1 / 21

Chapter 8

Chapter 8. Chemical Reactions. What a chemical equation looks like: yields 2 Na ( s ) + Cl 2 (g)  2 NaCl ( s ) coefficients symbols state of matter.  How to describe a chemical change 1. Word equations  Reactants  Products

hani
Download Presentation

Chapter 8

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. Chapter 8 Chemical Reactions

  2. What a chemical equation looks like: yields 2 Na (s) + Cl2(g)  2 NaCl (s) coefficients symbols state of matter

  3. How to describe a chemical change 1. Word equations  Reactants  Products  Examples: iron + oxygen  iron (III) oxide

  4. 2. skeleton equation  First step in an chemical equation  Does not show amounts  Uses common symbols

  5. 3. “Common symbols” a. solid (s) b. liquid (l) c. gas (g) d. aqueous solution (aq)- substance dissolved in water

  6. e. catalyst 1. Speeds up the reaction 2. Is not used up 3. Written on the arrow Δ –heat catalyst MnO4

  7. f. Examples MnO2 H2O2 (aq) ----> H2O (l) + O2(g) 4. skeleton examples a. Iron(III) oxide reacts with carbon monoxide to produce iron and carbon dioxide

  8. b. Heating potassium chlorate in the presence of MnO2 produces oxygen gas and potassium chloride as a solid

  9. Balancing Chemical Equations 1. 2H2(g) + O2(g)  2 H2O (l) 2. Only numbers you may write are coefficients. 3. YOU MAY NEVER CHANGE SUBSCRIPTS!

  10. 4. Leave H and O go until last. 5. Reduce if possible, lowest whole number ratios. 6. Examples: a. AgNO3 + H2S  Ag2S + HNO3

  11. b. HCl + NaOH --> NaCl + H2O c. Al(OH)3 + H2CO3 --> Al2(CO3)3 + H2O d. Al + S8 --> Al2S3 e. N2 + H2 --> NH3

  12. Types of Chemical Reaction A. Combination reaction (synthesis) 1. Two or more elements combine to form ONE product 2. A + X  AX 2K(s) + Cl2(g)  2KCl (s)

  13. B. Decomposition 1. one reactant breaks into products 2. AX  A + X 3. Ex. H2CO3 (aq)  H2O (l) + CO2 (g)

  14. C. Single displacement 1. A + BX  AX + B element + compound  compound + element 2. Ex. Cu + 2 AgCl CuCl2 + 2 Ag

  15. D. Double displacement 1. positive ions switch with positive ions 2. AX + BY  BX + AY 3. NaOH + HClNaCl + H2O

  16. E. Combustion 1. always a hydrocarbon (C and H) added to oxygen 2. products are always carbon dioxide and water 3. Ex. 2 C2H6 + 7 O2 4 CO2 + 6H2O

  17. F. See packet to do this

  18. G. Net Ionic Equation 1. Spectator ions – “watch” do not really do anything 2. Break only (aq) ions apart 3. Do not break (s) apart

  19. 4. Examples: • AgNO3(aq) + NaCl(aq) AgCl(s) + NaNO3(aq) • Pb (s) + AgNO3 (aq) Ag (s) +Pb(NO3)2(aq)

  20. F. Combustion reactions 1. always reacts with oxygen 2. hydrocarbon (some form of CH) plus oxygen always gives carbon dioxide and water

  21. 3. Examples: a. C6H6 + O2

More Related