Related Experiment Video
Updated: Feb 25, 2026

06:53
Photoelectron Imaging of Anions Illustrated by 310 Nm Detachment of F−
Published on: July 27, 2018
9.2K
Size Effect in the Ionization Energy of PAH Clusters
C Joblin1, L Dontot1, G A Garcia2
1IRAP, Université de Toulouse, CNRS, UPS, CNES , 9 Av. du Colonel Roche, 31028 Toulouse Cedex 4, France.
The Journal of Physical Chemistry Letters
|July 26, 2017
Summary
Scientists measured ionization energies for polycyclic aromatic hydrocarbon (PAH) clusters, finding they decrease with size. This research supports PAH presence and ionization in space.
Area of Science:
- Physical Chemistry
- Astrochemistry
- Quantum Mechanics
Background:
- Polycyclic Aromatic Hydrocarbons (PAHs) are abundant in space.
- Understanding PAH ionization is crucial for astrochemistry.
- Previous studies lacked experimental ionization data for PAH clusters.
Purpose of the Study:
- To experimentally measure near-threshold photoionization spectra of pyrene and coronene clusters.
- To compare experimental ionization energies with theoretical calculations.
- To investigate the influence of cluster size and temperature on ionization energy.
Main Methods:
- Utilized imaging photoelectron-photoion coincidence spectrometry.
- Employed a VUV synchrotron beamline for measurements.
- Performed electronic structure calculations for ionized molecular clusters.
Main Results:
- Observed a consistent decrease in ionization energy with increasing cluster size for both pyrene and coronene.
- Achieved quantitative agreement between experimental and theoretical ionization energies when including temperature effects.
- Identified a discontinuity in the ionization energy trend for the pyrene hexamer.
Conclusions:
- The study validates theoretical models for describing the electronic structure of PAH clusters.
- PAH clusters are likely ionized in astronomical environments.
- Experimental data provides benchmarks for theoretical advancements in PAH cluster research.
Related Concept Videos
Ionization Energy
43.8K
The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its first ionization energy (IE1). The first ionization energy for an element, X, is the energy required to form a cation with 1+ charge:
43.8K
The Energies of Atomic Orbitals
30.4K
In an atom, the negatively charged electrons are attracted to the positively charged nucleus. In a multielectron atom, electron-electron repulsions are also observed. The attractive and repulsive forces are dependent on the distance between the particles, as well as the sign and magnitude of the charges on the individual particles. When the charges on the particles are opposite, they attract each other. If both particles have the same charge, they repel each other.
30.4K
π Electron Effects on Chemical Shift: Overview
1.7K
An applied magnetic field causes loosely bound π-electrons in organic molecules to circulate, producing a local or induced diamagnetic field over a large spatial volume. As the molecules tumble in solution, the field generated by π-electrons in spherical substituents results in a zero net field. However, the net field generated by π-electrons in non-spherical substituents is not zero. The effect of this induced field depends on the orientation of the molecule with respect to B0,...
1.7K
Atomic Radii and Effective Nuclear Charge
62.6K
The elements in groups of the periodic table exhibit similar chemical behavior. This similarity occurs because the members of a group have the same number and distribution of electrons in their valence shells.
62.6K
π Electron Effects on Chemical Shift: Aromatic and Antiaromatic Compounds
2.0K
In aromatic compounds, such as benzene, the circulation of (4n + 2) π-electrons sets up a diamagnetic or diatropic ring current around the perimeter of the molecule. This current induces a magnetic field that opposes the external field inside the ring and reinforces it on the outside. The protons in benzene are deshielded and exhibit high chemical shifts in the range 6.5–8.5 ppm. The shielding effect at the center of the ring is evident in complex aromatic molecules, such as...
2.0K
Ionic Radii
34.2K
Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it is smaller than the atom from which it is derived. For example, the covalent radius of an aluminum atom (1s22s22p63s23p1) is 118 pm, whereas the ionic radius of an Al3+ (1s22s22p6) is 68 pm. As electrons are removed from the outer valence shell, the remaining core electrons occupying smaller shells experience a greater effective nuclear...
34.2K

