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