We are asked which of the following statements will be true for a Lewis and Bronstead-Lowry acid.
Based on the Lewis definition:
Lewis acid is an electron pair acceptor.
Some characteristics of a Lewis acid:
• When hydrogen is connected to an electronegative element such as P, O, N, S or halogens
▪ hydrogen gains a partially positive charge → makes hydrogen act as a Lewis acid
• Positively charged metal ions
▪ can accept negative electron pairs → can act as Lewis Acids
Let’s define a Bronsted-Lowry Acid. Recall also that Bronsted-Lowry acids and bases occurs in pairs called conjugate acid/base pairs.
Bronsted-Lowry acid → proton (H+) donor
Conjugate base → one less hydrogen form of the Bronsted-Lowry acid
A large molecule X is classified as a Lewis acid, and another molecule, Y, is a Bronsted-Lowry acid. Which of the following best describes a comparable behavior in aqueous solution?
a. Both molecules will tend to acquire a net positive charge
b. Both molecules will release hydroxide ions
c. Only molecule Y will react with the water
d. Both molecules will release hydrogen gas
e. Both molecules will tend to acquire a net negative charge
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