Oxidizing capacity is less then ozone but much stronger than chlorine and chloramines. Chlorine dioxide sanitizes through oxidation. It is the main biocide that is an atomic free radical. It has 19 electrons and has an inclination for substances that takes an electron. On the other hand chlorine when reacts with any substance it adds chlorine molecule or substitutes chlorine atom from substance.
Other amide types include RC(O)NHR and RNH2. Amides are found in a wide variety of things, they are used in the production of drugs such as paracetamol and LSD, but are also found in DNA. Amides are similar to amines (RNH2) in that they are both derivatives of ammonia and are both bases, though amides are considerably weak when compared to amines (amines have a pKa of around 9.5, while amides have a pKa of around -0.5). Therefore amides do not have clearly noticeable acid-base properties in water. The lack of basicity within amide is due to the C=O, or carbonyl group, within the amide as it has electron withdrawing properties causing the lone pair of electrons within nitrogen to become delocalised.
This was proved by utilizing the IR spectrum to verify the C=O was not in the final product as it lacked the 1640 cm-1 peak. The melting point of 113-115 degrees C proved that the final product obtained was the E-Stilbene. The TLC plate proved that the E and the Z product was produced, show cased by the double intensity of the DCM spot to the final product’s spot, both which had an Rf of 0.92. The double intensity proved that both products were produced, but through heating and filtering, the Z-Stilbene was
The formula for sodium acetate is NaC2H3O2, it is quite soluble in water, soluble in ether and slightly soluble in ethyl alcohol. While the chemical compound melts at 622.8℉, it does not have a boiling point for it will decompose. A hydrate is a chemical compound that forms when one or more water molecules are added to the molecules of another substance. Since sodium acetate is a trihydrate (NaC2H3O2·3H2O), it has three molecules of water for every molecule of sodium acetate and because of this, anhydrous sodium acetate quickly transitions into a trihydrate. This is due to sodium acetate being quite hygroscopic, meaning it readily absorbs moisture from the air.
9. Theoretical yield = (150.22g/mol)(3.5 x 10^-3 mol of nucleophile) = 0.525 g Actual yield = 0.441 g, Percent Yield = (0.441g/0.525g) x 100% = 84% 10. Percent recovery from recrystallization = (0.172g/0.441g) x 100% = 38% 11. The data table provided below obtained melting point data for crude product, pure product, and mixture of the pure and 4-tert-butylbenzyl. 12.
Reacting specific alkyl and aryl halides with magnesium metal will result an in organomagneisum compound known as a Grignard reagent (RMgX) (Ketcha, 155). To properly create a Grignard reagent, a few rules must be follow. First, aliphatic Grignard reagents are prepared by alkyl iodides, bromides and chlorides (Ketcha, 155). Aryl and vinylic Grignard reagents are prepared normally with iodides and bromides (Ketcha, 155). Second, “anhydrous, inert and basic (polar aprotic) solvent such as diethyl ether or tetrahydrofuran (THF) is required to solvate the magnesium” (Ketcha, 155).
Ytterbium is a rare earth metal, one of the elements found in Row 6 of the periodic table. It has an atomic number of 70, an atomic mass of 173.04, and a chemical symbol of Yb. Ytterbium is a typical metal that is both ductile and malleable. It has a melting point of 1,515°F (824°C), a boiling point of 2,600°F (1,427°C), and a density of 7.01 grams per cubic centimeter. Ytterbium is a relatively reactive element that is usually stored in sealed containers to prevent its reacting with oxygen of the air.
Due to water’s polar structure, ions in some compounds attract and form bonds with water molecules, forming hydrates. A hydrate is a salt that has water molecules trapped within its crystals. Every hydrate has a certain number of water molecules weakly bonded to the salt as follows: salt • number of water molecules Anhydrous salts are salts that can form hydrates but which have had all the water driven off, usually by heat. By heating the Copper (II) sulphate hydrate until its color changes from blue to white, the compound can be decomposed into CuSO4, a white crystal, and H2O gas, represented as follows: CuSO4 • xH2O(s) ←⎯→ CuSO4(s) + xH2O(g) Because of the mass conservation law and the fixed proportion of water molecules, the mole of H2O can be calculated by calculating the mass difference of the substance before and after the reaction: Mole of H2O = (Mass of substance before the reaction) (Mass
Explain why ethanal gives a positive iodoform test. • Ethanal is the only aldehyde to give a the positive result because the reaction requires a methyl group connected to a carbon atom with a keto or an OH- substituent. 2- In semicarbazone formation only one of the two –NH2groups in semicarbazide undergoes nucleophilic addition to the carbonyl group. Explain the difference in the reactivity of these two –NH2 groups, using resonance structures. • Within the semicarbazone formation there are two –NH2 groups.