Chapter 2: Acids and Bases, Functional Groups

Question 1

Unit for measuring bond dipole moments?

Answer 1

debyes

Question 2

Dipole moments are due to differences in?

Answer 2

Electronegativity

Question 3

3 kinds of intermolecular forces?

Answer 3

London dispersion, hydrogen bonding, and dipole-dipole

Question 4

What are intermolecular forces?

Answer 4

Forces between MOLECULES

Question 5

What 3 things can intermolecular forces influence?

Answer 5

Boiling point, melting point, and solubility of compounds

Question 6

What kinds of molecules have dipole-dipole interactions?

Answer 6

Polar molecules

Question 7

In dipole-dipole interactions, is attraction or repulsion of the positive and negative ends more common?

Answer 7

Attractive

Question 8

What causes London dispersion forces?

Answer 8

Temporary dipoles

Question 9

What is the main intermolecular force in nonpolar molecules?

Answer 9

London dispersion forces

Question 10

How are the size of an atom and temporary dipoles related?

Answer 10

Larger atoms are more polarizable

Question 11

What is the relationship between surface area and boiling point?

Answer 11

Boiling point of a molecule increases as the surface area of the molecule increases

Question 12

What is the relationship between branching and surface area?

Answer 12

Surface area decreases if a molecule has more branching

Question 13

Organic molecules must have a BLANK bond OR a BLANK bond to form a hydrogen bond?

Answer 13

N-H OR O-H

Question 14

Are hydrogen bonds strong?

Answer 14

Yes! They’re a strong kind of dipole-dipole interaction

Question 15

Is O-H more polar than N-H?

Answer 15

Yes

Question 16

What are Arrhenius Acids?

Answer 16

Dissociate in water to form H3O+

Question 17

What are Arrhenius Bases?

Answer 17

Dissociate in water to form OH-

Question 18

What are Bronsted-Lowry acids?

Answer 18

Donate proton

Question 19

What are Bronsted-Lowry bases?

Answer 19

Accept proton

Question 20

What is a conjugate acid?

Answer 20

Species that forms when a base accepts a proton

Question 21

What is a conjugate base?

Answer 21

Species that forms when an acid donates a proton

Question 22

What does Ka stand for?

Answer 22

Acid ionization constant

Question 23

What 2 values can be used to express the extent of an acid’s ionization in water?

Answer 23

Ka and pKa

Question 24

Do acid-base reactions favor weaker acids and bases or stronger acids and bases?

Answer 24

Weaker acids and bases

Question 25

What kind of arrow is usually (BUT NOT ALWAYS, LIKE IN THE CASE OF THE 6 STRONG ACIDS and 6 STRONG BASES) used for acid-base reactions?

Answer 25

Equilibrium area

Question 26

What is the relationship between the strength of an acid and the strength of its conjugate base?

Answer 26

Inversely related

Question 27

The weaker the acid, the BLANK the pKa?

Answer 27

Larger

Question 28

The weaker the base, the BLANK the pKa?

Answer 28

Larger

Question 29

Are weaker acids and weaker bases always on the same side or different side of the equation?

Answer 29

Always on the same side; they're either both reactants or both products

Question 30

What does amphoteric mean?

Answer 30

The substance can react with an acid or a base

Question 31

What is a common amphoteric molecule?

Answer 31

Water

Question 32

What is the conjugate base of water?

Answer 32

OH-

Question 33

What is the conjugate acid of water?

Answer 33

H3O+

Question 34

What is the relationship between the electronegativity of an atom on an acid, the stability of the conjugate base of that acid, and that acid's strength?

Answer 34

If the atom is more electronegative, the conjugate base of the acid will be more stable and the acid will be stronger

Question 35

When do you use electronegativities when comparing acid strength?

Answer 35

When you are comparing atoms in the same row/period

Question 36

When do you use atomic size when comparing acid strength?

Answer 36

When you are comparing atoms in the same group/column

Question 37

What is the relationship between the size of an atom, strength of the acid, and the stability of the conjugate base?

Answer 37

As the size of the atom increases, the strength of the acid increases due to increased stability of the conjugate base

Question 38

What do electron-withdrawing atoms and groups do to conjugate bases? What is this called?

Answer 38

They stabilize the conjugate base, and this is called an inductive effect

Question 39

What 3 factors does the magnitude of an inductive effect depend on?

Answer 39

The distance between the electronegative element and the site of the negative charge, the strength of the electron-drawing group, and the number of electron-withdrawing groups

Question 40

More "s" character in hybridization leads to a more stable BLANK and stronger BLANK

Answer 40

More stable conjugate base and therefore stronger acid

Question 41

What is the effect of resonance on acid strength?

Answer 41

The more resonance structures possible for the conjugate base, the more delocalized the negative charge is, the more stable the conjugate base, and the stronger the original acid

Question 42

What is a Lewis base/nucleophile?

Answer 42

Have available electrons to donate

Question 43

What is a Lewis acid/electrophile?

Answer 43

Accepts pair of electrons from nucleophile

Question 44

When breaking a bond, which atom receives the electrons?

Answer 44

The more electronegative atom

Question 45

When forming a bond, what is the direction of the arrow?

Answer 45

Negative to positive

Question 46

6 types of hydrocarbons?

Answer 46

alkanes, cycloalkanes, alkenes, cyclo alkenes, alkynes, aromatic