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) (sodium hydroxide)
  • KOH(s) (potassium hydroxide)
  • Ba(OH)2(s) (barium hydroxide)
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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) (sodium oxide)
  • K2O(s) (potassium oxide)
  • BaO(s) (barium oxide)
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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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  • metal + oxygen → metal oxide
  • nonmetal + oxygen → nonmetallic oxide
  • metal oxide + water → metallic hydroxide (base) 
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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
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