Chapter 9: liquids, solids, Chapter 9: liquids, solids, and solutionsand solutions

The Rock CycleThe Rock Cycle

                                                                          

Igneous

metamorphic

Sedimentary

The Rock Cycle

Igneous

The Rock Cycle

Igneous means “born of fire”

                  

Magma

Bedrock

But then theEARTH

Won’t leaveThe poor rock alone!

•Ice•Wind •Water ice

water

wind

                                                

Compression of sedimentsCompression of sedimentsis One way is One way

Sedimentary Rock Sedimentary Rock can be formedcan be formed

Igneous

metamorphic

Sedimentary

The Rock Cycle

?

Igneous

metamorphic

Sedimentary

The Rock Cycle

squished

kindamelted

                                                

HOT!

                                                

                         

         

Bands (can) form

Metamorphicmeans

“changed”

igneous

metamorphic

Sedimentary

The Rock Cycle

liquidsliquids

Made up of particles in constant motionMade up of particles in constant motion Particles closer together than gasesParticles closer together than gases Less KE than gasesLess KE than gases

Definite volumeDefinite volume FluidityFluidity Relatively high densityRelatively high density Relatively incompressibleRelatively incompressible Dissolving abilityDissolving ability Ability to diffuseAbility to diffuse Tendency to evaporate and boilTendency to evaporate and boil Tendency to solidifyTendency to solidify

Solids (2 types)Solids (2 types)

Crystalline (crystal): particles in orderly Crystalline (crystal): particles in orderly geometric patterngeometric pattern

Amorphous: random arrangementAmorphous: random arrangement

Definite shapeDefinite shape Definite volumeDefinite volume NonfludityNonfludity Definite melting pointDefinite melting point High densityHigh density IncompressibilityIncompressibility Slow rate of diffusionSlow rate of diffusion

Changes of stateChanges of state

Solid Solid liquid ( liquid (meltingmelting))

Solid Solid gas ( gas (sublimationsublimation))

Liquid Liquid solid ( solid (freezingfreezing))

Liquid Liquid gas: ( gas: (vaporizationvaporization))

Gas Gas liquid: ( liquid: (condensationcondensation))

Gas Gas solid: ( solid: (depositiondeposition))

Phase diagramPhase diagram

Triple pointTriple point: solid, liquid, gas coexist at : solid, liquid, gas coexist at equilibriumequilibrium

for water = 273.16 for water = 273.16 kelvins (0.01 °C) and a pressure of (0.01 °C) and a pressure of 611.73 pascals (ca. 6.1173 millibars, 0.0060373057 611.73 pascals (ca. 6.1173 millibars, 0.0060373057

atm).atm).

Critical temperatureCritical temperature: gas can not be : gas can not be converted to a liquid no matter how much converted to a liquid no matter how much pressure is exerted beyond the critical pressure is exerted beyond the critical temp.temp.

for water =374°C (647.096 K)for water =374°C (647.096 K)

Water cycleWater cycle

SolutionsSolutions

Homogeneous mixturesHomogeneous mixtures

ElectrolyteElectrolyte

Substance that dissolves in water and Substance that dissolves in water and gives a solution that conducts electric gives a solution that conducts electric current, e.g. NaClcurrent, e.g. NaCl

NonelectrolyteNonelectrolyte

Does not conduct electricity, e.g.sugarDoes not conduct electricity, e.g.sugar WHY??WHY??

SolventSolvent

Dissolving mediumDissolving medium

SoluteSolute

Substance dissolvedSubstance dissolved

Types of SolutionsTypes of Solutions

1. Gaseous, e.g. air1. Gaseous, e.g. air

2. Liquid, e.g. vinegar2. Liquid, e.g. vinegar

3. Solid, e.g. brass 3. Solid, e.g. brass

(solution of copper (solution of copper

and zinc)and zinc)

+ =+ =

AlloyAlloy

Mixtures in which 2 or more elements Mixtures in which 2 or more elements (usually metals) are uniformly mixed(usually metals) are uniformly mixed

SolubilitySolubility

The amt. of a substance required to form The amt. of a substance required to form a saturated soln. with a specific amt. of a saturated soln. with a specific amt. of solvent at a given temp.solvent at a given temp.

Effect of temperatureEffect of temperature

Increase in temp. usually Increase in temp. usually decreases decreases solubility of a gassolubility of a gas in a liquid in a liquid

Increase in temp. usually Increase in temp. usually increases increases solubility of a solidsolubility of a solid in a liquid in a liquid

Solubility of a gas in Solubility of a gas in waterwater

Factors affecting Factors affecting solubilitysolubility

Types of solvents, solutesTypes of solvents, solutes PressurePressure temperaturetemperature

Heat vs. temperatureHeat vs. temperature

TemperatureTemperature is a number that is related is a number that is related to the to the average kinetic energyaverage kinetic energy of the of the molecules of a substance. molecules of a substance.

HeatHeat is a measurement of the is a measurement of the total total energyenergy in a substance in a substance

Saturated solutionSaturated solution

Max. amt. of dissolved soluteMax. amt. of dissolved solute

Unsaturated soln.Unsaturated soln.

Less solute than sat. solnLess solute than sat. soln

Supersaturated solnSupersaturated soln

More solute than sat. solnMore solute than sat. soln

SuspensionsSuspensions

Heterogeneous mixture, particles settle Heterogeneous mixture, particles settle out, e.g. muddy waterout, e.g. muddy water

ColloidsColloids

Particles intermediate in size between Particles intermediate in size between solutions and suspensions, e.g. a cloudsolutions and suspensions, e.g. a cloud

Factors affecting rate of Factors affecting rate of dissolvingdissolving

Increased surface areaIncreased surface area Agitating solnAgitating soln HeatingHeating

Freezing point Freezing point depressiondepression

the difference between the freezing the difference between the freezing points of a pure solvent and a solution points of a pure solvent and a solution mixed with a solute. It is directly mixed with a solute. It is directly proportional to the concentration of the proportional to the concentration of the solutionsolution

Boiling point elevationBoiling point elevation a solution will have a higher boiling point a solution will have a higher boiling point

than that of a pure solvent after the than that of a pure solvent after the addition of a dissolved soluteaddition of a dissolved solute

ConcentrationConcentration

Measurement of the amt. of solute in a Measurement of the amt. of solute in a given amt of solvent given amt of solvent

Molarity (Molarity (MM))

The number of moles of solute in one liter The number of moles of solute in one liter of solutionof solution

molarity = # moles of solutemolarity = # moles of solute

# L of solution# L of solution

0.500 mol of NaOH is dissolved in 0.500 mol of NaOH is dissolved in enough water to yield 1.00 L of solutionenough water to yield 1.00 L of solution

0.500 mol NaOH0.500 mol NaOH

Molarity =Molarity = 1.00 L soln. 1.00 L soln.

= 0.500 = 0.500 MM NaOH NaOH

What is the molarity of 2.5 L of soln that What is the molarity of 2.5 L of soln that contains 80.0 g of NaCl?contains 80.0 g of NaCl?

80.0 g NaCl x 1 mol NaCl x 180.0 g NaCl x 1 mol NaCl x 1

58.4 g NaCl 2.5 L soln58.4 g NaCl 2.5 L soln

= 0.55 = 0.55 MM NaCl NaCl

((MM = mol/ L) = mol/ L)

How many g of NaCl are needed to make How many g of NaCl are needed to make 2,0 L of a 0.40 2,0 L of a 0.40 MM soln? soln?

0.40 mol NaCl x 58.4 g NaCl 0.40 mol NaCl x 58.4 g NaCl

1 mol NaCl1 mol NaCl

= 23.36 g/L= 23.36 g/L

23.36 g x 2.0 L = 47 g NaCl in 2 L soln23.36 g x 2.0 L = 47 g NaCl in 2 L soln

Diluting SolutionsDiluting Solutions

(M(Mii) (V) (Vii) = (M) = (Mff) (V) (Vff))

You are given a solution of commercially available You are given a solution of commercially available

aqueous ammonia (14.8 aqueous ammonia (14.8 MM NH NH33). How many mL ). How many mL of this soln is required to prepare 100.0 mL of of this soln is required to prepare 100.0 mL of 1.00 1.00 MM NH NH33 when diluted? when diluted?

MMii V Vi i = M = Mff V Vff

VVii = M = MffVVff

MMii

=(1.00=(1.00MM) (100.0 mL)) (100.0 mL)14.8 14.8 MM

= 6.76 mL= 6.76 mL

Standard DeviationStandard Deviation

Most common measure of statistical Most common measure of statistical dispersion (how widely spread the values dispersion (how widely spread the values in a data set are)in a data set are)

If the data points are If the data points are close to the meanclose to the mean, , then the standard deviation is then the standard deviation is smallsmall

If many data points are If many data points are far from the far from the meanmean, then the standard deviation is , then the standard deviation is largelarge

Standard deviation calculated as follows:Standard deviation calculated as follows: For each value For each value xxii calculate the difference calculate the difference

between between xxii and the average value . and the average value .

Calculate the squares of these differences. Calculate the squares of these differences. Find the average of the squared differences. Find the average of the squared differences.

This quantity is the variance σ2. This quantity is the variance σ2. Take the square root of the variance. Take the square root of the variance.

WaterWater

Most abundant liquid on EarthMost abundant liquid on Earth 70-90% of living mass70-90% of living mass Covalent bonds between atoms Covalent bonds between atoms withinwithin

moleculemolecule Hydrogen bonds Hydrogen bonds betweenbetween molecules molecules Highest density at 4 deg. C Highest density at 4 deg. C biological/ biological/

ecological implicationsecological implications

Structure of waterStructure of water

Crystal structure of iceCrystal structure of ice

Water cycleWater cycle

JEOPARDYJEOPARDY

SOLIDSSOLIDS LIQUIDSLIQUIDS SOLNSSOLNS WATERWATER

400400 400400 400400 400400

300300 300300 300300 300300

200200 200200 200200 200200

100100 100100 100100 100100

SCORESSCORES

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