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Module 1 > Pharm Chem > Flashcards

Pharm Chem Flashcards

1
Q

Solid - Gas

A

Sublimation

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2
Q

Plasma - Gas

A

Recombination

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3
Q

Liquid - Gas

A

Vaporization

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4
Q

Solid - Liquid

A

Melting

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5
Q

Gas - Solid

A

Deposition

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6
Q

Gas - Plasma

A

Ionization

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7
Q

Gas - Liquid

A

Condensation

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8
Q

Liquid - Solid

A

Freezing

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9
Q

Another words of melting

A

Fusion/Liquefaction/Thawing

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10
Q

Employed in distillation (Rotary Evaporator)

A

Vaporization and Condensation

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11
Q

Simplest form of substance

A

Element

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12
Q

> 2 elements chemically united (separated via chemical means)

A

Compound

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13
Q

> 2 substance wherein individual substance identifies are retained (separated via physical means): alcohol + water via distillation

A

Mixture

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14
Q

Example of extrinsic property

A

Length, mass/weight, volume, pressure, entropy, enthalpy, electrical resistance

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15
Q

Example of intrinsic property

A

Density/Spgr, Viscosity, Velocity, Temperature, Color

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16
Q

Mass/Matter is always constant (neither created nor destroyed)

A

Law of Conservation of Mass/Matter by Antoine Lavoisier

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17
Q

Elements combine in fixed ratio to form compounds.

A

Law of Definite/Constant Proportions by Proust’s Law

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18
Q

When 2 elements form >1 compounds, it can be expressed in a fixed whole number (by mass)

A

Law of Multiple Proportions by John Dalton

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19
Q

Proportions by weight when chemical reaction takes place can be expressed in small integral unit.

A

Law of Combining Weights

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20
Q

Atomos “indivisible”

A

Democritus

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21
Q

Billiard ball model

A

John Dalton

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22
Q

Plum Pudding/Raisin bread

A

JJ Thompson

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23
Q

Nuclear Gold Foil/ a-scat

A

Ernest Rutherford

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24
Q

Planetary model

A

Neil Bohr

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25
Q

Quantum mechanical/electron cloud

A

Erwin Schrodinger

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26
Q

Who discovered proton?

A

Ernest Rutherford

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27
Q

Who discovered the electron?

A

JJ Thompson & R.A Millikan

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28
Q

Oil drop experiment: Measure accurate charge & mass of electron

A

R.A Millikan

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29
Q

Who discovered neutron?

A

James Chadwick

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30
Q

Cathode ray tube: electron m/z ratio

A

JJ Thompson

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31
Q

Who discovered anode rays?

A

Eugene Goldstein

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32
Q

Particle separation based on electron

A

Electrochemistry

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33
Q

Separation of compounds based on electrophoretic mobility

A

Capillary Electrophoresis

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34
Q

Anode undergoes?

A

Oxidation

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35
Q

Cathode undergoes?

A

Reduction

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36
Q

What is ISOTOPES?

A

Same proton/atomic number/element but different in atomic mass

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37
Q

What is ISOBARS?

A

Same atomic mass but different elements

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38
Q

What is ISOTONES?

A

Same neutrons but different elements

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39
Q

What is ISOMERS?

A

Same molecular formula but different structure

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40
Q

What are the main isotopes?

A

H, C, N, S, Cl, O, Br

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41
Q

Aggregate of >2 atoms in definite arrangement held together by chemical bonds.

A

Molecules

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42
Q

Strongets IFA and examples

A

Hydrogen bonding

ex. H+S,O,N,X

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43
Q

Weakest IFA and examples

A

London Dispersion

ex. Aromatics (Benzene - Benzene)

ID-ID

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44
Q

Example of Keesom orientation

A

Water-Water
D-D

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45
Q

Example of Debye

A

Water-Benzene
D-ID

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46
Q

What type of bond is non metal+ non metal (glycosidic & peptide bond)

A

Covalent Bond

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47
Q

What type of bond is metal + non metal (NaCl)

A

Ionic bond

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48
Q

Ether bond is?

A

Glycosidic bond

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49
Q

Peptide bond is?

A

Amide bond

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50
Q

Pair of valence electron that are not shared with another atom in covalent bond

A

Lone Pair

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51
Q

What angle is linear? and its example?

A

180°
Alkynes (sp)
CO2

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52
Q

What angle is trigonal planar? and its example?

A

120°
Alkenes (sp²)

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53
Q

What angle is tetrahedral bent? and its example?

A

109.5°
Alkanes (sp³)
CCl4
H20

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54
Q

What are the exception to the octet rule?

A

Trigonal Bipyramidal
Octahedral

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55
Q

States that bond are formed by sharing of electron from overlapping atomic orbitals (covalent)

A

Valence Bond Theory

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56
Q

States that bonds are formed from interaction of atomic orbitals from molecular orbitals.

A

Molecular Orbital Theory

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57
Q

stronger bond; headways overlap

A

o bond
s = spherical

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58
Q

weaker bond; sideways overlap

A

π bond
p = dumbbell

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59
Q

Bonding & antibonding

A

Molecular orbitals

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60
Q

It is stable, ground state, bonding pair

A

Lower energy

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61
Q

It is unstable, excited state, antibonding

A

Higher energy

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62
Q

A + B —> AB
(Ammonia Production/Haber’s Process)

A

Synthesis/Combination/Direct Union

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63
Q

AB —> A+B

A

Decomposition/Analysis

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64
Q

AB + X —> AX + B

A

Single Displacement

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65
Q

AB + CD —> AC + BD

A

Double Displacement/Metathesis/Exchange

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66
Q

Reaction between acid & base to produce salt & H2O

A

Neutralization

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67
Q

Reaction with O2 in the presence of heat

A

Combustion

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68
Q

Reactivity Series of metal

A

Li > K > Ba > Ca > Na > Mg > Al > Mn > Zn > Cr > Fe > Cd > Co > Ni > Sn > Pb> H2 > Cu > Ag > Hg > Pt > Au

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69
Q

Reactivity Series of non metal

A

F > Cl > Br > I

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70
Q

Avogadro’s number:
1 mole = ?

A

6.022 x 10²³

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71
Q

Formula of Molarity/Formality

A

M = n solute/L solution

72
Q

Formula of Molality

A

M = n solute/kg solvent

73
Q

Formula of Normality

A

N = GEW/L or M × f

74
Q

It shows how the electrons are distributed among the various atomic orbitals in an atom.

A

Electronic Configuration

75
Q

Atoms may be built by progressive filling of energy of main energy sub level

A

Aufbau Principle

76
Q

Magic Number

A

1223343 454564567 567 677

*Si Susi Pumasok Sa Pinto
*Si Daddy Pumasok Sa Door
*Pumasok Si Father Daddy (2x)
*Pumasok Father Daddy Father

77
Q

Main energy level; size of orbital (e- cloud), distance of e- from nucleus

A

Principal (n = 1 to 7)

78
Q

Angular momentum & shape of orbital; subshell

A

Azimuthal ( l = 0 to 3 )

79
Q

Orientation; charge ( + or - )

A

Magnetic (ml)

80
Q

Magnetic moment/Rotation; direction of spin

A

Spin (ms)

81
Q

No unpaired electron

A

Diamagnetism

82
Q

At least 1 unpaired electron

A

Paramagnetism

83
Q

No two electrons will have same set of quantum number (exclusive)

A

Pauli’s Exclusion Theory

84
Q

Debunks Erwin Schrodinger (electron cloud model of an atom)
Impossible to predict/accurately determine the particles velocity (position & momentum)

A

Heisenberg’s Uncertainty Theory

85
Q

Orbitals are filled up singly before pairing up

A

Hund’s Rule

86
Q

Boyle’s Law constant & formula

A

T (in K)
P1V1 = P2V2

87
Q

Charles Law constant & formula

A

P (in atm)
T1/V1 = T2/V2

88
Q

Gay Lussac’s law constant & formula

A

V (in L)
P1/T1 = P2/T2

89
Q

Combined gas

A

P1V1/T1 = P2V2/T2

90
Q

Ideal gas (Universal gas constant)

A

R = 0.08205

91
Q

Ideal gas formulas

A

PV = nRT
M = n solute/L
P = MRT

92
Q

Avogadro’s formula

A

V1/n1 = V2/n2

93
Q

Mixture of non-interacting gases exerts a pressure that is the sum of their individual pressures.
Pt = P1 + P2 + P3 + …..

A

Dalton’s Law of Partial Pressure

94
Q

Effusion (& diffusion) rate of 2 gases are inversely proportional to the square roots of their densities providing the temp & pressure are same for 2 gases.

A

Grahams

95
Q

Rate at which 2 gases mix

A

Diffusion

96
Q

Rate at which gas escapes through a pinhole in vacuum.

A

Effusion

97
Q

Diffusion rate (flux) of liquid or gas is directly proportional to the concentration gradient (from high to low concentration)

A

Fick’s 1st Law

98
Q

Decrease temperature, increase pressure (i.e., sealed container), more CO2 is dissolved in water.

A

Henry’s

99
Q

How to get °C

A

°C = (°F-32)/1.8

100
Q

How to get °F?

A

°F = (°C x 1.8) + 32

101
Q

How to get °F?

A

°F = (°C x 1.8) + 32

102
Q

How to get K?

A

K = °C + 273.15

103
Q

Study of energy conversion/transformation in the universe

A

Thermodynamics

104
Q

Isolated from the rest by boundary or wall

A

System

105
Q

Everything outside the system

A

Surrounding

106
Q

If 2 systems are in thermal equilibrium respectively with a 3rd system, they must be in thermal equilibrium with each other.

A

Zeroth Law

107
Q

Energy/Mass are always constant! (neither created nor destroyed but can be transformed from one form to another)

A

1st Law of Thermodynamics: Law of Conservation of Energy

108
Q

Enthalpy (heat/reaction energy) change is independent of reactions/steps that occurred (only the initial & final steps would be the basis)

A

Hess’s Law

109
Q

Cold (absorbed heat)

A

Endothermic Reaction (+/_\H)

110
Q

Hot (release heat)

A

Exothermic reaction (-/_\H)

111
Q

For an isolated system, total entropy can never decrease over time.
No way but up

A

2nd Law of Thermodynamics: Law of Entropy

112
Q

Measure of systems’ thermal energy per unit temp; disorderliness or randomliness

A

Entropy (/_\S)

113
Q

Increase (irreversible) - real case

A

/_\S (+) Spontaneous

114
Q

Constant (reversible) - ideal case (in a steady state/equilibrium)

A

/_\S (-) Non-spontaneous

115
Q

If an object reaches absolute zero temperature, its atoms will stop moving.
Entropy of perfectly crystalline substance is zero!

A

3rd Law of Thermodynamics

116
Q

Thermodynamics state function that combines entropy & enthalpy

A

Gibb’s Free Energy

117
Q

Formula of Gibb’s Free Energy

A

/\G = /\H - T/_\S

118
Q

/_\G = 0:

A

Equilibrium

119
Q

/_\G (-):

A

Spontaneous

120
Q

/_\G (+):

A

Non spontaneous

121
Q

Study of reaction rates and reaction mechanism

A

Chemical Kinetics

122
Q

reactant —> product

A

reaction mechanism

123
Q

Change in reactant or product concentration with time

A

Reaction rate (M/s)

124
Q

Expresses the relationship of reaction rate to rate constant (k) & reactant concentrations raised to some power.

A

Rate Law

125
Q

What are the reaction rate theories?

A

Collision Theory
Transition State Theory

126
Q

Reaction rate is proportional to the number of collisions per time

A

Collision Theory

127
Q

Requirements for effective collision

A

Proper Orientation
Activation Energy

128
Q

Minimum amount of energy require to initiate chemical reaction

A

Activation Energy

129
Q

Rate depends on activation energy require to form intermediate/transition state (where new bonds formed & old bonds broken)

A

Transition State Theory

130
Q

Factors affecting Reaction Rate

A

•Reactant’s nature
• Concentration (except: zero order)
• Catalyst
•Surface area
•Temperature

131
Q

Speeds up the chemical reaction by lowering Ea

A

Enzyme

132
Q

Reaction rate is proportional to the product of the concentrate of the reactants to the power of its coefficient in a balanced equation

A

Law of Mass Action

133
Q

Keq = 1:

A

No shift or Equilibrium

134
Q

Keq > 1:

A

Favors product formation (to the right forward)

135
Q

Keq < 1:

A

Favors reactant formation (to the left backward)

136
Q

If an external stress is applied to a system at equilibrium, the system adjusts to partially offset the stress as the system reaches a new equilibrium.

A

Le Chatelier’s Principle

137
Q

Taste of acids

A

Sour

138
Q

Taste of bases

A

Bitter

139
Q

pH of acids

A

<7

140
Q

pH of bases

A

> 7

141
Q

Hard soap manufacture

A

NaOH

142
Q

Soft soap manufacture

A

KOH

143
Q

Bronsted Lowry in acid

A

Proton donor

144
Q

Bronsted Lowry in base

A

Proton acceptor

145
Q

Lewis in acid

A

Electron acceptor

146
Q

Lewis in base

A

Electron donor

147
Q

Thermodynamically stronger interaction

A

Hard-Hard/Soft-Soft

148
Q

Thermodynamically weaker interaction

A

Hard-Soft/Soft-Hard

149
Q

Hard acid + Hard base

A

Ionic complexes

150
Q

Soft acid + Soft base

A

Covalent complexes

151
Q

Resist pH change upon addition of small amounts of either acid or base

A

Buffer solution

152
Q

Buffer capacity

A

Van Slyke

153
Q

Number of grams of solute dissolved in 1L of saturated solution

A

Solubility

154
Q

Number of moles of solute dissolved in 1L of saturated solution

A

Molar solubility

155
Q

Q < Ksp

A

Unsaturated

156
Q

Q = Ksp

A

Saturated

157
Q

Q > Ksp

A

Supersaturated

158
Q

Dissolution rate is directly proportional to the solute surface area, solute concentration at boundary layer & diffusion coefficient

A

Noyes Whitney Equation

159
Q

Ability to be pounced into thin sheets

A

Malleable

160
Q

Ability to be drawn into wires

A

Ductile

161
Q

What elements are s&p block

A

Representative elements

162
Q

What element is d block?

A

Transition elements

163
Q

What element is f block?

A

Actinides & Lanthanides (Inner transition elements)

164
Q

Energy required to remove electron in neutral atom.

A

Ionization potential/energy

165
Q

Energy released when neutral atom gains extra electron

A

Electron affinity

166
Q

Atom’s ability to attract electron to itself.

A

Electronegativity

167
Q

Most electronegative

A

F

168
Q

2nd most electronegative

A

O2

169
Q

Electron found in outermost shell

A

Valence electron

170
Q

What are the 3 triad?

A

Iron triad
Light triad
Heavy triad

171
Q

Densiest metal

A

Os

172
Q

Discovered transuranic elements: >U exhibit radioactivity

A

Glenn Seaborg

173
Q

What are the 4 new elements?

A

Nihonium
Moscovium
Tennessine
Oganesson

174
Q

They can penetrate body tissues

A

Beta & Gamma

175
Q

Most penetrating
Photon of electromagnetic radiation

A

Gamma

Module 1 (4 decks)

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