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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

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unit 10 gases liquids and solids
Unit 10 - Gases, Liquids and Solids

General Properties:

I. Gases:

1. Expansion

2. Compressible

3. Fluid

4. Low density

5. Diffusion

6. Effusion

slide2
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

slide3
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

slide4
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

slide6
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

slide7
II. Liquids:

1. Tiny particles

2. Constant motion (limited)

3. Elastic collisions

4. Some intermolecular attractions

5. Closely fit together

slide8
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
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 …..

slide10
Liquids: elements and compounds

Elements: Hg, Br

Compounds: HOH, C3H2OH, C3H5(OH)3, C2H5OH, C8H18 …

slide11
Solids: elements and compounds

Elements: most metals (Except Hg)

nonmetals P, S, I, C

Compounds: NaCl, NaHCO3, CuSO4,

MgSO4, AlNa(SO4)2,

C6H12O6, C12H22O11…

slide12

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
Types of Crystals
  • Ionic – Hard, Brittle, High melting pt.

examples: NaCl, CuSO4, AgNO3

  • Covalent – Soft, Low melting pt.

examples: NH3, HOH, CH4

  • Network - hardness vary, High MP

examples: diamond, graphite, quartz

  • Metallic – MP range, hardness range

examples: Cu, Fe, Al,…

slide14
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

slide15

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
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

phase changes
Phase Changes

I. Chart-

G

Evaporate/

Condense

boil

Deposition

L

Sublimation

Solidify

Melt

S

slide20

II. Graph-

release energy

T

E

M

P

G

condense

boil

L

solidify

add energy

melt

S

E N E R G Y

slide21

III. Diagram-

4

  • Melting Pt
  • Boiling Pt
  • Triple pt
  • 4. Critical pt

P

S

L

1

2

1 atm

G

3

Temp

slide22
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.

slide25

Le Chatelier & Stress

I’ll start will an easy concept!

equilibrium le chatelier stress
Equilibrium (Le Chatelier & Stress)

Open System:

Evaporation

Condensation

cool

Room Temp

slide27

Closed System:

Dynamic Equilibrium:

evaporation = condensation

at one specific temperature

Equilibrium: Two Opposing changes occur at equal rate

slide28

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
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
slide30

Stress Heat or Cool:

HEAT

COOL

Explosion

Implode

Equilibrium will shift to ease stress

water
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

slide34
3.Colorless, transparent, odorless, tasteless4. 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

slide35
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)

slide36
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

slide37
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)

slide38

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

slide39
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

slide40
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

slide41
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

slide42
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)

slide45

MATH CONCEPTS

Remember the rules

sig figsig figsig fig

sci not sci notsci not

UNITS

slide46

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.

slide47

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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