1 / 12

6.2 Types of Reactions

6.2 Types of Reactions. Objectives Distinguish among the five major types of chemical reactions. Classify a reaction as belonging to one of five major types. Why Reactions Are Classified. So that scientists could have an idea about what is going to happen when a particular reaction occurs.

bbates
Download Presentation

6.2 Types of 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. 6.2 Types of Reactions Objectives Distinguish among the five major types of chemical reactions. Classify a reaction as belonging to one of five major types.

  2. Why Reactions Are Classified • So that scientists could have an idea about what is going to happen when a particular reaction occurs. • To know what type of products to expect and what precautions need to be taken.

  3. Major Classes of Reactions • Synthesis • Decomposition • Single-Displacement • Double-Displacement • Combustion

  4. Major Classes of Reactions

  5. Synthesis • Synthesis- two or more substances combine to form one product. • Examples • 2 Na(s) + Cl2(g)  2 NaCl(s) • 4 Fe(s) + 3 O2(g)  2Fe2O3(s) • 2 CO(g) + O2 (g)  2 CO2 (g)

  6. Decomposition • Decomposition – a compound breaks down into two or more simpler substances. • Examples • 2 H2O(l)  2 H2(g) + O2(g) • 2 HgO(l) 2 Hg(l) + O2(g) • 2 H2O2(aq)  2 H2O(l) + O2(g)

  7. Single-Displacement • Single-Displacement - one element takes the place of another in a compound • Examples • Fe(s) + CuSO4(aq)  FeSO4(aq) + Cu(s) • Cl2(g) + 2 NaBr(aq)  2 NaCl(aq) + Br2(l) • Cl2(g) + 2 KBr(aq)  2 KCl(aq) + Br2 (aq)

  8. Double-Displacement • Double-Displacement – positive portions of two ionic compounds are interchanged. • One of the products is either a precipitate or water • Examples • Pb(NO3)2(aq) + 2 KI(aq)  PbI2(s) + 2 KNO3 (aq) • PbCl2(s) + Li2SO4(aq)  PbSO4(s) +2 LiCl(aq) • BaCl2(aq) + H2SO4(aq) 2 HCl(aq) + BaSO4(s)

  9. Combustion • Combustion – a substance rapidly combines with oxygen to form one or more oxides. • Examples • 2 C2H2(g) + 5 O2(g)  4 CO2(g) + 2 H2O(g) • CH4(g) + 2 O2(g)  CO2(g) + 2 H2O(g) • C6H12O6(s) + 6 O2(g)  6 CO2(g) + 6 H2O(g)

  10. Table 6.1 Types of Reactions

  11. Review • What are the five major types of reactions? • Describe each and give an example.

  12. Homework • Page 209 #1-3 • Page 225 #6

More Related