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CHEMICAL BONDS

CHEMICAL BONDS. CHAP 9. For Science Fair Judges Write a 1 – 2 page word-processed report evaluating 2 projects. If you are not a judge, you may submit this assignment for 15 extra- credit points or as a lab make-up. Composition of Ionic Compounds. Common names : “salt” → sodium chloride

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CHEMICAL BONDS

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  1. CHEMICAL BONDS CHAP 9

  2. For Science Fair Judges Write a 1 – 2 page word-processed report evaluating 2 projects. If you are not a judge, you may submit this assignment for 15 extra- credit points or as a lab make-up.

  3. Composition of Ionic Compounds Common names: “salt” → sodium chloride “lye” → sodium hydroxide “rust” → iron oxide “baking soda” → sodium bicarbonate “chalk” → calcium carbonate

  4. Fig. 9.12 Three substances containing sodium and some form of the carbonate ion

  5. Names for Ionic Compounds containing only two different elements • Metal (positive) ion is written and spoken first • Negative element is written/spoken second • Subscripts used to produce an electrically • neutral compound • e.g. NaCl, CaO, KI, Fe2O3, CaC2

  6. Fig 11.6 NaCl dissolving in water

  7. Box Fig. 9.1 Conductivity tester for determining if a solution contains ions Fact: Dissolving an ionic compound in water results in ions being pulled apart from the crystal lattice to form free ions + −

  8. Chemical Reactions Chapter 10

  9. Homework for Chap 10 Read p 253 – 257; 261 - 271 Applying the Concepts # 1 – 17

  10. molecular empirical H2O Chemical Formulas An empirical formula shows the simplest whole-number ratio of the atoms in a substance A molecular formula shows the actual number of atoms of each element in the smallest unit of a substance H2O CH2O C6H12O6 O3 O N2H4 NH2

  11. Fig. 10.2 Several ways to express common molecules

  12. 3 ways of representing the reaction of H2 with O2 to form H2O reactants products A process in which one or more substances is changed into one or more new substances is a chemical reaction A chemical equation uses chemical symbols to show what happens during a chemical reaction

  13. Fig. 10.4 The Combustion of Charcoal “Carbon reacts with oxygen to yield carbon dioxide” C + O2→ CO2

  14. Fig. 10.5 The meaning of subscripts and coefficients

  15. Fig. 10.6 Illustration of the Law of Conservation of Mass

  16. Fig. 10.8 Hydrocarbons and Carbohydrates C12H22O11 C8H18 C3H8

  17. Types of Chemical Reactions • Oxidation-Reduction (Redox) • Combination • Decomposition • Replacement • Ion Exchange

  18. 2Mg (s) + O2 (g) 2MgO (s) Oxidation-Reduction Reactions (electron transfer reactions) Oxidation – an atom loses electrons Reduction – an atom gains electrons O2 is the oxidizing agent (takes electrons) Mg is the reducing agent (supplies electrons)

  19. Fig. 10.9 Example of an oxidizing agent (“chlorine”) Others: 1) Bleach 2) Hydrogen peroxide 3) Oxygen 4) Ultraviolet light

  20. Types of Chemical Reactions • Oxidation-Reduction (Redox) • Combination • Decomposition • Replacement • Ion Exchange

  21. 4 Fe (s) + 3 O2 (g) 2 Fe2O3 (s) Fig. 10.10 Iron combines with oxygen to form rust (iron oxide)

  22. Types of Chemical Reactions • Oxidation-Reduction (Redox) • Combination • Decomposition • Replacement • Ion Exchange

  23. Fig. 10.11 Decomposition of Mercury Oxide heat 2 HgO (s)→ 2 Hg (l) + O2(g)

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