1. Chem 1151 Review Chapters 1-4

2. Chap 1 The edge of a cube is 39.3 cm. What is the volume in cm 3 ? m 3 ? gal? Note SF 1 in = 2.54 cm and 1 gal = 231 in 3 (56.1 – 51.1)/6.58 = Convert 3.18 μs to ms Pt has a density of 21.4 g/cm 3. What is the mass of a Pt sample of volume 5.0 in 3 ? 0.00015 x 54.6 + 1.002 =

3. Chap 1 Memorize T 1.2 from kilo to pico 1 cm 3 = 1 mL Density of water = 1 g/cm 3

4. Chap 2 Nuclide symbol for the species with 14 p+ and 14 n0. Nuclide symbols for ions Atomic wt for this element  Write the formulas for and name –Co 2+ and Br - –Na + and PO 4 3- –Cr 3+ and O 2- –Ca 2+ and HCO 3 - –Cs + and S 2- Mass (amu) Frac abund 84.91180.7215 86.90920.2785

5. Chap 2 Write formulas for –Nitrogen tribromide, oxygen difluoride, dichlorine pentoxide, dinitrogen tetrafluoride Laws: conservation of mass, def proportions, multiple proportions Theory: Dalton’s Atomic Theory Memorize T2.5, Fig 2.22, strong acids, bases Nomenclature rules (Types I, II, III)

6. Chap 3 Balance chem eqns Conversions from g to mol to # atoms –Convert 0.15 mol Na to g to # Na atoms –Convert 2.78 g Hg(NO 3 ) 2 to # O atoms –Convert 10.0E20 N atoms in Hg(NO 3 ) 2 to mol molecule –# Ca 2+ in 2 mol Ca 3 (PO 4 ) 2 Determine empirical formula for 50.0% C, 5.6% H, 44.4% O

7. Chap 3 3TiO 2 +4C + 6Cl 2  3TiCl 4 + 2CO 2 + 2CO –Calc g CO if 100 g TiO 2 reacts w/xs C and Cl 2 –Calculate g C needed to produce 1.0 kg TiCl 4 –If the reaction yield is 70%, how many g C are needed in previous question? –If you start with 4.15g TiO 2 and 6.78g Cl 2 and xs C, how many g of TiCl 4 will be produced? –How many g of the xs reagent (not counting C) will remain at the end of the rxn?

8. Chap 4 Memorize solubility rules, OX# rules, balancing redox rxn rules, defn of molarity Predict solubility of aqueous solns of PbS, Na 2 CO 3, Li 3 P, AgBr, BaSO 4, NH 4 Br, Fe(OH) 2, PbS, Write the net ionic eqn for aq solns of –Silver nitrate + sodium bromide –Lead(II) nitrate + potassium sulfate –Hydrobromic acid + strontium hydroxide –Sodium carbonate + magnesium iodide

9. Chap 4 What is the molarity of a 50.0 mL solution containing 0.798 g KMnO 4 ? What volume of 0.120 M CuSO 4 contains 0.150 mol solute? Prepare 1.50 L of a 0.50 M solution of HCl from 12.4 M HCl stock soln. What is the molarity of sodium ions in a 0.33 M soln of sodium phosphate?

10. Chap 4 Na 2 CO 3 (aq) + Ca(OH) 2 (aq)  CaCO 3 (s) + 2NaOH(aq) What volume of 0.350M Na 2 CO 3 is required to react with 49.8 mL of 0.150M Ca(OH) 2 ? How many g of CaCO 3 will be produced when 33.0 mL of 0.250M Na 2 CO 3 reacts with 57.0 mL of 0.200M Ca(OH) 2 ?

11. Chap 4 Determine the OX# of N in NO, NO 2, N 2 O, NH 2 -, N 2, N 2 O 5, NO 2 -, N 2 O 4 Br 2 + SO 2  Br - + SO 4 2- balance in acid MnO 4 - + I -  MnO 2 + IO 3 - bal in base In the reactions above, what is oxidized?, reduced? What is the RA?, OA? #e- transferred?

12. Chap 4 KI(aq) + AgNO 3 (aq)  KNO 3 (aq) + AgI(s) Excess silver nitrate was added to a 10.0 mL sample of KI soln. If 2.183 g AgI was produced, what is the molarity of the KI soln? If the rxn above has an 80% yield, what is the molarity of the KI soln?