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Stage 1 Pharmacy > Chemistry > Flashcards

Chemistry Flashcards

1
Q

Antacid

A

A weak base

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2
Q

Arrhenius Theory

A

Acid - proton donor

Base - hydroxyl donor

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3
Q

Brønsted-lowry theory

A

Acid - proton donator
Base - proton acceptor
Water is amphoteric
Strong acid- strong tendency to give up proton
Weak acid- weak tendency to give up proton

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4
Q

Lewis theory

A

Lewis acid - electron pair acceptor
Lewis base - electron pair donor
Both combine to make adduct
Uses valence electron (outer e-)

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5
Q

pH and [H3O+] equation?

A 
pH= -log[H3O+] 
[H3O+]= 10-pH
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6
Q

Kw equation and what is it at 25°C?

A

Kw= [H3O+][OH-]

25°C kw is 1x10-14

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7
Q

Strong acids? Strong base?

A

HCL HBr HI H2SO4

NaOH KOH

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8
Q

Weak acid? Weak base?

A

Acetic acid (ethanoic acid) HF H2O

NH3 HS- H2O

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9
Q

Ka and pKa equation?

A

Ka= [H3O+][A-] ÷ [HA]

pKa= -logKa Ka= 10-pKa

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10
Q

Acid strength of pKa?

A

The stronget the acid the lower the pKa

The weaker the acid the higher the pKa

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11
Q

pH and pKa ionisation?

A 
Acids
pH = pKa 50% ionized 
pH = pKa +1 90%
pH = pKa +2 99%
pH = pKa +3 99.9%

Base
pH = pKa 50% 
pH = pKa -1 90%
pH = pKa -2 99%
pH = pKa -3 99.9%
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12
Q

What is pKa?

A

Measure of how easily a molecule will release a proton

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13
Q

Electronegativity?

A

The ability of an atom to pull bonding electrons towards itself. F is most electronegative

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14
Q

Hybridization

A

Promoting an electron to an empty p orbital to form an sp3 orbital

2e- = linear = 180° = sp 
3e- = trigonal planar = 120° = sp2 
4e- = tetrahedral = 109.5° = sp3

Single bond is sigma
Double bond is one sigma and one pie bond

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15
Q

Buffer?

A

The ability to resist changes in pH upon the addition of small amounts of either acid or base
Equivalence point is when the pH and Base are at the same point

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16
Q

Henderson Hasselbalch equation

A

pH = pKa + log ([conjugate base] ÷ [acid])

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17
Q

Alkane pKa

A

> 50

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18
Q

Alkynes pKa

A

44

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19
Q

First law of thermodynamics

A

Energy can’t be created or destroyed, it can only be converted from one form to another

20
Q

Energy equation

A

Change in energy = final - initial

21
Q

Exothermic and Endothermic

A

A change that releases heat = decrease in enthalpy (negative number)

A change that absorbs heat = increase in enthalpy (positive number)

22
Q

Heat capacity equation

A

Q= C x change in T

23
Q

Rate equation and arrhenius equation

A

Rate = k[A]n[B]m

K = Ae^(-Ea/RT)

23
Q

Alcohol pKa

A

15.5-18

Water is 15.7

24
Q

How to prioritise atoms attached naming it R/S?

A 
Drawn in 3D
Prioritise using atomic number 
Make sure 4th atom at back 
Clockwise = R
Anticlockwise = S
25
Q

2 exceptions for enantomers?

A

Plane polarised light filters it

Optical activity

26
Q

Meso stereoisomers

A

Molecules with 2 identical chiral carbon atoms have 3 stereoisomers

27
Q

Separating enantiomers?

A

Resolution- separation from racemic mixture or enantiomerically enriched mixture. One crystallised and filtered and other evaporated

Chiral chromatography- racemic solution is passed over chiral stationary phase giving rapid and reversible diastereotopic interaction

28
Q

Lipinski rule?

A

No more than 5 h bond donors
No more than 10 h bond acceptors
Molecular weight under 500 dalton’s
Partition coefficient log P less than 5

Used for assessing drug likeness and suitability for oral administration

29
Q

Phenol pKa

30
Q

Carboxylic acid pKa

31
Q

Anomer

A

2 sugars that’s differ in configuration at the carbon that’s the C=O in the open chain form

32
Q

Separation of amino acids?

A

pI separation by electrophoresis
By polarity - chromatography
In exchange chromatography

33
Q

Amide pKa

A

Neutral 35

RCO2H 5

34
Q

Semi-synthetic substance

A

Some compounds either can not be purely synthesized or can not be isolated from natural sources in low cost. Therefore, the natural intermediate of such drugs could be used for the synthesis of a desired product

35
Q

HCl pKa

36
Q

Inductive effect

A

An atoms ability to polarise a bond

can cause polarisation

37
Q

pH of abdomen

A

Stomach - 1-3
Small intestines - 6-7.5
Large intestines - 7-8
Colon - 5-7

38
Q

Carboxylic derivative reactivity order

A 
OH (carboxylic acid)
Cl (acid chloride)
OC(O)R' (anhydride)
OR' (ester)
NR2 (amide)
39
Q

water pKa

40
Q

H3O pKa

41
Q

Single, double and triple

A

Single - sigma
Double - 1 sigma, 1 pie
Triple - 1 sigma, 2 pie

42
Q

SN1 vs SN2

A

SN1 forms and intermediate whereas SN2 doesn’t

43
Q

Second law of thermodynamics

A

Entropy of the universe increases in a spontaneous process and remains unchanged in an equilibrium process

44
Q

HLB

A

more soluble in water if more than 10

Stage 1 Pharmacy (6 decks)

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