photochemistry basics

11/20/12 Photochemistry

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The first law of photochemistry, the Grotthuss-Draper law, states that light must be absorbed by a compound

in order for a photochemical reaction to take place.

The second law of photochemistry, the Stark-Einstein law, states that for each photon of light absorbed by a

chemical system, only one molecule is activated for subsequent reaction. This "photoequivalence law" was

derived by Albert Einstein during his development of the quantum (photon) theory of light.

Type of Glass Wavelength Cut-off

Photochemistry

Photochemistry

The study of chemical reactions, isomerizations and physical behavior that may occur under the influence of visible and/or

ultraviolet light is called Photochemistry. Two fundamental principles are the foundation for understanding photochemical

transformations:

The efficiency with which a given photochemical process occurs is given by its Quantum Yield (). Since many

photochemical reactions are complex, and may compete with unproductive energy loss, the quantum yield is usually

specified for a particular event. Thus, we may define quantum yield as "the number of moles of a stated reactant

disappearing, or the number of moles of a stated product produced, per einstein of monochromatic light absorbed.", where

an einstein is one mole of photons. For example, irradiation of acetone with 313 nm light (3130 ) gives a complex mixture

of products, as shown in the following diagram. The quantum yield of these products is less than 0.2, indicating there are

radiative (fluorescence & phosphorescence) and non-radiative return pathways (green arrow). The primary photochemical

reaction is the homolytic cleavage of a carbon-carbon bond shown in the top equation. Here the asterisk represents an

electronic excited state, the nature of which will be defined later.

Several secondary radical reactions then follow (shown in the gray box), making it difficult to assign a quantum yield to the

primary reaction. The biacetyl product, formed in the third reaction, may itself be excited by light or accept excitation energy

from an excited acetone molecule, further complicating this process.

By comparison, the light induced chlorination of methane, or other alkanes, has a large quantum yield, often near 106,

because of the secondary chain reactions that follow the primary cleavage of the Cl-Cl bond. Equations illustrating such

halogenation reactions have been presented elsewhere in this text.

Mechanistic Background

Absorption of visible and/or ultraviolet light by a molecule introduces energy

sufficient to break or reorganize most covalent bonds. From the relationship E =

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Pyrex < 275 nm

Corex < 260 nm

Vycor < 220 nm

Quartz < 170 nm

hc / , we see that longer wavelength visible light (400 to 800 nm) is less energetic(70 to 40 kcal/mole) than light in the accessible shorter wavelength (200 to 400

nm) near ultraviolet region (150 to 70 kcal/mole). Consequently, ultraviolet light is

most often used to effect photochemical change. Care must also be taken to

construct lamps and reaction vessels from glass that is transparent to the desired

wavelength range. The low wavelength cut-off for some common glass types are

given in the table on the right.The light required for a photochemical reaction may come from many sources. Giacomo Ciamician, regarded as the

"father of organic photochemistry", used sunlight for much of his research at the University of Bologna in the early 1900's.

Depending on the compounds being studied and the information being sought, bright incandescent lamps (chiefly infrared

and visible light), low, medium and high pressure mercury lamps (185 - 255 nm, 255 -1000 nm & 220 -1400 nm

respectively), high intensity flash sources and lasers have all been used. In careful studies of specific chromophores,

sources of monochromatic light may be desired.In this section we shall focus chiefly on the nature and behavior of the electronic excited states formed when a photon is

absorbed by a chromophoric functional group. As a rule, such excitation results in a change in molecular orbital

occupancy, an increase in energy, and changes in local bonding and charge distribution. The principles set forth in the UV-

Visible Spectroscopy chapter will provide a helpful foundation.

We begin by considering the electronic excitation of a simple diatomic molecule such as Cl2 or Br2. Both absorb light,

chlorine in the 300 to 380 nm region. and bromine in the 360 to 510 nm region. The

diagram on the right illustrates the initial electronic excitation. Both the ground (lowest

energy electronic state) and excited states are shown as energy profiles populated by

vibrational energy states (green lines) as well as rotational states (not shown). The

electron reorganization that occurs when the ground electronic state is excited by

absorption of a photon takes place much more rapidly than any movement of the atom

nuclei that eventually follow. In other words, electron shifts, when viewed from the

perspective of the nuclear coordinates, occur as if the heavier nuclei were fixed in

place. This consequence of the Born-Oppenheimer approximation led James Franck

and R. Condon to formulate the Franck-Condon Principle: Electronic transitions

occur much faster than nuclei can respond.

Overall bonding in an excited state is usually lower than in the ground state. Thus, the

XX bond length is increased in the excited state. At normal temperatures essentially

all molecules will exist in the ground vibrational state (zero level). The Franck-Condon

principle requires that excitation occur by a vertical transition, shown by the red line, resulting in the population of higher

vibrational levels in the excited state. Several events may then take place.

1. The vibrational energy may be lost as heat, relaxing the excited state to its zero vibrational level.

2. The excited state may return to the ground state by emitting a photon (light blue line). If this happens from the zero

vibrational level the frequency or energy of the emitted light will be lower than that of the initially absorbed light. This

radiative decay is called fluorescence if it takes place rapidly from the initial excited state. It is termed

phosphorescence if it occurs slowly by way of other excited states.

3. If a higher vibrational level of the excited state is populated, either by the initial Franck-Condon transition or by

collisional activation, the molecule may cleave into two X atoms. Note that vibrational level 5 of the excited state is

roughly coincident with bond breaking.

Virtually all organic compounds have more than two atoms, so the potential energy state diagram of X2 must be adjusted

for the increased number of bonding relationships. One way of doing this is to retain the energy coordinate while

dispensing with the dimensional (r) coordinate. The Jablonski diagram shown below is an example, in which the spatial

orientation of the various electronic states is not specified. Nevertheless, Franck-Condon transitions are expected.

One important feature conveyed by the diagram is that more than one electronic excited state is likely to exist for a given

molecule, six are drawn and labeled in the diagram. Each electronic state will have a group of vibrational (and rotational)

states, depicted by light blue lines above each state marker. Transitions between electronic states often occur to higher

vibrational levels which then relax to lower levels by collisional loss of heat (translational energy).

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Excited states may be classified as singlet or triplet based upon their electron spin angular momentum. The electrons in

most non-metallic organic compounds are paired (opposite spins) in bonding and non-bonding orbitals, resulting in a net

zero spin diamagnetic molecule for the ground state. Such states have a single energy state in an applied magnetic field,

and are called singlets. Electronic states in which two electrons with identical spin occupy different orbitals (the Pauli

exclusion principle) have a net spin of 1 (2 1/2) and are paramagnetic. In a magnetic field such states have three energy

levels (+1, 0, -1) and are called triplets. Molecular oxygen is a rare example of a triplet ground electronic state.

The distinction between singlet and triplet states is important because photon induced excitation always leads to a state of

the same multiplicity, i.e. singlet to singlet or triplet to triplet. Since most ground states are singlets, this means that the

excited states initially formed by absorption of light must also be singlets. Internal conversion of excited states to lower

energy states of the same multiplicity takes place rapidly with loss of heat energy (relaxation). Alternatively, an excited state

may return to the ground state by emitting a photon (radiative decay). In the study of acetone described above, nearly 80%

of the excited singlet states lose energy by internal conversion and about 3% by fluorescence. Conversion of a singlet state

to a lower energy triplet state, or vice versa, is termed intersystem crossing and is slower than internal conversion.

Radiative decay from a triplet state is called phosphorescence and is generally quite slow. The approximate timescales for

these transitions are given in the following table.

Process Transition Timescale (sec)

Light Absorption (Excitation) S0 Sn ca. 10-15 (instantaneous)

Internal Conversion Sn S1 10-14 to 10-11

Vibrational Relaxation Sn* Sn 10

-12 to 10-10

Intersystem Crossing S1 T1 10-11 to 10-6

Fluorescence S1 S0 10-9 to 10-6

Phosphorescence T1 S0 10-3 to 100

Non-Radiative Decay S1 S0

T1 S0

10-7 to 10-5

10-3 to 100

The non-radiative decay noted in the last row may take place by intermolecular energy transfer to a different molecule. This

collisional process is termed quenching if the focus is on the initially excited species, or sensitization if the newly created

excited state is of interest. Photochemical sensitization commonly occurs by a T1 + S0 S0 + T1 reaction, where the

bold red-colored species is the sensitizer. The new triplet excited state may then undergo characteristic reactions of its

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own.

Photochemical Reactions

Alkene Isomerization

A photochemical reaction occurs when internal conversion and relaxation of an excited state leads to a ground state

isomer of the initial substrate molecule, or when an excited state undergoes an intermolecular addition to another reactant

molecule in the ground state. The cis-trans photochemical isomerization of stilbene is a reaction of the first kind, as shown

in the following diagram. Both cis and trans-stilbene undergo * electron excitation by absorption of uv light. Whereas

isolated double bonds require 180 nm light for such excitation, conjugation with the phenyl substituents lowers the

transition energy to about 300 nm, a more easily achieved source. The molar absorptivity of the cis-isomer is less than that

of the trans-isomer because steric crowding of the ortho sites causes the phenyl groups to twist slightly out of coplanarity.

The stability of the stereoisomers of stilbene is due to a 62 kcal/mole barrier to rotation about the double bond produced by

the -bond. This bonding is absent in the * excited state (magenta curve in the diagram). Both the initial S1 states

formed from the cis and trans ground states are slightly twisted (the cis by 25 & the trans by 13) with the C=C double

bond being lengthened by about 4.5%. These local S1 states quickly relax to a common lower energy twisted configuration

( 90). Non-radiative internal conversion of this S1 twisted state leads to the transition state region of S0, which decays

equally to the ground states of the cis and trans isomers. This simple configurational isomerization about a single double

bond is referred to as a One-Bond-Flip (OBF) event.

A small proportion (6%) of the trans-S1 state fluoresces back to the trans-isomer, but there is less than 0.1% fluorescence

from the cis-S1 state. Triplet states (not shown) may also be formed, but there is no observable phosphorescence in

solution, and non-radiative decay from such states results in similar cis-trans isomerization. The quantum yield of trans to

cis isomerization decreases in viscous solvents, accompanied by an increase in fluorescent decay. Freezing the solutions

to a rigid glass halts the isomerization and results in maximum fluorescence efficiency.

Inspection of the cis-S1 local minimum near = 0 shows that only 70% of the molecules in this state relax to the lower

energy twisted S1 state. The remaining 30% undergo an electrocyclic rearrangement to an isomeric 4a,4b-

dihydrophenanthrene (DHP) S1 state, as illustrated above by clicking on the diagram. Molecules occupying this new

excited state then relax to either DHP or cis-stilbene ground states. Over time, DHP accumulates and may be converted to

phenanthrene by mild oxidation with air or iodine. Substituted phenanthrenes thus become available from trans-stilbene

precursors prepared by Wittig or Grignard procedures.

Another minor product from the photolysis of stilbene has been identified as 1,2,3,4-tetraphenylcyclobutane (distilbene),

shown in the following diagram. Unlike the previously described unimolecular isomerizations, this compound is formed by a

bimolecular reaction between an electronically excited stilbene and a ground state stilbene molecule. The dimer

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Photosensitized Stilbene Isomerization

Sensitizer Triplet Energy Cis:Trans Ratio

benzophenone 69 kcal/mole 60:40

accumulates slowly, irradiation of a 0.07 M solution of trans-stilbene in benzene producing 27% (as two stereoisomers)

after two months of exposure. As expected, higher stilbene concentrations increase the rate of dimer formation. Thus, a

0.56 M solution of trans-stilbene in ethyl acetate yielded 11% dimer in four hours of irradiation. Mercury lamps were used as

the uv light source in all these cases.

Electron donating substituents on the benzene rings facilitate the dimerization, as does restricting the ability of the double

bond to isomerize or achieve orthogonally twisted excited states. Examples of these influences will be displayed above by

clicking on the diagram.

The stilbene reactions described above have been attributed to singlet excited states. Triplet excited states exist, but their

formation by intersystem crossing is inefficient. In order to study the behavior of triplet excited states it is often necessary

to generate them by energy transfer from a higher triplet excited state of a suitable sensitizer molecule. Spin conservation

requires that spin exchange take place during the collisional energy transfer. Thus, a sensitizer triplet (Zt), generated from

sensitizer molecule Zs, reacts with a ground state stilbene molecule (Ms) in the following manner:

Zt() + Ms() Zs() + Mt().

The following diagram illustrates important features of this sensitization reaction. The ideal sensitizer (Z) absorbs light

preferentially with respect to the substrate (M), and undergoes efficient intersystem crossing to a triplet excited state (T1).

This energetic state then serves to activate a substrate molecule to a lower energy triplet state by collisional exothermic

energy and spin exchange, returning the sensitizer to its ground state. A variety of useful sensitizers have been identified,

and by clicking on the diagram a few of these will be drawn below.

In the early 1960's Prof. George Hammond's group at California Institute of Technology undertook an extensive study of the

photosensitized isomerization of stilbene and related alkenes and dienes.

A few of their findings are presented in the table on the

right, the same photostationary cis:trans ratio being

observed from either isomer as the starting point. By

clicking on the diagram a second time a diagram

illustrating this system will be displayed above. The

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benzil 53 kcal/mole 85:15

pyrene 47 kcal/mole 90:10

eosin 43 kcal/mole 0:100

unexpected change in steady state isomer distribution withthe triplet energy of the sensitizer could not be rationalized

as a single classical energy transfer. All sensitizers having

a greater triplet energy than 60 kcal/mole act by rapid

collisional vertical energy transfer (heavy blue arrows) to

the first encountered stilbene isomer. The initial cis and trans triplets undergo fast, and in the case of trans reversible,

conversion to a lower energy twisted triplet, which then decays to cis and trans-stilbene at rates that favor cis by a factor of

1.5. As the triplet energy of the sensitizer drops below 57 kcal/mole, two changes occur. First, the efficiency of energy

transfer to cis-stilbene diminishes and the trans isomer is selectively activated, resulting in a greater [cis]/[trans]

photostationary state. Next, direct nonvertical excitation to the trans and twisted triplets may take place (light blue wavy

arrows). These competing excitations and subsequent decay to cis and trans ground states lead to remarkable variations

in isomer ratios. Finally, the very low energy triplet state of eosin is unable to effect any electronic excitation of stilbene, and

simply catalyzes thermal equilibration, which strongly favors the trans-isomer (trans is 6 kcal/mole more stable than cis)

These sensitized isomerizations do not give any significant amount of the electrocyclic rearrangement or dimerization

reactions observed from singlet excited states.

Carbonyl Compounds

Background

Conjugated ketones are often good sensitizers, thanks to the efficiency of intersystem crossing from the n * singlet to

the triplet. However, before discussing this application it will be helpful to consider the bonding structure of the carbonyl

group itself. In the case of the simple compound formaldehyde, the Lewis formula consists of two CH sigma bonds, a C

O sigma bond, a C=O pi bond and two non-bonding electron pairs. As

shown in the diagram on the right, two Lewis structures, differing in the

hybridization of oxygen, may be drawn, The structure on the left is a

common representation in which an sp2 oxygen replaces one of the

CH2 groups of an ethylene molecule. However, based on the principle

that stable molecules will adopt the strongest bonding possible, the right

hand structure becomes an attractive alternative. An sp2sp sigma

bond should be stronger and shorter than a sp2sp2 sigma bond, and the shorter bond distance will enhance the pi-

bonding. Double bonds are of course shorter and stronger than equivalent single bonds. The average values given in the

following table indicate that C=C is 13% shorter and 76% stronger than a CC bond, whereas C=O is 15% shorter and

over 100% stronger than a CO bond, possibly reflecting the sp hybridization of the oxygen. An important difference

between these models is found in the nature of the non-bonding electron pairs on oxygen. In the sp2-oxygen model these

occupy very similar (degenerate) orbitals, but in the sp-oxygen model one pair is in a relatively low energy sp-orbital and the

other in a higher energy p-orbital. Molecular orbital calculations clearly show that the latter model is a better representation

than the former.

Bond Length, CC, 1.54 C=C, 1.34 CO, 1.44 C=O, 1.22

Bond Energy, kcal/mole CC, 84 C=C, 146 CO, 86 C=O, 177

To examine the molecular orbitals of formaldehyde Click Here.

A general diagram illustrating the two major electronic excitations of a carbonyl group is shown below. This terminology

has been defined in the UV-Visible Spectroscopy chapter. The weak nature of the n * absorption is due to the poor

overlap of the p-orbital housing the higher energy electron pair with the * orbital (they are essentially orthogonal). In

contrast, and * orbitals overlap almost completely, so the probability of a * excitation being achieved by a photon

of proper energy is high. This spatial overlap requirement has been termed a selection rule by spectroscopists. A second

important selection rule concerns the probability of electronic transitions between states of different spin multiplicity, the

spin selection rule. This rule reflects the high probability of transitions between different singlet states, or between

different triplet states, but the low probability of singlet-triplet or triplet-singlet transitions. A table summarizing these rules is

given below.

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Formaldehyde, acetaldehyde and acetone show strong * absorption at 180 to 190nm ( = 103 to 104), and weak n

* absorption at 280 to 300 nm ( = 12 to 20). Conjugation with the -electrons of a double bond or a benzene ring

shifts both absorptions to longer wavelength and increases the strength of absorption.

Compound Cyclohexanone (CH3)2C=CHCOCH3 C6H5CHO C6H5COCH3

max * 200 nm ( 2000) 230 nm ( 12,300) 242 nm ( 14,000) 238 nm ( 13,000)

max n * 285 nm ( 14) 325 nm ( 90) 328 nm ( 50) 320 nm ( 40)

Aryl ketones such as acetophenone (right hand compound in the table above), undergo rapid intersystem crossing of the n

* singlet excited state to an energetically close * triplet state. The latter then quickly decays to the lower energy

n * triplet, as shown for benzophenone in the diagram below. This circuitous route for the low probability direct

conversion reflects modified selection rules formulated by Prof. M. A. El Sayed of UCLA (last two entries in the following

table). This pathway is not available to most aliphatic ketones, so their intersystem crossing rates from n * singlets to

triplets are slow.

As noted in the diagram, there is very little fluorescent decay from the S1 state, and radiationless decay to S0 is less than

1% of the intersystem crossing to T2. In the absence of quenching reactions, T1 returns to S0 by a mixture of

phosphorescent and radiationless decay.

Benzophenone Excited States


8/20

Some Carbonyl Selection Rules

Transition Probability Factor

S0 S1(n , *)

S0 S1( , *)

forbidden

----------------

allowed

orbital overlap

in space

(also symmetry)

Sn S1 S0Tn T1

allowedno change in

spin multiplicity

S(n , *) T(n , *)

S( , *) T( , *)forbidden

change in

spin multiplicity

S(n , *) T( , *)

S( , *) T(n , *)allowed

change in

orbital configuration

Reactions

H Abstraction, Bond Cleavage & Cycloaddition

The n * excited states of carbonyl compounds display a rich chemistry in their own right.

Since the oxygen has an unpaired electron, it behaves in much the same way as an alkoxy

radical, as noted in the chapter on free radical chemistry. Hydrogen abstraction and addition

to double bonds are typical reactions. Cleavage of neighboring carbon-carbon bonds may

also occur, the two most common of these being designated Type I and Type II. General equations for these primary

reactions, starting from aryl ketone excited states, are described in the following diagram. The n * excited state shown

in brackets at the center of the diagram may also be described as the resonance hybrid drawn on the right. Note that the

ground state polarity of the carbonyl group has been reversed in this excited state.

The triplet excited state of aryl ketones has a lifetime of about 100 ns, and most of the subsequent reactions are very fast

(rates range from 104 to 109 M-1 sec-1). Consequently, the effect of quenchers such as 1,3-pentadiene on product

distribution provides valuable information about the mechanisms. These quenchers have T1 energies much lower and S1energies higher than corresponding ketone states. The rate of quenching is nearly diffusion controlled, and is therefore

proportional to the concentration of the quencher. Since the ground state triplet of oxygen reacts rapidly with triplet excited

states, air must be excluded when studying these reactions.

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Examples of hydrogen abstraction and alkene addition reactions will be displayed above by clicking on the diagram.

Reduction of benzophenone to benzpinacol is common in most hydrocarbon solvents, even in pure benzene. The

diphenylmethanol radical formed by hydrogen abstraction is relatively stable and, once formed, dimerizes to benzopinacol

in nearly quantitative yield. In contrast, the more reactive isopropanol radical is converted to acetone by transferring its

hydroxyl hydrogen to benzophenone, thus forming another diphenylmethanol radical.

The photoaddition of carbonyl compounds to olefins had been observed by the Italian chemist E. Paterno in 1909, but the

structure of the oxetane products remained unknown until elucidated by Bchi and coworkers (M.I.T.) in 1954. This reaction

is now known as the Paterno-Bchi reaction. The mechanism shown here was established for the electron-rich alkene

dioxene, a compound that favors electron transfer to benzophenone. Other alkenes are also believed to react by way of a

1,4-biradical intermediate, and significant regioselectivity is found with many unsymmetrical alkenes. Two additional

examples of this reaction are drawn in the gray-shaded box at the bottom. The second illustrates the intramolecular variant.

A related example of carbonyl addition to alkenes is the use of benzophenone as a light activated initiator of polymerization

for monomers such as styrene and methyl methacrylate.

Examples of type I fragmentations are displayed below. These reactions are fast, and often proceed with a high quantum

yield. The first example, shown at the top, illustrates a typical homolytic cleavage of a carbonyl substituent, followed by a

fast hydrogen atom transfer between the caged radical pair. Three intramolecular type I reactions, all proceeding by way of

biradical intermediates, demonstrate the variety of products that may be formed by hydrogen transfer disproportionation

and/or ring closure. The cyclic transition states for such intramolecular hydrogen transfer usually include five or six, and

occasionally seven atoms.

By clicking on the diagram, examples of type II reactions will be displayed. These reactions all begin by an intramolecular

hydrogen atom abstraction, similar to the intermolecular abstraction in the reductive dimerization of benzophenone.The

general example at the top of the diagram shows how a key 1,4-biradical intermediate, formed by intramolecular hydrogen

abstraction, may disproportionate to several different products, including type II cleavage to the enol tautomer of a ketone

(green shaded box) and ring closure to a cyclobutanol (the Yang Reaction). In hydrocarbon solvents intramolecular

hydrogen transfer back to carbon is common, reducing the quantum yield of these products by over 50%. This reverse

hydrogen transfer is inhibited by hydrogen bonding solvents, which stabilize the newly formed OH group. As expected, the

rate at which the biradical is formed is sensitive to substitution at the -carbon. If R=H (a methyl group) the rate is 100

times slower than if R=CH3 (abstraction of a 3- hydrogen). This reactivity order reflects the bond dissociation energies of

the CH bonds in the same fashion as noted for free radical halogenation of alkanes. Also, replacement of all -hydrogens

by deuterium reduces the rate of biradical formation substantially.

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The ratio of type II cleavage and Yang cyclization products from a given substrate depends on several factors. The steroid

ketone in example 2 gives both reactions, with cyclization predominating. Example 3 is instructive, first because the rate of

biradical formation is much higher than in many other cases, as a result of conformational bias favoring the reactive

orientation (as drawn); and second, because cyclobutanol formation induces severe strain. Only type II fragmentation is

observed. Finally, example 4 proceeds by a -hydrogen abstraction (7-membered cycle), as the only possible

transformation of its kind. The resulting 1,5-biradical then closes to the product shown. Remarkably, phosphorescence

studies indicate that this reaction occurs from a low-lying * triplet state, rather than the n * triplet usually

associated with this class of reaction.

Type II reactions depend, of course, on close approach of the carbonyl oxygen to a -hydrogen. The conformational

mobility of the examples drawn above permits this to occur within the lifetime of the excited triplet. However, it is not difficult

to find molecules for which this is not possible. Benzoylcyclohexane, shown at the top of the following diagram, is such a

compound. Because of its equatorial location on the six-membered ring, the carbonyl oxygen cannot reach any of the -

hydrogens. If the benzoyl group is forced into an axial orientation by a large cis-tert-butyl group on c-4, then the oxygen can

easily reach the axial cis -hydrogens (colored red. The resulting type II photochemistry depends on the other C-1

substituent. If R = H, type II cleavage is the only product; however this changes to exclusive stereoselective cyclization if R

= CH3. The conformational drawings in the gray-shaded box suggest a reason for this remarkable change. Following the

initial hydrogen abstraction, the 1,4-biradical is well aligned for ring closure, but the benzyl radical must be rotated 90

before it is properly aligned for bond cleavage (far right structure). A C-1 methyl substituent hinders this rotation, leading to

formation of the strained cyclobutanol product.

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To learn more about Type II reactions Click Here.

Photoenolization

When the reactive carbonyl function and a -hydrogen are conjugated via an aromatic ring or double bond, the 1,4-diradical

created by hydrogen abstraction quickly relaxes to a conjugated enol tautomer. This is illustrated in the following diagram

for a -hydroxyl substituent, examples on the left, and an ortho-tolyl ketone on the right. If an aromatic ring has been

disrupted by the photoenolization, as in all the cases but avobenzone (lower left), the enoltautomer is unstable and rapidly

reverts to the initial aromatic carbonyl compound. This might appear to be a useless transformation, but it finds practical

application as a sunscreen ingredient. The three compounds on the left are examples of current sunscreen components.

Oxybenzone screens UVA, salicylate esters (R=C8 to C10) screen UVB and avobenzone screens both.

Careful studies of the photoenolization of ortho-alkyl benzophenones and acetophenones have enhanced our

understanding of this deceptively simple transformation. By clicking on the diagram the behavior of ortho-

methylacetophenone will be elaborated. Excitation of the anti and syn mixture of this ketone leads to two stereoisomeric

n * triplet states, TE and TZ respectively. The former has a much longer lifetime () than the latter since it must undergo

a conformational change before -H abstraction from the ortho-methyl substituent can take place. In both instances a

twisted triplet biradical is formed. This biradical may be intercepted by electron transfer to PQ2+ followed by rapid proton

loss. This event is easily monitored by the intense blue color of the PQ+ radical cation, and serves to set the lifetime of the

biradical at 580 nsec. Relaxation of the biradical leads to a mixture of (E) and (Z)-xylylenols, the latter undergoing rapid H-

transfer back to the starting ketone. (Z)-Xylylenol formation directly from a syn n * singlet state is possible and would

not be detected.

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Depending on the reaction conditions, (E)-xylylenols may undergo a variety of reactions or slowly relax back to the initial

ketone. Clicking on the above diagram a second time will show examples of other reactions (Part 3). Unlike benzophenone

itself, the ortho substituted compound in the upper left corner does not undergo any pinacol reduction. Instead, -H

abstraction produces a mixture of interconverting twisted biradicals which decay predominantly to (E,E) and (Z,E)-

xylylenols. Only the former is sufficiently long lived to yield distinctive products. At temperatures below 0 C conrotatory

electrocyclization forms cis-1,2-diphenylbenzocyclobutenol in high yield. At room temperature or above, conrotatory ring

opening regenerates the (E,E)-xylylenol which may be trapped by cycloaddition to maleic anhydride.

Competition between photoenolization and type II cleavage has been explored in the manner shown above, by clicking on

the diagram a third time (Part 4). The syn conformer of butyl (and isoamyl) o-tolyl ketone gives exclusive photoenolization,

60% from the n * singlet state, the corresponding triplet state undergoing xylylenol formation faster than type II

cleavage. The anti conformer reacts exclusively from the triplet state, which either isomerizes to the syn triplet or

generates the biradical precursor to type II products. As noted in the previous section, t-butanol favors type II cleavage. The

8-methyl-1-tetralone served as a reference molecule, constrained with the carbonyl oxygen syn to the methyl substituent.

Conjugated -Orbital Functions

Dienes and Polyenes

Acyclic conjugated dienes, trienes and polyenes absorb strongly in the 220 to 300 nm region of the near ultraviolet. The

resultant singlet excited states undergo a variety of reactions, as shown in the following diagram for 1,3,5-hexatriene and

two 2,5-dialkyl derivatives. Two configurational isomers (E & Z) are possible, together with three coplanar s-cis and s-trans

conformations for each (the cEt structure is not drawn). The E-configuration is normally more stable than its Z-isomer, and

for R=H or CH3 the elongated tEt conformation is preferred. The various conformers of both the E & Z-isomers are rapidly

interconverted at room temperature, the equilibrium composition depending on the size of substituents such as R. The light

induced isomerization about the central double bond of the trienes (e.g. EZ) is an example of OBF.

Now, electronic * excitation of any triene increases the -bonding between carbons 2 & 3 as well as 4 & 5, as may

be seen in the HOMO (3) and LUMO (4*) molecular orbitals of the parent triene. Taken together with the very short

lifetimes of these excited states (10 nsec), this suggests that photochemical products should reflect the rotamer

composition of the ground state. Put another way, excited state rotamers are not expected to equilibrate prior to reaction,

the NEER principle (Non-Equilibration of Excited Rotamers). An example of NEER is found in the absence of 1,3-

cyclohexadiene among the photoproducts from the parent triene (R=H), compared with its increased quantum yield as R is

changed to methyl and then tert-butyl (increased cZc concentration).

For E as well as Z-trienes, reactivity parallels an increase in the population of non-planar s-cis rotamers. Furthermore, 1,2-

divinylcyclopentene (drawn in the gray-shaded box) is photochemically unreactive and exhibits fluorescence in solution,

demonstrating that twisting about the central (3,4-) double bond of the triene is an essential factor in these reactions.

Irradiation of trans,cis,cis-1,3,5-cyclononatriene, shown at the bottom of the diagram, by 254nm light establishes a 60:40

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photoequilibrium with the cis-fused bicyclononadiene on its right. This equilibrium is shifted to the right by longer

wavelength 300nm light, which also induces further electrocyclization to tricyclo[4.3.0.0]non-3-ene. As a rule,

cyclohexadienes absorb light at longer wavelength than similar non-cyclic hexatrienes. Higher temperatures permit the

thermal electrocyclization of trans,cis,cis-1,3,5-cyclononatriene to the trans-fused bicyclononadiene on its left.

Finally, diradical mechanisms for the formation of allylcyclopropene (ACP), vinylcyclobutene (VCB) and bicyclohexene

(BHE) products will be shown above by clicking on the diagram. ACP may be formed from either the tEt or cZt excited

states, but VCB and BHE require the latter rotamer. The MVCP product on the left is unique to R = CH3.

As noted above, the reduced bond order of a formal double bond in its first excited state leads to the OBF mechanism for

isomerization in fluid solution. The torsional movement in this change is sensitive to the viscosity of the solution and to

other structural constraints that may exist. Thus, the facile isomerization and weak fluorescence, typical for trans-stilbene

in fluid solutions, change to low isomerization and strong fluorescence in rigid media at low temperatures. Here, the rapid

radiationless deactivation of the excited state by OBF is impeded and a normally non-fluorescent compound becomes

fluorescent.

A more complex, higher energy motion that achieves double bond isomerization in restrictive environments has been

described and named the Hula-Twist. As shown for a cis-stilbene derivative in the following diagram, the OBF process

involves a 180 flip of the aryl group on the right side of the double bond. By contrast, the HT process proceeds by

simultaneous rotation of a small CH moiety (light blue ellipse) about the double bond and an adjacent single bond (both

colored brown). This not only converts the cis-isomer to its trans-configuration, but also effects a conformational change

(note the orientation of the red hydrogen relative to the aryl substituent on its left).

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Show Hula-Twist Isomerization

The difference between OBF and HT isomerization of a Z to E-triene will be shown above by clicking on the diagram. It has

been proposed that photoisomerization of biologically important polyenes, such as retinal and calciferol may occur by the

HT mechanism because translocation of a single H-atom is less volume demanding than the turning over of one-half the

molecule, as required by the OBF process. This would be especially important when the chromophore is encapsulated in a

protein or bilayer membrane.

Instructive examples of the photochemical behavior of biologically important polyenes may be examined by clicking these

buttons.

Rhodopsin Bilirubin Vitamin D

Enone Reactions

[2+2]-Cycloaddition

In the earlier discussion of stilbene photoisomerization a [2+2]-cyclodimerization was noted. The construction of

cyclobutane rings from alkene components is rare in ground state chemistry, so a general photochemical synthesis of this

kind would provide a valuable addition to our assortment of useful carbon-carbon bond forming reactions. Double bonds

activated by conjugation with a carbonyl group have proven especially effective in this respect, both in forming [2+2] dimers

and adding to isolated alkene functions. A particularly important example of photodimerization involves the damage to DNA

caused by uv light. Thymine (or uracil in the case of RNA) is one of four heterocyclic base components of nucleic acids.

On exposure to ultraviolet light, thymine may undergo [2+2]-dimerization with a suitably oriented nearby thymine, as shown

in the diagram below. When this happens toxic products are generated that are directly responsible for cell death via

mutagenic action, suppression of DNA transformation and/or activation of carcinogenic pathways. A natural repair

mechanism employing a photolyase enzyme system reverses the dimerization.

Four possible dimers of thymine (and uracil) may be formed. The cis-syn isomer shown above is the chief dimer formed

by irradiation of DNA, or from frozen aqueous solutions of thymine or uracil. Other isomers are formed in varying amounts

from room temperature solutions of these bases. By clicking on the diagram a drawing showing the pertubation of DNA by

this dimerization will be displayed.

In reactions with unsymmetrically substituted alkenes, cyclic enones yield fused cyclobutane rings with variable regio and

stereoselectivity. As shown in the following diagram, the addition of 2-cyclopentenone to propene gives a mixture of

regioisomers, both having a cis-fused bicyclo [3,2,0] heptane unit. In contrast, addition of 2-cyclohexenone to 1,1-

dimethoxyethene proceeds with good regioselectivity and modest stereoselectivity favoring a trans-ring fusion. The last

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(i) Cyclization to a fused cyclobutane product.

(ii) Disproportionation by a 1,5-hydrogen transfer, yielding an or alkenyl-substituted ketone.

(iii) Fragmentation back to the starting compounds.

example demonstrates that unsaturated carbonyl functions other than ketones may lead to cycloaddition products, and that

functional substituents on the alkene moiety may influence the regioselectivity.

By clicking on the diagram, three more examples will be displayed, The first two confirm the modest [2+2] regioselectivity

noted in the first display and show additional monocyclic products. The third reaction discloses there is very low retention

of configuration in the cycloaddition of alkene stereoisomers. This stands in marked contrast to the high selectivity that

characterizes [4+2] cycloadditions known as the Diels-Alder reaction. A similar lack of stereoselectivity is found in

intramolecular [2+2] cycloadditions, as may be seen by clicking the diagram a second time. Three additional examples of

the intramolecular variant (I. II & III) are also presented in this new display. The importance of this method for the assembly

of complex molecules is shown by the short efficient synthesis of the sesquiterpene isocomene accomplished by M.

Pirrung.

The poor selectivities and modest quantum yields observed for these cycloaddition reactions have engendered several

mechanistic interpretations. Identification of the enone excited state as a * triplet comes from selective quenching

studies as well as transient absorption spectroscopy. Bauslaugh's proposal that this triplet adds to the alkene to form a

1,4-biradical proposal is still the simplest and most satisfying explanation of the facts. As shown in the following diagram,

the initial bonding may take place at either the or -carbon of the enone. The resulting biradicals would also be triplets,

and on intersystem crossing to a singlet could yield ground state products by one of three paths.

The latter event accounts for low quantum yields, and is presumed to be fast because isomerization of recovered alkene is

small when cis and trans-2-butene are used as the alkene reactant. For the addition of cyclopentenone to isobutene, four

possible biradicals may be drawn, the estimated stability order being II > I > III > IV. Finally, although the biradical species

are very short lived (ca. 60 ns), it has been possible to trap them by use of the foul-smelling, highly-toxic, hydrogen donor

hydrogen selenide. The results of such a trapping study will be displayed below by clicking on the diagram.

Several important conclusions were reached in this case. First, no initial addition to the more substituted carbon of the

alkene took place, since tert-butyl substituted cyclopentanones would have been produced (via III & IV) and none were

found. Second, although initial bonding at the -carbon (yielding II) was nearly twice as fast as -bonding, over 96% of II

fragmented to starting materials, compared with 79% of I. Consequently most of the trapped products came from I. These

products were formed either by hydrogen atom delivery to both radical sites (giving saturated compounds) or hydrogen

delivery followed by hydrogen abstraction by HSe. (giving unsaturated compounds), as noted in the gray-shaded box

bottom-right..

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The formation of trans-fused bicyclo [4,2,0] octane products from 2-cyclohexenone has been explained by considering the

conformations of the 1,4-biradical intermediates. This will be illustrated above by clicking the diagram a second time. Here,

three rotamers (1, 2 & 3) for both the and chains are drawn. When the radical sites are far apart (2 and 3),

fragmentation of the biradical is likely. The trans-ring fusion will be formed from conformation 1, and cis from 3. The

latter bonding will be subject to some axial hindrance. For the -manifold, 1 should yield a cis-fused product and 2 the

trans-isomer. However the latter bonding would again be hindered.

The de Mayo Reaction

In 1962 Paul de Mayo (Univ. Western Ontario) found that the enol of pentane-1,3-dione gave a 2-acetyl-1-

methylcyclobutanol adduct when irradiated in the presence of a cycloalkene. As shown by the top reaction in the following

diagram, this cyclobutanol (R1 = R2 = CH3) may then undergo a facile base-catalyzed retroaldol fragmentation to a 1,5-

diketone. This sequence thus achieves the attachment of a short alkyl chain to each carbon atom of the double bond.

Further base induced reactions, such as epimerization of the initial cis-configuration, and aldol cyclization of the diketone

may follow. Following its initial report, this powerful [2+2]-cycloaddition reaction sequence has been put to many uses. One

of these is the synthesis of -tropolone shown by the bottom equation.

Two additional applications of the de Mayo reaction in synthesis will be displayed above by clicking on the diagram. The

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upper reaction is noteworthy for the unexpectedly high regioselectivity of the [2+2] cycloaddition. Ring opening of the

bicyclo[3.2.0]heptane moiety proceeds by an ethylagous elimination or Grob fragmentation. Conversion of the resulting

bicyclic ketoacetal to -himachalene was straightforward. The lower reaction demonstrates that poor stereoselectivity in

the cycloaddition does not necessarily present a problem. Here, the four new stereocenters in the cycloadduct are lost

and/or epimerized by the retroaldol opening of the four-membered ring and subsequent aldol cyclization.

Cyclohexadienone Reactions

Cross-Conjugated Derivatives

Derivatives of 2,5-cyclohexadienone are common in nature, and their photochemical transformations posed a challenge to

early researchers. Some reactions of 4,4-diphenyl-2,5-cyclohexadienone are presented in the following diagram. Although

2,3-diphenylphenol was a product from irradiation in aqueous dioxane, it is actually formed from 6,6-

diphenylbicyclo[3.1.0]hex-3-ene-2-one, the initial rearrangement product. It should be noted that a similar

bicyclo[3.1.0]hexane isomer was formed by irradiation of 4,4-diphenyl-2-cyclohexenones, as shown in the gray-shaded box

at the bottom right.

These photochemical rearrangements occur by way of triplet excited states, which are conveniently depicted as diradicals.

Mechanisms for these reactions will be displayed above by clicking on the diagram. Bond reorganization may take place in

the triplets, which eventually intersystem cross to singlet species. Charge separation in these states may then lead to

rearrangement to a stable product.

The photo-isomerization shown above is one example of a general family of reactions known as di--methane

rearrangements, other examples of which are illustrated in the following diagram. These transformations are often photo-

sensitized, indicating they proceed by way of triplet excited states. As the name suggests, substrates exhibiting this

rearrangement are comprised of two -functions separated by a saturated (sp3-hybrid) carbon atom (designated by a red

dot in the illustration). In the event, a 1,2-shift of one ene-group, followed by a bond formation between the terminal sites of

the remaining -function leads to a vinylcyclopropane product. One of the unsaturated functions may be a carbonyl or

imine group, as in examples 2. and 3.

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A photo-isomerization of this kind was used by H. Zimmerman (Wisconsin) to prepare the novel self-replicating diene

semibullvalene from barrelene.

Conjugated Derivatives

Derivatives of 6,6-disubstituted 2,4-cyclohexadienones are also photochemically reactive. Some examples are given in the

following diagram. Electrocyclic ring opening to an unsaturated ketene is the favored transformation. Since nucleophilic

compounds such as water, alcohols and amines add rapidly to ketenes, the resulting carboxylic acid or derivative is the

final isolated product. If no nucleophilic reactants are present, the conjugated ketene diene will recyclize to the starting

compound. Slower reactions leading to phenolic products may then occur. In the last (bottom) example, additional methyl

substituents reduce the reactivity of the trans-ketene intermediate, so that only strongly nucleophilic amines are able to trap

it. The ketene is removed by light induced isomerization and cyclization. As in the previous dienones, a triplet excited state

undergoes decay to polar singlets that are thought to decompose in the manner depicted in the gray-shaded area.

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Among the natural dienones displaying interesting photochemical behavior, the sesquiterpene santonin is exceptional, and

has been the subject of exhaustive study. Click the button to learn more about this subject.

Santonin

The names and association (at the time of their major work) of many chemists whose research has led to the development

of modern photochemistry are presented in the following table.

Name Location

D. H. R. Barton Imperial College, London

G. H. Bchi Massachusetts Institute of Technology

O. Chapman Iowa State University

P. de Mayo University of Western Ontario

G. S. Hammond California Institute of Technology

R. S. Liu University of Hawaii

D. C. Neckers Bowling Green State University

J. Saltiel Florida State University

J. C. Scaiano Ottawa Chemistry Institute

G. B. Schuster Georgia Institute of Technology

N. J. Turro Columbia University

P. J. Wagner Michigan State University

A. Weedon University of Western Ontario

N. C. Yang University of Chicago

H. E. Zimmerman University of Wisconsin

For more click here.

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photochemistry basics

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