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Chemical Reactions

Chemical Reactions. Classifying Reactions. The five general types of reaction are combination, decomposition, single-replacement, double-replacement, and combustion. Synthesis/ Combination.

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Chemical Reactions

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  1. Chemical Reactions

  2. Classifying Reactions The five general types of reaction are combination, decomposition, single-replacement, double-replacement, and combustion.

  3. Synthesis/Combination A combination reaction is a chemical change in which two or more substances react to form a single new substance. Magnesium + nitrogen yields magnesium nitride

  4. Synthesis/Combination Products: • It will always just produce ONE product • Group A metal and a nonmetal react, the compound is the metal cation and the nonmetal anion 2K(s) +Cl2(g) 2KCl(s) • When two nonmetals react in a combination reaction, more than one product possible S(s) + O2(g) SO2(g) 2S(s) + 3O2(g) 2SO3(g) • More than one product may also result from the combination reaction of a transition metal and a nonmetal Fe(s) + S(s) FeS(s) 2Fe(s) + 3S(s) Fe2S3(s)

  5. Practice with Synthesis Reactions Complete and balance this equation for a combination reaction. Be + O2 Write and balance the equation for the formation of magnesium nitride (Mg3N2) from its elements.

  6. Decomposition A decomposition reaction is a chemical change in which a single compound breaks down into two or more simpler products. Copper chloride decomposes to copper and chloride

  7. Decomposition Products: • The products can be any combination of elements and compounds. • Usually difficult to predict. • A simple binary compound will break down to its constituents. • Most decomposition reactions require energy in the form of light, heat or electricity 2HgO(s) 2Hg(l) + O2(g)

  8. Practice with Decomposition Complete and balance this decomposition reaction HI Write the formula for the binary compound that decomposes to the products H2 and Br2

  9. Single Replacement A single replacement reaction is a chemical change in which one element replaces a second element in a compound. Magnesium replaces hydrogen in hydrochloric acid to make magnesium chloride and hydrogen gas HCl+ MgH2+MgCl2

  10. Single Replacement Reaction Whether one metal will displace another metal from a compound depends upon the relative reactivities of the two metals. A reactive metal will replace any metal listed below it in the activity series.

  11. Single Replacement A halogen can replace another halogen from a compound. The activity of the halogens decrease as you go down. Br2(aq) + NaI(aq) NaBr(aq) + I2(aq) Br2(aq) + NaCl(aq) No Reaction

  12. Practice with Single Replacement Reactions Complete the equations for these single replacement reactions in aqueous solution. Balance each equation. Put “no reaction” if a reaction does not occur. Fe(s) + Pb(NO3)2(aq) Cl2(aq) + NaI(aq) Ca(aq) + H2O(l)

  13. Double Replacement Reaction A chemical change involving an exchange of positive ions between two compounds.

  14. For a Double Replacement Reaction to Take Place: • One of the products is only slightly soluble and precipitates from solution. • One of the products is a gas. • One product is a molecular compound such as water.

  15. Practice with Double Replacement Write the products of these double-replacement reactions. Then balance each equation. NaOH(aq) + Fe(NO3)3(aq) (Iron(III)hydroxide is a precipitate) Ba(NO3)2(aq) + H3PO4(aq) (Barium phosphate is a precipitate)

  16. Combustion Reactions A combustion reaction is a chemical change in which an element or a compound reacts with oxygen, often producing energy in the form of heat and light. 2C8H18(l) + 25O2(g) 16CO2(g) + 18H2O(l) The complete combustion of a hydrocarbon produces carbon dioxide and water.

  17. Practice with Combustion Reactions Write a balanced equation for the complete combustion of each compound. Formic acid (HCOOH) Heptane (C7H16)

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