Pharm Chem Flashcards
1
Q
Solid - Gas
A
Sublimation
2
Q
Plasma - Gas
A
Recombination
3
Q
Liquid - Gas
A
Vaporization
4
Q
Solid - Liquid
A
Melting
5
Q
Gas - Solid
A
Deposition
6
Q
Gas - Plasma
A
Ionization
7
Q
Gas - Liquid
A
Condensation
8
Q
Liquid - Solid
A
Freezing
9
Q
Another words of melting
A
Fusion/Liquefaction/Thawing
10
Q
Employed in distillation (Rotary Evaporator)
A
Vaporization and Condensation
11
Q
Simplest form of substance
A
Element
12
Q
> 2 elements chemically united (separated via chemical means)
A
Compound
13
Q
> 2 substance wherein individual substance identifies are retained (separated via physical means): alcohol + water via distillation
A
Mixture
14
Q
Example of extrinsic property
A
Length, mass/weight, volume, pressure, entropy, enthalpy, electrical resistance
15
Q
Example of intrinsic property
A
Density/Spgr, Viscosity, Velocity, Temperature, Color
16
Q
Mass/Matter is always constant (neither created nor destroyed)
A
Law of Conservation of Mass/Matter by Antoine Lavoisier
17
Q
Elements combine in fixed ratio to form compounds.
A
Law of Definite/Constant Proportions by Proust’s Law
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
19
Q
Proportions by weight when chemical reaction takes place can be expressed in small integral unit.
A
Law of Combining Weights
20
Q
Atomos “indivisible”
A
Democritus
21
Q
Billiard ball model
A
John Dalton
22
Q
Plum Pudding/Raisin bread
A
JJ Thompson
23
Q
Nuclear Gold Foil/ a-scat
A
Ernest Rutherford
24
Q
Planetary model
A
Neil Bohr
25
Quantum mechanical/electron cloud
Erwin Schrodinger
26
Who discovered proton?
Ernest Rutherford
27
Who discovered the electron?
JJ Thompson & R.A Millikan
28
Oil drop experiment: Measure accurate charge & mass of electron
R.A Millikan
29
Who discovered neutron?
James Chadwick
30
Cathode ray tube: electron m/z ratio
JJ Thompson
31
Who discovered anode rays?
Eugene Goldstein
32
Particle separation based on electron
Electrochemistry
33
Separation of compounds based on electrophoretic mobility
Capillary Electrophoresis
34
Anode undergoes?
Oxidation
35
Cathode undergoes?
Reduction
36
What is ISOTOPES?
Same proton/atomic number/element but different in atomic mass
37
What is ISOBARS?
Same atomic mass but different elements
38
What is ISOTONES?
Same neutrons but different elements
39
What is ISOMERS?
Same molecular formula but different structure
40
What are the main isotopes?
H, C, N, S, Cl, O, Br
41
Aggregate of >2 atoms in definite arrangement held together by chemical bonds.
Molecules
42
Strongets IFA and examples
Hydrogen bonding
ex. H+S,O,N,X
43
Weakest IFA and examples
London Dispersion
ex. Aromatics (Benzene - Benzene)
ID-ID
44
Example of Keesom orientation
Water-Water
D-D
45
Example of Debye
Water-Benzene
D-ID
46
What type of bond is non metal+ non metal (glycosidic & peptide bond)
Covalent Bond
47
What type of bond is metal + non metal (NaCl)
Ionic bond
48
Ether bond is?
Glycosidic bond
49
Peptide bond is?
Amide bond
50
Pair of valence electron that are not shared with another atom in covalent bond
Lone Pair
51
What angle is linear? and its example?
180°
Alkynes (sp)
CO2
52
What angle is trigonal planar? and its example?
120°
Alkenes (sp²)
53
What angle is tetrahedral bent? and its example?
109.5°
Alkanes (sp³)
CCl4
H20
54
What are the exception to the octet rule?
Trigonal Bipyramidal
Octahedral
55
States that bond are formed by sharing of electron from overlapping atomic orbitals (covalent)
Valence Bond Theory
56
States that bonds are formed from interaction of atomic orbitals from molecular orbitals.
Molecular Orbital Theory
57
stronger bond; headways overlap
o bond
s = spherical
58
weaker bond; sideways overlap
π bond
p = dumbbell
59
Bonding & antibonding
Molecular orbitals
60
It is stable, ground state, bonding pair
Lower energy
61
It is unstable, excited state, antibonding
Higher energy
62
A + B ---> AB
(Ammonia Production/Haber's Process)
Synthesis/Combination/Direct Union
63
AB ---> A+B
Decomposition/Analysis
64
AB + X ---> AX + B
Single Displacement
65
AB + CD ---> AC + BD
Double Displacement/Metathesis/Exchange
66
Reaction between acid & base to produce salt & H2O
Neutralization
67
Reaction with O2 in the presence of heat
Combustion
68
Reactivity Series of metal
Li > K > Ba > Ca > Na > Mg > Al > Mn > Zn > Cr > Fe > Cd > Co > Ni > Sn > Pb> H2 > Cu > Ag > Hg > Pt > Au
69
Reactivity Series of non metal
F > Cl > Br > I
70
Avogadro's number:
1 mole = ?
6.022 x 10²³
71
Formula of Molarity/Formality
M = n solute/L solution
72
Formula of Molality
M = n solute/kg solvent
73
Formula of Normality
N = GEW/L or M × f
74
It shows how the electrons are distributed among the various atomic orbitals in an atom.
Electronic Configuration
75
Atoms may be built by progressive filling of energy of main energy sub level
Aufbau Principle
76
Magic Number
1223343 454564567 567 677
*Si Susi Pumasok Sa Pinto
*Si Daddy Pumasok Sa Door
*Pumasok Si Father Daddy (2x)
*Pumasok Father Daddy Father
77
Main energy level; size of orbital (e- cloud), distance of e- from nucleus
Principal (n = 1 to 7)
78
Angular momentum & shape of orbital; subshell
Azimuthal ( l = 0 to 3 )
79
Orientation; charge ( + or - )
Magnetic (ml)
80
Magnetic moment/Rotation; direction of spin
Spin (ms)
81
No unpaired electron
Diamagnetism
82
At least 1 unpaired electron
Paramagnetism
83
No two electrons will have same set of quantum number (exclusive)
Pauli's Exclusion Theory
84
Debunks Erwin Schrodinger (electron cloud model of an atom)
Impossible to predict/accurately determine the particles velocity (position & momentum)
Heisenberg's Uncertainty Theory
85
Orbitals are filled up singly before pairing up
Hund's Rule
86
Boyle's Law constant & formula
T (in K)
P1V1 = P2V2
87
Charles Law constant & formula
P (in atm)
T1/V1 = T2/V2
88
Gay Lussac's law constant & formula
V (in L)
P1/T1 = P2/T2
89
Combined gas
P1V1/T1 = P2V2/T2
90
Ideal gas (Universal gas constant)
R = 0.08205
91
Ideal gas formulas
PV = nRT
M = n solute/L
P = MRT
92
Avogadro's formula
V1/n1 = V2/n2
93
Mixture of non-interacting gases exerts a pressure that is the sum of their individual pressures.
Pt = P1 + P2 + P3 + .....
Dalton's Law of Partial Pressure
94
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.
Grahams
95
Rate at which 2 gases mix
Diffusion
96
Rate at which gas escapes through a pinhole in vacuum.
Effusion
97
Diffusion rate (flux) of liquid or gas is directly proportional to the concentration gradient (from high to low concentration)
Fick's 1st Law
98
Decrease temperature, increase pressure (i.e., sealed container), more CO2 is dissolved in water.
Henry's
99
How to get °C
°C = (°F-32)/1.8
100
How to get °F?
°F = (°C x 1.8) + 32
101
How to get °F?
°F = (°C x 1.8) + 32
102
How to get K?
K = °C + 273.15
103
Study of energy conversion/transformation in the universe
Thermodynamics
104
Isolated from the rest by boundary or wall
System
105
Everything outside the system
Surrounding
106
If 2 systems are in thermal equilibrium respectively with a 3rd system, they must be in thermal equilibrium with each other.
Zeroth Law
107
Energy/Mass are always constant! (neither created nor destroyed but can be transformed from one form to another)
1st Law of Thermodynamics: Law of Conservation of Energy
108
Enthalpy (heat/reaction energy) change is independent of reactions/steps that occurred (only the initial & final steps would be the basis)
Hess's Law
109
Cold (absorbed heat)
Endothermic Reaction (+/_\H)
110
Hot (release heat)
Exothermic reaction (-/_\H)
111
For an isolated system, total entropy can never decrease over time.
No way but up
2nd Law of Thermodynamics: Law of Entropy
112
Measure of systems' thermal energy per unit temp; disorderliness or randomliness
Entropy (/_\S)
113
Increase (irreversible) - real case
/_\S (+) Spontaneous
114
Constant (reversible) - ideal case (in a steady state/equilibrium)
/_\S (-) Non-spontaneous
115
If an object reaches absolute zero temperature, its atoms will stop moving.
Entropy of perfectly crystalline substance is zero!
3rd Law of Thermodynamics
116
Thermodynamics state function that combines entropy & enthalpy
Gibb's Free Energy
117
Formula of Gibb's Free Energy
/_\G = /_\H - T/_\S
118
/_\G = 0:
Equilibrium
119
/_\G (-):
Spontaneous
120
/_\G (+):
Non spontaneous
121
Study of reaction rates and reaction mechanism
Chemical Kinetics
122
reactant ---> product
reaction mechanism
123
Change in reactant or product concentration with time
Reaction rate (M/s)
124
Expresses the relationship of reaction rate to rate constant (k) & reactant concentrations raised to some power.
Rate Law
125
What are the reaction rate theories?
Collision Theory
Transition State Theory
126
Reaction rate is proportional to the number of collisions per time
Collision Theory
127
Requirements for effective collision
Proper Orientation
Activation Energy
128
Minimum amount of energy require to initiate chemical reaction
Activation Energy
129
Rate depends on activation energy require to form intermediate/transition state (where new bonds formed & old bonds broken)
Transition State Theory
130
Factors affecting Reaction Rate
•Reactant's nature
• Concentration (except: zero order)
• Catalyst
•Surface area
•Temperature
131
Speeds up the chemical reaction by lowering Ea
Enzyme
132
Reaction rate is proportional to the product of the concentrate of the reactants to the power of its coefficient in a balanced equation
Law of Mass Action
133
Keq = 1:
No shift or Equilibrium
134
Keq > 1:
Favors product formation (to the right forward)
135
Keq < 1:
Favors reactant formation (to the left backward)
136
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.
Le Chatelier's Principle
137
Taste of acids
Sour
138
Taste of bases
Bitter
139
pH of acids
<7
140
pH of bases
>7
141
Hard soap manufacture
NaOH
142
Soft soap manufacture
KOH
143
Bronsted Lowry in acid
Proton donor
144
Bronsted Lowry in base
Proton acceptor
145
Lewis in acid
Electron acceptor
146
Lewis in base
Electron donor
147
Thermodynamically stronger interaction
Hard-Hard/Soft-Soft
148
Thermodynamically weaker interaction
Hard-Soft/Soft-Hard
149
Hard acid + Hard base
Ionic complexes
150
Soft acid + Soft base
Covalent complexes
151
Resist pH change upon addition of small amounts of either acid or base
Buffer solution
152
Buffer capacity
Van Slyke
153
Number of grams of solute dissolved in 1L of saturated solution
Solubility
154
Number of moles of solute dissolved in 1L of saturated solution
Molar solubility
155
Q < Ksp
Unsaturated
156
Q = Ksp
Saturated
157
Q > Ksp
Supersaturated
158
Dissolution rate is directly proportional to the solute surface area, solute concentration at boundary layer & diffusion coefficient
Noyes Whitney Equation
159
Ability to be pounced into thin sheets
Malleable
160
Ability to be drawn into wires
Ductile
161
What elements are s&p block
Representative elements
162
What element is d block?
Transition elements
163
What element is f block?
Actinides & Lanthanides (Inner transition elements)
164
Energy required to remove electron in neutral atom.
Ionization potential/energy
165
Energy released when neutral atom gains extra electron
Electron affinity
166
Atom's ability to attract electron to itself.
Electronegativity
167
Most electronegative
F
168
2nd most electronegative
O2
169
Electron found in outermost shell
Valence electron
170
What are the 3 triad?
Iron triad
Light triad
Heavy triad
171
Densiest metal
Os
172
Discovered transuranic elements: >U exhibit radioactivity
Glenn Seaborg
173
What are the 4 new elements?
Nihonium
Moscovium
Tennessine
Oganesson
174
They can penetrate body tissues
Beta & Gamma
175
Most penetrating
Photon of electromagnetic radiation
Gamma
