Unit 10 - Gases, Liquids and Solids
General Properties:
I. Gases:
1. Expansion
2. Compressible
3. Fluid
4. Low density
5. Diffusion
6. 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 shape
2. Definite volume
3. Not fluid
4. Melt
5. High density
6. Incompressible
7. Slow diffusion
8. 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…
Types of Solids
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 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
o
0C
Phase Changes
I. Chart-
G
Evaporate/
Condense boil
Deposition
L
Sublimation
Solidify
Melt
S
II. GraphT
release energy
E
M
solidify
melt
P
condense
boil
L
G
add energy
S
ENERGY
III. Diagram4
P
S
1. Melting Pt
2. Boiling Pt
L
3. Triple pt
1
2
1 atm
G
3
Temp
4. Critical pt
Terms
Melting: solid to liquid (add heat)
Evaporation: liquid to gas without boiling
Boiling: change of liquid to bubbles of vapor
that appear throughout the liquid
Condensation: gas to liquid (release heat)
Solidification/Freezing: liquids to solids
Sublimation: solid to gas without becoming
a liquid Ex: I2, CO2, paradichlorobenzene
Deposition: 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
Room Temp
Condensation
cool
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
Vapor pressure=atmospheric pressure
Boiling Point changes with
Pressure and / or Altitude changes :
Increase pressure,
BP (pressure cooker)
Decrease pressure, BP (high Mt range)
BOILING and ELEVATION
•
•
•
•
•
•
•
DEATH VALLEY CA
HAZLET NJ
BOULDER CO
LEADVILLE CO
MT WHITNEY CA
MT McKINLEY CA
MT EVEREST TIBET
100.3C
100.0C
94.0C
89.0C
85.0C
79.0C
70.0C
Stress
Heat or Cool:
HEAT
Explosion
COOL
Implode
Equilibrium will shift to ease stress
Water
Ocean (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 bubbles
5. 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 air
Ex: 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
Csp: heat capacity
m: mass
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
Heavy
Water