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Wade (6e) Study Problem 1-25 Draw a Lewis structure for each species. (a) N2H4 (b) N2H2 (c) (CH3)4NCl (d) CH3CN (e) CH3CHO (f) CH3S(O)CH3

(g) H2SO4 (h) CH3NCO (i) CH3OSO2OCH3 (j) CH3C(NH)CH3 (k) (CH3)3CNO Solutions Your Lewis structure may look different from these. As long as the atoms are connected in the same order and by the same type of bond, they are equivalent structures. For now, the exact placement of the atoms on the page is significant.

1-26 Draw a Lewis structure for each compound. Include all nonbonding pairs of electrons.

(a) CH3CHCHCH2CHCHCOOH (b) NCCH2COCH2CHO (c) CH2CHCH(OH)CH2CO2H (d) CH3CH(CH3)CH2C(CH2CH3)2CHO

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1-27 Draw a line-angle formula for each compound in 1-26. Solutions In each set below, the second structure is a more correct line formula. Since chemists are human(surprise!), they will take shortcuts where possible; the first structure in each pair uses a common abbreviation, either COOH or CHO. Make sure you understand that COOH does not stand for C—O—O—H. Likewise for CHO.

1-28 Draw Lewis structures for

(a) two compounds of formula C4H10 (b) two compounds of formula C2H7N (c) three compounds of formula C3H8O2 (d) two compounds of formula C2H4O

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Solutions Resonance forms must have atoms in identical positions. If any atom moves position, it is a different structure.

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Study Problems

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