State of

MatterChemistry AS level Cambridge University press

By: Danica Prinzessin (Danica Putri)

States of matter

Gas:1. No fixed

shape or volume

2. Randomly arraged

3. Far apart, can be compressed

4. Move freely in all directions

Liquid:1. Follow the shape of

the container2. Close together3. Fixed volume4. Compressed slighty5. Arraged fairly

randomly6. Limited movement in

all directions

Solid:1. Fixed shape and

volume2. Touching each other3. Can’t be compressed4. Regular arrangement5. Can vibrate only

diagram of objects changes in form

The Gasseous State

Kinetic Theory of Gases:1. The gas molecule move rapidly and

randomly.2. The distance between the gas molecule

is much greater than the diameter of the volume.

3. No attraction or repulsion between the molecules.

4. All collision between particle are elastic.5. The temperature of the gas is related to

the average kinetic energy of the molecules.

Ideal Gases:The volume depends on:1. Pressure, measure in pascals (Pa)2. Temperature, measure in Kelvin (K), 0

celcius=273K

General gas equation:General gas equation

Gas pressure

Where:p=pressure [Pa; N / m2]V=volume [m3]m=mass [kg]M=molar mass [kg / kmol]R=general gas constant R = 8.314510 kJ / (kmol K)T=thermodynamic temperature [K]n=molecular number density [1 / m3]k=Boltzmann's constant k = 1.380 x10-

23 J/K

General gas e.q combined with the gass law:

Limitations of the ideal gas laws:Real gas don’t obey the K.E.Theory in 2 ways:1. There isn’t zero attraction between the

molecules.2. Can’t ignore the volume of the

molecules themselves.

These differences are especially noticeable at very high pressures and very lown temperatures, under this conditions:1. The molecule are close to each other.2. Not negligible volume compared with

the volume of the container.3. Van der Waals’ or dipole-dipole forces

attraction.4. Attractive forces pull the molecules

towards each other.5. The effective volume is smaller than

expected for an ideal gas.

Deviated to ideal gas: HClNot approaches ideal gas behavior: NH4

Approaches ideal gas behavior: He

The Liquid StateBoiling Point:Liquid to Gass Energy transferred make the particles

move faster. The forces attraction of the prticles

weaker. The particle with most energy are the first

to escape from the forces holding. Evaporates. Move fast and randomly , then the particles

spread out.Melting Point:Solid to LiquidThe particles vibrate more vigorously.The forces attraction of particles are weaker. Temperature is higher than 0 degree celcius.Freezing Point:Liquid to SolidLoss kinetic energy.Increasing forces attraction of particles .

The Solid State Lattice: Ions, atoms, or molcules arrangement in the solid substance.

Structure of solid

1. Ionic latticesCharacteristic: Hard. Brittle. High melting points. High boiling points. Many of them are soluble in water. Only conduct electricity when molten or

in solution.Giant Ionic: (e.g. NaCl, MgO) Dissolvent in water. Free ions. Conduct electricity.

Ionic bond of NaCl, it also Giant ionic same as MgO

2. Metallic Lattices

Characteristic: The layers can slide over each other. Delocalised elestron. Lattice of kations. Shiny. Malleable. Conduct electricity. When the layer slide, new metallic

bond are easily re-formed between ions.

Mixture of 2 or more metals or metal with non-metal.The metal added to create the alloy becomes part of the crystal lattice of the other metal.

Characteristic: The presence of different sized

metal ions makes the arrangement of tle lattices less regular.

Layers can’t slide easily. Stronger than pure metal.

e.g.1. Zinc 30% and Copper 70%.

2. Aluminium with other elements (such as coper, magnesium, silicone, manganese).

3. Alloys

4. Simple molecular

Characteristic:Can forms crystals.Weak van der waals’ forces.Strong covalent bonds.Easily broken when heatedForms crystal lattice.

Allotrops: different crystalline or molecular forms of the same element.

Hydrogen bond:H binds with element F,N, and OCharacteristic: High boiling point Interact with other atoms are negative or

electron-rich.

Iodine crystal and its’ structure

5. Giant mollecular structure

GraphiteThe carbon atoms are arranged in

planar layer, form hexagon layers.Each carbon atom is joined to 3 other

carbon atoms by strong covalent bonds.

4th electron of each carbon atom occupies at p orbital.

Softness, the layers can slide.Good conductor of electricity.High melting and boiling points.

e.g. Pencil, lubricant.

Diamond Each carbon atom forms 4 covalent

bonds with other carbon atoms. High melting points and boiling

ponts. Hardness. Doesn’t conduct electricity or heat.

Artifical diamonds can be made by heating other forms of carbon under high pressure.

Silicon (IV)oxide Structure smiliar to diamond. Each oxygen atom is bonded to only

2 silicon atoms. Each silicon atom is bonded to 4

oxygen atoms. Colourless crystals. High melting point and boiling

point. Doesn’t conduct electricity. Hardness.

6. Ceramics

Ceramics: An inorganic non-metallic solid which is prepared by heating a substance or mixture of substances to a high temperature. Characteristic: Very high melting point and boiling

points. Don’t conduct electricity, they’re

electrical insulators. Don’t conduct heat, no free

electrons. Retain strength at high temperature

above 550 degree celcius (refractories).

Hard. Unreactive chemically.

Uses of ceramics: Ceramics containing Magnesium

oxide: Refractory in furnace linings. Electrical insulators in industrial

electrical cabel. Fire resistant wall furnaces.

Ceramics containing Aluminium Oxide: Refractory in furnace linings. As an abrasive for grinding hard

materials. In transparent aluminium oxide for

furnaces and military vechiles.

Ceramics containing silicon(IV)oxide: Refractory in furnace linings. As an abrasive. Manufacture of glass.

Conserving material

There is only a limited supply of metal ores in the earth.

Huge wasre dumps and landfill sites scarring the landscape and problem swith litter.

Recycling advantages: Saves energy. Conserves supplies of the ore. Less waste. Landfill sites don’t get filled up

fast. Cheaper than extracting the

metal from the ore.

2 metals are easily to recycle: Copper and Aluminium.

Copper:Less energy is needed to extract and refine the recycled copper.Less energy is needed to recycle copper than is needed to transport copper ore to the smelting plant and extract copper from it.

Aluminium:Isn’t necessary to extract the aluminium is much cheaper than extracting aluminium from bauxite ore.Doesn’t need the treatment of bauxite.The aluminium scrap needs less energy to melt it.The expensive electrolysis of aluminium oxide doesn’t need to be carried out.

Thanks