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Chemistry

Chemistry. Chapter 10 Notes #1. Covalent Compounds -Review. Common Diatomic molecules Hydrogen (gas), Oxygen, Nitrogen, Fluorine, Chlorine, Bromine, Iodine Acids – Binary and Oxy Hydrochloric, Hydrosulfuric, Sulfuric, Sulfurous, Chlorous Regular Compounds

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Chemistry

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  1. Chemistry Chapter 10 Notes #1

  2. Covalent Compounds -Review • Common Diatomic molecules • Hydrogen (gas), Oxygen, Nitrogen, Fluorine, Chlorine, Bromine, Iodine • Acids – Binary and Oxy • Hydrochloric, Hydrosulfuric, Sulfuric, Sulfurous, Chlorous • Regular Compounds • Carbon Dioxide, Carbon tetrachloride, diphosphorus pentoxide

  3. Covalent Compounds • Nonmetal + nonmetal • Use prefixes to tell how many of each (find it on the pink sheet) • 2nd element, change the ending to –ide • Example Fluorine becomes Fluoride • Example: CO2 - Carbon Dioxide • Example: N2O4 – dinitrogen tetraoxide

  4. Ionic Compounds - Review • Cation + Anion (positive + negative) • Charges matter!!!!!! • Roman numerals tell charge for transitions • Polyatomics don’t end in –ide (mostly) • Need your cheat sheet • Examples • Tin (IV) oxide, lead (II) sulfite, strontium carbonate, aluminum oxide, magnesium chloride, calcium oxide, potassium iodide, potassium iodate

  5. Ionic Compounds • Metal + nonmetal • Find charge on periodic table for elements, on pink sheet for polyatomics • Ions come together to balance charge • NO charges (superscripts) in the formulas, just subscripts • EX: Mg2+ and Cl- = MgCl2 • Name: Name the metal, change the nonmetal ending to –ide • EX: MgCl2 = Magnesium Chloride

  6. Chemical Reactions- Review • Change in the composition and properties of a substance, or substances, as the result of a chemical reaction. • Ex. Souring of Milk • Ex. Rusting of iron • Ex. Change in color • Burning./Combustion • Chemical reactions change substances

  7. Chemical Reactions- Review • Signs of Chemical Change • Combustion (Flame, Smoke, Ash) • New substance formed • Color change • Precipitate (solid formed when mixing 2 liquids) • Bubbling/fizzing (Production of a gas) • Change in Temp (warmer or cooler) • Disappearance of a metal • Formation of liquid droplets • Odor

  8. Reactions • Breaking bonds require energy • Forming bonds releases energy • 2 terms for describing the overall energy transfer in a chemical reaction • Exothermic • Endothermic Reactions

  9. Chemical Reactions • Exothermic Reactions • Chemical reactions that overall release energy • They use energy to break bonds, but more energy is released in the formation of the products than was used to break the bonds • Endothermic Reactions • Chemical reactions that overall use energy • They use more energy to break bonds than is released in the formation of the products

  10. Chemical ReactionsExothermic Endothermic

  11. Chemical Reactions • Original bonds are broken • Atoms rearrange • New bonds form • Reactants: starting substances that will undergo a chemical change • Product: substance that is the result of a chemical change/reaction

  12. Chemical Reactions • Energy is conserved in chemical reactions • Law of conservation of energy • Chemical energy – energy stored in the bonds of the compounds • Total energy on the reactant side of an equation equals the total energy on the product side • This includes the energy given off….

  13. Chemical Reactions • Reactants -> Products • Word Equation • Isooctane + oxygen -> carbon dioxide + water • Skeleton Equation • C8H18 + O2 -> CO2 + H2O • Chemical Equation • 2C8H18 + 25O2 -> 16CO2 + 18H2O

  14. Chemical Reactions • In a balanced chemical equation energy and mass is conserved • You can only change coefficients • NO CHANGING SUBCRIPTS! • Changing the subscripts changes the chemicals, therefore it changes the entire reaction • Changing coefficients is just changing the amounts of chemicals necessary to carry out the reaction

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