1 / 12

Chemical Reactions

Chemical Reactions. Types of Reactions. 5 Types of Reactions. Synthesis or Combination Decompostion Single Replacement Double Replacement Combustion. Synthesis or Combination Reaction. Two or more substances combine to form another substance Example: A + B  AB

sarai
Télécharger la présentation

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. Chemical Reactions Types of Reactions

  2. 5 Types of Reactions • Synthesis or Combination • Decompostion • Single Replacement • Double Replacement • Combustion

  3. Synthesis or Combination Reaction • Two or more substances combine to form another substance • Example: A + B  AB • 2H2 (g) + O2 (g)  2H2O (g)

  4. Decomposition Reaction • One substance breaks down or decomposes into two or more simpler substances • Example: AB  A + B • 2H2O  2H2 + O2 • Just the opposite of a synthesis reaction

  5. Single Replacement Reaction • Occurs when one element replaces another in a compound • Example: AB + C  AC + B • Ba (cr) + FeBr2(aq)  BaBr2 (aq) + Fe (cr)

  6. Double Replacement Reaction • Takes place if a precipitate, water, or a gas forms when two ionic compounds in solution are combined • A precipitate is an insoluble compound formed during this type of reaction • Example: AB + CD  AC + BD • AgNO3 (aq) + NaCl (aq)  AgCl (cr) + NaNO3 (aq)

  7. Combustion Reaction • A chemical change in which an element or a compound reacts with oxygen often producing energy in the form of heat and light • Often the other reactant is a hydrocarbon which is a compound composed of hydrogen and carbon • The products of a combustion reaction are usually CO2 and H2O

  8. Example • 2 C8H18(l) + 25 O2(g) 16 CO2(g) + 18 H2O(l) • Notice the reactants and products • Reactants – Hydrocarbon reacting with Oxygen • Products – CO2 and H2O • Is this a combustion reaction • 2 Mg(s) + O2(g)  2 MgO (s) • Yes, because it reacts with oxygen producing heat and light • It can also be classified as a synthesis or combination reaction

  9. Energy and Chemical Reactions • In all chemical reactions, energy is either released or absorbed • Bonds must be broken or formed • To break bonds energy is required • To form bonds energy is released

  10. Exothermic Reaction • In many chemical reactions, less energy is required to break the original bonds than is released with the formation of new bonds • Heat is given off • Examples: Burning of wood; Explosion • Reactants  Products + Energy

  11. Endothermic Reaction • More energy is required to break the original chemical bonds than is given off. • Heat is absorbed so the container feels colder • Reactants + Energy  Products

  12. What type of reaction? • 2 NaBr + 1 Ca(OH)22 CaBr2 + 2 NaOH • 2 NH3+ 1 H2SO41 (NH4)2SO4 • 3 Pb + 3 H3PO43 H2 + 1 Pb3(PO4)2

More Related