Melting point is the temperature at which the lattice is collapses and the solid is converted into liquid. The trend in structure is from the metallic oxides containing giant structures of ions on the left of the period via a giant covalent oxide in the middle to molecular oxides on the right. Sodium peroxide‚ magnesium oxide and aluminum oxide are metallic oxide which have high melting and boiling point compared to other period 3 oxide. This is due to their giant ionic structure and the strong ionic
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Experiment #9 – Identification of Aldehydes and Ketones Introduction Aldehydes and ketones share the carbonyl functional group which features carbon doubly bonded to oxygen. In the case of ketones there are two carbon atoms bonded to the carbonyl carbon and no hydrogens. In the case of aldehydes there is at least one hydrogen bonded to the carbonyl carbon; the other attachment may be to a carbon or a hydrogen. In all cases the carbon(s) that are attached to the carbonyl group may be aliphatic (not
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Semester 1 Revision The list below will assist you to check your understanding of the main concepts studied in Semester One. Work carefully through the list below and make sure that you can do what the statement says. This is not a course summary. It is a checklist for you to use to identify areas where you need extra work and a guide for your study. Macroscopic properties of matter I can | | | Classification
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and metallic bonds are formed by combinations of metals and nonmetals. * Metal + nonmetal = ionic bond * Nonmetal + nonmetal = covalent bond * Metal + metal = metallic bond When two elements engage in ionic bonding‚ one or more electrons are transferred from the metal to the nonmetal‚ forming ions (charged atoms). The metal‚ having lost one or more electrons‚ forms a cation‚ an ion with a positive charge; the nonmetal‚ having gained one or more electrons‚ becomes an anion‚ an ion with
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Solids • metals (good electrical/heat conductors) • semiconductors • insulators (poor electrical/heat conductors) Bonding in solids: Ionic solids Ionic solid crystals (e.g. NaCl) are held together by the Coulomb attractive interaction between ions with opposite sign (ionic bonding) e2 b U = −αk + m r r (α = 1.7476 for Na +Cl − ) (m ~ 10) k = 1 / 4πε 0 Madelung constant Ionic cohesive energy: 11 U0 = min U (r ) = −αk 1 − m r0 mb r0 = αk 1 m −1
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1.0 INTRODUCTION Flame photometry‚ also referred to as ’flame atomic emission spectrometry ’ is a quick‚ economical and simple way of detecting traces of metal ions‚ primarily Sodium‚ Potassium‚ Lithium‚ Calcium‚ and Barium‚ in a concentrated solution. The process is an extension of the principles used in a flame test‚ with the main differences having more precision in the results‚ and the use of more advanced technology. This report focuses on the theory‚ applications‚ limitations and analysis
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complications. The present article discusses various issues associated with biological corrosion of different kinds of implants used as cardio stents‚ orthopedic and dental implants. As the materials used for these implants are manifold starting from metallic materials such as stainless steel (SS)‚ cobalt chromium‚ titanium and its alloys‚ bioceramics‚ composites and polymers are in constant contact with the aggressive body fluid‚ they often fail and finally fracture due to corrosion. The corrosion
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it emits the absorbed energy in the form of light. A platinum or nichrome wire was dipped into aconcentrated HCL and was heated to clean it. The wire was dipped into different salt solutionsand heated in order to determine the metallic ion’s color and wavelength. Metal ions emitting aviolet-colored flame has the largest amount of energy while those that emit red-colored flamehave the least amount of energy. Introduction An atom is the smallest particle of an element‚ which can exist and still
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Chemical bond From Wikipedia‚ the free encyclopedia Jump to: navigation‚ search A chemical bond is an attraction between atoms that allows the formation of chemical substances that contain two or more atoms. The bond is caused by the electrostatic force of attraction between opposite charges‚ either between electrons and nuclei‚ or as the result of a dipole attraction. The strength of chemical bonds varies considerably; there are "strong bonds" such as covalent or ionic bonds and "weak bonds"
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Purpose: To determine the colors of the Atomic Emission Spectra of several metallic ions. Materials: Safety glasses 10 test tubes Test tube rack Paper Pencil 50 mL beaker Bunsen burner Nichrome wire Barium Nitrate Copper Nitrate Strontium Nitrate Lithium Nitrate Potassium Nitrate Sodium Chloride Calcium Nitrate Unknown solutions A‚B‚ & C Hydrochloric Acid Wash bottle (with distilled water) Procedure: 1. Label the test tubes with the names of the solutions and unknowns. 2. Place
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