Unit 10 - Gases, Liquids and Solids
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Transcript of Unit 10 - Gases, Liquids and Solids
Unit 10 - Gases, Liquids and Solids
General Properties:I. Gases:
1. Expansion2. Compressible3. Fluid4. Low density5. Diffusion6. Effusion
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
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
III. Solids:1. Definite shape2. Definite volume3. Not fluid 4. Melt 5. High density6. Incompressible7. Slow diffusion8. Sublimation (solid to gas)9. Rigid form
Diffusion: move from area of high concentration to low concentration
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
II. Liquids:
1. Tiny particles
2. Constant motion (limited)
3. Elastic collisions
4. Some intermolecular attractions
5. Closely fit together
III. Solids:
1. Tiny particles
2. Constant vibratory motion
3. Strong intermolecular forces
4. Rarely move position
5. Closely packed (fixed position)
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 …..
Liquids: elements and compounds
Elements: Hg, Br
Compounds: HOH, C3H2OH, C3H5(OH)3, C2H5OH, C8H18 …
Solids: elements and compounds
Elements: most metals (Except Hg)
nonmetals P, S, I, C
Compounds: NaCl, NaHCO3, CuSO4,
MgSO4, AlNa(SO4)2,
C6H12O6, C12H22O11…
1) Crystalline: crystal lattice (3-D)
Shapes: unit cells – cubic, body center or face center
Basic crystal systems:
a) isomeric cubic d) orthorhombic
b) tetragonal e) monoclinic
c) trigonal f) triclinic
g) hexagonal
Types of Solids
Types of Crystals
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,…
Forming Crystals: evaporation or from magma SLOW cooling: large perfect crystal
Defect: flaws (mistake in crystals)
a) foreign atom /ion (changes color )
b) internal misalignment (fuzzy)
c) dislocation - edge - screwed
Edge dislocation: extra layer of atoms extends part of the way into a crystal
Screwed dislocation: unequal growth while the crystal form
2) 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
Types of Solids:3) 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
Phases
Below 0oC
Phase Changes
G
L
S
Deposition
I. Chart-
Condense
SolidifyMelt
Evaporate/boil
Sublimation
T
E
M
P
E N E R G Y
S
L
G
solidifymelt
boilcondense
II. Graph-
add energy
release energy
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
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.
Get your thinking caps on this will
be FUN!!!!!!
Holy Moley!!!!!
Le Chatelier & Stress
I’ll start will an easy concept!
Equilibrium (Le Chatelier & Stress)
Open System:
Evaporation
cool
Condensation
Room Temp
Closed System:
Dynamic Equilibrium:
evaporation = condensation
at one specific temperature
Equilibrium: Two Opposing changes occur at equal rate
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
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
Stress Heat or Cool:
Implode
Equilibrium will shift to ease stress
HEAT COOLExplosion
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
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
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)
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
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)
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
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
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
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
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)
Holy Moley Math!!!!!!!!!!!!!!!!
MATH CONCEPTS Remember the rules
sig fig sig fig sig fig
sci not sci not sci not
UNITS
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.
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
FIN
This is what you need for HeavyWater