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Chapter 4.1 & 5.3

Chapter 4.1 & 5.3. SYNTHESIS AND DECOMPOSITION REACTIONS ELEMENTS AND THEIR OXIDES. Another good one:. http://www.funnyjunk.com/channel/Chemistry+Jokes+are+fun/cpmqGpc. Predicting Chemical Reactions.

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Chapter 4.1 & 5.3

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  1. Chapter 4.1 & 5.3 SYNTHESIS AND DECOMPOSITION REACTIONS ELEMENTS AND THEIR OXIDES

  2. Another good one: http://www.funnyjunk.com/channel/Chemistry+Jokes+are+fun/cpmqGpc

  3. Predicting Chemical Reactions • Using the periodic table, we can figure out the properties of the elements Ex. H, N, O, F, Cl, Br, I elements are all diatomic • Since the properties of the elements are predictable, the chemical reactions they undergo are also predictable Ex. Na and K are both alkali metals that react with Cl to form very stable compounds

  4. Synthesis Reactions • Two reactants combine to make a larger, more complex product Synthesis reaction between sodium and chlorine: http://www.youtube.com/watch?v=Mx5JJWI2aaw

  5. Synthesis of Ionic Compounds • Metal + Non-Metal  Ionic Compound Ex. 2 K(s) + Cl2 (g)  2 KCl (s) REMEMBER: Always apply the criss cross rule when making ionic compounds!

  6. Synthesis of Molecular Compounds • Non-metal + Non-metal  Molecular compound • Can involve: • HYDROGEN: Easy to predict because H usually forms molecular compounds and follows general pattern of synthesis Ex. H2 (g) + F2 (g)  HF (g) • NO HYDROGEN: difficult to predict because the reaction depends on reaction conditions. Ex. C and O can make CO or CO2 depending on the amount of oxygen available to react

  7. Oxides– A Special Type of Synthesis • Oxide: a compound made up of any element and oxygen • Basic oxidesMg + O2 MgOMgO + H2O  Mg(OH)2 • Acidic oxidesCO2 (g) + H2O (l)  H2CO3 (aq)SO3 (g) + H2O (l)  H2SO4 (aq) NO2(g) + H2O (l)  HNO3 (aq) + HNO2 (aq)

  8. Recall: • pH < 7 = acidic solution, pH= 7 neutral solution, pH > 7= basic solution • Acids produce H+ ions in solution • Bases produce OH- ions in solution

  9. Decomposition Reactions • A compound breaks down to form two or more simpler products • Generally need energy (heat, catalyst, electricity) to get started

  10. Decomposition of Ionic Compounds • Ionic compound  Element + Element Ex. 2 KCl (l) 2 K (s) + Cl2 (g) This reaction involves passing electricity through KCl to break it down into its elements K and Cl

  11. Decomposition Involving Compounds • Compounds with polyatomic ions or molecular compounds are difficult to predict • Use chemical tests to detect what the products are (often testing for presence of gas)Ex. 2 KClO32 KCl + 3 O2 Ex. CaCO3 CaO + CO2 Note: Both reactions require heat

  12. Examples Identify the reaction type: • 2 HCl H2 + Cl2 • Cl2O (g) + H2O (l)  2 HClO (aq) • 2 AlCl3(s)  2 Al (s) + 3 Cl2 (g) • KO(g) + H2O (l)  2 KOH (aq)

  13. Some Helpful Links • Synthesis and decomposition reactions explained:http://www.youtube.com/watch?v=yS8noHTIJ_E • Basic and acidic oxides:http://www.youtube.com/watch?v=MtL64hRoTzQ

  14. Homework pg. 161 # 1, 2, 4 pg. 204 #3, 4, 9

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