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CHEMICAL REACTIONS!

CHEMICAL REACTIONS!. BUBBLES PRECIPITATE COLOR CHANGES EVOLUTION OF HEAT & LIGHT (FIRE!). Chemical Equations. The “sentence” that describes the reaction. Reactants – parts before the reaction Yield sign – arrow representing the actual reaction.

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CHEMICAL REACTIONS!

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  1. CHEMICAL REACTIONS! • BUBBLES • PRECIPITATE • COLOR CHANGES • EVOLUTION OF HEAT & LIGHT (FIRE!)

  2. Chemical Equations • The “sentence” that describes the reaction. • Reactants – parts before the reaction • Yield sign – arrow representing the actual reaction. • Products – parts remaining after the reaction has occurred.

  3. Chemical Equations • MUST INCLUDE ALL REACTANTS & PRODUCTS • COMPOUNDS MUST BE WRITTEN WITH CORRECT FORMULAS ACCORDING TO OXIDATION NUMBERS • MUST SATISFY THE LAW OF CONSERVATION OF MATTER

  4. 7 DIATOMIC ELEMENTS • HYDROGEN • NITROGEN • OXYGEN • FLUORINE • CHLORINE • BROMINE • IODINE Mr & Mrs BrINClHOF

  5. Organic Nomenclature(organic means carbon based) Alkane – carbon chain held together with single bonds. General formula – CnH2n+2 Cyclic alkanes - CnH2n

  6. TYPES of CHEMICAL REACTIONS 1. Combustion – an organic molecule (carbon based) burns with oxygen and always produces CO2 and H2O. Alkanes CnH2n+2 1. methane 6. hexane 2. ethane 7. heptane 3. propane 8. octane 4. butane 9. nonane 5. pentane 10.decane

  7. Continued… 2. Synthesis – Two or more reactants combine to form one product. A + B  AB Examples sodium + sulfur hydrogen + oxygen

  8. TYPES of CHEMICAL REACTIONS 3. Decomposition – One reactant breaks apart to form two or more products. AB  A + B

  9. Types of Decomposition Reaction • binary compounds  • metal carbonate  • metal hydroxide  • metal chlorate  • acids 

  10. Continued… 4. Single Replacement – a single element replaces the similar element within a compound. • Cation exchange – positive ion is replaced • Anion exchange – negative ion is replaced

  11. Activity Series • A list of elements organized according to the ease with which they undergo reactions. • Established with single-replacement reactions - most active on top, least active on bottom.

  12. Activity Series… • Elements on the activity series chart can replace any element below it on the activity series. • Examples- • sodium + zinc chloride  • sodium + barium chloride  • chlorine + potassium iodide  • chlorine + potassium fluoride 

  13. Last but not least… 5. Double Replacement reactions – (aka- metathesis) reaction between two compounds where similar ions exchange places.

  14. Reactions in Aqueous Solutions Aqueous Solutions? Net ionic equations Spectator ions

  15. Types of D.R. Reactions • Precipitate – reaction between solutions of soluble compounds that yield an insoluble product. Example – K2SO4 + Ba(NO3)2

  16. Molecular – ionic reactions that yield a covalent product. (i.e. – water) Example – NaOH + HCl

  17. Gas – reactions that produce some type of gas that bubbles away. • Example – HCl(aq) + FeS(s)

  18. Gases to Look For as Products • H2S • NH4OH NH3 + H2O • H2CO3  H2O + CO2

  19. Examples • HBr + LiOH  • CaCO3(s) + HCl(aq)  • (NH4)2S(aq)+ LiOH(aq) • K2CrO4(aq) + AgNO3(aq) • Ca(NO3)2(aq) + RbCl(aq) 

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