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8 Chemical Bonding Solutions to Exercises (a) TiCl4, metal and nonmetal, Ti(IV) is a relatively high oxidation state, molecular (by contrast with which is definitely ionic), titanium tetrachloride metal and nonmetal, ionic, calcium fluoride (b) two nonmetals, molecular, chlorine trifluoride VF₃, metal and nonmetal, ionic, vanadium(III) fluoride (c) SbCl₅, metalloid and nonmetal, molecular, antimony pentachloride AIF₃, metal and nonmetal, ionic, aluminum fluroide Lewis Structures; Resonance Structures (sections 8.5 and 8.6) 8.47 Analyze. Counting the correct number of valence electrons is the foundation of every Lewis structure. Plan/Solve. (a) Count valence electrons: 4 + (4 1) = 8 4 pairs. Follow the procedure in Sample Exercise 8.6. H H-Si-H H (b) Valence electrons: 4 + = 10 5e⁻ pairs (c) Valence electrons: [6 + (2 = 20 10 pairs i. Place the S atom in the middle and connect each F atom with a single bond; this requires pairs. ii. Complete the octets of the F atoms with nonbonded pairs of electrons; this requires an additional pairs. iii. The remaining pairs complete the octet of the central (d) (Draw the structure that obeys the octet rule, for now.) 32 valence 16 pairs H (e) Follow Sample Exercise 8.8. 20 valence 10 e- pairs (f) 14 valence 7 e- pairs H Check. In each molecule, bonding e- pairs are shown as lines, and each atom is surrounded by an octet of electrons (duet for H). 203