What Is The Interaction Of Small Cobalt Clusters With Circumcoronene?

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CHE 131 Experiment 8, General Chemistry 1 Lab, 1 Quarter 2015-2016, DePaul University. [Online] https://www.d2l.depaul.edu (November 09, 2015).

The students created a macroscopic, three-dimensional (3D) model of several properties of the periodic table. They explained in their own words the following terms: atomic radii, ionic radii, first ionization energy, and electronegativity. Lastly, they identified, described, and explained the patterns observed in the 3D periodic tables for the following element properties: atomic radii, ionic radii, first ionization energy, and electronegativity.

References are properly cited within the paper; reference page includes all citations; proper title page and introduction are present and evidence of spell check and grammar check are not obvious. Seven to 10 errors noted.

In order to synthesize our metal complexes, we were able to make both Copper and Ruthenium metals. From this, we combined each metal complex with DMSO by refluxing the compound. The metal complexes were analyzed through their melting point and IR spectroscopy to determine whether the metal bonded to a Sulfur atom or an Oxygen atom of the DMSO. After analyzing the IR spectrum, it was determined that S=O shifted to a lower wavenumber in CuCl2~2DMSO and that S=O shifted to a higher wavenumber in RuCl2~4DMSO.

This explains how the presence of a single fluoride atom instead of a hydrogen impacts the structure and charge distribution of the cyclic hydrocarbon. In turn adding a Fluoride atom also increases the energy of the cyclic hydrocarbon creating less stable structures in boat, twist and half chair increasing ΔG and decreasing the amount of other conformers in a solution compared to chair.

In final analysis, the electronegativity and density periodic trends trends are fairly consistent. Electronegativity decreases when going down groups, while density increases. However, the outliers of these trends are the noble gases, because of their stable, unreactive properties. In addition to helping students learn about periodic trends, it also demonstrated to students how these trends were of great use for previous scientists when they worked together to discover new elements that were missing on the periodic

This source is relevant and important because as I stated in the summary, it allows you to see

14. Egeland, GM, Sweney, MH, Fingerhut, M. Halperin, W., Willie, and K. Schnorr, T. (2007).

Chang, R. (2010). Chemistry. 10th ed. 1221 Avenue of the Americans, New York: McGraw- Hill Companies, Inc.

The electronic structure of the doped fullerene interacting with L-Alanine compared to pure fullerene C20 has been calculated with the B3LYP/6-31G basis set. The molecular orbital theory, the chemical reactivity of a molecular system can be estimated using HOMO and LUMO energies and overlaps of molecular orbital [12-14]. In our present investigation the HOMO-LUMO gaps of C19Si-L-Alanine (Si-N) and C20-L-Alanine (C-N) are 2.48768 and 1.81637eV respectively so C19Si-L-Alanine has the more molecular kinetic stability. These energy gap values of C19Si-L-Alanine are higher than fullerene with amino acids. The HOMO and LUMO energy gap is an important measure for stability indexes in various chemical and biochemical systems.

I do not recommend any major changes to the paper; however, I do recommend a couple of minor changes:

value of 0.087 micro g. These results support and expand our understanding of the mechanisms

Both physicists and chemists have investigated the CO2 anion extensively over the past few decades because of its importance in atmospheric chemistry, gas lasers, and a multitude of different industrial applications. It has been observed in a variety of experimental processes such as electron collisions and high-energy applications. As is well-known, electrons cannot permanently attach to the CO2 molecule; as such, all CO¬2 anion states are inherently metastable and have finite lifetimes. Despite the many studies, both experimental and theoretical, there are still a number of unanswered questions, especially concerning the relationship between short-lived and long-lived temporary anion states. Direct electron attachment to the CO2 molecule produces only short-lived anion states with lifetimes in the femtosecond range. These short- lived species consist most importantly of the low lying anionic states 2Πu and 2Σg+ 1–6. They are the main contributor to the electron scattering from neutral CO2. The 2Σg+ virtual state is responsible for the zero-energy peak in scattering experiments with energies for electron scattering below 1eV, while the 2Πu resonance state can be attributed to the observed peak in scattering cross sections at about 3.8eV. Long-lived CO2 anion states on the other hand, have been observed with lifetimes in the microsecond, even millisecond range7,8. They can be produced in processes such as double electron attachment to CO2+ ions9,10, sputtering techniques11,

When CO2 interacts, a charge polarization mechanism takes places in which a metal ion polarizes the nearby CO2 molecule and a weak van der Waals’ interaction formed between the CO2 molecule and MOF-5. Furthermore, the bonding between the metal ion and CO2 molecule at this site also might be through a simple dispersion and electrostatic interaction [76x].