ability to conduct heat and electricity  Example: copper wire

14. The “sea” of electrons

15. 2 ways to determine bond type (fold up your bottom flap) 1. Location on the periodic table metal + nonmetal = Ionic nonmetal + nonmetal = Covalent metal + metal = Metallic

16. 2. taking the difference in the electronegativity (subtract!!!) Sulfur and Hydrogen 2.5 – 2.1 = 0.4 Nitrogen and Cesium 3.0 – 0.7 = 2.3 Chlorine and Bromine 3.0 – 2.8 = 0.2 Polar covalent Ionic Nonpolar covalent 4.0 ionic 1.7 polar cov 0.3 nonpolar cov

17. Now you try… Electronegativity & Bond Type Homework Don’t forget Chemis-Tree project!!! Google ideas! Look what I found online…

18. Happy Thanksgiving!!! I am thankful for each of you. It’s crazy to me that I get paid to do something I love. I love your personalities, your laughter, your passion about life and your face when you’re successful at learning something difficult. Be safe next week and don’t eat too much! Love ya! Duley