Chromophore

Source: Wikipedia, the free encyclopedia.
Leaves change color in the fall because their chromophores (chlorophyll molecules) break down and stop absorbing red and blue light.[1]

A chromophore is a

leaves
. The color that is seen by our eyes is that of the light not absorbed by the reflecting object within a certain wavelength spectrum of visible light. The chromophore indicates a region in the molecule where the energy difference between two separate molecular orbitals falls within the range of the visible spectrum (or in informal contexts, the spectrum under scrutiny). Visible light that hits the chromophore can thus be absorbed by exciting an electron from its ground state into an excited state. In biological molecules that serve to capture or detect light energy, the chromophore is the moiety that causes a conformational change in the molecule when hit by light.

Healthy plants are perceived as green because chlorophyll absorbs mainly the blue and red wavelengths but green light, reflected by plant structures like cell walls, is less absorbed.[2]
β-carotene
molecule are highlighted in red.

Conjugated pi-bond system chromophores

The porphyrin moieties in our red blood cells, whose primary function is to bind iron atoms which capture oxygen, result in the heme chromophores which give human blood its red color. Heme is degraded by the body into biliverdin (which gives bruises their blue-green color), which in turn is degraded into bilirubin (which gives patients with jaundice a yellow skin tone).
In the mammalian eye, the molecule retinal is a conjugated chromophore. Retinal begins as 11-cis-retinal, which, upon capturing a photon γ (light) of the correct wavelength, straightens out into all-trans-retinal which pushes against an opsin protein in the retina, which triggers a chemical signaling cascade which results in perception of light or images by the brain.

Just like how two adjacent p-orbitals in a molecule will form a

pi-bond, three or more adjacent p-orbitals in a molecule can form a conjugated pi-system. In a conjugated pi-system, electrons are able to capture certain photons as the electrons resonate along a certain distance of p-orbitals - similar to how a radio antenna detects photons along its length. Typically, the more conjugated (longer) the pi-system is, the longer the wavelength of photon can be captured. In other words, with every added adjacent double bond we see in a molecule diagram, we can predict the system will be progressively more likely to appear yellow to our eyes as it is less likely to absorb yellow light and more likely to absorb red light. ("Conjugated systems of fewer than eight conjugated double bonds absorb only in the ultraviolet region and are colorless to the human eye", "Compounds that are blue or green typically do not rely on conjugated double bonds alone.")[3]

In the

Woodward–Fieser rules can be used to approximate ultraviolet-visible maximum absorption wavelength in organic compounds with conjugated pi-bond systems.[citation needed
]

Some of these are metal complex chromophores, which contain a metal in a

heme group (iron in a porphyrin ring) of hemoglobin, or magnesium complexed in a chlorin-type ring in the case of chlorophyll. The highly conjugated pi-bonding system of the macrocycle ring absorbs visible light. The nature of the central metal can also influence the absorption spectrum of the metal-macrocycle complex or properties such as excited state lifetime.[4][5][6] The tetrapyrrole moiety in organic compounds which is not macrocyclic but still has a conjugated pi-bond system still acts as a chromophore. Examples of such compounds include bilirubin and urobilin
, which exhibit a yellow color.

Auxochrome

An auxochrome is a functional group of atoms attached to the chromophore which modifies the ability of the chromophore to absorb light, altering the wavelength or intensity of the absorption.

Halochromism

Main article: Halochromism

Halochromism occurs when a substance changes color as the

molecular structure changes upon certain changes in the surrounding pH. This change in structure affects a chromophore in the pH indicator molecule. For example, phenolphthalein
is a pH indicator whose structure changes as pH changes as shown in the following table:

Structure
pH 0-8.2 8.2-12
Conditions acidic or near-neutral basic
Color name colorless pink to fuchsia
Color

In a pH range of about 0-8, the molecule has three

carbon atom in the middle which does not make the π-bonding in the aromatic rings conjugate. Because of their limited extent, the aromatic rings only absorb light in the ultraviolet region, and so the compound appears colorless in the 0-8 pH range. However, as the pH increases beyond 8.2, that central carbon becomes part of a double bond becoming sp2 hybridized and leaving a p orbital to overlap with the π-bonding in the rings. This makes the three rings conjugate together to form an extended chromophore absorbing longer wavelength visible light to show a fuchsia color.[7] At pH ranges outside 0-12, other molecular structure changes result in other color changes; see Phenolphthalein
details.

Common chromophore absorption wavelengths

Functional group or compound Absorption wavelength
Bromophenol blue (yellow form) 591 nm[8]
Malachite green 617 nm[9]
Cyanidin 545 nm[citation needed]
β-carotene
 452 nm[citation needed]

See also

References

  1. PMID 26919572
    .
  2. doi:10.1080/00219266.2020.1858930
    .
  3. ^ Lipton, Mark (Jan 31, 2017). "Chapter 1: Electronic Structure and Chemical Bonding, Chapter 1.10: Pi Conjugation". Purdue: Chem 26505: Organic Chemistry I (Lipton), LibreTexts edition. Purdue University.
  4. NAID 10005456738
    .
  5. ISBN 978-1-4020-4515-8
    .
  6. ^ Shapley, Patricia (2012). "Absorbing light with organic molecules". Archived from the original on 2013-06-21. Retrieved 2012-12-14.
  7. ^ Clark, Jim (May 2016). "UV-Visible Absorption Spectra". chemguide.co.uk.
  8. ISBN 9781464135385
    .
  9. OCLC 851381738
    .

External links
Retrieved from "https://en.wikipedia.org/w/index.php?title=Chromophore&oldid=1223468929"