brass and bronze‚ are very important Has various oxidation states: 0 in elemental copper‚ +1‚ and +2 which is observable in corroded brass/bronze Oxidation states n n n Oxidation state is an indicator of the degree of oxidation of an atom The formal oxidation state is the theoretical charge the atom would have of all bonds were 100% ionic Oxidation is loss of electrons‚ reduction is gain of electrons (OIL RIG) Oxidation States of Copper n n n n n 0
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that all three alcohols should have a different level of reactivity. The hydrogen atom on the hydroxyl functional group can be easily substituted because of its enhanced acidity. This is the basis of a halogenation reaction‚ and controlled oxidation reaction‚ which will be observed through this investigation. Purpose: To observe and compare the reactivity of the isomers of butanol as examples of 1°‚ 2° ‚ and 3° alcohols. Hypothesis: The reactivity of primary alcohol will be lower than
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subsequent oxidation in solution to adipic acid using an excess of strong nitric acid. This report deals with KA oil/cyclohexanol production by various routes‚ followed by the common step of nitric acid oxidation. KA oil production from cyclohexane by the cobalt catalyst and boric acid air oxidation routes is reviewed. Production of KA oil from phenol is also covered‚ as is the Asahi process for cyclohexanol production from benzene via cyclohexene. Appropriately adjusted nitric acid oxidation is appended
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Module 7 Exam Review ANSWER KEY 1. Define acid. (7.01) An acid is a substance that produces hydrogen ions‚ H+ or hydrodium ionsH3O+ in solution. 2. Compare the three theories of acids. (7.01) An Arrhenius acid is a substance the increases the concentration of hydrogen ion‚ H+ or hydronium ions H3O+when dissolved in water. You must have water. A BrØnsted-Lowry acid is any substance that donates a hydrogen ion‚ H+ to another substance. A Lewis acid is any substance that accepts a lone pair
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electrode and electrolyte and a salt bridge. In a galvanic cell one metal can undergo reduction and the other oxidation. A typical galvanic cell is based on the spontaneous redox reaction: Net Ionic Equation Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s) Half Equations Zn(s) → Zn2+(aq) + 2e– Cu2+(aq) + 2e– → Cu(s) The anode will undergo reduction (Zinc) and the cathode will undergo oxidation (Copper) The two half cells must be physically separated so that the solutions do not mix together. A salt
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eukaryotic organelles (mitochondria‚ chloroplasts) CELLULAR RESPIRATION GLUCOSE 1 2 GLYCOLYSIS 1 PYRUVATE OXIDATION2 KREBS CYCLE 3 2 ELECTRON TRANSPORT 4 CHAIN 2 NET ATP PRODUCED = 36 Nelson‚ 2003 Redox Reactions • Reduction-oxidation reactions – Transfer electrons from donor to acceptor atoms • Donor is oxidized as it releases electrons • Acceptor is reduced as it accepts electrons Cellular Respiration Series of chemical reactions and electron exchanges that convert
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electrolysis‚ or if a voltage is created by a chemical reaction as in a battery‚ it is an electrochemical reaction. In contrast‚ chemical reactions where electrons are transferred between molecules are called oxidation/reduction (redox) reactions. In general‚ electrochemistry deals with situations where oxidation and reduction reactions are separated in space or time‚ connected by an external electric circuit to understand each process. |Contents
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Usually the more expensive the essential oil‚ the less of it you will need to use. There are also many different families of aromatherapy smells. Citrus‚ Floral‚ Veracious‚ Camphor‚ Spicy‚ Resin‚ Woody‚ and Earthy are the majority of the aromatherapy smells. There are approximately 400 plants that can actually produce essential oils and we only use about 300 of them. Essential oils also contain many therapeutic properties. Therapeutic
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! ! To review oxidation-reduction reactions and their stoichiometry. To learn the concept and technique of redox titration. To determine the percent (m/v) of an active ingredient‚ sodium hypochlorite (NaOCl)‚ in a commercial bleaching agent. B. Theoretical Background Whereas acid-base reactions involve the transfer of a proton‚ oxidation-reduction or redox reactions involve the transfer of electrons from one substance to another‚ resulting in changes in oxidation numbers of two or more
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Writing Half Reaction and Net Ionic Equation Going back to our first concept or topic‚ we’ve learn how to identify the Oxidizing and Reducing agent and the Oxidation as well as the Reduction. In this part of the Redox reaction or in this step‚ it is very important that you already know the Oxidizing and Reducing agent for us to find the half reaction. In this step or part‚ we will also learn how to balance using the addition of electrons in both sides if necessary. After this step we can now write
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