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Science 10 Chapter 4.3 Balancing Chemical Equations

Science 10 Chapter 4.3 Balancing Chemical Equations. Today. Learning check  Review chemical compounds and formulas Chemical Reactions!!!. Silver chloride__________ 2. Sulphur dioxide__________ 3. Lead (II) acetate decahydrate _______________ Silver dichromate__________

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Science 10 Chapter 4.3 Balancing Chemical Equations

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  1. Science 10 Chapter 4.3 Balancing Chemical Equations

  2. Today • Learning check  • Review chemical compounds and formulas • Chemical Reactions!!!

  3. Silver chloride__________ 2. Sulphur dioxide__________ 3. Lead (II) acetate decahydrate_______________ Silver dichromate__________ Silicon tetraflouride__________ 6. Ammonium phosphate __________ 7. Copper (I) iodide__________ 8. Iron (II) fluoride nonahydrate_____________ 9. Zinc hydrogen sulphite______________ 10. Manganese (IV) monohydrogen phosphate trihydrate ________________ Try Some Name into Formula

  4. Try Some Formula into Name 1. NI3 _______________________________ 2. Ca(OH)2 _______________________________ 3. Fe2(SO4)3.H2O _______________________________ 4. (NH4)2C2O4 _______________________________ 5. Co3(PO4)2.8H2O_______________________________ 6. H3PO4 _______________________________ 7. HClO2 _______________________________ 8. N3O _______________________________ 9. HI _______________________________ 10. Mg3P2 _______________________________

  5. Chemical Changes • Nothing is created or destroyed, only rearranged • Reactants = products • 200 yrs ago John Dalton realized atoms rearrange • # of each atom in reactants = # of each atom in products

  6. The LAW: Conservation of mass • Antoine and Marie-Anne Lavoisier in the 1700’s • Atoms are neither created or destroyed in chemical reactions • Mass reactants = mass products

  7. Indicators of chemical change • Colour changes • Temperature changes • A gas is produced • A precipitate (solid form

  8. Chemical Reactions • Occur when new substances are created reactants  products Can be written as: • A word equation: nitrogen monoxide + oxygen  nitrogen dioxide • A symbolic equation: 2NO(g) + O2(g)  2NO2(g)

  9. Word equations (the simplest) Potassium metal + oxygen gas  potassium oxide Provides limited information

  10. Skeletal Equations (Symbolic) • Show formulas of compounds/elements, but not quantities of atoms e.g., K + O2 K2O

  11. Symbolic Equations 2NO(g) + O2(g)  2NO2(g) Coefficients – indicate ratio of cmpds State of matter – dissolved in water/aqueous (aq), solid (s), liquid (l), or gas (g)

  12. Balanced chemical equation • Shows all atoms and their quantities • Number of each atom should be equal on both sides of the reaction arrow • Always use smallest whole-number ratio • To balance, change coefficients, never subscripts e.g., 4K + O2 2K2O HgO  Hg + O2

  13. Helpful hints • Balance metals first • Count polyatomic groups as 1 atom • Balance oxygen atoms last • Odd/even problem? Double it! ____Mg + ____HCl → ____MgCl2 + ____H2 ____H2 + ____ N2 → ____ NH3 ____ Fe + ____ Br2 → ____ FeBr3

  14. Try these! ____Sn(NO­2)4___K3PO4 → ___KNO2 ___Sn3(PO4)4 ____P4 + ____I2 → ____PI3 ____Al + ____O2 → ____Al2O3

  15. Today • Learning check • Review chemical compounds and formulas • Chemical Reactions #X#(s)A  B • Due tomorrow: workbook pages 71 and 73 • Due Monday: workbook pages 77, (78-79 even #’s), 80

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