chapter 3. light emitting diod. electron configuration
TRANSCRIPT
Chapter 3. Light emitting diod
Electron configuration
Covalent bond
Organic semiconductors: extensively conjugated molecular systems such as fully conjugated polymers or cata-condensed polyacenes (PAH, e.g., anthracene)
Electron density sections through central molecular plane, with each contour line representing an increase of 500 electrons/nm3
-electron clound in anthracene
Molecular orbitals
types of electronic transitions in polyatomic molecules
The total spin quantum number S = Σ si
The multiplicities M = 2S + 1
Spin of electrons
Statistical states
Ms:Magnetic quantum number
Energetics of spin states
Zero-field splitting EZF ~ 0.1 cm1 ~ 1 kG
Externally applied H ~ 1 to 10 kG
Spin interaction
Coulomb repulsion
Electronic excitation and de-excitation in organic molecules
Jabloński Diagram
probability of transition. The Beer-Lambert Law. Oscillator strength
The molecules whose absorption transition moments are parallel to theelectric vector of a linearly polarized incident light are preferentially excited.
The probability of excitation is proportional to the square of the scalar product of the transition moment and the electric vector. This probability is thus maximum when the two vectors are parallel and zero when they are perpendicular.
Frank-Condon principle
Electronic transition ~ 10-15 sVibration ~ 10-10 – 10-12 s
Vertical transition
Bathochromic: red-shiftHyposochromic: blue-shift
Effects of domain overlap & corresponding wave amplitudes
Mirror image rule
Mirror image rule
Rigorous relatioship between absorption & fluorescence
Kasha’s rule
Radiative & non-radiative processes
Internal conversionInternal conversion is a non-radiative transition between two electronic states of the same spin multiplicity.
FluorescenceEmission of photons accompanying the S1 S0 relaxation is called fluorescence.
In most cases, the absorption spectrum partly overlaps the fluorescence spectrum. At r. t., a small fraction of molecules is in a vibrational level higher than 0 in the ground state as well as in the excited state. At low temp, this departure from the Stokes Law should disappear.
It should be noted that emission of a photon is as fast as absorption of a photon (~1015 s). However, excited molecules stay in the S1 state for a certain time (a few tens of picoseconds to a few hundreds of nanoseconds, depending on the type of molecule and the medium) before emitting a photon or undergoing other de-excitation processes (internal conversion, intersystem crossing).
From S1, internal conversion to S0 is possible but is less efficient than conversion from S2 to S1, because of the much larger energy gap between S1 and S0.
Experimental schematic for detection of the Stokes’ shift
The energy of the emission is typically less than that of absorption. Hence, fluorescence typically occurs at lower energies or longer wavelengths.
After the 1850s, Stokes became involved in administrative matters, and his scientific productivity decreased.
Some things never change.
Stokes shift
Intersystem crossing and subsequent processes
Intersystem crossingis a non-radiative transition between two isoenergetic vibrational levels belonging to electronic states of different multiplicities.
Delayed fluorescenceT1S1 can occur when the energy difference between S1 & T1 is small and when the lifetime of T1 is long enough.
Triplet-triplet annihilationIn concentrated solutions, a collision between two moleculesin the T1 state can provide enough energy to allow one of them to return to the S1 state leads to a delayed fluorescence emission.
Triplet-triplet transitionsOnce a molecule is excited and reaches triplet state T1, it can absorb a different wavelength because triplet-triplettransitions are spin allowed.
Energy transfer
Distinction between radiative and non-radiative transfer
hopping
Excitation energy transfer
heterotransfer
homotransfer
Radiative energy transfer
(rate constant)
(lifetime of excited state)
Non-radiative energy transfer
EET: excitation energy transfer or electronic energy transferRET: resonance energy transfer
FRET: fluorescence resonance energy transfer
Energy transfer can result from different interaction mechanisms. The interactions may be Coulombic and/or due to intermolecular orbital overlap.
* * The Coulombic interactions consist of long-range dipole-dipole interactions (Forster’s mechanism) and short-range multi-polar interactions.
* * The interactions due to intermolecular orbital overlap, which include electron exchange (Dexter’s mechanism) and charge resonance interactions, are of course only short range.
It should be noted that for singlet-singlet energy transfer, all types of interactions are involved, whereas triplet-triplet energy transfer is due only to orbital overlap.
The total interaction energy can be expressed as a sum of two terms: a Columbic term Uc and an exchange term Uex. The Coulombic term corresponds to the energy transfer process in which the initially excited electron on the donor D returns to the ground state orbital on D, while simultaneously an electron on the acceptor A is promoted to the excited state. The exchange term corresponds to an energy transfer process associated with an exchange of two electrons between D and A.
CI: Coulombic interaction
EE: electron exchange
Formation of excimers and exciplexes
Excimers
An excimer is located at wavelengths higher than that of the monomer and does not show vibronic bands.
P3HT PL heating-1
500 550 600 650 700 750 800 8500
50
100
150
200
250Heating-1 30 oC
70 oC
110 oC
150 oC
190 oC
210 oC
220 oC
230 oC
240 oC
250 oC
260 oC
exc
= 470 nm
HT-PL of PT-6 (fresh toluene solution cast), exc
= 550 nm (95/03/27)
Em
issio
n in
tens
ity (a
. u.)
Wavelength (nm)
S
C6H13
[ ]n
Exciplexes
Lifetimes and quantum yields
Lifetimes and quantum yieldsExcited-state lifetimes
The rate constants for the various processes will be denoted as follows:
A very short pulse of light at time 0 brings a certain number of molecules A to the S1 excited state by absorption of photons. These excited molecules then return to So.The rate of disappearance of excited molecules is expressed by the following differential equation:
iF(t), the -pulse response of the system, decrease according to a single expontial.
Quantum yields
When the fluorescence quantum yield and the excited-state lifetime of a fluorophore are measured under the same conditions, the non-radiative and radivative rate can be easily calculated by means of the following relations:
τr = 1/krs
quenching
The sum kM of the rate constants for de-excitation processes is equal to the reciprocal excited-state lifetime :
Kq : the observed rate constant for the bimolecular process
The fluorescence characteristics (decay time and/or fluorescence quantum yield) of M* are affected by the presence of Q as a result of competition between the intrinsic de-excitation and these intermolecular processes.
Overview of the intermolecular de-excitation of excited molecules leading to fluorescence quenching
4.2.1 Phenomenological approach
(static quenching)
Dynamic quenching
Stern-Volmer kinetics (ignore the transient effects)
i(t) = i(0) exp (-t/)
KSV : Stern-Volmer constant
I0/I vs. [Q] Stern-Volmer plot
Static quenching
The term static quenching implies either the existence of a sphere of effective quenching or the formation of a ground-state non-fluorescent complex (Figure 4.1)
Sphere of effective quenching
Formation of a ground-state non-fluorescent complex
I ~ [M]
Simultaneous dynamic and static quenching
dynamic
static non-fluorescent complex
static
Sphere of effective quenching