Lecture 5: Introduction to Acids and Bases

Question 1

Bronsted-Lowry definition of Acid

Answer 1

Proton Donor

Question 2

Bronsted-Lowry definition of Base

Answer 2

Proton Acceptor

Question 3

Lewis definition of Acid

Answer 3

Electron pair acceptor

Question 4

Lewis definition of Base

Answer 4

Electron pair donore.

Question 5

Transfer of a proton from an acid to a base.

Answer 5

Proton Transfer Reaction

Question 6

An acid donates a proton and becomes a _____

Answer 6

Conjugate Base

Question 7

A Lewis acid is one of these:

Answer 7

Electrophile

Question 8

A Lewis base is one of these:

Answer 8

Nucleophile

Question 9

The measure of a molecule’s tendency to lose a proton.

Answer 9

Acidity

Question 10

The measure of a molecule’s affinity for a proton

Answer 10

Basicity

Question 11

The stronger the acid, the _____ the conjugate base

Answer 11

Weaker

Question 12

In an acid/base reaction, equilibrium favors the side of the reaction producing the _____ acid.

Answer 12

Weaker

Question 13

The level to which an acid dissociates in an aqueous environment.

Answer 13

Ka

Question 14

Ka values _____ as the strength of the acid increases.

Answer 14

Increase

Question 15

The amount of [H+] or [H3O+] present in aqueous solutions.

Answer 15

pH

Question 16

Has the ability to act as an acid or base under certain circumstances.

Answer 16

Amphoteric

Question 17

A _____ acid produces a weak conjugate base.

Answer 17

Strong

Question 18

Acidity increases across a row as the _____ increases.

Answer 18

Electronegativity

Question 19

Acidity increases as the atomic radius of the element _____

Answer 19

increases

Question 20

Aluminum and Boron are only present in _____ acids

Answer 20

Lewis

Question 21

Lewis Acid/Base reactions always have ____ product(s)

Answer 21

1

Question 22

Bronsted-Lowry Acid/Base reactions always have _____ product(s)

Answer 22

2