1 / 16

Chemical Reactions

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

cleta
Download Presentation

Chemical Reactions

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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.

  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.

  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.

  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. 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)

  15. 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.

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

More Related