reaction of alkanes with bromine

Published by on November 13, 2020

In the case of the reaction with propene, 1,2-dibromopropane is formed. UV light is not required for this reaction. . 4:49 (Triple only) Understand how to write the structural and displayed formula of a polyester, showing the repeat unit, given the formulae of the monomers from which it is formed, including the reaction of ethanedioic acid and ethanediol: 4:50 (Triple only) know that some polyesters, known as biopolyesters, are biodegradable, (d) Energy resources and electricity generation, 4:28 describe how bromine water can be used to distinguish between an alkane and an alkene, 6.07 describe how to use two permanent magnets to produce a uniform magnetic field pattern, 4:17 describe how long-chain alkanes are converted to alkenes and shorter-chain alkanes by…, 2:37 describe the reactions of hydrochloric acid, sulfuric acid and nitric acid with metals,…, 3:02 describe simple calorimetry experiments for reactions such as combustion, displacement,…, 4:36 (Triple only) describe the reactions of aqueous solutions of carboxylic acids with…, d) Relative formula masses and molar volumes of gases, e) Chemical formulae and chemical equations, b) Group 1 elements: lithium, sodium and potassium, c) Group 7 elements: chlorine, bromine and iodine, d) The industrial manufacture of chemicals. Talk me through these mechanisms . 1:01 understand the three states of matter in terms of the arrangement, movement and energy of the particles, 1:02 understand the interconversions between the three states of matter in terms of: the names of the interconversions, how they are achieved and the changes in arrangement, movement and energy of the particles, 1:03 understand how the results of experiments involving the dilution of coloured solutions and diffusion of gases can be explained, 1:04 know what is meant by the terms: solvent, solute, solution, saturated solution, 1:05 (Triple only) know what is meant by the term solubility in the units g per 100g of solvent, 1:06 (Triple only) understand how to plot and interpret solubility curves, 1:07 (Triple only) practical: investigate the solubility of a solid in water at a specific temperature, 1:08 understand how to classify a substance as an element, a compound or a mixture, 1:09 understand that a pure substance has a fixed melting and boiling point, but that a mixture may melt or boil over a range of temperatures, 1:10 describe these experimental techniques for the separation of mixtures: simple distillation, fractional distillation, filtration, crystallisation, paper chromatography, 1:11 understand how a chromatogram provides information about the composition of a mixture, 1:12 understand how to use the calculation of Rf values to identify the components of a mixture, 1:13 practical: investigate paper chromatography using inks/food colourings, 1:14 know what is meant by the terms atom and molecule, 1:15 know the structure of an atom in terms of the positions, relative masses and relative charges of sub-atomic particles, 1:16 know what is meant by the terms atomic number, mass number, isotopes and relative atomic mass (Aᵣ), 1:17 be able to calculate the relative atomic mass of an element (Aᵣ) from isotopic abundances, 1:18 understand how elements are arranged in the Periodic Table: in order of atomic number, in groups and periods, 1:19 understand how to deduce the electronic configurations of the first 20 elements from their positions in the Periodic Table, 1:20 understand how to use electrical conductivity and the acid-base character of oxides to classify elements as metals or non-metals, 1:21 identify an element as a metal or a non-metal according to its position in the Periodic Table, 1:22 understand how the electronic configuration of a main group element is related to its position in the Periodic Table, 1:23 Understand why elements in the same group of the Periodic Table have similar chemical properties, 1:24 understand why the noble gases (Group 0) do not readily react, (e) Chemical formulae, equations and calculations, 1:25 write word equations and balanced chemical equations (including state symbols): for reactions studied in this specification and for unfamiliar reactions where suitable information is provided, 1:26 calculate relative formula masses (including relative molecular masses) (Mᵣ) from relative atomic masses (Aᵣ), 1:27 know that the mole (mol) is the unit for the amount of a substance, 1:28 understand how to carry out calculations involving amount of substance, relative atomic mass (Aᵣ) and relative formula mass (Mᵣ), 1:29 calculate reacting masses using experimental data and chemical equations, 1:31 understand how the formulae of simple compounds can be obtained experimentally, including metal oxides, water and salts containing water of crystallisation, 1:32 know what is meant by the terms empirical formula and molecular formula, 1:33 calculate empirical and molecular formulae from experimental data, 1:34 (Triple only) understand how to carry out calculations involving amount of substance, volume and concentration (in mol/dm³) of solution, 1:35 (Triple only) understand how to carry out calculations involving gas volumes and the molar volume of a gas (24dm³ and 24,000cm³ at room temperature and pressure (rtp)), 1:36 practical: know how to determine the formula of a metal oxide by combustion (e.g. copper(II) oxide), 1:37 understand how ions are formed by electron loss or gain, 1:38 know the charges of these ions: metals in Groups 1, 2 and 3, non-metals in Groups 5, 6 and 7, Ag⁺, Cu²⁺, Fe²⁺, Fe³⁺, Pb²⁺, Zn²⁺, hydrogen (H⁺), hydroxide (OH⁻), ammonium (NH₄⁺), carbonate (CO₃²⁻), nitrate (NO₃⁻), sulfate (SO₄²⁻), 1:39 write formulae for compounds formed between the ions listed in 1:38, 1:40 draw dot-and-cross diagrams to show the formation of ionic compounds by electron transfer, limited to combinations of elements from Groups 1, 2, 3 and 5, 6, 7 only outer electrons need be shown, 1:41 understand ionic bonding in terms of electrostatic attractions, 1:42 understand why compounds with giant ionic lattices have high melting and boiling points, 1:43 Know that ionic compounds do not conduct electricity when solid, but do conduct electricity when molten and in aqueous solution, 1:44 know that a covalent bond is formed between atoms by the sharing of a pair of electrons, 1:45 understand covalent bonds in terms of electrostatic attractions, 1:46 understand how to use dot-and-cross diagrams to represent covalent bonds in: diatomic molecules, including hydrogen, oxygen, nitrogen, halogens and hydrogen halides, inorganic molecules including water, ammonia and carbon dioxide, organic molecules containing up to two carbon atoms, including methane, ethane, ethene and those containing halogen atoms, 1:47 explain why substances with a simple molecular structures are gases or liquids, or solids with low melting and boiling points.

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