Presentation on theme: "Water, Water Everywhere, But Where’s the Solution?"— Presentation transcript:
1 Water, Water Everywhere, But Where’s the Solution? Chapter 13 Chemistry
2 Please select a Team.Team 1Team 2Team 3Team 4Team 5
3 Water is A polar molecule A nonpolar molecule A polar bear Bipolar 10 5A polar moleculeA nonpolar moleculeA polar bearBipolar10
4 A Review of WaterWater’s hydrogen bonds create a unique compound that is less dense in the solid phase and needs lots of energy to break IMF bonds.Water is a polar molecule made up of one oxygen atom and two hydrogen atoms, H2O
5 The force that acts on the surface of a liquid and tends to minimize the area of the surface is: 5Surface areaSurface tensionSurfing tensionSurface10
6 Surface TensionThe inward force, or pull, that tends to minimize the surface area of a liquid is called surface tension.All liquids have a surface tension, but water’s surface tension is higher than most.
7 A surfactant is:5Any substance that interferes with hydrogen bonding and reduces surface tensionAny substance that strengthens hydrogen bonding and increased surface tensionI have no ideaI really have no idea!10
8 Surfactant FactoidsSoaps and detergents are surfactants. Adding a detergent to beads of water on a greasy surface will cause them to collapse and spread out.
9 Solutions are: Hard to find Homogeneous mixtures 5Hard to findHomogeneous mixturesUnable to be separated by filteringAnswers 1-3None of theseI really have no idea10
10 In a solution A solvent dissolves the solute 5A solvent dissolves the soluteA solute dissolves the solvent10
11 Solvents and Solutes NaCl (aq) Solvents DISSOLVE solutes. In sugar water, water is the solvent and sugar is the solute. Solvents and solutes can be solids, liquids, or gas. Solute particles can be atoms, ions, or molecules.Heating the solvent decreases dissolving rates by adding kinetic energy and increasing rate of movement..An aqueous solution is one that contains dissolved substances.NaCl (aq)
12 15.2Solvents and SolutesIf you filter a solution through filter paper, both the solute and the solvent pass through the filter.A solution cannot be separated by filtration. The small size of the solute particles allows them to pass through filter paper.
13 Saturation is: The state of my brain currently The rings of Saturn A solution that cannot dissolve any more solute10
14 Saturation/Unsaturated Saturated: a solution that cannot dissolve any more solute under the given conditionsUnsaturated: a solution that contains less soluted than a saturated solution and can dissolve more soluteSupersaturated: a solution holding more dissolved solute than what is required to reach equilibrium
15 Solvation is:5The process where you deduce the answer to solve a problemThe process where positive and negative ions of a ionic solid become surrounded by solvent moleculesThe process where dipole covalent molecules are surrounded by solvent moleculesThe way to heaven10
16 SolvationAs individual solute ions break away from a crystal, the negatively and positively charged ions become surrounded by solvent molecules, and the ionic crystal dissolves.
17 Polar solvents such as water dissolve ionic compounds and polar compounds. 5TrueFalse10
18 Nonpolar solvents such as gasoline dissolve nonpolar compounds. 5TrueFalse10
19 Like Dissolves LikePolar solvents dissolve polar substances and nonpolar solvents dissolve nonpolar substances.Sharpie “permanent” markers are actually waterproof. The ink is a nonpolar substance which a polar substance like water cannot dissolve. What nonpolar solvent could you use?Oil is nonpolar and does not dissolve in water, a polar solvent.
20 Team Scores 766.67 Team 2 700 Team 3 633.33 Team 5 625 Team 4 525
21 The word miscible means: Liquids that cannot dissolve into each otherLiquids that attract ionsLiquids that are able to dissolve into each otherA young woman named Sybil that isn’t married.10
22 Miscible/Immiscible The obvious result of “Likes Dissolve Likes” Oil and Water DON’T MIX!!!Water and Oil are polar/non-polar liquids, and are IMMISCIBLE.
23 Which makes a solute dissolve FASTER into a solvent? Increase the temperature of the solventAgitate or stir itUse the biggest size of solute available.All of the above1 and 21 and 310
24 3 Things to Faster Dissolution Rates Increase the temperature of the solventAgitate or stir it to add kinetic energyINCREASE the amount of surface area with SMALLER pieces for greater exposure (i.e., granules NOT chunks).
25 An electrolyte is:5A compound that conducts an electric current when it is in an aqueous solution or a molten stateA compound that cannot conduct electric currentA compound that conducts electric current only in a solid state10
26 ElectroltyesAn electrolyte is a compound that can conduct an electric current when it is in an aqueous solution or molten state.The bright glow shows that sodium chloride is a strong electrolyte because nearly all the dissolved sodium chloride exists as separate Na+ and Cl– ions.All ionic compounds are electrolytes because they dissociate into ions, which carry charges. Is sugar an electrolyte?
27 A compound that contains water of hydration is called an aquifer. 5TrueFalse10
28 HydratesA compound that contains water of hydrationCuSO4 5H2O
30 A suspension is: A bridge that hangs over the PeeDee River 5A bridge that hangs over the PeeDee RiverA mixture in which particles settle upon standing.A mixture in which particles cannot be separated by filtrationA compound that must have no contact with a surface10
31 SuspensionsA suspension differs from a solution because the particles of a suspension are much larger and do not stay suspended indefinitely.Suspensions are heterogenous because at least two substances can be clearly identified.
32 Which one is a colloid? Milk Whipped cream Marshmallow Fog 1 and 4 5MilkWhipped creamMarshmallowFog1 and 4All of the above10
33 ColloidsA colloid is a heterogeneous mixture containing particles that range in size from 1 nm to 1000 nm, between a suspension and solution.
34 Coagulation of Colloids A colloidal system can be destroyed, or coagulated, by the addition of ions having a charge opposite to that of the colloidal particles.The added ions neutralize the charged colloidal particles. The particles can clump together to form heavier aggregates and precipitate from the dispersion.