1 / 38

Chapter 9

Chapter 9. Classifying Chemical Reactions. Types of Reactions. We will consider five types of reactions : Single displacement reactions Double displacement reactions Decomposition reactions Synthesis reactions Combustion reactions. 1. Single Replacement Reactions.

juancopeland
Download Presentation

Chapter 9

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 9 Classifying Chemical Reactions

  2. Types of Reactions • We will consider five types of reactions : • Single displacement reactions • Double displacement reactions • Decomposition reactions • Synthesis reactions • Combustion reactions

  3. 1. Single Replacement Reactions • Single Replacement Reactionsoccur when one element replaces another in a compound. • A metal can replace a metal (+) OR a nonmetal can replace a nonmetal (-). • element + compound compound + element A + BC  AC + B (if A is a metal)OR A + BC  BA + C (if A is a nonmetal) (remember the cation always goes first!) In a single replacement reaction it is better to write H2O as HOH because it will split into H+ and OH- (not H+ and O2- !!)

  4. Single Replacement • A small piece of lithium metal is added to water.

  5. Single Replacement Reaction

  6. Single Replacement Reactions • Sodium chloride solid reacts with fluorine gas NaCl(s) + F2(g)  NaF(s) + Cl2(g) unbalanced

  7. Single Replacement Reactions • Zinc metal reacts with aqueous nickel (II) nitrate Zn(s)+ Ni(NO3)2(aq) Zn(NO3)2(aq) + Ni(s)

  8. 2. Double Replacement Reactions • Double Replacement Reactionsoccur when the cations in two compounds switch places. • compound + compound  compound + compound • AB + CD  AD + CB

  9. Double Replacement Reactions • KOH + H2SO4 → K2SO4 + HOH • FeS + HCl → FeCl2 + H2S • NaCl + H2SO4 → Na2SO4 + HCl • NH4NO3 + NaCl → NH4Cl + NaNO3

  10. Decomposition Reactions • Decomposition reactions occur when a compound breaks up into two or more substances. • Some examples of decomposition reactions are: • Potassium chlorate when heated breaks into oxygen gas and potassium chloride. • 2KClO3→ 2KCl + 3O2 • Heating sodium bicarbonate decomposes into sodium carbonate and water and carbon dioxide. • 6NaHCO3→ 3Na2CO3 + 3H2O + 3CO2 ∆ ∆

  11. 3. Decomposition Reactions • Thesimplest decomposition reactions occur when a binary compound breaks up into its elements. Compound  Element + Element • In general: AB  A + B • Example: 2 H2O  2H2 + O2 • Example: 2 HgO  2Hg + O2

  12. Decomposition Reaction

  13. This reaction is highly endothermic

  14. Energy Changes • “Many” decomposition reactions involve large changes in energy (they are highly endothermic or highly exothermic).

  15. Toluene A A A

  16. Trinitrotoluene

  17. Tri-Nitro-Toluene

  18. Nitroglycerin Nitroglycerin is a contact explosive (physical shock can cause it to explode) and it degrades over time to even more unstable forms. This makes it extremely dangerous to transport or use.

  19. Alfred Nobel • Nobel found that when nitroglycerin was added to an absorbent inert substance it became safer. • He patented this in 1867 as dynamite.

  20. Alfred Nobel “The Merchant of Death is Dead”

  21. Alfred Nobel“The Merchant of Death is Dead” • The erroneous publication in 1888 of a premature obituary of Alfred Nobel by a French newspaper, condemning him for his invention of dynamite, is said to have brought about his decision to leave a better legacy after his death. • The obituary stated "The merchant of death is dead" and went on to say, "Dr. Alfred Nobel, who became rich by finding ways to kill more people faster than ever before, died yesterday.” • In reality the newspaper had instead confused Alfred for his brother who had passed away.

  22. Nobel Prizes • Nobel signed his last will and testament and set aside the bulk of his estate to establish the Nobel Prizes.

  23. Synthesis Reactions • Synthesis reactions occur when two or more substances combine to form a compound. (Sometimes these are called combination or addition reactions.) • sulfur trioxide reacts with water to make sulfuric acid. • H2O + SO3 → H2SO4

  24. 4. Synthesis reactions • The simplest Synthesis reactions occur when two elements combine and form a binarycompound. element + element  compound • Basically: A + B  AB • Example: 2H2 + O2  2H2O • Example: Fe+ Cl2  FeCl2

  25. Synthesis Reaction

  26. 5. Combustion Reactions • Combustion reactionsoccur when a hydrocarbon reacts with oxygen gas. • This is also called burning!!! • The products of combustion are carbon dioxide and water.

  27. Combustion Reactions • Example: - CxHy + O2  CO2 + H2O • Combustion is used to heat homes and run automobiles (example: octane in gasoline, is C8H18). • Combustion also got you to school today.

  28. Cellular Respiration C6H12O6 + 6O2 → 6CO2 + 6H2O

  29. Combustion Reactions • CxHy + O2  CO2 + H2O • This is an example of completecombustion. • Products in complete combustion are “ALWAYS” carbon dioxide and water. • Combustion may also be incomplete in which other products will form .

  30. Complete vs. Incomplete Combustion • Determined by the amount of oxygen. • Incomplete combustion occurs when there isn't enough oxygen to allow the fuel (usually a hydrocarbon) to react completely.

  31. Incomplete Combustion • Incomplete Combustion occurs when hydrocarbons are burned in limited oxygen • Either we limit the oxygen available or there is simply not enough oxygen – think of a car running in an enclosed garage. • we produce carbon monoxide instead of carbon dioxide, or in extremely limited oxygen we produce pure carbon (soot). • 2C3H8 + 7O2 → 6CO + 8H2O (limited oxygen) • C3H8 + 2O2 → 3C + 4H2O (extremely limited oxygen)

  32. Complete and Incomplete Combustion • In most combustion reactions both incomplete and complete combustion occur at the same time and so we form all the previously mentioned products. C9H20 + O2→ CO2+ CO + C + H2O

  33. Complete and Incomplete Combustion • We will however consider combustion to be complete when predicting the products of reactions. C9H20 + O2 → C9H20+ O2→ CO2 + H2O

  34. Gas Lighting and CO Poisoning • People who lived in 19th century cities were often poisoned by exposure to carbon monoxide from illuminating gas, which was a flammable mixture of gas suitable for lighting purposes that is made from coal and contained extremely high levels of CO.

  35. Poe's face has one eye drooping lower than the other while his mouth slants the other way. This same abnormality can be seen in the faces of people poisoned by CO today.  It is caused by the effect of repeated CO exposure on facial nerves and can be partially if not completely reversed with months of daily oxygen therapy.(very high levels of CO exposure, in comparison, can cause complete paralysis or coma)

  36. Was Poe suffering from CO poisoning or just a troubled soul? • Poe described many symptoms of CO poisoning in his letters, poems and tales. • People poisoned by CO often have the same bizarre physical and mental symptoms he describes.

  37. Homework • Reaction Type and Balancing Worksheet (Due in two days).

More Related