Question: What will happen to different halide salts found in the body if various compounds are added to the halide? How will the halides react? Introduction: For this lab we tested 6 halide salts found in the body‚ and their reactivity when a compound is added. We tested the halides NaF‚ NaCl‚ KBr‚ KI‚ and two unknown halides. To find the reaction of the halide‚ we are adding drops of Ca(NO3)2‚ AgNO3‚ AgNO3 + Na2S2O3‚ and NaOCI + Starch to the halides. Each halide will be separated from each other and
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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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SYNTHESIS OF AN ALKYL HALIDE S.M. BLANCAFLOR1 1INSTITUTE OF BIOLOGY‚ COLLEGE OF SCIENCE UNIVERSITY OF THE PHILIPPINES‚ DILIMAN‚ QUEZON CITY 1101‚ PHILIPPINES DATE SUBMITTED: 3 JANUARY 2012 DATE PERFORMED: 8 DECEMBER 2011 ------------------------------------------------- ABSTRACT Alkyl halides are molecules which have a carbon atom attached to a halogen atom (e.g.‚ chlorine‚ iodine‚ or bromine.) Alkyl halides are very important since they are used in many of the products used today
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3/22/2012 ARYL HALIDES 2. displacement reactions of diazonium salts ARYL HALIDES General formula: Ar–X where X = F‚ Cl‚ Br or I Examples Structure: C-X bonds are shorter and stronger Bond C-Cl C-Br Ar-X 1.69 A° 1.86 A° R-X 1.77 1.91 Dipole moments are unusually small. Bond C-Cl Preparation: 1. electrophilic aromatic substitution – useful only if one product is obtained C-Br Ar-X 1.7 D 1.7 D R-X 2.10 D 2.15 D Dipole moments may cancel out depending on the geometry of the
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I https://www.oppapers.com/join.php#submit . Experiments with Metals and Ions of Metals Introduction Metals are similar in their physical properties in general‚ but they are not identical. Most of the metals are solids; few of them are liquids‚ such as mercury and cesium. Density of metals is not similar also. For example‚ sodium has density of 0.97g/cm3 while lead has density of 11.4g/cm3. Melting point of sodium is 98.0oC while for lead it is 327.6oC. Metals have the capability
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Relative Reactivity of Anilines Abstract: Various Anilines were tested with Br2/HBr solution‚ the products were crystallized and melting points attained to verify relative reactivity. My assignment‚ 2‚4-Dibromoanisol‚ was prepared in a yield of 52% with a melting point of 55-58 C . Reaction: Mechanism: Procedure: Anisole (0.35mL‚ 0.0378mol) was obtained and placed in a pre-weighed 25 mL round bottom flask‚ along with 2.5 mL of glacial acetic acid and a magnetic stir bar. Then the
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Preparation and SN1 Reactivity of 2-Bromobutane Whitney Bellido Department of Chemistry‚ Illinois State University‚ Normal‚ IL 61790-4160 Submitted: April 4th‚ 2013 Introduction The overall goal of this experiment is to understand and be familiar of SN1 reactivity. We also learned how to prepare 2-Bromobutane by learning how to distill and extract this product from its organic layer. Finally‚ another goal was to specifically understand the relative reactivity of alkyl halides under SN1 conditions
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CLASSIFICATION TESTS FOR ORGANIC HALIDES James Anand L. Regala‚ Sabrina Nicolle G. Sarte‚ Ann Michelle Siao‚ Michael Sibulo‚ Victoria Tan Group 8 2C Pharmacy Organic Chemistry Laboratory ABSTRACT This experiment is done to classify organic halides. Most organic halides are synthetic and are not flammable. One way to classify organic halides is by classifying its -carbon atom as primary‚ secondary or tertiary. If the -carbon is attached to one R group‚ it is then primary. If the -carbon is
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Testing for Ions Analysis Chemical Changes of Test Solutions Test Solution Silver Nitrate Barium Chloride Potassium Thiocyanate Sodium Sulfate - Stayed white in color - Turned cloudy in color - Precipitation formed in solution - Stayed white in color Potassium Chloride - Turned cloudy in color - Precipitation formed in solution - Stayed white in color - Stayed white in color Iron (III) Nitrate - Stayed orange in color - Stayed orange in color - Changed color from orange
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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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