Sodium Borohydride Reduction: Diphenylmethanol from Benzophenone

Halogenation is when one or more hydrogens in a compound are replaced with a halogen, for example fluorine, chlorine, bromine or iodine. In a halogenation of the alkane, the

with oxygen. The catalyst is the yeast and it helps remove the oxygen from the hydrogen

The overall goal in this lab was to oxidize borneol, a secondary alcohol, into camphor, which is a ketone. For the purposes of oxidation chromic acid was utilized, which was prepared by adding a 1:1 ratio of chromium trioxide to dilute sulfuric acid.

The Purpose of this experiment is for the students to learn how to use sodium borohydride to reduce benzil to its secondary alcohol product via reduction reaction. This two-step reaction reduces aldehydes by hydrides to primary alcohols, and ketones to secondary alcohols. In order for the reaction to occur and to better control the stereochemistry and yield of the product, the metal hydride nucleophile of the reducing agents such as LiH, LiAlH4, or NaBH4 must be carefully chosen. Being that LiAlH4 and NaBH4 will not react with isolated carbon-carbon double bonds nor the double bonds from aromatic rings; the chosen compound can be reduce selectively when the nucleophile only react with

This type of reaction is an oxidation-reduction (or redox) reaction. This reaction is also [anabolic/catabolic] and [endergonic/exergonic].

A chemical reaction involving the transfer of electrons rather than molecules is classified as a Redox reaction. A reaction involving the loss of electrons is called Oxidation, and a reaction involving the gain of electrons is called Reduction. Oxidation and Reduction always occur together, as one reactant loses electrons, and the other gains them. This exchange often effects the physical states of molecules, as their solubility is changed with their charge.

In this experiment, benzopinacol was to be synthesized through photochemical reaction and its acid-catalyzed rearrangement product benzopinacolone.

82. Oxidation occurs when there is a removal of electrons and/or hydrogen atoms from a

In radical halogenations lab 1-chlorobutane and 5% sodium hypochlorite solution was mixed in a vial and put through tests to give a product that can then be analyzed using gas chromatography. This experiment was performed to show how a radical hydrogenation reaction works with alkanes. Four isomers were attained and then relative reactivity rate was calculated. 1,1-dichlorobutane had 2.5% per Hydrogen; 1,2-dichlorobutane had 10%; 1,3-dichlorobutane had 23%; and 1,4-dichlorobutane had 9.34% per Hydrogen.

2. What are catalysts? What is a type of catalyst and why is it needed?

Through an oxidation-reduction reaction sequence, Borneol is converted to isoborneol. First, borneol is oxidized through a reaction with sodium hypochlorite at 400C to form camphor. When the camphor is then reduced by sodium borohydride, isoborneol is formed. The percent yeild of isoborneol collected was 56.4%, and the melting point range was found to be between 174.2-179.90C. Through analysis of the product through 1H NMR spectroscopy the percent purity is found to be 77.2% pure isoborneol.

Experiments 2-1 and 2-2 study the production of hydrogen gas by different chemical reactions. By using a hydrogen gas collection apparatus and the principles of chemistry, we were able to evaluate the data and reach our goal. Experiment 2-1 uses zinc, magnesium and aluminum and how much hydrogen gas they produce to predict the volume of hydrogen gas produced for different masses of each metal. In this experiment we see that each metal has an increasing amount of hydrogen gas as mass goes up, however each metal had different amount of hydrogen gas for the same mass. Zinc produced the least amount of hydrogen gas, then increasing with magnesium, and aluminum produced the highest amount. The

The brewer jar has a high-vacuum pump that evacuates oxygen that gets replaced with a 95% mixture of nitrogen and 5% carbon dioxide. There are platinum catalysts in the jar lid that binds residual oxygen with hydrogen which forms water. The second is the GasPak system. The disposable hydrogen and carbon dioxide envelope generator. The system requires it to be in room temperature catalyst that doesn't need electrical activation to be used. Hydrogen reacts with oxygen to help yield water. The last technique is the chromium sulfuric acid method. Hydrogen is generated in a desiccator jar that reacts with 15% of sulfuric acid with chromium powder. Hydrogen evolves and gets forced out of the desiccator jar and gets replaced with hydrogen.

A fuel cell is, in principle, a very simple electrochemical device. The chemical reaction that powers hydrogen fuel cells is the same as that which occurs when hydrogen burns. The chemical equation for this reaction is: 2H2 + O2 ( 2H2O + energy. "Normally hydrogen burns, reacting with oxygen from the air, producing water, heat and light. ... In the fuel cell the chemical reaction is exactly the same, but instead of producing light and heat energy, electrical energy is produced."2 All fuel cells consist of an electrolyte (a substance that allows only the passage of ions) sandwiched between two electrodes. When a fuel containing hydrogen is passed over the negative electrode, otherwise known as an anode, it is ionized. Ionization of the fuel, often accomplished with the assistance of a catalyst, removes electrons from the hydrogen creating positively charged hydrogen ions and negatively charged free electrons. Since only the ions can pass through the electrolyte situated between the electrodes, the electrons must find another route to the positive electrode or cathode, where they will be reunited with the hydrogen ions and combined with oxygen atoms to form water. The electrons passing around the electrolyte constitute an electric current, and thus can be used to provide power during their journey from anode to cathode.3

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