Term
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Definition
| pKa = -log Ka
Ka is the acid dissociation constant.
Ka is the equilibrium constant for the dissociation of a weak acid.
Acid dissolves producing Hydronium ions and conjugate base
HA <--> H+ + A-
Ka = [H+][A-] / [HA]
pKa = -log Ka |
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Term
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Definition
| H+ donor
proton(H) donor
has an H+ that can be easily ripped off by a base |
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Term
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Definition
| H+ acceptor
proton (H) acceptor
able to pull off H+ from an acid |
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Definition
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Definition
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Term
| Strength of an acid is based on... |
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Definition
| ...the stability of it's conjugate base |
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Term
| strong acids have ___________ conjugate bases |
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Definition
| strong acids have stable conjugate bases |
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Term
| A weak acid has a less/more stable conjugate base than a strong acid |
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Definition
| A weak acid has a LESS stable conjugate base than a strong acid |
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Term
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Definition
| the acid once it has been deprotonated |
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Term
| Features that determine the stability of a negative charge: |
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Definition
- The electronegativity of the atom with the negative charge
- The size of the atom with the negative charge
- Stabilization of the negative charge with resonance
- Stabilization of the negative charge by adjacent electronegative atoms
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Term
| Which is more acidic?
H2 OR NH3
water ammonia |
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Definition
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Term
Which is more electronegative?
oxygen or nitrogen |
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Definition
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Term
| Negative charges prefer to rest on larger atoms because... |
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Definition
The charge can be spread over a much larger region of space.
This makes it more stable. |
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Term
Which is more acidic?
HI or HF |
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Definition
| HI
F- is more electronegative than I-, but, I- is significantly larger than F-
SIZE TRUMPS ELECTRONEGATIVTY |
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Term
| Why is phenol a million times stronger acid than cyclohexanol?
[image] |
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Definition
| Because the conjugate base of phenol is more stable than the conjugate base of cyclohexanol.
Phenol's conj base has a resonance structure. The anion can delocalize the negative charge throughout the ring through resonance. Thus stabilizing it.
Cyclohexanol's conj base has no resonance structure.
cyclohexane is a weaker acid!![image] |
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Term
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Definition
| ethanoic acid
CH3COOH
a carboxylic acid |
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Definition
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Definition
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Term
| Why is [image] the Chlorine substitued acetic acid more acidic than the hydrogen containing acetic acid? |
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Definition
| The electronegative Chlorine atom is pulling some of the electron density away from the oxygens, making the oxygens not having to bear all of the negative charge by themselves. |
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Term
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Definition
| Have the formula:
CnH2n+2
Hydrogen saturated since they have the maximum number of hydrogens possible |
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Term
| Hydrocarbons that contain a single alkene or a single ring... |
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Definition
| ...contain a single degree of unsaturation
because adding either a ring or a double bond requires the loss of two hydrogens.
CnH2n |
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Term
| Calculate the Degrees of Unsaturation |
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Definition
| Degrees of Unsaturation =
[(Number of Carbons x 2) +
2 - Number of Hydrogens]
/ 2
Halides(F, Cl, Br, I) count as hydrogens
Nitrogen counts as a 1/2 |
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Term
Double bonds add _____ degree(s) of unsaturation
Rings add _____ degree(s) of unsaturation.
Triple bonds add _____ degree(s) of unsaturation. |
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Definition
| Double bonds add ONE
Rings add ONE
Triple bonds add TWO degree(s) of unsaturation. |
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Term
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Definition
| need a definition for alkyne |
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Definition
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Definition
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Definition
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Definition
| three carbon alkyl substituent
-C3H7 |
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Term
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Definition
| also isopropanol
propan-2-ol
[image]
isomer of propanol |
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Term
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Definition
| also isopropanol
propan-2-ol
[image]
isomer of propanol |
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Term
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Definition
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Term
| first and second simplest alkene |
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Definition
| ethylene (ethene)
C2H4
propene
C3H6
[image] |
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Term
trans
cis
(high/low priority) |
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Definition
trans: opposite sides
"E"
cis: same sides
"Z" |
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Term
| bp of butane vs. bp of isobutane |
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Definition
| butane bp: -.5o
isobutane bp: -11.7o |
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Term
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Definition
| positively charged carbon atom |
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Definition
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Definition
| also called ethanyl
-CH=CH2
a derivative of ethylene
[image] |
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Term
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Definition
| -C2H5
Abbreviated -Et
[image] |
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Term
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Definition
| formula:
CnH2n+1
ex:
methyl
ethyl
butyl
etc.
very reactive when by itself. it is a free radical |
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Definition
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Definition
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Definition
same formula
different connectivity |
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Term
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Definition
same connectivity, same formula
just rotated around a bond |
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Term
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Definition
electron rich
nucleus loving |
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Term
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Definition
electron loving
electron deficient |
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Term
| What removes the mercury in an oxymercuration reaction? |
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Definition
| Sodium Boro-hydrate
NaBH4 |
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Term
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Definition
| CH3-CH2-O-CH2-CH3
[image] |
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Term
| effect of halogens and other electronegative groups |
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Definition
electron withdrawing polar effect
they will PULL electrons toward themselves and away from the carbon |
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Term
| electron donating polar effect |
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Definition
| some groups will raise the pKa or reduce the acidity of nearby carboxylic acid groups. |
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Term
| what are 2 structural effects that affect Bronsted acidity? |
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Definition
Element effect
polar effect
element effect is dominated by the change in bond dissociation energies with a column and by the change in electron effiniies within a row
polar effect: caused by the interactions of charges formed in the acid-base reaction with polar bonds or other charged groups in the acid or base molecule |
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Term
| if you have more substituents, then it is More/less stable |
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Definition
MORE stable
because of the hyperconjugation |
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