Chapter 9: liquids, solids, and solutions. The Rock Cycle.
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Transcript of Chapter 9: liquids, solids, and solutions. The Rock Cycle.
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
TEAM 1TEAM 1 TEAM 2TEAM 2 TEAM 3TEAM 3 TEAM 4TEAM 4