INVESTIGATION investigating the properties of Period 3 oxides Aim The purpose of this experiment is to examine the oxides of Period 3 elements and describe their bonding and structure. Introduction You carry out an investigation along similar lines to the work you did on the chlorides of the elements in Period 3 (Experiment 4.12). However‚ you will not be asked to test the oxides with cyclohexane because unlike the covalent chlorides‚ most of the oxides are not composed of discrete molecules. Therefore
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Aim: to perform a firsthand investigation to compare the physical and chemical properties of magnesium and oxygen when they are experimented to form magnesium oxide Theory: The empirical formula of a compound is the formula that tells us the ratio in which the atoms are present in the compound. To calculate an empirical formula: - Write down the masses of all of the elements present - Convert masses to moles (by dividing by atomic weights in grams) - Divide through by the smallest number of
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Oxides Research 1. Assess evidence‚ which indicates increases in atmospheric concentration of oxides of sulfur and nitrogen. Thorough collection of data‚ surveys‚ and tests from the 1950’s indicate a rising trend in atmospheric concentrations of oxides of sulfur and nitrogen. An enhancement in funding‚ technological and information resources‚ has led to wider and more detailed analyses of oxides of sulfur and nitrogen concentrations‚ and as the diagrams indicate (see diagrams) there is a clear
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metal found represent by the atomic number of 12. This experiment involves combining Magnesium with Oxygen which is a gas represented by the chemical element 8. The word equation for the result of this experiment is Magnesium + Oxygen= Magnesium Oxide. The equation is Mg + O =MgO Definitions Word Definitions Mass Number The Mass number is the amount of Protons and Neutrons in the Nucleus. Atomic Number The amount of protons found in the nucleus. Element A pure substance made up of 1 type
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number of atoms of oxygen in the formula Al(ClO3)3.6H2O? - 15 22. Write the correct formulas for the following binary ionic compounds. Compounds | Formulas | Lithium fluoride | LiF | Calcium oxide | CaO | Aluminum nitride | AlN | Beryllium Chloride | BeCl2 | Potassium iodide | KI | Aluminum oxide | Al2O3 | 23. Write the correct formulas for the following binary molecular compounds. Compounds | Formulas | Carbon monoxide | CO | Boron tribromide | BBr3 | Sulfur hexafluoride | SFl3
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The Law of Definite Proportions states that a chemical compound contains the same element in exactly the same proportions by mass regardless of the size of the sample or source of the compound. This relates to the magnesium oxide lab because we tested out this theory to see if it is true that the law of definite proportions says that a chemical compound contains the same element in exactly the same proportions by mass regardless of the size of the sample or source of the compound. In this experiment
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Nitric Oxide Filiberto Moncada Nitric Oxide Herbs That Increase Nitric Oxide Jul 4‚ 2011 | By Janet Contursi [pic] Janet Contursi has a Ph.D. in anthropology from the University of Minnesota and has been a freelance writer for over 23 years. Her articles have appeared in professional journals‚ magazines‚ newspapers and on the web. Contursi has a Master Herbalist diploma from the American College of Healthcare and Sciences. Her interests are the environment‚ herbal medicine and
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Zinc oxide in a mixture with a about 0.5% iron(III) oxide (Fe2O3) is called calamine and is used in calamine lotion. There are also two minerals‚ smithsonite and hemimorphite‚ which have been called calamine historically (see: calamine (mineral). Zinc peroxide‚ ZnO2 .½ H2O‚ is a white to yellow powder that is used in antiseptic ointments. Zinc white is used as a pigment in paints and is more opaque than lithopone‚ but less opaque than titanium dioxide. It is also used in coatings for paper
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Working out the Formula of Magnesium oxide Aims When magnesium is heated in air‚ it reacts with oxygen. During this oxidation reaction‚ magnesium oxide is produced. This increases the mass. If we know the mass of magnesium at the start‚ and the mass of magnesium oxide produced at the end‚ we can work out the mass of oxygen which has been combined with the magnesium. We can use these masses to work out the formula of magnesium oxide. Apparatus Googles
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COMBUSTION OF MAGNESIUM OXIDE DESIGN Aim/Purpose: To calculate the number of moles and the empirical formula of magnesium oxide. Safety precautions: 1) Wear lab coat 2) Wear gogles. 3)Make sure the bunsen burner is working properly and their is no leakage. 4) Wear gloves. Hypothesis: The weight of the magnesium ribbon increases after burning‚ so this indicated that their was a change in mass. This change happened because of the magnesium ribbon inside the crucible which reacted with Oxygen
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