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Organic Chemistry > Ch. 2 - Acids & Bases > Flashcards

Ch. 2 - Acids & Bases Flashcards

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1
Q

What is a Bronsted-Lowry acid?

A

proton donor

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2
Q

What is a Bronsted-Lowry base?

A

proton acceptor

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3
Q

What must a BL acid have?

A

a hydrogen atom

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4
Q

What must a BL base have?

A

a lone pair or pi bond

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5
Q

What are counterions?

A

spectator ions (usually salts) that balance negative charge

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6
Q

What is the possible net charge of BL acids?

A

negative, positive or zero

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7
Q

What is the possible net charge of a BL base?

A

negative or zero

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8
Q

What is an oxyacid?

A

acid in which the protons are placed on the oxygen

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9
Q

What do you do when you see a salt in a reaction?

A

immediately split it into its ions and decide which ions are involved, make the other a spectator ion

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10
Q

What does a loss of a proton form?

A

conjugate base

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11
Q

What does the gain of a proton form?

A

conjugate acid

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12
Q

What does a starting material with a positive net charge indicate?

A

it is an acid

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13
Q

What does a starting material with a negative net charge indicate?

A

it is a base

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14
Q

What is acid strength?

A

the tendency of an acid to donate a proton

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15
Q

The stronger the acid, the ______ the Ka.

A

larger

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16
Q

The stronger the acid, the ______ the pKa.

A

smaller

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17
Q

What is the relationship between pKa and Ka?

A

pKa = -log(Ka)

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18
Q

What is the pKa range for a typical organic compound?

A

+5 to +50

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19
Q

What are the six strong acids? What are generally their pKas?

A

HCl, H2SO4, HBr, HNO3, HI, HClO4

negative pKas

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20
Q

What are the common strong bases?

A

NaOH, KOH, LiOH (anything with -OH)

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21
Q

How do you calculate Ka?

A

[products]/[reactants]

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22
Q

A strong acid forms a ______ conjugate base.

A

weak

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23
Q

A strong base forms a ______ conjugate acid.

A

weak

24
Q

What does the position of equilibrium rely on in acid/base reactions?

A

strength of acid/base

equilibrium will favor the formation of the weaker acid/base

25
Q

What is the general rule of acidity? (think stable!)

A

anything that stabilizes a conjugate base (A-) makes the starting acid more acidic

26
Q

What is the pKa of acetic acid (weak acid)?

A

5

27
Q

What is the pKa of water and alcohol?

A

16

28
Q

What is the pKa of ammonia (weak base)?

A

38

29
Q

What is the pKa of methyl amine?

A

40

30
Q

What is the pKa of methane/ethane?

A

50

31
Q

What are the four effects that make acids more acidic?

A

element, inductive, resonance, hybridization

32
Q

What is the most important factor of acidity?

A

element effects

33
Q

What are element effects?

A

the location of A (from HA) on the ptable

rows: acidity increases as A is more EN (right)
columns: acidity increases as A gets bigger (down)

34
Q

What are inductive effects?

A

presence of atoms that are more electronegative than carbon
- withdraws electron density from C, pulls through sigma bonds
- stabilizes negative charge
» acidity INCREASES with presence of electron withdrawing groups (more EN, closer to neg charge, greater the effect)

35
Q

What are resonance effects?

A

delocalization of electron density stabilizes conjugate bases and makes them weaker

acidity of HA increases when conj base is resonance stabilized

36
Q

What are hybridization effects?

A

Lower hybridization (increased % s character) = more stable conj base and acid is more acidic

37
Q

How many bonds are formed in an acid-base reaction?

A

one

38
Q

Does an atom with a filled octet have an available electron pair?

A

no

39
Q

Can unpaired electrons be used in acid-base reactions?

A

no

40
Q

Equilibrium tends to the side with a ______ Ka value?

A

smaller

41
Q

What is the correct formula for the conjugate acid of CH3NH2?

A

CH3NH3+

42
Q

What is the cause of the inductive effect?

A

the difference of EN of the atoms involved

43
Q

In an acid-base reaction, the equilibrium always favors the formation of what species?

A

weak acids and weak bases

44
Q

Acid strength is ______ by any factor that makes the conjugate base more stable.

A

increased

45
Q

What is an an electrophile?

A

an electron-deficient species

46
Q

What is a nucleophile?

A

an electron-rich species

47
Q

What is TsOH and what is it’s pKa?

A

p-toluenesulfonic acid, strong organic acid with pKa of -7

48
Q

What are the three common types of bases?

A

negative charged oxygen bases (-OH + derivatives)
negative charge nitrogen bases (-NH2 + derivatives)
hydrife (H-)

49
Q

What are pKa values of strong bases?

A

pKa > 12

50
Q

Do all strong bases have a negative charge?

A

Yes, but not all species with a negative charge are strong bases.

51
Q

What is a carbanion?

A

negatively charged carbon atom

52
Q

What is a Lewis acid?

A

electron pair acceptor

53
Q

What is a Lewis base?

A

electron pair donor

54
Q

What must a Lewis base have?

A

available electron pair or pi bonds

55
Q

T/F: All BL acids are Lewis acids?

A

True, but not all Lewis acids are BL acids

56
Q

How many bonds are broken and formed in a Lewis reaction?

A

one formed, none broken (forms lewis acid-base complex)

Organic Chemistry (26 decks)

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