Imagine each of the molecules shown below was found in an aqueous solution. Can you tell whether the solution is acidic, basic, or neutral? molecule The solution is... H3Ń ○ acidic basic O neutral ○ (unknown) H₂N CH C ○ acidic ○ basic CH2 CH3-CH-CH3 O neutral ○ (unknown) H³Ñ OH HO O acidic ○ basic O neutral ○ (unknown) H3N-CH- HO CH CH3 OH ○ acidic basic O neutral ○ (unknown)

For oxyacids, how does acid strength depend on a. the strength of the bond to the acidic hydrogen atom? b. the electronegativity of the element bonded to the oxygen atom that bears the acidic hydrogen? c. the number of oxygen atoms? How does the strength of a conjugate base depend on these factors? What type of solution forms when a nonmetal oxide dissolves in water? Give an example of such an oxide. What type of solution forms when a metal oxide dissolves in water? Give an example of such an oxide.

Use Table 13-2 to order the following from the strongest to the weakest acid. HClO2,H2O,NH4+,HClO4

1. Which of the following can act as a Lewis acid? (Hint : In each case, draw the Lewis electron dot structure of the molecule or ion. Are there lone pairs of electrons on the central atom? If so, it can be a Lewis base. Does the central atom lack an electron pair? If so, it can behave as a Lewis acid.) PH3 BCl3 H2S HS−