1. Calculate the molar mass for the following compounds a. silver nitrate b. chromium (II) perchlorate c. lead (II) carbonate d. nickel (II) hydroxide e. sodium sulfate 2. Perform the following conversions a. 0.75 g silver nitrate moles b. 1.50 moles lead (II) carbonate grams c. 0.256 g nickel (II) hydroxide atoms d. 1.29x1018 atoms chromium (II) perchlorate moles e. 0.0259 g of sodium sulfate moles 3. Convert 25.62 grams of hydrophosphoric acid to moles. 4. Calculate the % of oxygen in strontium phosphate Calculate the % of potassium in potassium oxide Calculate the percent of nitrogen in magnesium nitride. 5. Find the empirical and molecular of the compound given below. 1. 56.15 g C, 9.43 g H, 74.81 g O, 13.11 g N, and 21.49 g Na. ; molar mass = 591.2 amu 6a. The molecular formula of a compound is P6S4. What is the empirical formula of this compound? b. The molecular formula of a compound is C4H4. Determine the empirical formula of this compound. 7. What is the molecular formula of a compound that has an empirical formula of C2H7 and a molar mass of 93 g/mol. 8. Calculate the empirical formula for a compound that is found to contain 85.64% carbon and 14.36% hydrogen by mass. 9. Draw the following structures Determine the shape Determine the polarity NH4+ CO32- Carbon dioxide Dihydrogen monoxide Hydrofluoric acid Nitrogen trihydride Carbon tetrachloride 10. Be able to locate alkali metals, alkaline earth metals, transition metals, nonmetals, halogens, and noble gases on the periodic table 11. Determine the oxidation number (charge) for the following: Alkali metals Alkaline earth metals Halogens Noble gases 12. Determine protons, neutrons, and electrons for the following: Chlorine – 37 Copper – 66 54 Cr 14 N 31 3- P 13. Define ionic bond. 14. Define covalent bond.