Day 6 1-17 Group Quest: Previewing Assignment: Read / review section 15.1 and complete #s 1-7 on page 493 Day 6 1-17 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Q of the Day Day 1 12-5 Day 3 1-30 Calculate and record your % grade. Quest 5 = ____ Did you meet your goal? Why or why not. 3. SPECIFIC study (preparation) plan for next test? Next time I will study by … 4. Record your new goal: - If you met your goal you must improve by at least one point. If not your goal stays the same. Day 1 12-5 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Assignment page 493 #s 1-7 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Chapter 15 Water and Aqueous Systems 15.1 Water and Its Properties 15.2 Homogeneous Aqueous Systems 15.3 Heterogeneous Aqueous Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

PERIOD 1 = Friday 2-7 day 1 PERIOD 3 = Monday 2-10 day 2 Quarterly #2 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

What properties of water make it essential to life on Earth? CHEMISTRY & YOU What properties of water make it essential to life on Earth? Water covers about three quarters of Earth’s surface. All known life forms are made mostly of water. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State Molecule has net polarity Polar bonds δ– δ+ Liquid water Hydrogen bond Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State Many unique and important properties of water—including its high surface tension, low vapor pressure, and high boiling point—result from hydrogen bonding. Liquid water Hydrogen bond Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Liquid State Vapor Pressure Hydrogen bonding between water molecules also explains water’s unusually low vapor pressure. An extensive network of hydrogen bonds holds the molecules in liquid water to one another. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Solid State As water begins to cool, it behaves initially like a typical liquid. It contracts slightly, and its density gradually increases. When the temperature of the water falls below 4˚C, the density of water actually starts to decrease. Density of Liquid Water and Ice Temperature (˚C) Density (g/cm3) 100 (liquid water) 0.9584 50 0.9881 25 0.9971 10 0.9997 4 1.0000 0 (liquid water) 0.9998 0 (ice) 0.9168 normal unique to water Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Solid State Below 4˚C, water no longer behaves like a typical liquid. Ice, which forms at 0˚C, has about a 10% lower density than water at 0˚C. Ice is one of only a few solids that floats in its own liquid. Density of Liquid Water and Ice Temperature (˚C) Density (g/cm3) 100 (liquid water) 0.9584 50 0.9881 25 0.9971 10 0.9997 4 1.0000 0 (liquid water) 0.9998 0 (ice) 0.9168 unique to water Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Solid State Why is ice less dense than liquid water? The structure of ice is a regular open framework of water molecules in a hexagonal arrangement. The hexagonal symmetry of a snowflake reflects the structure of the ice crystal. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Solid State The unique properties of ice are a result of hydrogen bonding. Extensive hydrogen bonding in ice holds the water molecules farther apart in a more ordered arrangement than in liquid water. Hydrogen bond Ice Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Water in the Solid State The fact that ice floats has important consequences for all organisms. The liquid water at the bottom of an otherwise frozen body of water is warmer than 0˚C, so fish and other aquatic life are better able to survive. If ice were denser than liquid water, bodies of water would tend to freeze solid during the winter months, destroying many types of organisms. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

CHEMISTRY & YOU What properties of water that result from hydrogen bonding make it essential to life on Earth? The low vapor pressure of water keeps the liquid water in all of Earth’s lakes and oceans from evaporating rapidly. If water did not have such a high boiling point, it would be a vapor at the usual temperatures found on Earth. The fact that ice floats allows fish and other aquatic life to survive the winter months. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Bonding and Interactions BIG IDEA Bonding and Interactions Water molecules are held together through hydrogen bonds. The hydrogen bonding interactions between water molecules account for the unique properties of water, including its high surface tension, low vapor pressure, and high boiling point. Hydrogen bonding also accounts for the fact that ice is less dense than liquid water. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

I. What is a solution? water solvent A. An aqueous solution is formed when ________ is the _________. water solvent An aqueous solution is water that contains dissolved substances. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Solutions Solvents and Solutes In a solution, the dissolving medium is the solvent. The dissolved particles in a solution are the solute. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

I. What is a solution? alcohol solvent solute solvent B. A tincture is formed when _________ is the _________. C. Concentration is the amount of ________ dissolved in a given amount of _________ alcohol solvent solute solvent Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

I. What is a solution? concentration M = 1. Molarity, M or M a. Most widely-used unit of __________________ b. Formula c. Ex: concentration # mols of solute M = # L of solution 5g glucose in 100mL sol’n C6H12O6  6(12) + 12(1) + 6(16) = 1 mol x 5 g = 0.0278 mol ÷ .1L = 0.278 M 180 g Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

(Volume of Conc.)(M Conc.) = (Volume of Dilute)(M of Dilute sol’n) I. What is a solution? 2. Other units of concentration include ___________________, _______________, _________, and ____________ D. Dilution is adding more ________ to a solution to reduce the ________________. 1. Used to prepare solutions from _______________ solutions. 2. Formula mass percentage mole fraction molality normality solvent concentration stock or conc. VcMc = VdMd (Volume of Conc.)(M Conc.) = (Volume of Dilute)(M of Dilute sol’n) 21 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Vc(10 M K2Cr2O7) = (250 mL)(5 M K2Cr2O7) I. What is a solution? 3. Ex. How much 10M K2Cr2O7 should you use to prepare 250 mL of 5M K2Cr2O7? VcMc = VdMd Vc(10 M K2Cr2O7) = (250 mL)(5 M K2Cr2O7) Vc= Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Assignment page 493 #s 1-7 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Period 1 = Double = Prelab Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.