Unit 10- Gases, Liquids, and Solids General Properties I. Solids: 1. Definite shape 2. Definite...
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Transcript of Unit 10- Gases, Liquids, and Solids General Properties I. Solids: 1. Definite shape 2. Definite...
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Unit 10- Gases, Liquids, and SolidsGeneral PropertiesI. Solids:
1. Definite shape2. Definite volume3. Not fluid 4. Melt 5. High density6. Incompressible7. Slow diffusion8. Sublimation (solid to gas)9. Rigid form
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II. Liquids:
1. Definite volume 2. Fluid
3. High density 4. Diffuse
5. Incompressible 6. Dissolve solids
7. Surface tension 8. Boil / evaporate
9. Solidify
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III. Gases:1. Expansion2. Compressible3. Fluid4. Low density5. Diffusion6. Effusion
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7. Condense to liquid
8. No definite shape
9. No definite volume
10. Change volume with Temperature
11. Change volume with Pressure
12. Deposition (to solid)
Fluid: Substance that can flow and take shape of container
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Diffusion: move from area of high concentration to low concentration
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Kinetic Properties (KMT): (Movement)
I. Gases:
1. Tiny particles
2. Constant straight line motion
3. Elastic collisions
4. Little or no attraction forces
5. Average kinetic energy
KE = ½ mv2
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II. Liquids:
1. Tiny particles
2. Constant motion (limited)
3. Elastic collisions
4. Some intermolecular attractions
5. Closely fit together
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III. Solids:
1. Tiny particles
2. Constant vibratory motion
3. Strong intermolecular forces
4. Rarely move position
5. Closely packed (fixed position)
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Examples of Gases, Liquids, and Solids
Gases: elements and compounds
Elements: a) monatomic gases – He, Ne, Ar, Kr, Xe, Rn
b) diatomic gases – H2, N2, O2, F2, Cl2
Compounds: CO, CO2, NO, NO2, N2O, N2O3, NH3, C2H6, C3H8,
SO2, SO3, AsH3 …..
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Liquids: elements and compounds
Elements: Hg, Br
Compounds: HOH, C3H2OH, C3H5(OH)3, C2H5OH, C8H18 …
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Solids: elements and compounds
Elements: most metals (Except Hg)
nonmetals P, S, I, C
Compounds: NaCl, NaHCO3, CuSO4,
MgSO4, AlNa(SO4)2,
C6H12O6, C12H22O11…
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Types of SolidsI. Crystalline : rigid unit cells, specific melting points, and crystal lattice.
Shapes: It can be cubic, tetragonal, trigonal, or thorhombic, monoclinic, triclinic, and hexagonal
Unit cell: cubic (8), body centered (9), face centered (14), hexagonal (12)
Basic Crystal systems: 7 shapes above which based on their angles, length of sides, and # of sides
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Forming Crystals: SLOW cooling, Evaporation, Pressure/ Heat to produce large perfect crystals
Defect: a) flaws with an atom – missing or extra
b) foreign atom /ion (changes color )
Ex: diamond: orange, yellow, purple, green, blue, pink
c) dislocation – off track
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crystaline types:
1) Ionic – Hard, Brittle, High melting pt.
examples: NaCl, CuSO4, AgNO3
2) Covalent – Soft, Low melting pt.
examples: NH3, HOH, CH4
3) Network - hardness vary, High MP
examples: diamond, graphite, quartz
4) Metallic – MP range, hardness range
examples: Cu, Fe, Al,…
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II. Microcrystalline Fullerines / Buckyballs contain carbon (graphite)16–128atoms
sulfur 4 – 8 atoms phosphorus 30 +/- atoms
Properties: strong, durable, hollow, fluffy shapes are spheres or tubes network bonding
Examples: tennis racket frames golf club shafts airplanes frame / outer covering
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III. Amorphous: is also called meta-stable liquids or super -cooled liquids
Properties: -melting pt range
-weak intermolecular forces
-temperature sensitive
-random molecular arrangement
Examples: Glass, Rubber, Plastics, Waxes
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Phases
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Below 0oC
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Phase Changes
G
L
S
Deposition
I. Chart-
Condense
SolidifyMelt
Evaporate/boil
Sublimation
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T
E
M
P
E N E R G Y
S
L
G
solidifymelt
boilcondense
II. Graph-
add energy
release energy
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III. Diagram-
Temp
1 atm
P
4
1 2
3
S L
G
1. Melting Pt
2. Boiling Pt
3. Triple pt
4. Critical pt
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TermsMelting: solid to liquid (add heat)Evaporation: liquid to gas without boilingBoiling: change of liquid to bubbles of vapor
that appear throughout the liquidCondensation: gas to liquid (release heat)Solidification/Freezing: liquids to solidsSublimation: solid to gas without becoming
a liquid Ex: I2, CO2, paradichlorobenzeneDeposition: gas to solid without passing liq.
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Get your thinking caps on this will
be FUN!!!!!!
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Holy Moley!!!!!
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Le Chatelier & Stress
I’ll start will an easy concept!
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Equilibrium (Le Chatelier & Stress)
Open System:
Evaporation
cool
Condensation
Room Temp
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Closed System:
Dynamic Equilibrium:
evaporation = condensation
at one specific temperature
Equilibrium: Two Opposing changes occur at equal rate
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Boiling Point
Boil at same temperature until all liquid has vaporized
Boiling Point changes with
Pressure and / or Altitude changes :
Increase pressure, BP (pressure cooker)
Decrease pressure, BP (high Mt range)
Vapor pressure=atmospheric pressure
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BOILING and ELEVATION
• DEATH VALLEY CA 100.3C
• HAZLET NJ 100.0C
• BOULDER CO 94.0C
• LEADVILLE CO 89.0C
• MT WHITNEY CA 85.0C
• MT McKINLEY CA 79.0C
• MT EVEREST TIBET 70.0C
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Stress Heat or Cool:
Implode
Equilibrium will shift to ease stress
HEAT COOLExplosion
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WaterOcean (saltwater), river, lakes and glaciers
(freshwater), cover about 75% of earth’s surface. Living things are 70% - 90% HOH.
Physical Properties of Water: 1. Ice(s), Water(l), Vapor(g)2. Angular molecule O
1050 H H
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3.Colorless, transparent, odorless, tasteless 4. Intermolecular forces (Hydrogen bond)
5. Highly polar
6. Rigid structure as solid “hex” shape
7. Most dense 4oC
8. FP 0oC / BP 100oC at STP
9. D(l) = 1.00 g/cm3
10. D(s) = .917 g/cm3 Ice floats in water
11. D(g) = .000748 g/cm3 as vapor
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12. Hf = 334 joules/g; Hv = 2260 j/g
13. Csp = 4.18 j/goC (l); 2.06 j/goC (s) ;
2.02 j/goC (g)
14. Universal solvent
Chemical Properties of Water:
1. Stable under standard conditions (STP)
STP= standard temperature (0oC) and pressure (1 atm)
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2. React with active metals H2
2 Na + 2 HOH 2NaOH + H2
3. It decomposes to H2 and O2
4. Metal oxide + HOH Bases
BaO + HOH Ba(OH)2
5. Nonmetal Oxide + HOH Acids
SO3 + HOH H2SO4
6. It promotes chemical changes.
Aqueous reactions
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Used as a Standard for:
1. Temperature at sea level(thermometer)
2. Pressure (Barometer)
3. Volume (Liter)
4. Mass (Gram)
5. Density (specific gravity)
6. Heat (calorie/joule)
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Heavy Water:
D2O (deuterium oxide)
a) 2400 liters HOH 83 ml D2O
b) more dense d= 1.2 g/cm3
c) BP 101.4 oC / MP 3.8 oC
d) used as “tracer” in chem RXNs
chemical and biological
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Terms:
1. Water of crystallization: homogeneous particles bounded by surface making definite angles. The slower the crystals form, the more perfect they are.
2. Hydrated crystal: a crystallized substance containing HOH
3. Anhydrate: substance without water
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4. Effervescence: rapid evolution of small gas bubbles5. Efflorescence: hydrated crystals lose HOH when expose to the air
Ex: Na2CO3.10HOH fast process
CuSO4.5HOH slow process
6. Deliquence: take up water from the air
Ex: NaOH fast / CaCl2 slow 7. Hydroscope: insoluble material take up
water vapor from the airEx: hair, wool, silk
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8. Miscible: two liquids can dissolve freely in one another in any portion.
Ex: water + isopropanol
9. Immiscible: two liquids are not soluble in each other. Ex: water + oil
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10. Effuse: gas particles pass through a tiny opening
11. Viscosity: the resistance of a liquid to flow. Ex: syrup
12. Lattice: 3-D arrangement of particles of a crystal
13. Unit cell: 3-D pattern of the entire lattice (repeating pattern)
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Holy Moley Math!!!!!!!!!!!!!!!!
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MATH CONCEPTS Remember the rules
sig fig sig fig sig fig
sci not sci not sci not
UNITS
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Csp = specific heat capacity; energy needed to raise 1.00 g of substance 1.0 oC
metals – low Csp
nonmetals – moderate Csp
compounds – varied Csp
H = m x Csp x T
H: energy in calories or joules m: mass
Csp: heat capacity T: change in temp.
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Ex: A 15.00 g sample of HOH is raised from 21oC to 37 oC. How much energy is needed?
H = 15.0 g x 4.18 j/goC x (37-21) oC
= 1003 joules
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FIN
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This is what you need for HeavyWater