AP Chemistry II Review – Flashcards
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Hydrogen
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H |
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Lithium
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Li |
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Boron
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B |
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Copper
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Cu |
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Arsenic
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As |
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Bromine
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Br |
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Helium
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He |
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Beryllium
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Be |
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Carbon
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C |
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Zinc
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Zn |
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Selenium
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Se |
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Rubidium
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Rb |
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Strontium
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Sr |
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Neon
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Ne |
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Plutonium
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Pu |
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Oxygen
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O |
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Tin
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Sn |
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Sodium
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Na |
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Silver
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Ag |
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Cobalt
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Co |
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Antimony
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Sb |
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Fluorine
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F |
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Uranium
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U |
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Magnesium
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Mg |
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Cadmium
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Cd |
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Nickel
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Ni |
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Iodine
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I |
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Aluminum
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Al |
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Cesium
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Cs |
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Silicon
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Si |
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Gold
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Au |
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Francium
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Fr |
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Barium
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Ba |
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Calcium
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Ca |
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Iron
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Fe |
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Phosphorus
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P |
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Bismuth
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Bi |
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Radium
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Ra |
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Tungsten
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W |
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Chromium
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Cr |
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Argon
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Ar |
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Sulfur
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S |
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Astatine
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At |
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Mercury
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Hg |
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Platinum
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Pt |
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Nitrogen
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N |
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Chlorine
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Cl |
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Manganese
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Mn |
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Potassium
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K |
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Lead
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Pb |
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Lead |
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Pb |
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When the name of the anion ends in "-ide" the acid name begins with the prefix "_________" , and the stem of the anion has the suffix "________". |
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prefix: "hydro" suffix: "-ic" |
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When the anion name ends in "-ite", the acid name is the _____ of the anion with the suffix _____". |
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acid name is the stem suffix: "-ous" |
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When the anion name ends in "-ate", the acid name is the ______ of the anion with the suffix "____". |
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acid name is the stem suffix: "-ic" |
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Oxidation Number |
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A number assigned to an atom in a molecular compound or molecular ion that indicates the general distribution of electrons among the bonded atoms. |
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Strong Acids |
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100% ionized in aqueous solutions to form the hydronium ion, H3O+ (also written as H+(aq)) and the anion. |
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Strong Bases |
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100% ionized in aqueous solution to form the hydroxide ion, OH-, and the cation. |
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HCl |
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hydrochloric acid |
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HBr |
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hydrobromic acid |
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HI |
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hydroiodic acid |
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HNO3 |
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nitric acid |
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H2SO4 |
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sulfuric acid |
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HClO4 |
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perchloric acid |
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HClO3 |
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chloric acid |
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Alkali metal hydroxides and the more soluble alkaline earth hydroxides are... |
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NaOH(s) |
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sodium hydroxide |
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KOH(s) |
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potassium hydroxide |
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Ba(OH)2(s) |
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barium hyroxide |
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Alkali metal oxides and the more soluble alkaline earth oxides are.. |
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Na2O(s) |
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sodium oxide |
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K2O(s) |
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potassium oxide |
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BaO(s) |
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barium oxide |
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polyatomic ions |
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these are ions that include more than one element, but they remain together as a group and have one overall charge for the group of atoms involved. |
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C2H3O2- |
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acetate |
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CN- |
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cyanide |
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OH- |
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hydroxide |
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NO2- |
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nitrite |
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NO3- |
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nitrate |
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ClO- |
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hypochlorite |
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ClO2- |
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chlorite |
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ClO3- |
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chlorate |
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ClO4- |
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perchlorate |
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BrO3- |
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bromate |
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SCN- |
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thiocyanate |
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HSO4- |
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hydrogen sulfate |
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HCO3- |
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hydrogen carbonate |
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MnO4- |
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permanganate |
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IO3- |
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iodate |
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CO32- |
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carbonate |
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S2O32- |
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thiosulfate |
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C2O42- |
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oxalate |
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SO32- |
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sulfite |
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SO42- |
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sulfate |
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O22- |
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peroxide |
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O21- |
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superoxide |
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HPO42- |
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hydrogen phosphate |
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CrO42- |
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chromate |
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Cr2O72- |
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dichromate |
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PO43- |
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phosphate |
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NH41+ |
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ammonium |
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Hg22+ |
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Mercury(I) ion |
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Hg2+ |
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Mercury(II) ion |
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Metal + oxygen → ________ |
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metal oxide |
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nonmetal + oxygen → _____ |
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nonmetallic oxide |
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metal oxide + water →_____ |
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metallic hydroxide (base) |
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types of synthesis reactions |
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combustion reaction |
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when oxygen combines with another compound to form water and carbon dioxide |
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synthesis reaction |
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when two or more simple compounds combine to form a more complicated one |
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decomposition reaction |
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the opposite of a synthesis reaction - a complex molecule breaks down to make simpler ones |
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single displacement reaction |
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when one element trades places with another element in a compound |
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double displacement reaction |
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when the anions and cations of two different molecules switch places, forming two entirely different compounds |
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acid base reaction |
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a special kind of double displacement reaction that takes place when an acid and base react with each other. The H+ ion in the acid reacts with the OH- ion in the base, causing the formation of water. Generally, the product of this reaction is some ionic salt and water |