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PCP > Inorganic and Phychem > Flashcards

Inorganic and Phychem Flashcards

1
Q

Element is composed of tiny, indivisible, & Indestructible particles call atoms

A

Atomic Theory by Dalton

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2
Q

After 50 years, evidence was seen that atoms are divisible by

A

Marie Curie

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3
Q

Who named atoms from atomos which means indivisible?

A

Democritus

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4
Q

The pudding model is by

A

Joseph John thomson

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5
Q

What model of the atom where electrons are distributed evenly on a sphere of positive charge?

A

Pudding model (jj thomson)

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6
Q

Who discovered electron?

A

Joseph john thomson

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7
Q

Who gave the name electron?

A

G. Johnstone stoney

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8
Q

Caltech of electron charge

A

Shift 7 3

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9
Q

Which experiment and who discovered the eletric charge?

A

Millikan oil drop experiment by Robert Millikan

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10
Q

Who discovered proton?

A

Ernest rutherford

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11
Q

Cathode rays (by jj thomson) produced electron, what rays produced proton and by who?

A

Anode rays by eugen goldstein

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12
Q

What experiment bombarded a gold foil with alpha particles?

A

Alpha particle scattering experiment by Ernest rutherford

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13
Q

Who discovered neutron?

A

James chadwick

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14
Q

James chadwick bombarded what element w/ alpha radiation to produce neutron?

A

Beryllium

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15
Q

He proposed that light and other electromagnetic waves were emitted in discrete packets of energy called quanta

A

Max Planck

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16
Q

Energy formula

A

E=hf=hc/ÿ

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17
Q

A theory that describes matter as acting both as particle and wave

A

Quantum theory of atoms

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18
Q

Atoms produces what kind of spectra

A

Line spectra

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19
Q

Molecules produces what kind of spectra

A

Band spectra (group of lines close to each other)

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20
Q

Bohr’s Model Formula

A

E=2.18x10^-18z^2(1/n1^2 - 1/n2^2)

J/photon

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21
Q

Number of Proton and electron is equal to Z, What is Z

A

Atomic Number

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22
Q

How to get the number of neutrons of an element

A

Atomic mass (A) - Atomic Number (Z)

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23
Q

Photoelectric Effect Formula KE

A

KE=1/2 mv^2 =hf - ø (ø work function of metal)

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24
Q

Compton scattering Formula Wavelength

A

Ÿ’ - ÿ= (h/mc) (1-cosö)

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25
Q

He suggests that matter might exhibit wave-like properties

A

De Broglie Wavelength by Louis de Broglie

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26
Q

Formula for De Broglie’s Wavelength

A

Ÿ=h/mv

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27
Q

What is this principle “ It is impossible to know exactly both the position & momentum of an electron/small particle simultaneously and accurately”

A

Heisenberg’s Uncertainty Principle

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28
Q

Recite the Schrodinger’s Equation

A

Check nalang sa index!

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29
Q

“The wave function contains all the dynamical information about the system it describes”

A

Born Interpretation of wave function squared

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30
Q

Avogadro’s number

A

6.02x10^23 atom/mol

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31
Q

Quantum numbers: Principal

A

n=1-7

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32
Q

Quantum Numbers: Azimuthal, l

A

0=s
1=p
2=d
3=f

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33
Q

Quantum Numbers: Magnetic, ml

A

-1, 0, 1 or dpende sa azimuthal

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34
Q

Quantum Numbers: Spin, ms

A

+1/2 -1/2

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35
Q

Total electrons in the nth shell formula

A

2n^2

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36
Q

“No two electrons of an atom can have all the four quantum numbers the same” what principle and by who

A

Pauli’s Exclusion Principle by Wolfgang Pauli

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37
Q

“The filling of subshells by electrons are according to increasing order of energy and follows the (n+1) rule” what principle

A

Aufbau Principle

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38
Q

“The pairing up of electrons in an orbital of a subshell takes place only when all orbitals contain at least one electron” what rule

A

Hund’s rule of Maximum Multiplicity

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39
Q

Who discovered Radium and Polonium?

A

Marie Curie

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40
Q

Half life of C-14

A

5730

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41
Q

Our body has what kind of 2 carbons

A

C-12 and C-14

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42
Q

What is a Pitch blende

A

Ore of 238U3O8 • 11H2O

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43
Q

What isotope used as medicine for Thyroid?

A

I-181

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44
Q

What isotope/s used as medicine for Bones?

A

Ca-41 and P-32

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45
Q

What isotope used as medicine for Heart?

A

Th-282

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46
Q

Radioactive decay rate

A

N=NaMok/AW

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47
Q

1curie (Ci) is equal to

A

3.7x10^10/s

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48
Q

Geological Dating Formula

A

t=1.5x10^10 log(1+ Pb206/U238) years

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49
Q

Carbon-14 Dating Formula

A

t=1.9x10^4 log(rliving/rdead) years

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50
Q

Biggest Nuclear Plant

A

Kashiwazaki-Kariwa

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51
Q

Mass-energy equivalence Formula

A

E=mc^2

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52
Q

1amu is equal to how many grams

A

1.66x10^-24

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53
Q

1amu is equal to how many MeV

A

931

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54
Q

What experiment bombarded U-235 w/ neutron and obtained the element 56 & 36?

A

Nuclear Fission

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55
Q

Who lead the nuclear fission experiment?

A

HMS

Hahn, Meitner, Strassman

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56
Q

What elements are obtained in the nuclear fission experiment?

A

56 & 36

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57
Q

Nuclear fission experiment bombarded what element with neutron obtaining elements 56 & 36?

A

U-235

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58
Q

Fuel used in nuclear powerplant

A

U-235

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59
Q

Nuclear power plant fuel consumption formula

A

M=2.11x10^-4 x P/NaE g/day

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60
Q

Formula for Binding Energy

A

BE=[Z x Mh + (A-Z) x Mn-Ma) (931MeV/1amu)

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61
Q

Equivalent of Mh in binding energy

A

1.007825 u

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62
Q

Equivalent of Mn in binding energy

A

1.008665 u

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63
Q

Who classified the elements according to metals, non metals, gases, and earths

A

Antoine Lavoisier

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64
Q

Who discovered the law of triads

A

Johann Dobereiner

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65
Q

Who made the three dimensional arrangement of known elements

A

Alexandre Beguyer

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66
Q

Who discovered the law of octaves

A

John Newlands

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67
Q

Who first to recognize periodic trends in properties of elements

A

Julius lothar Meyer

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68
Q

Who arranged the elements in increasing order of their atomic masses

A

Dmitri Mendeleev

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69
Q

This law states that elements are periodic functions of their atomic number

A

Periodic law

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70
Q

Energy released when an electron is added to an isolated gaseous atom

A

Electron affinity

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71
Q

Measure of the relative tendency of an atom to attract shared electron pair

A

Electronegativity

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72
Q

What is used in electronegativity to measure the relative tendency of an atom to attract shared electron pair

A

Pauling scale

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73
Q

Determination of lattice energy of a compound between metals & nonmetals

A

Born haber cycle

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74
Q

Born-haber cycler formula

A

Q=S+I+1/2D+Ea+Uo

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75
Q

What bond shared electrons between non metals

A

Covalent bond

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76
Q

What bond transfers electrons from metal to non metal

A

Ionic bond

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77
Q

Equal sharing of bonding pairs

A

Non polar covalent bond

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78
Q

Unequal sharing of bonding pairs

A

Polar covalent

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79
Q

Result of electron transfer

A

Ionic Bond

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80
Q

What rule where atoms tend to gain lose or share electrons until surrounded by 8 valence electrons

A

Octet rule

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81
Q

Electrons are written as dots

A

Lewis structure

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82
Q

Formal charge formula

A

Valence e- -1/2 (bonding e-) - (Non-bonding e-)

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83
Q

Bond order formula

A

BO= [(e- in BMO) - (e- in ABMO)] / 2

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84
Q

Leo says ger meaning

A

Losing electrons is oxidation

Gaining electrons is reduction

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85
Q

Ideal gas equation

A

PV=nRT

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86
Q

Boyle’s Law

A

P1V1=P2V2

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87
Q

Charle’s law

A

V1/T1 = V2/T2

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88
Q

Gay Lussac’s Law

A

P1/T1 = P2/T2

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89
Q

Combined Gas Equation

A

P1V1/T1 = P2V2/T2

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90
Q

Dalton’s Law

A

P1/PT= n2/nT

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91
Q

Amagat’s Law

A

V1/VT = n2/nT

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92
Q

Ludwig Boltzmann Constant K Formula

A

K=R/NA =1.38x10^-23 j/molecules-K

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93
Q

Maxwell’s Distribution of Speeds Formula: Most Probable Speed

A

Sqr root of 2RT/M

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94
Q

Maxwell’s Distribution of Speeds Formula: Mean Speed

A

Sqr root of 8RT/piM

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95
Q

Maxwell’s Distribution of Speeds Formula: Root mean squared

A

Sqr root of 3RT/M

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96
Q

Graham’s Law of Diffusion Formula

A

ÛA/ÛB= sqr root of MWB/MWA

Or ÛA/ÛB= sqr root of Density A/Density B

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97
Q

Mean Free Path Formula

A

ÿ=[1/(sqr root of 2)(ô)] [RT/PNa]

Na= avogadro’s

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98
Q

Gas gas collision formula

A

Zgg=Vave/ÿ

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99
Q

Gas wall collision formula

A

Zgw=PANa/ sqr root of 2pi MRT

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100
Q

Compressibility Factor, Z formula

A

Z=PV/RT

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101
Q

Van Der Waals Formula

A

(P + n^2 a/V^2) (V-nb) = nRT

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102
Q

Boyle Temperature Formula

A

TB=a/bR

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103
Q

Ability of a fluid to escape

A

Fugacity (gas has fugacity and liquid has none)

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104
Q

Critical Constant, a formula:

A

a=27 R^2 Tc^2 / 64 Pc

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105
Q

Critical Constants, b formula:

A

b=R Tc/8 Pc

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106
Q

Barometric Pressure formula

A

P=Po e^-(g M Z / R T)

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107
Q

Po @ Sealevel pressure is

A

101.325 KPa or 1atm

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108
Q

Strongest intermolecular force

A

Ion dipole

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109
Q

Intermolecular force with H bond

A

Dipole dipole

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110
Q

Weakest intermolecular force

A

London dispersion

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111
Q

Dipole moment formula

A

û= qr=(n x e) (r)

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112
Q

Ionic Character formula

A

û obs / û theo

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113
Q

Intermolecular attraction between unlike molecules

A

Adhesive forces

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114
Q

Intermolecular attraction between same molecules

A

Cohesive forces

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115
Q

Ability of a liquid to flow in narrow spaces without external forces

A

Capillary action

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116
Q

Capillary action height formula

A

h=(2(gamma y) cos (alpha a))/(rho, p) g r

gamma, y= liquid air surface tension

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117
Q

Half bubble formula

A

Pi -Po=4y/r

gamma y

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118
Q

Full bubble formula

A

Pi -Po=2y/r

gamma y

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119
Q

What compound forms bubbles in soap

A

Surfactant

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120
Q

Solids not arranged in an orderly manner

A

Amorphous solids

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121
Q

Solids arranged in a definite manner

A

Crystalline solids

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122
Q

Different physical properties in different directions

A

Anisotropy

123
Q

Amount of energy required to completely separate the ions

A

Lattice energy

124
Q

1 atom are held together in a large network

A

Network covalent

125
Q

Who (3) discovered C-60 buckministerfullere or bucky ball

A

Harry kroto, Richard Smalley, and robert curl

126
Q

Total number of space lattices

A

14

127
Q

Body centered radius formula

A

4r=a sqr root of 3

128
Q

Face centered radius formula

A

4r=a sqr root of 2

129
Q

Simple crystal lattice radius formula

A

a=2r

130
Q

Packing fraction of simple crystal lattice

A

pi/6

131
Q

Packing fraction of body centered crystal lattice

A

pi sqr root of 3 / 8

132
Q

Packing fraction of face centered crystal lattice

A

pi sqr root of 2 / 6

133
Q

Density of crystal

A

p= n(AW)/NA (a)^3

134
Q

1 angstrom equal to m

A

10^-10

135
Q

Who discovered DNA via X-ray crystallography

A

Rosalind franklin

136
Q

Crystal are not only diffraction gratings but also reflection gratings

A

Bragg’s law

137
Q

Lawrence Bragg equation

A

ny=2dsin@=2dsin@/ sqr root of h^2 + k^2 + I^2

y gamma
@ theta

138
Q

Packing efficiency formula

A

PF= [ (# of atoms/unit cell) (atomic volume ] / volume of unit cell

139
Q

Enthalpy Formula

A

H=U+PV

140
Q

If Change of H is less than 0

Process is

A

Exothermic

141
Q

If Change of H is greater than 0

Process is

A

Endothermic

142
Q

Enthalpy formula for gases

A

Change of H = change of U + change of ng R T

Change of ng = product moles - reactant moles

143
Q

Hess law

A

Enthalpy change is independent of the way the process is carried out

144
Q

Measure of degree of disorder in the system

A

Entropy

145
Q

Unit of Entropy

A

J/mol K

146
Q

Used to calculate absolute zero entropies of pure substance at any temperature

A

Third law of thermodynamics

147
Q

gibbs free energy, G formula

A

G=H-TS

148
Q

Unit of Gibbs free energy

A

J/mol

149
Q

Energy freely available from the system which can put into useful work

A

Gibbs free energy

150
Q

@ Normal Boiling Point temperature, Pressure is

A

1 atm

151
Q

If change of G is less than 0, system is

A

Spontaneous

152
Q

If change of G is greater than 0, system is

A

Non spontaneous

153
Q

If change of G is equal to 0, system is

A

@ equilibrium

154
Q

If change of enthalpy is positive and change of entropy is positive system is

A

Spontaneous @ high T

155
Q

If change of enthalpy is positive and change of entropy is negative system is

A

Non spontaneous at all T

156
Q

If change of enthalpy is negative and change of entropy is positive system is

A

Spontaneous at all T

157
Q

If change of enthalpy is negative and change of entropy is negative system is

A

Spontaneous at low T

158
Q

Solid to vapor

A

Sublimation

159
Q

Vapor to solid

A

Solidification

160
Q

Solid to liquid

A

Fusion

161
Q

Liquid to solid

A

Freezing

162
Q

Liquid to vapor

A

Evaporation

163
Q

Vapor to liquid

A

Condensation

164
Q

Clapeyron equation

A

(P2-P1/T2-T1) = H of fusion / (T1+T2/2) (V2-V1)

V is specific Volume

165
Q

Clausius Clapeyron Equation

A

ln (P2/P1) = (-H/ R) (1/T2 -1/T1)

166
Q

Trouton’s rule in using Boyle’s Temp

A

Change of S = H vap/ Tb = 10.5R = 21 cal/mol K = 88 J/mol-K

167
Q

There is phase change but no change in temperature

A

Latent heat

168
Q

There is change in temperature but no phase change

A

Sensible heat

169
Q

Reaction Quotient, Q is less than K

A

Shift to right

170
Q

Reaction Quotient, Q is greater than K

A

Shift to left

171
Q

Reaction Quotient, Q is equal to K

A

@ equilibrium

172
Q

Van’t Hoff’s Equation

A

ln (k2/k1) = (-H/R) (1/T2 - 1/T1)

173
Q

Le Chatelier’s Principle,

If Change of H is exothermic temperature

A

Increases and shift to the left

174
Q

Le Chatelier’s Principle,

If Change of H is endothermic temperature

A

Decreases and shift to the right

175
Q

Le Chatelier’s Principle,

If pressure increases

A

It shifts to the side with less mole

176
Q

Le Chatelier’s Principle,

If pressure decreases

A

Shift to the side with more mole

177
Q

Le Chatelier’s Principle,

If concentration of reactant increases

A

Shifts to the right

178
Q

Le Chatelier’s Principle,

If concentration of product increases

A

Shift to the left

179
Q

State of solution is based on the state of

A

Solvent

180
Q

Is a mixture of gases a true solution

A

Yes

181
Q

Does true solution remains homogeneous with time?

A

Yes

182
Q

For solids, if Temperature increases, solubility

A

Solubility increases and vice versa

183
Q

For gases, if pressure increases solubility

A

Solubility increases and vice versa

184
Q

For gases, if temperature increases solubility

A

Solubility decreases and vice versa

185
Q

Raoult’s Law is by

A

Francois Marie Raoult

186
Q

Formula of Raoult’s law

A

Partial Pressure A = Xa (Vapor Pressure A)

PA = XA P*A
XA = moles in liquid 
YA = moles in vapor
187
Q

Raoult’s law formula for YA

A

YA= Alpha XA/(Alpha -1) Xa + 1

188
Q

Raoult’s Law formula of Alpha

A

Alpha= PA/PB

189
Q

Vapor pressure of each component are independent of each other

A

Immiscible Liquids

190
Q

Immiscible Liquids Formula

A

Pt= P1 + P2= P1 + P2

P1 and P2 are vapor pressure

191
Q

Freezing point depression formula

A

(0-Tf) = i m kf

m is molality

192
Q

Boiling point elevation formula

A

Tb-100 = i m kb

m is molality

193
Q

Osmotic Pressure formula

A

Pi=iCRT

C is molarity

194
Q

Ebullioscopic constant, kb

A

0.52c/m

195
Q

Cryoscopic constant, kf

A

1.86c/m

196
Q

gc is equal to

A

gc= 1kg m/ N s^2 or 32.174 lb ft/lbf s^2

197
Q

Most electronegative element

A

Fluorine

198
Q

Vant hoff constant, i formula

A

alpha= i-1 / v-1

199
Q

In Osmosis if Co is greater than Ci it is

A

Hypotonic or crenation

200
Q

In osmosis If Co is less than Ci it is

A

Hypertonic or hemolysis

201
Q

If in osmosis Ci = Co it is

A

Isotonic

202
Q

In electrochemistry, if chemical energy is converted to electricity it is

A

Galvanic or voltaic cell

203
Q

In electrochemistry, if electrical energy is converted to chemical energy it is

A

Electrolytic cell

204
Q

Is galvanic cell spontaneous or not?

A

Spontaneous

205
Q

Is electrolytic cell spontaneous or not?

A

Not spontaneous

206
Q

Faradays constant is equal to blank coulombs/mol

A

96500 coulombs/mol

207
Q

Electrolytic Cell formula

A

I (change of T) = m n F / MW

n is no. Of electrons

208
Q

Nerst Equation

A

E=Ecell - 0.0592/n log Q

209
Q

Nerst equation at equilibrium

A

Ecell= 0.0592/n log keq

210
Q

Does not meet the criteria of a primary standard but used subsequently as the titrant in a particular method

A

Secondary standard

211
Q

Formed due to solvation of salts, strong acids and bases into a solution

A

Electrolytes

212
Q

Enumerate the strong acids

A

HCl, HBr, H2SO4, H3PO4, and HNO3

213
Q

Enumerate strong based

A

Part of group 1 (OH)

And group 2 (OH)2

214
Q

For weak acid solution

A

Ka= x^2/c-x
x=H+
ph=-log(H+)

215
Q

For weak base solution

A

Kb= x^2/c-x
x=OH-
ph=14+log(OH-)

216
Q

Arrhenius Base

A

Produce OH-

217
Q

Arrhenius acid

A

Produce H3O+

218
Q

Bronsted-Lowry Acid

A

Donate H+

219
Q

Bronsted-lowry base

A

Accept H+

220
Q

Lewis Acid

A

Accept e- pair

221
Q

Lewis Base

A

Donate e- pair

222
Q

Acts as both acid and base

A

Amphoteric

223
Q

Possess both hydrophilic and lipophilic properties

A

Amphipatic

224
Q

Amphoteric that can accept or donate proton

A

Amphiprotic

225
Q

Amphoteric that contain both acidic and basic groups and exists as zwitterions

A

Ampholytes

226
Q

From acid to conjugate base

A

Just remove 1H from acid

227
Q

From base to conjugate acid

A

Just add 1 H sa base

228
Q

Ka of CH3COOH

A

1.8x10^-5

229
Q

Kb of NH3

A

1.8x10^-5

230
Q

Salt of weak acid (Weak Base) formula

A

OH-= sqr root of KwC/Ka

231
Q

Salt of weak base (Weak acid) formula

A

H+ = sqr root of KwC/Kb

232
Q

Salt of weak acid and base formula

A

H+ = sqr root of KwKa/Kb

233
Q

K of water or Kw is equal to

A

1x10^-14

234
Q

Diprotic H2X formula

A

Ka=x^2/c-x

H+

235
Q

Diprotic HX- formula

A

H+ = sqr root of (K1K2C-K1Kw)/K1+C

236
Q

Diprotic x^-2

A

Kb2=Kw/Ka2=x^2/c-x

OH-

237
Q

Triprotic H3X formula

A

Ka=x^2/c-x

238
Q

Triprotic H2X- Formula

A

H+ = sqr root of (K1K2C-K1Kw)/K2+C

239
Q

Triprotic HX^-2 formula

A

H+= sqr root of (K2K3C-K2Kw)/K2+C

240
Q

Triprotic X^-3 formula

A

Kb3=Kw/Ka3= x^2/c-x

OH-

241
Q

Buffer is composed of

A

Weak acid/base and conjugate salt

1H difference

242
Q

Henderson-Hasselbalch equation

A

pH=pka+log (base/acid)

243
Q

Organic compounds used in titration to provide color change

A

Indicators

244
Q

Normality formula

A

N=M x n
M molarity
n number of H+/OH-/e-

245
Q

Kjeldahl factor for cereals:

A

5.70

246
Q

Kjeldahl factor for meat products:

A

6.25

247
Q

Kjeldahl factor for dairy products:

A

6.38

248
Q

If there is salt in the solution the solubility of salt decreases

A

Common ion effect

249
Q

Uses AgNO3 as titrant producing brick red color

A

Argentometric titrations

250
Q

Color of ferric chloride

A

Orange

251
Q

Titration where reaction of Ag+ and Dichromate forms red silver dichromate

A

Mohr method

252
Q

Titration using KSCN as 2nd titrant

A

Volhard method

253
Q

Titration using a sodium fluoresceinate as indicator with no back titration because end point is sharp

A

Fajans Method

254
Q

How to spot end of titration

A

1sr trace of red

255
Q

Bending of molecular bonds

A

Molecular conformation

256
Q

Have one unshared pair of electrons capable of forming covalent bond w/ ion

A

Ligand

257
Q

Formed when metal ion bonds with monodentate ligand

A

Coordination complex or metal complex

258
Q

Metal ion bonds with polydentate ligand

A

Chelate complex

259
Q

Forms soluble complex molecules with a metal ion resulting to inactivation of the ion’s ability to react with other elements to produce precipitate

A

Chelants

260
Q

Indicators of EDTA

A

Eriochrome Black T
Murexide
Calmagite

261
Q

Gravimetric Factor formula

A

GF= (MWB/MWA) (a/b)

262
Q

Redox electrons: MnO4- in acid and color

A

5e- (pink)

263
Q

Redox electrons: MnO4- in base and color

A

3e- (brown)

264
Q

Redox electrons: C2O4^-2

A

2e-

265
Q

Redox electrons: As^3+

A

2e-

266
Q

Redox electrons: Fe^2+

A

e-

267
Q

Redox electrons: Solid Fe

A

2e-

268
Q

Redox electrons: Sn^2+

A

2e-

269
Q

Redox electrons: NO2-

A

2e-

270
Q

Redox electrons: H2O2

A

2e-

271
Q

Redox electrons: Mo^3+

A

3e-

272
Q

Redox electrons: Ti^3+

A

e-

273
Q

Redox electrons: Cr2O7^2-

A

6e-

274
Q

Redox electrons: U^4+

A

2e-

275
Q

Redox electrons: Cu+

A

e-

276
Q

Redox electrons: I2

A

2e-

277
Q

Redox electrons: S2O3^2-

A

e-

278
Q

Jones reductor uses

A

Zn (Amalgam Zn-Hg)

279
Q

Walden reductor uses

A

Ag in 1M HCl

280
Q

Spectrophotometry formula

A

1/T=f in Hz

281
Q

Shortest wavelength is

A

Gamma rays

282
Q

Shortest wavelength has the highest energy, true or false

A

True

283
Q

Wavelength for bond breaking

A

Xrays

284
Q

Wavelength for electronic excitation

A

Ultraviolet

285
Q

Wavelength for vibration

A

Infrared

286
Q

Wavelength for rotation

A

Microwave

287
Q

A prism/grating/filter that selects one wavelength

A

Monochromator

288
Q

Monochromatic means

A

1 color

289
Q

A fraction of the original light that passes through the sample

A

Transmittance

290
Q

Transmittance formula

A

T=P/Po < 1

291
Q

Absorbance formula

A

A=log (Po/P) = -log T

292
Q

Beer’s law formula

A

A=Ębc
Ę epsilon molar absorptivity 1/M-cm
b path length in cm
c concentration

293
Q

Part of molecule responsible for light absorption

A

Chromophore

294
Q

Flat, fused-silica (SiO2) faces

A

Cuget

295
Q

Electronic states: spins are opposed

A

Singlet state

296
Q

Electronic states: spins are parallel

A

Triplet state

297
Q

Vibrational and rotational state of a non-linear molecule

A

Vibration: 3n-6
Rotation: 3

298
Q

Vibrational and rotational state of a linear molecule

A

Vibration: 3n-5
Rotation: 2

299
Q

Transition between states with same spin quantum number

A

Internal conversion

300
Q

Transition between states with different spin quantum number

A

Intersystem crossing

301
Q

Sensitive enough to observe single molecules

A

Luminescence

302
Q

Emission of photon during transition with same quantum number

A

Fluorescence

303
Q

Emission of photon during transition with different quantum number

A

Phosphorescence

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