Abdul Gadoush Period 2 Chemistry Honors 1-16-14 Metal Gizmo 1. Purpose/Problem: The whole purpose to this experiment was to identify which metal of the following: Copper, Magnesium or zinc had the most occurring reactions in the constant chemicals that they were inserted in. The metal that had the least amount of reactions in each chemical would be the least reactant, and the metal that had the most occurring reactions in the chemical would be the most reactant. For this process to occur (make metal gizmos), Naugatuck Metal Works needs one highly reactive metal and another that isn't a reactive metal. - signs of chemical change = changes the shape and color, creates a gas, distributes heat, Etc.
The purpose of the lab was to determine which reactant was the limiting reactant, and to see how much of the other reactant was used. The true molarity of a compound can be defined as the amount of moles per liter of that substance. The equation of this single displacement chemical reaction done during this lab is 2Al(s) + 3CuCl(aq) → 3Cu (s) + 2AlCl2 (aq). In the reaction, the solid Aluminum replaces the Copper in Copper (II) Chloride to produce solid copper, and Aluminum Chloride. In order to find which reactant is the limiting reactant, an equation based on the molarity of the Copper (II) Chloride may be used, or the products of the reaction may be observed.
An aqueous solution of ammonium sulfate is allowed to react with an aqueous solution of lead(II) nitrate. Identify the solid in the balanced equation. A) (NH4 )2 SO4 B) Pb(NO3 )2 C) PbSO4 D) NH4 NO3 E) There is no solid formed when the two solutions are mixed. ____ 11. An aqueous solution of sodium carbonate is reacted with an aqueous solution of calcium chloride.
Kumari Biswas Chem 106 – 07 October 06, 2014 Menglu Shi Group member: Shemeika McLaren, Jose Suarez, Colleen Shum Lab 3: Redox Arena Redox Arena Lab Part I Observations and Data Observations of starting materials and standards Chemicals | Observations | The Four standards | Granular zinc | Silver-gray irregular solids | Iodine crystals | Purple-black spherical solids, strong smell | Zinc ion and iodine-iodide-triiodide ion in H2O | Red brown liquid | Zinc iodide | Gray white solid powder | Chemicals used for tests | 0.17 M acetic acid | Clear liquid | Mineral oil | Thick clear liquid | Silver nitrate (AgNO3) | Clear liquid | Magnesium turnings | Solid curled metals | 3 M HCl | Clear liquid | Other chemicals
| Centrifuge: used to isolate the solid from the solution | . Focus Questions: When acidified water is not used in the zinc and iodine synthesis, zinc hydroxide is formed. How can it be identified based on the amphoteric nature. When zinc and iodine react without the presence of acetic acid in the water, zinc hydroxide forms. This is evident because the substance tested positive for both the acid test and the base test for zinc hydroxide.
We resulted that lead, silver, and copper are the strongest oxidizing agents, and that magnesium and zinc are the weak oxidizing agents. The strong oxidizing agent oxidized the weak oxidizing agent and in turn the strong oxidizing agent got reduced while oxidizing the weak agent. When a reaction occurred, the solid metal reduced the ion, and in turn made it the more reactive metal. In part two we used a solvent extraction technique to derive an activity series for the halogens. With the use of this technique we placed chlorine, bromine, and iodine into solutions containing chloride, bromide, and iodide.
Although, Ionic bonding is when an atom gives away elections to another atom, which only happens in a metal and a nonmetal, and they have high melting points and are soluble. By investigating the unknown
In each part of the experiment, you will be observing a different property of electrolytes. Keep in mind that you will be encountering three types of compounds and aqueous solutions: Ionic Compounds These are usually strong electrolytes and can be expected to 100% dissociate in aqueous solution. Example: NaNO 3 (s) → Na+(aq) + NO 3 –(aq) Molecular Compounds These are usually non-electrolytes. They do not dissociate to form ions. Resulting solutions do not conduct electricity.
rtSeptember 17, 2012 NAME: Shelby Collins TITLE: What’s That Mineral OBJECTIVES: The objectives of the Mineral Identification lab is exactly what the title of the lab says, identifying minerals. In this lab, after making detailed observations of important minerals by using a tool kit, knowledge of classifying common rock forming minerals is to be gained. BACKGROUND: Before undertaking this lab, there are important concepts that must be understood that help with identifying and exploring important minerals. To identify a mineral, their physical properties must be examined. Such properties are luster, the way light is reflected off of a mineral and whither or not it is metallic or non-metallic, hardness, the resistance to scratching, gravity, the density of the mineral compared to water, fracture, irregular surface breakage and cleavage, breakage on flat planes.
(the 1st two), through the processes of weathering, metamorphism etc. (a) Essential minerals: These are the major constituents of the rock which help in the diagnosis of the rocks types. The disappearance of these minerals would cause the relegation of the rock to another type. (b) Accessory minerals: These are the minor constituents of a rock and their presence has no bearing on the nomenclature of the lock. The minerals commonly occurring in igneous rocks may be broadly classified into felsic and mafic varieties.