Abastract
The intermolecular interactions between halo-cyclopropenone derivatives (HC3OX;X= F, Cl, Br and I) and hypohalous acids (HOY; Y=F, Cl, Br and I) were investigated using the MP2 method with aug–cc-pVTZ basis set. Three types of complexes are forming by:1) hydrogen bond, 2) both hydrogen and halogen bonds, 3) halogen bond interactions. The results indicated that interactions in type 1 complexes are stronger than those in types 2 and 3. The H–O bonds show red shifts with complex formation in types 1 and 2, in which they are more considerable for type 1 complexes. The O–Y bonds display red shifts in the type 3 and blue shift in the type 2 complexes. Molecular electrostatic potential (MEP), quantum theory of atoms in molecules (QTAIM)
…show more content…
The graphical illustration of the representative configurations under consideration is depicted in Figure 2. Possible interactions which considered for HOY molecules with HC3OX are including hydrogen bonding (O···H) and halogen bonding (X···Y,O···X) which have been denoted as XYm. The X is representing the cyclopropenone (HC3OF, HC3OCl, HC3OBr, and HC3OI were defined as F, Cl, Br and I, respectively); Y shows the HOY molecules (HOF, HOCl, HOBr, and HOI were defined as F, Cl, Br and I, respectively) and m was applied for displaying the type of complex that formed between them. For example FI1 shows type 1 complex of HC3OF with HOI or BrBr2 is illustrating type 2 complex of HC3OBr with HOBr. The XY1 type shows O···H interactions, which HOY acts as hydrogen bond donor (HBD). In the XY2 type, the O···H and X···Y interactions have been assigned between HOY and HC3OX molecules. In the H···O interaction HOY acts as HBD while in the X···Y it might act as electron acceptor (Lewis acid) or electron donor (Lewis base) regarding the nature of X and Y atoms. In the XY3 model a halogen bond (XB) interaction was found between HC3OX and HOY in which Y atom of HOY as electron acceptor interact with O atom of HC3OX as electron donor. It should be noted that no halogen bond was observed between HC3OX and HOF (FF3, ClF3, BrF3 and IF3). The intermolecular distances for complexes and the bond lengths difference between complexes and isolated monomers are listed in Table 1. The O···H (Types 1 and 2), X···Y and O···Y distances are in the ranges of 1.762–1.809 Å, 1.746–1.823 Å, 3.064–4.182 Å, and 2.610–2.697 Å, respectively. The calculated intermolecular distances for O···H (Types 1 and 2) and O···Y are less than the sum of the van der Waals (vdW) radii of the corresponding atoms (vdW radii for H, O, F, Cl, Br and I are 1.20, 1.52, 1.47 , 1.75, 1.85 and 1.98 Å, respectively [40]), indicating attractive
Many sources of error were responsible for recovering a small amount of product. Introduction: The carbon-carbon bond formation is an important tool in organic chemistry to construct the simple as well as an organic compound. There are several
3.3. Frontier molecular orbital The electronic structure of the doped fullerene interacting with glycine compared to pure fullerene C20 has been calculated with density functional theory using the B3LYP/6-31G basis set. The molecular orbital theory, the relative chemical reactivity of a molecular system can be estimated using HOMO and LUMO energies and overlaps of molecular orbital [18-20]. The electronic transition from the HOMO to LUMO are mainly derived from the electron density transfer n orbital to p* orbital.
4.) I noticed that there is a relationship between the ionic radius and the atomic number of the representative elements in Group 1A. The higher the atomic number, the bigger the ionic radius is. So, while hydrogen has an atomic number of 1 and Francium has an atomic number of 87, it is safe to assume that FR has a higher ionic radius. This is true; the ionic radius for Hydrogen is 0.012, and for Francium, it is 0.194.
As different bonds require different amounts of energy to bend and stretch, they absorb and transmit different amounts of radiation. This data is then collected by the spectrometer and transposed into graph form. The different amounts of absorbance for various functional groups and types of bonds have been established and can be used to identify compounds. Also, an IR spectrum can be compared to known “fingerprint” spectra in order to identify the compound. When compared to the fingerprint spectrum for 1-bromobutane found in Experimental Organic Chemistry, the IR spectrum collected from the data was very similar.
Our latest lab covered a detailed description of atoms and molecules, laid out in a distinctive way using balls and sticks for valence electrons and bonds. We were given charts to fill out recoding our findings regarding several molecules and their electron count, type of bonds,
Firstly, intermolecular forces and strengths of different chemical substances could be identified using valence shell electron pair repulsion shapes and prior knowledge of various kinds of intermolecular forces: London Dispersion, Dipole-Dipole, and Hydrogen bonding. Knowing this, Acetone was seen to possess London Dispersion and Dipole-Dipole forces. Propanol was seen to possess London Dispersion, Dip0le-Dipole forces, and Hydrogen Bonding. Acetic Acid was seen to possess Hydrogen Bonding and Dipole-Dipole forces. Overall,
In the end, it was concluded that Unknown 30A may have a low molecular weight and was an amine because it turned the red litmus paper blue, after being soluble in water. Therefore, the solubility of the unknown occurred due to weak intermolecular attractive forces of hydrogen bonds. Small amines form hydrogen bonds in water. As a result, the litmus paper turned red to blue because the amine accepted protons from their bond with water molecules, and was basic.
For this experiment, stereochemistry was observed by analyzing both the isomerization of dimethyl maleate and carvones. The dimethyl maleate is formed by two methyl ester groups that are connected by an alkene. They are in a cis-conformation meaning they are on the same side of the alkene, therefore the esters are close to one another. This conformation is strained and sterically hindered due to electrons repelling each other and are enantiomers of one another. With the use of radical chemistry, the cis conformation can be changed into a trans configuration where the esters are on opposite sides of one another.
The constant variable is the amount of sodium hydroxide. Literature review A covalent bond is a chemical bond that involves the sharing of electron pairs between atoms. These electron pairs are shared pairs and bonding pairs, and the stable balance of attraction and a repulsive force between atoms, when they share electrons is called covalent bonding.
Aims of experiment • Determine the rate constants for hydrolysis of (CH3)3CCl in solvent mixtures of different composition (50/50 V/V isopropanol/water and 40/60 V/V isopropanol/water) • Examine the effect of solvent mixture composition on the rate of hydrolysis of (CH3)3CCl Introduction With t-butyl chloride, (CH3)3CCl, being a tertiary halogenoalkane, it is predicted that (CH3)3CCl reacts with water in a nucleophilic substitution reaction (SN1 mechanism), where Step 1 is the rate-determining step. The reaction proceeds in a manner as shown
The purpose of this experiment was to learn about the electrophilic aromatic substitution reactions that take place on benzene, and how the presence of substituents in the ring affect the orientation of the incoming electrophile. Using acetanilide, as the starting material, glacial acetic acid, sulfuric acid, and nitric acid were mixed and stirred to produce p-nitroacetanilide. In a 125 mL Erlenmeyer flask, 3.305 g of acetanilide were allowed to mix with 5.0 mL of glacial acetic acid. This mixture was warmed in a hot plate with constantly stirring at a lukewarm temperature so as to avoid excess heating. If this happens, the mixture boils and it would be necessary to start the experiment all over again.
In this experiment, hydride reducing agents were used, since hydrides have spare electrons that they can donate to other compounds. Two popular hydride reducing agents, lithium aluminum hydride and sodium borohydride, were considered for this experiment. Since hydride reducing agents were used in this reaction, the reaction would have been extremely sensitive to proton sources, since
The purpose of this experiment was to learn about metal hydride reduction reactions. Therefore, the sodium borohydride reduction of the ketone, 9-fluorenone was performed to yield the secondary alcohol, 9-fluorenol. Reduction of an organic molecule usually corresponds to decreasing its oxygen content or increasing its hydrogen content. In order to achieve such a chemical change, sodium borohydride (NaBH4) is used as a reducing agent. There are other metal hydrides used in the reduction of carbonyl groups such as lithium aluminum hydride (LiAlH4).
Bromination is a type of electrophilic aromatic substitution reaction where one hydrogen atom of benzene or benzene derivative is replaced by bromine due to an electrophilic attack on the benzene ring. The purpose of this experiment is to undergo bromination reaction of acetanilide and aniline to form 4-bromoacetanilide and 2,4,6-tribromoaniline respectively. Since -NHCOCH3 of acetanilide and -NH2 of aniline are electron donating groups, they are ortho/para directors due to resonance stabilized structure. Even though the electron donating groups activate the benzene ring, their reactivities are different and result in the formation of different products during bromination.
Properties of Substances Express Lab 1)The purpose of this lab was to compare the physical properties of different types of solids and how the properties of solids are determined by their intermolecular forces and their intramolecular bonds. Then we were to classify each type of solid as either ionic, metallic, non-polar molecular, polar molecular, or network. Paraffin wax classified as a non-polar molecular, Silicon dioxide was classifies as a network, Sodium chloride was classified as ionic, Sucrose was classified as polar molecular and Tin was classified as metallic. (2)The intermolecular forces that are present in Paraffin wax are dispersion forces, because it is non-polar and carries a negative charge. Followed by Sucrose that has