1 / 37

Types Of Chemical Reactions

Types Of Chemical Reactions. Objective. Distinguish between the 5 different types of reactions Predict the products of a reaction Predict the physical states of products. 5 Types of Reactions. Composition/Synthesis Decomposition Single Replacement Double Replacement Combustion.

cera
Download Presentation

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. Objective • Distinguish between the 5 different types of reactions • Predict the products of a reaction • Predict the physical states of products

  3. 5 Types of Reactions • Composition/Synthesis • Decomposition • Single Replacement • Double Replacement • Combustion

  4. Composition Reactions aka synthesis rxn • When two or more substances react to form a single product • 2 reactants → 1 product • A + X → AX • H2 + O2 → • MgO + CO2 → 2 H2O MgCO3

  5. Decomposition • Occurs when a compound is broken down into simpler substances • Single reactant yields two or more products • (1 reactant → 2 products) • forms a common gas as one of the products; CO2, O2, SO2, H2O

  6. Decomposition Examples • AX → A+ X • HgO → • CaCO3 → Hg + O2 CaO + CO2

  7. Single Replacement • One substance replaces another • A metal replaces a metal, if it is more active • A non-metal replaces a non-metal, if it is more active

  8. Single Replacement Examples • A and B are metals; X and Y are non-metals A + BX → AX + B OR Y + BX → BY + X • Mg + Zn(NO3)2 → • Cl2 + KBr → Mg (NO3)2 + Zn KCl + Br2

  9. Double Replacement • An exchange of partners • The metal replaces the metal and the non-metal replaces the non-metal • AX + BY → AY + BX • Na2S + Cd(NO3)2 → • BaCl2 + K2CO3 → NaNO3 + CdS BaCO3 + KCl

  10. Composition • Two elements or compounds combine to form a single substance • A + X → • Fe + O2 → • H2O + SO3 → AX FeO H2 SO4

  11. 5 Kinds of Decomposition Reactions • Metallic Carbonates • Metallic Hydroxides • Metallic Chlorates • Oxy Acids • Oxides

  12. Metallic Carbonates • CaCO3→ • Metal oxide and carbon dioxide formed CaO + CO2

  13. Metallic Hydroxides • Many metallic hydroxides (OH-), when heated, decompose into metallic oxides and water. • Ca(OH)2 → • Metal oxide and water formed • Exceptions to the rule: NaOH and KOH CaO + H20

  14. Metallic Chlorates • (ClO3-), when heated, decompose into metallic chlorides and oxygen • 2KClO3→ • metal chloride and oxygen formed 2KCl + 3O2

  15. Oxy Acids • Some oxy acids, when heated, decompose into nonmetallic oxides and water • Seltzer Water • H2CO3 → • Acid Rain • H2SO3 → CO2 + H2O SO2 + H2O

  16. Oxides • Some oxides, when heated, decompose. • 2HgO → • 2Pb O2 → 2Hg + O2 2PbO + O2

  17. 4 Kinds of Single Replacement Reactions • Metal w/ more active metal • Hydrogen in acids w/ more active metal • Hydrogen in water w/ by most active metals • Halogen w/ more active halogen

  18. Metal w/ more active Metal • Replacement of a metal in a compound by a more active metal (PCS Mazintl) • Zn + CuSO4 → • Zinc replaces the copper, therefore zinc is more active ZnSO4 + Cu (s)

  19. Hydrogen in acids w/ more active metals • Replacement of hydrogen, in acids, by metals more active than hydrogen (PCS Mazintl) • Zn + H2SO4 → • The corresponding metallic compound and hydrogen gas are formed Zn SO4 + H2 (g)

  20. Hydrogen in water w/ most active metals • Replacement of hydrogen, in water, by the most active metals. Which Metals? • All Group I and some of Group II • Ca + 2 H2O → • A hydroxide and hydrogen gas are formed Ca(OH)2 + H2 (g)

  21. Halogen w/ more active halogen • Replacement of a halogen by a more active halogen • Cl2 + 2 KBr → • Br2 + 2 KI → • MgBr2 + I2 → • The corresponding metallic compound and elemental halogen are formed 2 KCl + Br2 2 KBr + I2 no reaction because Br is more active than I, so I will not replace Br

  22. Activity Series of the elements • A + BX → AX + B • If A replaces B, then A is more active than B • If an element is above another element on the chart, then it is more active, and will replace the lower positioned element • All metals above hydrogen displace hydrogen from hydrochloric acid or dilute sulfuric acid.

  23. P.C.S. MazintlActivity of Halogens P potassium Fluorine C calcium Chlorine S sodium Bromine M magnesium Iodine a aluminum z zinc i iron n nickel t tin l lead HYDROGEN Copper Mercury Silver More Active

  24. Example • Zn (s) + CuSO4 (aq)→

  25. P.C.S. MazintlActivity of Halogens P potassium Fluorine C calcium Chlorine S sodium Bromine M magnesium Iodine a aluminum z zinc i iron n nickel t tin l lead HYDROGEN Copper Mercury Silver More Active

  26. Example • Zn (s) + CuSO4 (aq)→ • Mg (s) + Zn(NO3)2 (aq) → ZnSO4 (aq) + Cu (s) Mg (NO3)2 (aq) + Zn (s)

  27. Double Replacement • AX + BY → AY + BX • usually takes place in a solution of water…all reactant solutions are aqueous • 2 compounds → 2 different compounds • 1 of these will not be soluble in water…solid (s) • The soluble (dissolved) compound is aqueous…(aq) • In order for you to know if the reaction has occurred, a solid or gas must form • 1 product will typically be: • solid: precipitate • gas: CO2 SO2 NH3

  28. Solubility Rules for Double Dis(RE)placement Reactions • How to determine which product is the precipitate Na+ K+ NH4+ NO3- [ Will always be soluble in water. Tells you what won’t precipitate, so assume the other one will

  29. Examples • CaCO3 + 2 HCl → • Pb(NO3)2 + KI → • NaOH + KI → → CaCl2 + H2CO3 H2O + CO2 PbI2 + 2 KNO3 no reaction because both products are soluble NaI + KOH

  30. Combustion • An element or compound reacts with oxygen • Usually produces heat → Exothermic • Combustion of a hydrocarbon always produces carbon dioxide and water • 2 Mg + O2 → • 2 CH3OH + 3 O2 → 2 MgO + heat 2 CO2 + 4 H20 + heat

  31. Writing Molecular, Complete Ionic, and Net Ionic Equations • Molecular Equations: an equation showing the complete neutral formulas for every compound in the reaction. • AgNO3 (aq) + NaCl (aq)→ AgCl(s) + NaNO3 (aq)

  32. Complete Ionic Equations: equations that show reactants and products as they are actually present in solution. • Ionic compounds dissociate (dissolve) in water, so they are written as individual ions…if the compound is soluble…check your solubility rules • Complete Ionic Equation of : • AgNO3 (aq) + NaCl (aq)→ AgCl(s) + NaNO3 (aq)

  33. Spectator Ions: ions in solution that appear unchanged on both sides of the equation • Net Ionic Equation: equations which show only the species that actually participate in the reaction • Spectator ions are omitted from the net ionic equation

  34. Write the Net Ionic Equation for:Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq) → AgCl(s) + Na+ (aq) + NO3-(aq)

  35. Write the molecular, complete ionic and net ionic equations for the following: lead (II) nitrate reacts with lithium chloride.

  36. Write the molecular, complete ionic and net ionic equations for the following:Hydrobromic acid reacts with calcium hydroxide

  37. END

More Related