Mike Taylor Chemistry for CAPE by Susan Maraj and Arnold Samai Periodic Trends in Group II Elements in Group II The elements in Group II are called alkaline earth metals. Be‚ Mg‚ Ca‚ Sr‚ Ba‚ Ra Beryllium‚ Magnesium‚ Calcium‚ Strontium‚ Barium‚ Radium These elements bond by metallic bonds (intramolecular forces) to form giant metallic structures. The size of the atoms increases down the group Physical properties of Group II metals Ionization The
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01/27/2013 Abstract: What can be found from this experiment is as follows‚ Introduction/Background: This lab was about determining water hardness. Water hardness is the amount of metal ions in the water. The most common found ion in the water is calcium ions and typically with a charge of +2. Water hardness plays a big significance in our daily life because to many metal ions in our drinking water can have adverse effects on our body. You can measure the water hardness by EDTA titrations. EDTA
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an insufficient adenosine production as a result of decreased mitochondrial phosphorylation. A result of a decrease in adenosine triphosphate (ATP) is anaerobic metabolism‚ which contributes to a change in the intracellular ion balance of sodium‚ calcium‚ and potassium ions (McCance & Huether‚ 2013). Hypoxia Induced Sodium and Potassium Shifts
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four carboxylic acid groups has an electron pair to donate to a metal ion center‚ making EDTA a hexadentate (“six-toothed”) ligand which forms an octahedral complex. Fig. 2. Ethylenediaminetetraacetic acid (EDTA). Fig. 3. EDTA4– chelating a calcium ion. REV 2012-02-13 COMPLEXOMETRIC DETERMINATION OF WATER HARDNESS PAGE 1 OF 4 CHM152LL LAB MANUAL COMPLEXOMETRIC DETERMINATION OF WATER HARDNESS
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yield of product‚ increasing the limiting reactant‚ possibly‚ is the most effective. In this experiment we were able to calculate limiting reactants from the reaction of CaCl2. 2H2O + K2C2O4.H2O(aq). As a group‚ we obtained our salt mixture of calcium chloride and potassium oxalate‚ and weighed the mixture. We were able to make an aqueous solution from the mixture and distilled water. We boiled and filtered off the solution‚ leaving the precipitate. Once the precipitate was dried overnight‚ it was
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the mucus. This movement of water is a result of chloride and sodium transport across the membrane. This method‚ along with other mechanisms is what ensures fluidity of the mucus‚ resulting
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‘Kinetics’ is the study of chemical reactions. The speed of a reaction can vary depending on many variables such as the nature of the reactants‚ particle size‚ concentration and temperature. For a chemical reaction to occur‚ there must be a collision between reactants. The reaction rate is slower when the reactants are large and complex molecules because it takes longer for the molecules to combine together creating a chemical reaction. More than 2000 years ago‚ Democritus‚ who was a philosopher
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detection of anions in a given solution. Method: CO3 Solution Iodine Solution 6M Nitric Acid SO4 Solution Sulphric Acid(H2SO4) Chloride Solution 6M Asetic Acid(CH3COOH) Barrium Chloride(BaCl2) 6M HCl(Hydrochloric acid) Silver Nitrate(AgNO3) 1M Potassium Nitrate(KNO2) Calcium Chloride (CaCl2) Barrium Hydroxide Ammonium Hydroxide (NH3OH) Methylene Chloride Test Tube/Test Tube Holder Eye Dropper Eye Dropper Beaker Pipette Pipette Bulb Litmus Paper Hot Plate Observations/Calculations:
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Paragraph 1 The polymorphs involved are the halides in tetragonal rutile (TiO2) structure and the halides in so-called calcium chloride structure. As the name implies‚ the unit cell of halides in tetragonal rutile structure is tetragonal‚ with the lattice parameters a=b≠c and α=β=γ=90o. It belongs to the space group P42/mnm. On the other hand‚ the unit cell of halides in calcium chloride structure is orthorhombic‚ i.e. a≠b≠c and α=β=γ=90o. The space group of this CaCl2 structured polymorph is Pnnm.
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NSS Chemistry Part 3 Metals HKCEE Past Paper Questions – Structural Questions 1. HKCEE 1995 Q1 Rubidium (Rb) and potassium belong to the same group in the Periodic Table. The relative atomic mass of rubidium is larger then that of potassium. (a) Explain whether rubidium is more reactive than potassium. (b) Write a chemical equation for the reaction between rubidium and water. (State symbols should be given.) (c) Suggest how rubidium can be stored safely in the laboratory.
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