protons and neutrons. Aproton is the nucleus of the simplest atom - hydrogen. A proton and a neutron formeddeuterium‚ which then formed helium. (77%hydrogen‚ 23% helium) 7.Describe what must have happened after the Big Bang. The expanding universe was foggy and opaque‚ containing energy in the form of radiation.300 000 years after the big bang‚ the universe dropped to 3000°C. This allowed the electronsto be captured by hydrogen and helium nuclei to form new atoms and elements‚ and the fogstarted
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An example would be the reaction between silicon and hydrogen‚ where each silicon has an electron octet and each hydrogen has an electron duet. With that ratio being four hydrogen atoms bonding to each silicon atom‚ the empirical formula can be computed to be SiH4. In this experiment‚ I will write chemical equations using Lewis symbols and Lewis structures to represent
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things. * Proteins‚ DNA‚ carbohydrates‚ and other molecules that distinguish living matter from inorganic material are all composed of carbon atoms bonded to each other and to atoms of other elements. * These other elements commonly include hydrogen (H)‚ oxygen (O)‚ nitrogen (N)‚ sulfur (S)‚ and phosphorus (P). (CHONPS) Concept 4.1 Organic chemistry is the study of carbon compounds * The study of carbon compounds‚ organic chemistry‚ deals with any compound with carbon (organic compounds)
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Yet‚ this behavior does not correspond to Kekule’s structural formula‚ which says that three conjugated double bound should exist. Another critic brought to this formula is that she predicts the existence of for isomers than in reality. If two hydrogen atoms in the benzene’s molecule are substituted with two bromine atoms‚ then‚ according tot Kekule’s rule‚ there should be two isomers containing two bromine atoms connected to two nearby carbon atoms (positions 1‚2 and 1‚6) at one
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Experimenting with a Candle Justin Nguyen Mrs. Howley 11/16/11 Mod F Purpose: the purpose is to learn how the process of a candle burning. The goals of this experiment are to practice in the art of observation‚ the art of questioning‚ and the development of a better understanding of this process. Hypothesis: through this experiment‚ we will learn how candle is working. Materials: * Candle * Note card * Matches or butane lighter * Aluminum foil * 1L beaker * Balance
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Structure and bonding Ionic bonds are chemical bonds formed through an electrostatic attraction between two oppositely charged ions. Ionic bonds are formed between an metal and a non-metal. The metal loses an electron or electrons form its highest energy level becoming a positively charged Ion and the non-metal gains an electron or electrons in its highest energy level‚ becoming a negatively charged Ion. Covalent bonds are strong bonds between two non-metal atoms. A covalent bond forms when two
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Student Number Mark / 39 Chemistry Preliminary Course Final Examination • 2006 General Instructions • • • • • • • Reading time – 5 minutes Working time – 45 minutes Write using black or blue pen Draw diagrams using pencil Board-approved calculators may be used A Data Sheet and a Periodic Table are provided Write your Student Number at the top of this page Total Marks – 39 Part A – 10 marks • Attempt Questions 1 – 10 • Allow about 10 minutes for this part Part B – 29 marks • Attempt
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Copper sulphate experiment Introduction There are a number of different methods of making salts‚ such as the reaction of a metal with an acid. Copper metal‚ however‚ does not react with sulphuric acid and so another method must be used. In this experiment a basic copper compound (copper(II) oxide) will be reacted with sulphuric acid giving copper(II) sulphate as one of the products. Method 1. Wear goggles and keep your face away from the beaker during the reaction 2. Place 20 cmm3 sulphuric
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formed products based on a BALANCED chemical equation. Mass Molar Mass Mole Coeff Bal Eqn Mole Molar Mass Mass Example 2 • The Haber Process involves reacting gaseous nitrogen and gaseous hydrogen to form ammonia. Determine the mass in grams of hydrogen gas required to form 1.00 x 103 g ammonia. Your Turn 2 • If you react 52.9 g of potassium chlorate (KClO3) with excess phosphorus‚ what mass of tetraphosphorus decoxide (P4O10) would be produced. KClO3 (s) +
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test tube rack and add about 5mL of HCl. Carefully drop a piece of zinc metal and observe briefly. Quickly cover the test tube with a cork and after a minute‚ insert a lighted match on the mouth of the test tube. A “Pop” indicates the presence of hydrogen. Pour 5mL of CuSO4 in a clean test tube and add a piece of zinc metal. Let it stand in the rack for five minutes. Pour 5mL of CuSO4 in another test tube. Using a pipette‚ transfer the solution of the first test tube into another clean one. Observe
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