1 / 15

Types of Chemical Reactions

Types of Chemical Reactions. A chemical equation describes a chemical change. The Law of Conservation of Mass says that the number and kind of atoms going INTO a chemical reaction must be the same as the number and kind of atoms coming OUT.

chesna
Télécharger la présentation

Types of 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. Types of Chemical Reactions

  2. A chemical equation describes a chemical change. The Law of Conservation of Mass says that the number and kind of atoms going INTO a chemical reaction must be the same as the number and kind of atoms coming OUT. Balancing an equation makes it obey the Law of Conservation of Mass. Review

  3. The six types of chemical reactions we will discuss are: Synthesis Decomposition Single Displacement Double Displacement Acid-Base Combustion Types of Reactions

  4. Two or more substances combine to form one substance. The general form is A + X  AX Example: 2Mg + O2 2MgO Synthesis Reactions

  5. Decomposition Reactions One molecule breaks down to form two or more substances. The general form is AX  A + X Example: 2H2O  2H2 + O2

  6. Single Displacement Reactions A single element switches places with another element in a chemical compound. The general form is A + BX  AX + B Example: Ni + 2AgNO3 2Ag + Ni(NO3)2

  7. Example: Ni + 2AgNO3 2Ag + Ni(NO3)2 Single Displacement Reactions • Ni + 2AgNO3 • Nickel replaces the metallic ion Ag+. • The silver becomes free silver and the nickel becomes the nickel(II) ion.

  8. Double Displacement Reactions The cations of two compounds exchange places with each other. The general form is: AX + BY  AY + BX

  9. Double Displacement Example: NaOH + CuSO4 The Na+ and Cu2+ switch places. Na+ combines with SO42- to form Na2SO4. Cu2+ combines with OH- to form Cu(OH)2 2NaOH + CuSO4 Na2SO4 + Cu(OH)2

  10. Acid-Base Acid-base reactions are double displacement reactions which takes place when an acid and base react with each other. HA + BOH → H2O + BA AcidBase Example: HBr + NaOH → NaBr + H2O The H+ ion in the acid reacts with the OH- ion in the base, causing the formation of an ionic salt (NaBr) and water.

  11. Combustion Reaction When a compound containing carbon and hydrogen combines with oxygen, the products formed are heat, water, and carbon dioxide. CH4 + 2O2 CO2 + 2H2O

  12. Does the reaction look like this: X + O2 CO2 + H2O ? If yes - combustion reaction. 2) Is there only one product? If yes - synthesis reaction. 3) Is there only one reactant? If yes - decomposition reaction. 4) Are any reactants only one kind of element? If yes - single displacement reaction. 5) Is water a product of this reaction? If yes - acid base reaction. If not - double displacement reaction.

  13. Learning Check... Classify each of the following reactions: H2 + Cl2 2HCl Synthesis Ca + 2H2O  Ca(OH)2 + H2 Single displacement

  14. Classify each of the following reactions: 2CO + O2 2CO2 Synthesis 2KClO3 2KCl + 3O2 Decomposition Learning Check...

  15. Classify each of the following reactions: CH3SH + 3O2 CO2 + 2H2O + SO2 Combustion Zn + 2HCl ZnCl2 + H2 Single displacement Learning Check...

More Related