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Chem 31 > Module 2: Acids and Bases > Flashcards

Module 2: Acids and Bases Flashcards

1
Q

four main factors, in the following priority order, that affect the stability of the conjugate base

A
  1. Atom
  2. Resonance
  3. Induction
  4. Orbital
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2
Q

the acidity of H-A increases as the percent s-character of A increases

A

hybridization effects

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3
Q

measure of a compound’s affinity for a proton

A

basicity

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4
Q

Any species that is electron deficient and capable of accepting an electron also a?

A

lewis acid

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5
Q

The acidity relies on the stability of the?

A

conjugate base

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6
Q

Down the periodic table, the ___________________ determines the acidity

A

atomic size

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7
Q

acids that the net charge may be zero (+), or (-)

A

bronsted-lowry acids

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8
Q

The tendency of an acid to donate a proton

A

acid strength

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9
Q

these are more electronegative than p orbitals

A

s orbitals

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10
Q

Electron donor

A

lewis base

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11
Q

these contains a proton

A

all bronsted-lowry acids

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12
Q

this always favors formation of the weaker acid and base

A

equilibrium

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13
Q

the acidity of H-A inccreases both left-to-right across a row and down a column of the periodic table

A

element effects

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14
Q

this shows how greatly the acidity varied for different functional groups.

A

pKa table

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15
Q

this is the characteristic of a particular compound, which indicates the tendency of the compound to give up its proton.

A

pKa

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16
Q

Electron acceptor

A

lewis acid

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17
Q

the lewis acid is also called a ________________ or electron-rich

A

nucleophile

18
Q

Proton acceptor

A

bronsted-lowry base

19
Q

Increase the concentration of H+ions when dissolved in water

A

arrhenius acid

20
Q

the acidity of H-A increases with the presence of electron-withdrawing groups in A

A

inductive effects

21
Q

Increase the concentration of OH-ions when dissolved in water

A

arrhenius base

22
Q

this is used to describe the acidity (concentration of positively charged hydrogen ions) of a solution

A

pH scale

23
Q

The more readily the compound donates a proton, the?

A

stronger the acid

24
Q

these contain a lone pair of electrons or a pi bond

A

all bronsted-lowry base

25
Q

bases that the net charge may be zero or (-)

A

bronsted-lowry bases

26
Q

The use of curved arrows to show simple proton-transfer reactions.

A

The Lewis Definition

27
Q

Proton donor

A

bronsted-lowry acid

28
Q

the acidity of H-A increases when the conjugate base A is resonance stabilized

A

resonance effects

29
Q

An acid can be deprotonated by the conjugate base of any acid having a?

A

higher pKa

30
Q

from left to right, acidity increases as the electronegativity _________________

A

increases

31
Q

The ______________ the electronegativity, the stronger the inductive effect

A

stronger

32
Q

Structural effects on acidity and basicity of organic molecules

A

The Brønsted–Lowry Definition

33
Q

a lewis acid is also called an ________ or electron deficient

A

electrophile

34
Q

the closer the electronegative atom to the hydrogen, the stronger the?

A

acid

35
Q

this is due to differences in electronegativity (EN), the intrinsic ability of an atom to attract the shared electrons in a covalent bond

A

bond polarity

36
Q

a weaker conjugate base means a more?

A

stable conjugate base

37
Q

this is broader and more encompassing than the Bronsted-Lowry definition because it is not limited to substances that donate or accept protons only.

A

lewis definition of acids and bases

38
Q

these are structurally the same as Brønsted–Lowry bases. Both have an available electron pair—a lone pair or an electron pair in a π bond.

A

lewis bases

39
Q

measure of the tendency of a compound to give up a proton

A

acidity

40
Q

the stronger the acid, the weaker its?

A

conjugate base

Chem 31 (22 decks)

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