ࡱ> uwty bjbj .O{{M&&d$fal\\:qqq```````$be a2qq22 a a2`2`Y4m`p)r^:\>`6a0fa?\.f8f|m`fm`dqZ@ 4?qqq a a2qqqfa2222fqqqqqqqqq& F: Problem Session 2 Chapters: 6, 7, 11, 12, 13 Directions: Answer each of the following questions in complete sentences where appropriate. Be sure to show all of your work and report your answers to the correct number of significant figures. Question 1. Given the correct IUPAC name for the following compounds a. PCl3 _____________________ b. SF6 _____________________ c. Na2SO4 _____________________ d. MnO _____________________ e. (NH4)2O _____________________ f. RbClO4 _____________________ g. Cd(CN)2 _____________________ h. N2O5 _____________________ i. Ni(HSO4)2 _____________________ j. HCl (g) _____________________ k. HCl (aq) _____________________ l. FeCl26H2O_____________________ m. Al2O3 _____________________ n. V2O5 _____________________ o. H3PO3 (aq) _____________________ p. IF5 _____________________ Question 2. Write the correct formula for the following compounds: a. Vanadium(III) chlorate _________ b. Aresenic acid _________ c. Carbon tetrachloride _________ d. Hydrocyanic acid _________ e. Iodine trichloride _________ f. Dichlorine heptoxide _________ g. Sodium hydrogen sulfate _________ h. Mercury(II) phosphate _________ i. Stannous fluoride _________ j. Bismuth(III) cyanide _________ k. Tungsten(II) nitride _________ l. Boron trichloride _________ m. Hydrogen sulfide _________ n. Disulfur dichloride _________ o. Nickel(II) fluoride _________ tetrahydrate p. Xenon tetrafluoride _________ Question 3. A dandruff shampoo contains pyrithion, C10H8N2O2S2, which acts as an antibacterial and antifungal agent. What is the empirical formula of pyrithion? What is the molar mass of pyrithion? What is the percent composition of pyrithion? How many atoms of C are in 25.0 g pyrithion? How many moles of pyrithion contain 8.2 x 1024 atoms of nitrogen? How many grams of S are in 4.56 moles of pyrithion? Question 4. A sample contains 70.6% Hg, 12.5% Cl, and 16.9% O. If it has a molar mass of about 568 g/mol, what are the empirical and molecular formulas? Question 5. A 14.1 mg sample of a hydrocarbon was burned in air. The products were 38.8 mg of CO2 and 31.7 mg of water. What is the empirical formula of the hydrocarbon? Question 6. A 0.2417 gram sample of a compound known to be composed of C, H, O and Cl only, is burned in oxygen yielding 0.4964 grams of carbon dioxide and 0.0846 grams of water. A separate 0.1696 gram sample of the compound is fused with sodium metal, the products dissolved in water and the chloride quantitatively precipitated with silver nitrate to yield 0.1891 grams of AgCl. What is the simplest empirical formula for the compound (Challenge Problem)? Question 7. Write the shorthand electronic configuration for the following: Si: ________________________________________________ Pb: ________________________________________________ Cl: ________________________________________________ Cr2+: ________________________________________________ S2-: ________________________________________________ Pb4+: ________________________________________________ Question 8. Rank the following atoms in order of increasing radius: _____ N _____ Sb _____ Rb _____ Cs _____ F Question 9. Name the element that corresponds to each of the following: alkali metal with the smallest atomic radius _____ Group 5A element with the highest ionization energy _____ [Kr] 5s24d10 _____ Question 10. Identify each bond as ionic, polar covalent, or nonpolar covalent, use Figure 12.9, page 347 of the textbook. Show the distribution of charge. Sb-H _____________________ B-H _____________________ P-F _____________________ d. Rb-Br _____________________ Question 11. Consider the following redox reaction: ___Mg (s) + ___HCl (aq) ( ___MgCl2 (aq) + ___H2 (g) Draw the Lewis structures for each reactant and product and determine which reactant was oxidized and which was reduced. Question 12. Compare the electron dot formulas of BF3 and NF3. Why do these molecules have different shapes? Question 13. If a nonmetal has 5 valance electrons, how many bonds it is most likely to form? How many lone pairs will it most likely have? Question 14. For each molecule: a) draw the Lewis structure; b) give the electron pair geometry; c) give the molecular shape; d) give the bond angle; e) identify the molecule as polar or nonpolar. Dichloromethane, CH2Cl2Gallium trihydride, GaH3Chlorate ionCyanate ion, OCN- (resonance)ClNO2 (resonance)Nitrogen dioxide ion, NO2+ Question 15. Draw Lewis structures for the following organic molecules and identify the electronic and molecular geometry around each central atom. 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