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Chemical Changes (Reactions)

Chemical Changes (Reactions). Reactants Products Synthesis Single Replacement Double Replacement Decomposition. Chemical Reactions. Indicators Fizzing (gas produced) Color change Gets cloudy/precipitant (solid produced) Heat released or absorbed Light emitted Odor changes.

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Chemical Changes (Reactions)

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  1. Chemical Changes (Reactions) • Reactants • Products • Synthesis • Single Replacement • Double Replacement • Decomposition

  2. Chemical Reactions • Indicators • Fizzing (gas produced) • Color change • Gets cloudy/precipitant (solid produced) • Heat released or absorbed • Light emitted • Odor changes

  3. Chemical Reactionshttp://ed.ted.com/lessons/if-molecules-were-people-george-zaidan-and-charles-morton • Reactants  Products • H2O2 H2O + O2 • What are the reactants? What are the products?

  4. Chemical Reactions There are 4 kinds of Chemical Reactions that occur: Synthesis Decomposition Single Double Replacement Replacement

  5. Chemical Reactions • Synthesis • Two or more reactants are combined to form one product. +

  6. Chemical Reactions • Decomposition • One reactant breaks down into two or more products. +

  7. Chemical Reactions • Single Replacement • An element and a compound combine. • One element from the reactants replaces another in the products. + +

  8. Chemical Reactions • Double replacement • Two compounds combine. • Two elements in the reactants switch places in the products. + +

  9. Chemical Reactions-Practice Identifying • Example #1 • H2 + O2 H2O Which is it? • Synthesis • Decomposition • Single Replacement • Double Replacement

  10. Chemical Reactions Which is it? • Synthesis • Decomposition • Single Replacement • Double Replacement • Example #2 • Li3P  Li + P

  11. Chemical Reactions Which is it? • Synthesis • Decomposition • Single Replacement • Double Replacement • Example #3 • Na + MgCl2 Mg + NaCl

  12. Chemical Reactions • Example #4 • SiCl4 + O2 SiO + Cl2 Which is it? • Synthesis • Decomposition • Single Replacement • Double Replacement

  13. Chemical Reactions • Example #5 • C5O3 C + O2 Which is it? • Synthesis • Decomposition • Single Replacement • Double Replacement

  14. Chemical Reactions • Example #6 • Rb2O + AlF3 RbF + Al2O3 Which is it? • Synthesis • Decomposition • Single Replacement • Double Replacement

  15. Chemical Reactions Law of conservation of Matter Atoms are not created or destroyed The number of atoms at the START of a reaction, there must be the same number of atoms AFTER the reaction. Equations must be balanced!

  16. Chemical Reactions Balancing Chemical Equations STEPS: Count the number of atoms for each element in the reactants and in the products. Compare the numbers to see if each element is balanced (equal) with itself. Use WHOLE NUMBER coefficients to “fix” unbalanced elements. Do not change the subscripts!

  17. Chemical Reactions Balancing Chemical Equations STEPS: Whole number coeficients go in front of the compound or element in the equation and multiply every atom after it. Ex: NaCl3 has 1 Na atom and 3 Cl atoms but if I needed to have 2 Na atoms in my reactants or products, I would put a coefficient of 2 in front of the compound NaCl3….. 2NaCl3 and now I would have 2 Na atoms, but also 6Cl atoms You cannot put a coefficient in between a compound!ts!

  18. Chemical Reactions • Example #1 • H2 + O2 H2O • H-2 H-2 • O-2 O-1 • 2H2 + O22H2O BALANCED • H-4 H-4 • O-2 O-2

  19. Chemical Reactions • Example #2 • Li3P  Li + P • Li-3 Li-1 • P-1 P-1 • Li3P 3Li + P BALANCED • Li-3 Li-3 • P-1 P-1

  20. Chemical Reactions • Example #3 • C5O3 C + O2 • 2C5O310C + 3O2 BALANCED

  21. Chemical Reactions • Example #4 • Rb2O + AlF3 RbF + Al2O3

  22. Chemical Reactions • Example #5 SnO2 + H2 → Sn + H2O

  23. Chemical Reactions • Example #6 • Mg(ClO3)2 + Na  NaClO3 + Mg

  24. Chemical Reactions • Example #7 • Al2(SO4)3 + RbF  AlF3 + Rb2SO4

  25. Chemical Reactions • Identify and Balance • Al + F2 AlF3

  26. Chemical Reactions • Identify and Balance • Ca(MnO4)2 + FeCl4 CaCl2 + Fe(MnO4)4

  27. Chemical Reactions • Identify and Balance • Si3O  Si8 + O2

  28. Chemical Reactions • Identify and balance • Cs2O + N2 Cs3N + O2

  29. Warm Up • Classify the following chemical reactions as decomposition, single replacement, double replacement or synthesis: • For the first equation, what are the reactants and what are the products? • Write the chemical formula for Barium Nitride

  30. Acids and Bases

  31. Draw a Line Like this in the middle of your paper • 0 c 0 7 14 \ You will cut out the pictures you get on the paper and arrange them along the pH scale you have drawn. Do your best to guess where things might go…DO NOT glue them down until you check with me firstu

  32. Acidsproperties • Conduct electricity (electrolytes) • Produce H+ ions • Sour taste • Corrosive • pH values 0-6.9

  33. Acids • Acids • pH range = 0-6.9 • Examples: Citric Acids, Gastric Acid, Battery Acid, Sodas, tomatoes, etc. • Examples of Formulas: HCl, H2SO4, H3PO4, HNO3, etc SPOILED MILK

  34. Basesproperties • Conduct electricity (electrolytes) • OH- ions • Bitter taste • Corrosive • Have a slippery feeling (like soap) • pH values 7.1-14

  35. Bases • Bases pH range 7.1 to 14 • Examples: Soaps, Cleaning supplies, Hair Relaxers, etc. • Examples of Formulas:NaOH, KOH, Mg(OH)2, Al3(OH), NH3, NH4OH

  36. Acids & Bases-pH Scale

  37. Acids and Bases-Compare & Contrast

  38. 9. Electrolyte 10. pH = 13 11. pH = 4 12. H2SO4 13. HBr 14. FrOH 15. Corrosive 16. Bitter taste Acids and Bases--Identify • pH =2 • HF • pH= 7 • RbOH • Ca(OH)2 • pH= 9 • Sour taste • Slippery feel

  39. Acids & Bases • Neutralization Reactions • Only an Acid can neutralize a base Only a Base can neutralize an acid • H+ comes off of the Acid and OH- comes off of the Base (OH and H make water!) • Acid + Base  Water + Salt • Ex: HCl + KOH  H2O + KCl

  40. Acid/Base Neutralization • HBr + LiOH  _________ + _________ • FrOH + HCl  _________ + _________ • H2S + Mg(OH)2 ________ + _______ • ______ + HF  H20 + KF • ______ + CsOH  H20 + CsI

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