1 / 14

Reaction Types

Reaction Types. How do we know what will be produced in a chemical reaction?. Recognizing a pattern of reactivity gives a broader understanding than memorizing a large number of reactions Would expect elements of the same family to behave similar 2K + 2H 2 O → 2KOH + H 2

amaya-hartman
Download Presentation

Reaction Types

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. Reaction Types

  2. How do we know what will be produced in a chemical reaction? • Recognizing a pattern of reactivity gives a broader understanding than memorizing a large number of reactions • Would expect elements of the same family to behave similar • 2K + 2H2O → 2KOH + H2 • What will happen if Na combines with water?

  3. Five Types of Reactions • Combustion – rapid reaction that produces flame • Occurs in hydrocarbons (compounds of C, H, and sometimes O) • Reaction of hydrocarbon with oxygen to produce carbon dioxide and water • C3H8 + 5O2 → 3CO2 + 4H2O • 2CH3OH + 3O2 → 2CO2 + 4H2O

  4. Combination or Synthesis • Two reactants combine to form a single product • A + B → AB • Examples • C + O2→ CO2 • N2 + 3H2→ 2NH3 • CaO + H2O → Ca(OH)2

  5. Decomposition • Single reactant breaks apart to form two or more substances • AB → A + B • Examples • 2KClO3 → 2KCl + 3O2 • CaCO3 → CaO + CO2

  6. Single Replacement • One element replaces another similar element in a compound • A + BX → AX + B • Examples • Fe + 2HCl → FeCl2 + H2 • Zn + CuSO4 → ZnSO4 + Cu • Na + 2H2O → 2NaOH + H2

  7. Double Replacement • Atoms exchange partners • Also called metathesis reactions • AX + BY → AY + BX • We will look at two types of double replacement • Acid-base reactions • Precipitation reactions

  8. Acid-Base Reactions • Acid – substance that increases the H+ concentration in aqueous solutions • HCl → H+ + Cl- • H2SO4→ H+ + HSO4- • HSO4→ H+ + SO42-

  9. Base • Increases the OH- concentration • NaOH → Na + OH- • NH3 + H2O → NH4+ + OH-

  10. Neutralization • Acids and bases react together to produce a salt (ionic compound) and water • HCl + NaOH → NaCl + H2O • Write a balanced equation for the reaction of hydrobromic acid, HBr, with barium hydroxide, Ba(OH)2.

  11. Write the balanced equation for the reaction between phosphoric acid, H3PO4, and potassium hydroxide.

  12. Precipitation Reaction • Double replacement that forms a precipitate • KI (aq) + Pb(NO3)2 (aq) → PbI2 (s) + 2KNO3 (aq)

  13. Example • When sodium phosphate and barium nitrate are mixed, a precipitate of barium phosphate forms. Write the balanced equation.

  14. Example • When aqueous sodium hydroxide and magnesium nitrate are mixed, a magnesium hydroxide precipitate forms. Write the balanced chemical equation.

More Related