Chapter 17.9, Problem 17P

In the following compounds, the C atoms form a single ring.Draw a Lewis structure for each compound, identify cases for which resonance exists, and determine the carbon-carbon bondorder(s): (a) C₃H₄; (b) C₃H₆; (c) C₄H₆; (d) C₄H₄; (e) C₆H₆.

Draw the Lewis structure with lowest formal charges, and determine the charge of each atom in (a) OCS; (b) NO. (C)CN−; (d) ClO−.

Draw the complete Lewis structure of (CH3)2CHCH(NH2)CO2H and identify all H-bond donors and all H-bond acceptors.

From their Lewis structures, determine the number of sand p bonds in each of the following molecules or ions:(a) CO2; (b) cyanogen, 1CN22; (c) formaldehyde, H2CO;(d) formic acid, HCOOH, which has one H and two O atomsattached to C.

Draw the Lewis structure with lowest formal charges, and determine the charge of each atom in (a) OCS; (b) NO.

The carbon–carbon bond length in C2H2 is 1.20 Å, that inC2H4 is 1.34 Å, and that in C2H6 is 1.53 Å. Near which ofthese values would you predict the bond length of C2 tolie? Is the experimentally observed value, 1.31 Å, consistent with your prediction?

Write the Lewis structure for each of the following species,and indicate the structure of each: (a) SeO32 - ; (b) S2Cl2;(c) chlorosulfonic acid, HSO3Cl (chlorine is bonded tosulfur).

.For anion NO2-, (a) predict the stereochemistry. Justify your prediction with VSEPR theory and by formal charge; (b) indicate the hybridization appropriate to the stereochemistry; (c) describe the bond character of N-O for the resonance structure.

Like several other bonds, carbon-oxygen bonds havelengths and strengths that depend on the bond order. Draw Lewis structures for the following species, and arrange them in order of increasing carbon-oxygen bond length and then by increasing carbon-oxygen bond strength: (a) CO; (b) CO₃²⁻; (c) H₂CO;(d) CH₄O; (e) HCO₃(H attached to O).