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Reaction Types: Writing (balanced) Equations and Predicting Products

Reaction Types: Writing (balanced) Equations and Predicting Products. Simple reaction frequently follow one of these five basic patterns : Synthesis (Direct Combination): Two elements or compounds become one product Example: 2 NO + O 2  NO 2

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Reaction Types: Writing (balanced) Equations and Predicting Products

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  1. Reaction Types: Writing (balanced) Equations and Predicting Products

  2. Simple reaction frequently follow one of these five basic patterns: Synthesis (Direct Combination): Two elements or compounds become one product Example: 2 NO + O2 NO2 Decomposition: One compound decomposes to simpler compounds or elements. Carbonates decompose to oxides and CO2 CaCO3CaO + CO2 Hydroxides decompose to oxides and H2O Ca(OH)2CaO + H2O Chlorates* decompose to chlorides and oxygen gas 2 KClO3 2 KCl + 3 O2 *other halogen-oxides also decompose to their halides and oxygen gas Single Replacement (displacement): One element takes the place of another. Example: Zn + 2 HCl  ZnCl2 + H2 Can use the Activity Series to determine if a single replacement will occur. Double Replacement (displacement): Two atoms trade places (but always metal for metal, non-metal for non-metal). Example: 3 CaCl2 + 2 Na3PO4 Ca3(PO4)2 + 6 NaCl Combustion:A fuel and Oxygen gas (along with an ignition source) produce CO2, H2O and heat. Example: C3H8 + 5 O2 3 CO2 + 4 H2O + heat

  3. ***REMEMBER: All compounds must be “balanced” (their ions and charges must match). The diatomics (the 7 at 7: Hydrogen, Nitrogen, Oxygen, Fluorine, Chlorine, Bromine, and Iodine) Write the formulas of the products first. Then balance the equation (what goes in, must come out). Formulas in equations must be consistent with those predicted from the charges of common ions. The net charge (overall charge) in an ionic formula must add up to zero. Use Coefficients to balance equations. Never change the subscripts in formulas to “make it fit”.

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