3. Most laboratory experiments are performed at room temperature at 65 C. Express this temperature in: a. F b. Kelvin

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1 Do all work on a separate sheet of paper so that you can show your work. Section A: Measurement and Math 1. Convert the following and show your work: a. 200 meters = miles. b. 650 in = meters c. 4 years= seconds. d. 200 liters = ml 2. Classify each of the following as units of mass, volume, length, density, energy, or pressure. a. Kg b. Liter c. m 3 d. mm e. kg/m 3 f. Joule g. atm h. cal. i. Torr j. g/ml 3. Most laboratory experiments are performed at room temperature at 65 C. Express this temperature in: a. F b. Kelvin 4. How many significant figures are in each of the following? a mm b kj c x10 23 atoms d L e cm 3 f g h i j x 10 4 k x Record the following in correct scientific notation: a. 4050,000,000 cal b mol c Ǻ d. 700,000,000 atoms 6. Calculate the following to the correct number of significant figures. a g / cm 3 b g / L Page 1 of 6

2 7. A given sample contains 2.0 g of hydrogen, 33.1 g of sulfur, and g of oxygen. What is the total mass of the sample? a g b g c g d. 1.1 x 10 2 g e. 1.1 x 10-2 g 8. Give the chemical symbols for the following elements: a. Carbon b. Sulfur c. Titanium d. Nitrogen e. Helium f. Krypton g. Fluorine h. Scandium I. Arsenic J. Potassium K. Sodium l. Chloride m. Iron n. Zinc 9. The density of copper is 8.96 g/cm 3. What is the mass of cm 3 of pure copper? 10. The density of a piece of metal can be determined from mass and water displacement data. A piece of metal with a mass of g is placed in a flask with a volume of cm 3. It is found that g of water (d= g/cm 3 ) is needed to fill the flask with the metal in it. The density of the metal is most nearly (all answers in g/cm 3 ): (Show your work) a b. 1.7 c d. 9.5 e Page 2 of 6

3 Section B: Atoms, Molecules and Ions 1. Identify the following as a diatomic molecule, molecular compound, ionic compound, atomic element. a. F 2 b. Cl 2 c. C d. NaCl e. KF f. CO 2 g. H 2 h. Ag i. Rust (Fe 2 O 3 ) j. MgO k. O 2 l. I 2 m.co n. K 2 CO 3 2. What is the difference between a Chlorine and Chloride? 3. What is the difference between a Sodium atom and a sodium ion? 4. What is the difference between Carbon-12 and Carbon-13? 5. Complete the following table: # of protons # of neutrons # of electrons in atom Mass number Atomic number Net Charge when ion is formed Symbol Se Page 3 of 6

4 6. Name each of the following compounds (use the table of polyatomic ions in your notes when necessary): a. FeO b. Fe 2O 3 c. PCl 5 d.mg(oh) 2 e. V 2O 5 f. NaHCO 3 g. K 2SO 4 h. CoCrO 4 i. Hg 2O j. (NH 4) 3PO 4 7. Write the formula for following compounds: a. Calcium sulfate b. Ammonium phosphate c. Lithium nitrate d. Potassium perchlorate e. Barium oxide f. Zinc sulfide g. Sodium hydroxide h. Calcium iodide i. Aluminum carbonate 8. Identify each of the following elements: a. member of the same family as oxygen whose most stable ion contains 54 electrons b. noble gas with 18 protons in the nucleus c. halogen with 85 protons and 85 electrons d. member of the alkali metal family whose most stable ion contains 18 electrons e. member of group 17 whose most stable ion contains 10 electrons 9. Strontium consists of four isotopes with masses and their percent abundance of amu ( 0.5%), amu (9.9%), amu (7.0 %), and amu (82.6 %). Calculate the weighted average atomic mass of Strontium. Show your work. 10. Think about Group 2 on the periodic table. a. How many valence electrons do the atoms of group 2 have? b. Do the elements of group 2 lose or gain electrons when they become ions? c. What is the charge on group 2 elements when they become ions? d. How many valence electrons do group 2 elements have when they become an ion? How do you know? 11. Think about Group 17 on the periodic table. a. How many valence electrons do the atoms of group 17have? b. Do the elements of group 17 lose or gain electrons when they become ions? c. What is the charge on group 17 elements when they become ions? d. How many valence electrons do group 17 elements have when they become an ion? How do you know? Page 4 of 6

5 12. Write the formulas, with the charges, of the following ions: (Common monoatomic ions) I) Name ( Ion) Symbol( Ion) a) Sodium b) Potassium c) Cesium d) Beryllium e) Calcium f) Strontium g) Barium h) Aluminum i) Nitrogen j) Arsenic k) Oxygen l) Fluorine m) Chlorine n) Bromine o) Iodine Write the formulas (with charges) of the ions of the transition elements below: a) Chromium(III) c) Iron(II) or Ferrous d) Iron(III) or Ferric e) Cobalt(II) f) Nickel(II) or nickel g) Copper(II) or Cupric Page 5 of 6

6 Section C: Stoichiometry 1. Write complete balanced equations for each of the following: a. calcium oxide + hydrochloric acid à calcium chloride + water b. barium chloride + sodium sulfite à barium sulfite + sodium chloride c. benzene (C6H6) + oxygen à carbon dioxide + water d. lead(ii) nitrate + potassium iodide à lead(ii) iodide + potassium nitrate e. fluorine + calcium chloride à calcium fluoride + chlorine 2. Convert each of the following. Assume that all substances are at standard temperature and pressure(stp): a grams of NO 2 to liters b grams of CsI to molecules c. 2.6 x molecules of ammonium phosphate to grams d liters of carbon monoxide to moles e moles of sodium chloride to grams f moles of sodium chloride to grams 3. Tetrahydrocannabinol(THC), C21H30O2, is a psychoactive compound extracted from the resin of Cannabis sativa (marihuana, hashish). Show all of your work. a. Calculate the molar mass of THC. b. Calculate the percent composition of the elements in THC. c. What is the mass in grams of 6.66 moles of THC? d. How many molecules are there in 4.20 mg of THC? e. What is the mass of one molecule of THC? 4. Consider the reaction: N2 + 3H 2 à 2NH 3 a. How many molecules of NH 3 are produced from 30 molecules of N2? b. If you have 3 moles of N 2, how many moles of H 2 will you need to react with all of the N 2? c. If you have 50.0 L of N 2, how many Liters of NH 3 will you produce? d. How many grams of N 2 do you need to produce 28.0 g of NH 3? Page 6 of 6