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Identifying equations

Identifying equations. 5 types. Combination or synthesis reaction. Always has multiple compounds on the left and a single compound on the right A + B  AB Examples: 2K + Cl 2  2KCl S + O 2  SO 2. Combination or synthesis reaction. Decomposition reaction.

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Identifying equations

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  1. Identifying equations 5 types

  2. Combination or synthesis reaction

  3. Always has multiple compounds on the left and a single compound on the right • A + B  AB • Examples: • 2K + Cl2 2KCl • S + O2 SO2 Combination or synthesis reaction

  4. Decomposition reaction

  5. Always has on compound on the left that breaks down into multiple things on the right • AB  A + B • Examples: • CaCO3CaO + CO2 • 2HgO  2Hg + O2 Decomposition reaction

  6. Single replacement reaction

  7. One element trades places with another element to form a new compound • One element is always “dumped” • A + BC  B + AC • Single element + compound  single element + compound • Examples: • Mg + Zn(NO3)2 Mg(NO3)2 + Zn • Mg + 2AgNO3 Mg(NO3)2 + 2Ag Single replacement reaction

  8. Double replacement reaction

  9. Each compound “trades” an element • polyatomic ions can act like a single element • Compound + compound  Compound + compound • AB + CD  AD + BC • Examples: • Na2S + Cd(NO3)2CdS + 2NaNO3 • 2NaCN + H2SO4 Na2SO4 + 2HCN Double replacement reaction

  10. Sometimes elements will not react, depending on where they are on the activity series • Mg + LiNO3 no reaction • Zn + HCl H2 + ZnCl2 • Cu + HCl  no reaction • K + NaCl  Na + KCl Increasing reactivity Lithium Li Potassium K Calcium Ca Sodium Na Magnesium Mg Aluminum Al Zinc Zn Iron Fe Lead Pb (Hydrogen) (H)* Copper Cu Mercury Hg Silver Ag Decreasing reactivity Activity series

  11. Combustion reaction

  12. Element or compound reacts with oxygen to release energy. • Hydrocarbon + oxygen  carbon dioxide + water • Examples: • CH4 + 2O2 CO2 + 2H2O • C8H18O3 + 11O2  8CO2 + 9H2O Combustion reaction

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