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Properties of Ionic and M o lecular Compounds

Properties of Ionic and M o lecular Compounds. Solubility and Properties of Water Section 2.3. Objectives. C lassify ionic and molecular compounds based on their properties U se a solubility chart to predict whether an ionic compound is soluble in water

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Properties of Ionic and M o lecular Compounds

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  1. Properties of Ionic and Molecular Compounds Solubility and Properties of Water Section 2.3

  2. Objectives • Classify ionic and molecular compounds based on their properties • Use a solubility chart to predict whether an ionic compound is soluble in water • Relate the molecular structure of water to its properties

  3. Solubility • Solubility: the ability to dissolve (in our case, in water) • Aqueous (aq) : when something is very soluble • Solid (s) : when something is slightly soluble/doesn’t dissolve well • Decide this by using a solubility table: • page 57 in textbook and on your data sheet

  4. Demonstration • Copy the following table into your notes and fill in during the demonstration:

  5. How to use a solubility table • page 57 in textbook and on your data sheet • Break the compound up into its ions: • The negative ions (anions) are across the top • Find your negative ion and then look down into the chart to find the positive ion • “all” : all compounds with those ions • “most” : most compounds with those ions • “only with” : only compounds containing what’s listed • Which elements are group 1? Group 2?

  6. Solubility Table • Find the solubility/state of the following compounds using the solubility table: • (NH4)2S • AgCl • PbSO4 • Sr(OH)2 • Fe(OH)3 • Au(NO3)3 • AgCH3COO • potassium carbonate • iron (III) nitrate • ammonium sulfite • lead (IV) bromide

  7. Demo Results • Which compounds produced solids? • Could we have predicted which ones would form solids? • Can you identify which compound made the precipitate? How? • What ions do I have? How will they recombine?

  8. Properties of Water • Water is polar • Has a positive (hydrogen) and a negative (oxygen) end • Bent shape and unequal sharing of electrons • What does this mean can happen? • Water molecules are attracted to one another • Because polar, has several important properties: • Boils at higher temp • Why is this important? Hint: Think of how much of the earth is covered in water • Bodies of water serve to regulate temperatures (absorb heat during the summer and release in winter)

  9. Formation of Ice • Is ice more or less dense than liquid water? • How do you know? • Water molecules spread out as it freezes making six-sided rings • Look at a snowflake: how many points does it have? • Space in between water molecules • Makes ice less dense • Why is this important? What might be affected if ice didn’t float?

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