Metal-Only Lewis Pairs with Transition Metal Lewis Basas

CHE 135 Experiment 2, General Chemistry III Lab, Spring Quarter 2015-2016, DePaul University. [Online] htps://www.d2l.depaul.edu (April 19, 2016).

Typically an ionic bond occurs between one metal and one non-metal ion. One atom borrows one or more electrons from another atom. An ionic bond is a type of chemical bond that occurs when one atom loses an electron to form a positive ion and the other atom gains an electron to form a negative ion, which then result in attraction.

Redox reactions are an important class of reactions in organic chemistry that involve the transfer of electrons from

In metallic bonding, the reason it is so good at conducting heat and electricity, is the electrons are loosely held in the atom. Also, the structural pattern of metals is hexagonal-close-packing (Francis, E . . .). Metallic bonds are when the electrons are shared and are able to move and how C models show that. The idea of the electrons being able to move, delocalized electrons, helps produce its characteristics like conductivity and malleability, etc. (Anderson . . .). In a redox reaction, oxidation and reduction happens. Also you can’t have reduction happening without oxidation also happening along with it. Redox reactions oxidation is the loss of electrons
and reduction is the gain of electrons (Redox . .

The free radical chlorination of 1-chlorobutane resulted in a mixture of at least 4 different possible products from the reaction. Gas chromatography-mass spectrometry helped in figuring out which of the products are most abundant in the sample product created as well as in discovering the ratio of relative reactivities of the hydrogens. This experiment showed that the ratio of relative reactivities was found to be 1.0 : 3.5 : 6.2 : 2.4, which indicates that the secondary hydrogens are more reactive than the primary hydrogens and that reactivity further increases the further away the hydrogen is from the chlorine on the 1-chlorobutane. The results agree with the conjecture that the primary hydrogens are less reactive than

Grignard Reactions Introduction Grignard reactions are of extreme importance in synthesis of many organic compounds. Because of the extreme nucleophilic tendencies of the Grignard reagent (typically denoted RMgX, where R is an organic nucleophile, and X is a halide), we find that Grignard reagents are extremely useful for the addition of organic fragments. The Grignard reagent’s extreme nucleophilicity can be explained by its unique bonding abilities. Because the carbon-magnesium bond is neither fully covalent nor fully ionic, this creates a very stable yet reactive region at the pseudohalide. Furthermore, the relatively similar electronegativities of the two adjacent atoms create a strong pole between the two, while still stable enough to

[27] Aluminium (III) isopropoxide is widely versatile catalyst giving different reactivity in different type of solvents. Aluminium (III) isopropoxide do not exist in single molecules but as trimers or tetramers that do not have the same reactivity. [7] As seen in figure 7, an equilibrium state can be achieved between trimers and tetramers with tetramers being more stable. The actual catalyst-initiator for ROP of e-caprolactone is prepared by dissolving the trimers in e-caprolactone which separates itself into single molecule to form a six-coordinated aluminium complex, figure 8. [28]

My participation in the SURC conference will allow me to practice sharing the findings discovered in my research in Dr. Ferreira's lab for the investigation of the photoredox catalysis. This practice will be valuable for my growth as a researching scientist, who will be practicing research and presenting the work to others in the future. Attending this conference would enable me to continue practicing this pertinent skill in the realm of research. My involvement with the conference would be great practice from the usual presentations in the lab group meeting as I must be able to articulate the purpose and data to scientists, who may be unfamiliar with organometallic catalysis and the efforts towards synthetic method development. This topic of research was not widely represented at SURC the previous year, and the exhibition of my research would add to the overall diversity of the types of research presented at SURC.

This is a reaction between some metals and oxygen. Electrons jump from the metal to the oxygen and form a layer of oxidation on the metal (nobelprize.org, 1992). This reaction is also an example of a reaction reduction and is called a redox reaction (stands for reduction-oxidation)(thoughtco.com, N.D). In this practical, the heat released in the chemical

Free-radical chain reactions involve the formation of halides and alkyl halides by reacting diatomic halogens with reactive hydrogens attached to hydrocarbons. In this experiment, diatomic bromine was reacted with various arenes to produce hydrobromic acid and alkyl halides. The mechanism behind this reaction can be characterized by three distinct phases: initiation, propagation, and termination. During the initiation step, bromine radicals are produced via thermal or photochemical homolysis. These bromine radicals then react with hydrogens attached to a hydrocarbon in the propagation step to produce hydrobromic acid and a carbon radical. The chain reaction continues since the carbon radical formed can react with another diatomic bromine molecule, producing a carbon-bromine bond and regenerating a bromine radical. The termination step ends the reaction by reacting two bromine radicals with each other, lowering the concentration of highly reactive bromine radicals in solution.

Olmsted, John III; Williams, Greg; Burk, Robert C. Chemistry, 1st Canadian ed.; John Wiley and Sons Ltd: Mississauga, Canada, 2010, pp 399 - 406

De re modality refers to the quantification of possibility and necessity claims in regards to the object or individual; rather than relying on a statement for quantification claims. To put this another way, when we make possibility and necessity claims we refer to the actual object rather than the statement itself.

As a class, we were able to compare and contrast the colors of the aromatic azo compounds from several different coupling partners as well as different substitution patterns for each (i.e. ortho, para, meta). This type of synthesizing molecules to create an array of potentially useful compounds is known as combinational chemistry. In combinatorial synthesis, when using a compound with multiple points of diversity, or R groups which can be substituted, a substantial number of possible structures can be found depending on the number of substituents utilized. Laboratories can use automated technologies to perform these types of reactions on an industrial scale but scientists can also utilize these methods to synthesize and compare a select few molecules [2]. More specifically, the type of combinatorial synthesis utilized by our lab is known as “parallel synthesis”. In parallel synthesis, a number of reactants are available to react individually with a number of substrates which produces a substantial number of unique and potentially useful compounds. One way of organizing the information about these reactions is to create a table with the reactants

Green chemistry shapes the ways in which chemical processes or products can become ‘greener’. Green chemistry is also defined as sustainable chemistry, chemistry that reduces its negative effects of the environment, and life forms within, both long term and short term. Within green chemistry there are 12 primary principles; atom economy, less hazardous chemical synthesis, designing safer chemicals, safer solvents and auxiliaries, design for energy efficiency, use of renewable feedstocks, reduce derivatives, catalysis, design for degradation, real-time analysis from pollution prevention and inherently safer chemistry for accident prevention, all of which branch under the key principle; prevention.

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].