purpose of this lab is to identify the different features that come about by using oxidation reduction and recording the observations‚ these tests will help determine the specific qualities each solution has. Hypothesis I theorize that nothing will happen with Magnesium because it is such a soft metal. Zinc should turn a greener color‚ because that’s what happens to a lot of statues and sculptures. I theorize that iron will tarnish badly because in air it can get tarnished so oxidation must do something
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Purpose: The purpose of this lab is to identify the different features that come about by using oxidation reduction and recording the observations‚ these tests will help determine the specific qualities each solution has. Materials: 1 Paper towels 1 Well-Plate 1 Tweezers‚ plastic Experiment Bag Oxidation-Reduction Activity Series 1 Copper (II) Sulfate‚ 1 M - 3 mL in Pipet 1 Iron (III) Chloride‚ 2 M - 3 mL in Pipet 1 Iron Metal‚ 2 pc in Bag 2"x 3" Magnesium Metal (ribbon) - 2 Small Pieces in Bag
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The purpose of this lab was to measure the reduction potentials of metals and to understand how a reduction-oxidation relationship works to produce spontaneity. Lastly‚ these results were used to determine the Faraday’s constant and Avogadro’s number by electrolysis‚ which is chemical decomposition produced by passing an electrical current through a solution with ions. The primary objective of part one of this experiment was to discover how the properties of an electrochemical cell works. An electrochemical
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took place by using the oxidation numbers in the equation. Variables: 1. I cleaned the reaction surface to limit contamination 2. I held the chemicals at approximately a 90 degree angle for consistency Introduction: Redox reactions occur when both oxidation and reduction take place. All atoms can be assigned an oxidation number‚ which is a positive or negative number that help in determining the reducing and/or oxidizing agents in an equation. An increase in the oxidation number of an atom from
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Oxidation Lab Part 1: Purpose: You are going to investigate the ease with which different metals undergo oxidation and reduction. Materials: | 4 samples of each of: lead‚ zinc‚ iron‚ copper | spot plates steel wool/sand paper | | | | Solutions of: | copper(II) sulfate Ferric nitrate Silver nitrate Lead (II) nitrate | | Procedure: 1. Obtain 4 samples of each metal and clean with steel wool or sand paper. Wash your hands after cleaning the metals so you are not exposed to lead
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STK 1084 Inorganic Chemistry I‚ LU 3 Oxidation – Reduction Reactions‚ Prepared By: Dr. Tay Meng Guan‚ Faculty of Resource Science and Technology‚ Universiti Malaysia Sarawak. LU 3 Oxidation and Reduction Reactions 3.1 Ideas of Oxidation and Reduction Oxidation of an atom can be occurred in the following conditions: 1. Losing an electron from the orbitals. e.g.: A A+ + e- 2. Adding an electronegative element (e.g.: F‚ Cl‚ Br‚ O) to a molecule. e.g.: A + F AF 3. Losing hydrogen
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Oxidation and Reduction Mnemonic: OILRIG Oxidation Is Loss‚ Reduction Is Gain Oxidation → the loss of electrons from an atom or an ion→ always happens at anode (positive electrode) → think anOde (O2 in the electrolysis of water xp) Redox reactions: Reactions involving the transfer of electrons e.g. burning‚ rusting‚ photosynthesis‚ respiration and the browning of apples. happens in three types of reactions: 1. addition of oxygen 2. removal of hydrogen 3. increase in valency (how easily an atom
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DEFINITIONS OF OXIDATION AND REDUCTION (REDOX) This page looks at the various definitions of oxidation and reduction (redox) in terms of the transfer of oxygen‚ hydrogen and electrons. It also explains the terms oxidising agent and reducing agent. Oxidation and reduction in terms of oxygen transfer Definitions • Oxidation is gain of oxygen. • Reduction is loss of oxygen. For example‚ in the extraction of iron from its ore: [pic] Because both reduction and oxidation are going on side-by-side
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moles/1000 mL = .0005 moles/10 mL = moles of hydroxylammonium chloride Ratio of Fe+2 to NH3OH+ = 2:1 2e- + 2Fe+3 --> 2Fe+2 so transfer of 2 electrons NH3OH+ --> something + 2e- Oxidation number of N in NH3OH+ is -1‚ therefore the oxidation number for N on the product side must be +1 because it gains 2 electrons. N2O has an oxidation number of +1 for N‚ so that would work. Data:Equation 1: NH3OH+ + 2Fe+3 --> something + 2Fe+2 Equation 2: 8H+ + 5Fe+2 + MnO4- --> 5Fe+3 + Mn+2 + 4H2O Equation 3: 6H+ +
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Making an Activity Series of Metals using different Solutions Purpose/ Hypothesis: The purpose of this lab was to clearly identify the reactivity of magnesium‚ zinc and copper. The metals reactivity will be exemplified as it will be tested with different solutions such as zinc sulfate (ZnSO4)‚ copper sulfate (CuSO4)‚ hydrochloric acid (HCL)‚ magnesium sulfate (Mg2SO4)‚ iron (II) sulfate (FeSO4) and tin (II) chloride (SnCl2). This will allow us in creating an activity series to visually see the reactivity
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