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NOTEPACK: UNIT 2 – Matter and Change

NOTEPACK: UNIT 2 – Matter and Change. Conceptual Chemistry. Unit 2 Objectives. 1) Read and express information given in chemical formulas. 2) Classify matter as a pure substance or a mixture.

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NOTEPACK: UNIT 2 – Matter and Change

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  1. NOTEPACK: UNIT 2 – Matter and Change Conceptual Chemistry

  2. Unit 2 Objectives 1) Read and express information given in chemical formulas. 2) Classify matter as a pure substance or a mixture. 3) Distinguish between chemical and physical properties of matter, as well as chemical and physical changes. 4) Balancing chemical equations. 5) Describing chemical reactions and calculate percent yield and percent error.

  3. OBJECTIVE 4: Balancing chemical equations. • Today we will practice balancing and writing chemical equations.

  4. Chemical Equation • Describes the original beginning substances (called reactants) using chemical formulas. Then an arrow points to the newly created substances (called products)using chemical formulas again. • Reactants  Products

  5. Symbols used in chemical equations:

  6. Symbols used in chemical equations:

  7. Symbols used in chemical equations:

  8. Symbols used in chemical equations:

  9. Symbols used in chemical equations:

  10. Symbols used in chemical equations:

  11. Symbols used in chemical equations:

  12. Symbols used in chemical equations:

  13. Symbols used in chemical equations:

  14. Symbols used in chemical equations:

  15. Balancing Equations • The law of conservation of mass states that matter cannot be created or destroyed. So, the number of atoms reacting must equal the number of atoms produced. However, a chemical change rearranges these atoms into new substances.

  16. To balance equations, follow these steps: 1) Count atoms on each side of the arrow. They should be equal. If not, you need to balance them.

  17. To balance equations, follow these steps: 1) Count atoms on each side of the arrow. They should be equal. If not, you need to balance them. 2) Balance both sides by using coefficients. Remember, they multiply through everything inside of that compound. NEVER change subscripts.

  18. To balance equations, follow these steps: 1) Count atoms on each side of the arrow. They should be equal. If not, you need to balance them. 2) Balance both sides by using coefficients. Remember, they multiply through everything inside of that compound. NEVER change subscripts. 3) Double-check work.

  19. Check if CORRECT! 

  20. OBJECTIVE 4 Practice Problems: ____KClO3 ____KCl + ____O2 ____AlBr3 + ____K2SO4 ____KBr + ____Al2(SO4)3 ____ C3H8 + ____ O2 ____ CO2 + ____ H2O Δ Δ

  21. OBJECTIVE 4 Practice Problems: 2 KClO3 2 KCl + 3 O2 ____AlBr3 + ____K2SO4 ____KBr + ____Al2(SO4)3 ____ C3H8 + ____ O2 ____ CO2 + ____ H2O Δ Δ

  22. OBJECTIVE 4 Practice Problems: 2 KClO3 2 KCl + 3 O2 2 AlBr3 + 3 K2SO4 6 KBr + 1 Al2(SO4)3 ____ C3H8 + ____ O2 ____ CO2 + ____ H2O Δ Δ

  23. OBJECTIVE 4 Practice Problems: 2 KClO3 2 KCl + 3 O2 2 AlBr3 + 3 K2SO4 6 KBr + 1 Al2(SO4)3 1 C3H8 + 5 O2 3 CO2 + 4 H2O Δ Δ

  24. OBJECTIVE 4 Practice Problems from in-class demos: Δ 1)H2 + O2 H2O

  25. OBJECTIVE 4 Practice Problems from in-class demos: Δ 1) 2 H2 + 1 O2 2 H2O

  26. OBJECTIVE 4 Practice Problems from in-class demos: Δ 1) 2 H2 + 1 O2 2 H2O 2)_Fe + O2 Fe2O3 Δ

  27. OBJECTIVE 4 Practice Problems from in-class demos: Δ 1) 2 H2 + 1 O2 2 H2O 2) 4 Fe + 3 O2 2 Fe2O3 Δ

  28. OBJECTIVE 4 Practice Problems from in-class demos: Δ 1) 2 H2 + 1 O2 2 H2O 2) 4 Fe + 3 O2 2 Fe2O3 3)C6H12O6 +O2 H2O + CO2 Δ Δ

  29. OBJECTIVE 4 Practice Problems from in-class demos: Δ 1) 2 H2 + 1 O2 2 H2O 2) 4 Fe + 3 O2 2 Fe2O3 3) 1 C6H12O6 + 6 O2 6 H2O + 6 CO2 Δ Δ

  30. OBJECTIVE 4 Practice Problems from in-class demos: Δ 1) 2 H2 + 1 O2 2 H2O 2) 4 Fe + 3 O2 2 Fe2O3 3) 1 C6H12O6 + 6 O2 6 H2O + 6 CO2 4)C3H8O +O2 H2O + CO2 Δ Δ Δ

  31. OBJECTIVE 4 Practice Problems from in-class demos: Δ 1) 2 H2 + 1 O2 2 H2O 2) 4 Fe + 3 O2 2 Fe2O3 3) 1 C6H12O6 + 6 O2 6 H2O + 6 CO2 4) 2 C3H8O + 9 O2 8 H2O + 6 CO2 Δ Δ Δ

  32. OBJECTIVE 4 Practice Problems from in-class demos: Δ 1) 2 H2 + 1 O2 2 H2O 2) 4 Fe + 3 O2 2 Fe2O3 3) 1 C6H12O6 + 6 O2 6 H2O + 6 CO2 4) 2 C3H8O + 9 O2 8 H2O + 6 CO2 5)H2O2H2O + O2 Δ Δ Δ MnO2

  33. OBJECTIVE 4 Practice Problems from in-class demos: Δ 1) 2 H2 + 1 O2 2 H2O 2) 4 Fe + 3 O2 2 Fe2O3 3) 1 C6H12O6 + 6 O2 6 H2O + 6 CO2 4) 2 C3H8O + 9 O2 8 H2O + 6 CO2 5) 2 H2O2 2 H2O + 1 O2 Δ Δ Δ MnO2

  34. OBJECTIVE 4 Practice Problems from in-class demos: Δ 6)CH4O(g) +O2(g)  H2O(g) +CO2(g)

  35. OBJECTIVE 4 Practice Problems from in-class demos: Δ 6) 2 CH4O(g) + 3 O2(g)  4 H2O(g) + 2 CO2(g)

  36. OBJECTIVE 4 Practice Problems from in-class demos: Δ 6) 2 CH4O(g) + 3 O2(g)  4 H2O(g) + 2 CO2(g) 7)KClO3(s)  KCl(s) + O2(g) Δ

  37. OBJECTIVE 4 Practice Problems from in-class demos: Δ 6) 2 CH4O(g) + 3 O2(g)  4 H2O(g) + 2 CO2(g) 7) 2 KClO3(s)  2 KCl(s) + 3 O2(g) Δ

  38. OBJECTIVE 4 Practice Problems from in-class demos: Δ 6) 2 CH4O(g) + 3 O2(g)  4 H2O(g) + 2 CO2(g) 7) 2 KClO3(s)  2 KCl(s) + 3 O2(g) 8)KI(aq) +Pb(NO3)2(aq)  KNO3(aq) +PbI2(s) Δ

  39. OBJECTIVE 4 Practice Problems from in-class demos: Δ 6) 2 CH4O(g) + 3 O2(g)  4 H2O(g) + 2 CO2(g) 7) 2 KClO3(s)  2 KCl(s) + 3 O2(g) 8) 2 KI(aq) + 1 Pb(NO3)2(aq)  2 KNO3(aq) + 1 PbI2(s) Δ Yellow!!!

  40. OBJECTIVE 4 Practice Problems from in-class demos: Δ 6) 2 CH4O(g) + 3 O2(g)  4 H2O(g) + 2 CO2(g) 7) 2 KClO3(s)  2 KCl(s) + 3 O2(g) 8) 2 KI(aq) + 1 Pb(NO3)2(aq)  2 KNO3(aq) + 1 PbI2(s) 9)Al(s) +CuCl2(aq)  AlCl3(aq) + Cu(s) Δ

  41. OBJECTIVE 4 Practice Problems from in-class demos: Δ 6) 2 CH4O(g) + 3 O2(g)  4 H2O(g) + 2 CO2(g) 7) 2 KClO3(s)  2 KCl(s) + 3 O2(g) 8) 2 KI(aq) + 1 Pb(NO3)2(aq)  2 KNO3(aq) + 1 PbI2(s) 9) 2 Al(s) + 3 CuCl2(aq)  2 AlCl3(aq)+ 3 Cu(s) Δ

  42. OBJECTIVE 4 Practice Problems from in-class demos: Δ 6) 2 CH4O(g) + 3 O2(g)  4 H2O(g) + 2 CO2(g) 7) 2 KClO3(s)  2 KCl(s) + 3 O2(g) 8) 2 KI(aq) + 1 Pb(NO3)2(aq)  2 KNO3(aq) + 1 PbI2(s) 9) 2 Al(s) + 3 CuCl2(aq)  2 AlCl3(aq)+ 3 Cu(s) 10)K(s) + H2O(l)  KOH(aq) + H2(g) Δ Δ

  43. OBJECTIVE 4 Practice Problems from in-class demos: Δ 6) 2 CH4O(g) + 3 O2(g)  4 H2O(g) + 2 CO2(g) 7) 2 KClO3(s)  2 KCl(s) + 3 O2(g) 8) 2 KI(aq) + 1 Pb(NO3)2(aq)  2 KNO3(aq) + 1 PbI2(s) 9) 2 Al(s) + 3 CuCl2(aq)  2 AlCl3(aq)+ 3 Cu(s) 10) 2 K(s) + 2 H2O(l)  2 KOH(aq) + 1 H2(g) Δ Δ

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