2. The following are four pairs of atoms. Consult Table 5.1 to answer these questions. N and C,N and H,S and O,S and F (Question \#5-pp214) a. What is the electronegativity difference between the atoms? b. Assume that a single covalent bond forms between each pair of atoms. Which atom attracts the electron pair in the bond more strongly? c. Arrange the bonds in orders of increasing polarity. 3. a. Draw the Lewis structure for the water molecule. b. Draw Lewis structures for the hydrogen ion and the hydroxide ion. c. Write a chemical reaction that relates all three structures from part of a and b. (Question \#10 - pp214) 4. The density of water at 0C is 0.9987g/cm3; the density of ice at this same temperature is 0.917g/cm3 (Question #11 on page 214 ) a. Calculate the volume occupied at 0C by 100.0g of liquid water and by 100.0g of ice. b. Calculate the percentage increase in volume when 100.0g of water freezes at 0C. 5. The acceptable limit for nitrate, often found in well water in agricultural areas, is 10ppm. If a water sample is found to contain 350mg/L, does it meet the acceptable limit? (Question \#18 - pp 215) 6. Solutions can be tested for conductivity using the apparatus shown in the chapter. Predict what will happen when each of these dilute solutions is tested for conductivity. Explain your predictions briefly. (Question #20 - pp215) a. CaCl2(aq) b. C2H5OH(aq) c. H2SO4(aq) 7. Classify the following aqueous solutions as acidic, neutral, or basic. (Question #26 pp215+4 extra questions) a. HI(aq) b. NaCl(aq) c. NH4OH(aq) f. [H+]=5107M d. [H+]=1108M e. [OH]=1102M g. [OH]=11012M 8. Explain how you would prepare these solutions using powdered reagents and any necessary glassware. (Question \#32 - pp215) a. Two liters of 1.50MKOH b. One liter of 0.050MNaBr