1. Work with your group – get as much done as possible – this will be collected!!!

2. #1 IONIC BOND Example: Draw the electron-dot symbols representing the following reactions: sodium atom + chlorine atom form ions to produce sodium chloride

3. #2 COVALENT BOND Ex: Use electron dot formulas to represent the reaction described. hydrogen atom + chlorine atom → HCl molecule

4. #3 ELECTRON DOT FORMULAS OF MOLECULES Example: Draw the Electron dot formula for each of the following molecules: a. H 2 S b. CH 2 Br 2 c. SO 3 d. HCN

5. #4 ELECTRON DOT FORMULAS OF POLYATOMIC IONS Example: Draw the Electron dot formula for each of the following polyatomic ions: a. NH 4 +1 b. NO 3 -1 c. PO 4 -3 d. CO 3 -2

6. Watch the following video before moving on (8 min) https://www.youtube.com/watch?v=AFqwtY7m2PI

7. #5 Empirical Formulas Write the empirical formula for the following compounds. C 6 H 6 C 8 H 18 WO 2 C 2 H 6 O 2 X 39 Y 13

8. #6 Empirical and Molecular Formulas A compound with an empirical formula of C 2 OH 4 and a molar mass of 88 grams per mole. What is the molecular formula of this compound? A compound with an empirical formula of C 4 H 4 O and a molar mass of 136 grams per mole. What is the molecular formula of this compound? A compound with an empirical formula of CFBrO and a molar mass of 254.7 grams per mole. What is the molecular formula of this compound?

9. #7 Empirical and Molecular Formulas A compound with an empirical formula of C 2 H 8 N and a molar mass of 46 grams per mole. What is the molecular formula of this compound? A well-known reagent in analytical chemistry, dimethylglyoxime, has the empirical formula C 2 H 4 NO. If its molar mass is 116.1 g/mol, what is the molecular formula of the compound? Nitrogen and oxygen form an extensive series of oxides with the general formula N x O y. One of them is a blue solid that comes apart, reversibly, in the gas phase. It contains 36.84% N. What is the empirical formula of this oxide?

10. #8 Empirical and Molecular Formulas A sample of indium chloride weighing 0.5000 g is found to contain 0.2404 g of chlorine. What is the empirical formula of the indium compound? An unknown compound was found to have a percent composition as follows: 47.0 % potassium, 14.5 % carbon, and 38.5 % oxygen. What is its empirical formula? If the true molar mass of the compound is 166.22 g/mol, what is its molecular formula? Rubbing alcohol was found to contain 60.0 % carbon, 13.4 % hydrogen, and the remaining mass was due to oxygen. What is the empirical formula of rubbing alcohol?

11. Unless you have a lot of time left – go on and challenge them to figure this stuff out

12. #9 SHAPES OF MOLECULES Ex. Give the electron dot formula, shape, and bond angles for CO 2 CH 2 O CH 4

13. #10 MOLECULES WHERE CENTRAL ATOM HAS ONE OR MORE LONE PAIRS AB 2 E: bent ⇒ central atom is bonded to two outer atoms (B) and has a lone pair of electrons (E) Ex. Give the electron dot formula, shape, and bond angles for SO 2

14. #11 AB 3 E: trigonal pyramid ⇒ central atom is bonded to two outer atoms (B) and has a lone pair of electrons (E) Ex. Give the electron dot formula, shape, and bond angles for NH 3.

15. #12 AB 2 E 2 : bent ⇒ central atom is bonded to two outer atoms (B) and has 2 lone pairs of electrons (E) Ex. Give the electron dot formula, shape, and bond angles for H 2 O

16. #13 REFER TO TABLE OF MOLECULAR SHAPES AND BOND ANGLES TO ANSWER THE FOLLOWING Example For the following molecules or ions(where the central atom is underlined): i. Draw the Electron dot formula. ii. Determine the shape of the molecule. iii. Determine the approximate bond angles a. CH 2 F 2 b. OF 2 c. phosphite ion, PO 3 –3

17. #14 POLAR COVALENT BONDS Example: For each of the bonds below: i. Use delta notation (δ+ and δ–) to indicate which atom is more electronegative, and ii. Use an arrow to point from the less electronegative atom to the more electronegative atom C – Cl N – O H – O

18. #15 Bond Types Example: Identify the type of bond described for each of the following: ionic bond: metallic bond: polar covalent: nonpolar covalent: The C–O bonds in CO 2 The C–C bonds in C 3 H 8 The bonds in F 2 The bonds in Ba The bonds in K 2 O The bonds in H 2 O

19. #16 SHAPES OF MOLECULES A molecule with polar bonds is polar if either of the following applies: 1) the central atom has one or more lone pair(s) of electrons, or 2) the atoms bonded to the central atom are not identical Ex. 1: Determine whether the following molecules are polar or nonpolar: CO 2 H 2 O SO 3