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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 - PowerPoint PPT Presentation
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Chemistry
Chapter 10Notes #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
Carbon Dioxide, Carbon tetrachloride, diphosphorus pentoxide
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
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
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
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
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
Reactions Breaking bonds require energy Forming bonds releases energy 2 terms for describing the overall energy
transfer in a chemical reaction Exothermic Endothermic Reactions
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
Chemical ReactionsExothermic Endothermic
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
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….
Chemical Reactions Reactants -> Products Word Equation
Isooctane + oxygen -> carbon dioxide + water
Skeleton Equation C8H18 + O2 -> CO2 + H2O
Chemical Equation 2C8H18 + 25O2 -> 16CO2 + 18H2O
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