AP Chemistry Dr. Istone Lab 3: Gravimetric Analysis of a Metal Carbonate Lab Objective: In this lab we will determine the identity of a group 1 metal carbonate compound by gravimetric analysis. The unknown is weighed and dissolved in water and the precipitate is filtered‚ dried‚ and weighed. From the data the formula weight and identity of the unknown metal carbonate is determined. Lab Procedure: 1. Set up the Bunsen burner and ring clamp‚ light the burner and heat the crucible
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Metals Physical Properties of Metals versus Non-metals Properties | Electrical conductivity | Heat conductivity | Melting and Boiling points | Malleability & ductility | Lustre | Metals | Good | Good | High | High | Shiny | Non-metals | Poor | Poor | Low | Low (Brittle) | Dull | Chemical Properties of Metals versus Non-Metals Properties | Metals | Non- metals | Reaction with oxygen | Form basic or amphoteric oxides | Form acidic or neutral oxides | Ionisation | Lose electrons
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of reaction of Alkali metals and Alkaline Earth meatals are compared in this lab. The pH of each of the resulting metal solutions are tested and the products of the reaction between calcium and water is discovered. The tested elements are sodium‚ lithium‚ potassium and calcium and each of them were placed in a beaker filled with water. The resulting solutions pH levels were tested with litmus paper. There were more steps for caclium because it is the only Alkaline Earth metal. For calcium‚ the gas
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extract a metal Industrial mineral- either has some direct practical use‚ or take part in some industrial process Gems and precious stones are an exception to industrial metals as they do have a direct ‘practical’ application but are dealt with separately. Some common minerals include: * * Silica- (silicon dioxide) most common mineral on earth * Calcite- (calcium carbonate) main mineral in limestone and marble Ore: A naturally occurring solid material from which a metal or valuable
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exchange of positive and negative ions between reacting solutions of two ionic compounds. Thus‚ in this example the precipitate must be either silver chloride‚ AgCl or sodium nitrate‚ NaNO3. Sodium nitrate dissolves readily in water and is therefore soluble. Thus we can conclude that silver chloride is the insoluble precipitate. We can represent the formation of this precipitate by a net ionic equation: Ag+ +NO3 ̄ +Na++Cl ̄→AgCl+NO3 ̄+Na+ Net: Ag+ (aq)+Cl ̄ (aq)→AgCl(s) Ions present in the solution but
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Purpose: To observe the characteristic colors produced when certain metallic ions are vaporized. Metallic Ion Color in Flame Na+ Light Orange K+ Pink / Orange Li Red Ca2+ Dark Orange Sr2+ Red Cu2 Green Co+2 Salmon Pink Ammonium Dichlorate Orange Sparks K2CR2O7 Orange Fe+1 No Reaction NaCl Orange Strantium Chloride Scarlet Red Ni+2 Dark Orange Copper Sulfate (solid) Green Fe+2
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next to it put a small drop of water‚ and let sit for few minutes to dry. Once dry‚ the fats will leave a grease spot behind. This can best be seen when you hold the paper up to a light source. The last macromolecule we explore in this lab is protein. In this lab we will test for the presence of protein using the CuSO4 test. A positive
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Identification of Metallic Ions Peter Jeschofnig‚ Ph.D. Version 42-0160-00-01 Kellie Long Purpose: To observe the different flames of alkali and alkaline metals. Procedure: Place a little bit of each element into the well plate. Then you soak a tip of a cotton swab in each solution. Then you place the cotton swab over the Bunsen burner until the flame changes color. observations The color of the flame is expected to be as follows: Metallic ion Flame color
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LAB 3.Ø.Ø: do ions combine in definite ratios PURPOSE The purpose of this investigation is to determine whether ions combine in definite ratios or not. To observe‚ and create a table of the different ions. QUESTION If copper (II) sulfate when mixed with sodium carbonate at different quantities combine to form ions in definite ratios. HYPOTHESIS / PREDICTION I believe that the ions will combine in definite ratios due to the fact that the valance electrons will not be changing throughout any
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Chemistry F332 Notes Ions in solids and solutions: Structure of an ionic lattice (Sodium Chloride): * Consists of sodium ions (Na+) surrounded by six chloride ions (Cl-) * Chloride ions also surrounded by six sodium ions. * Held together by attraction of oppositely charged ions. * Giant ionic lattice. * Electrostatic bonds hold lattices together. * Structure is simple cubic. * Some ionic crystals contain water. * Known as water of crystallisation. * These crystals
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