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Dubai

A Level Chemistry Edxcel State Of Matter

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Published in: Chemistry
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Here we will discuss about the solid , liquid , there properties ideal gas equation etc

Babar M / Dubai

10 years of teaching experience

Qualification: Master of science in chemistry(MSC CHEMISTRY), Bachelors of science in Chemistry, ( BSC biology) Biology , A levels , o levels

Teaches: Biology, Chemistry, Microbiology, Biochemistry, Molecular Biology, IGCSE/AS/AL, Science, Environmental Science, Maths, Home Science

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  1. EARN CHEMISTRY WITH BABAR A LEV L CHEMISTRY STAT OF MATTER EDXC L
  2. "SAC ASSUMPTAONS OF THEORY o Ideal Gas: a gas whose volume varies in proportion to temperature and inverse to pressure. Noble gases such as helium and neon approach ideal behaviour because of their low intermolecular forces. o Ideal Gas Laws: Gas molecules move rapidly and randomly The distance between gas molecules is greater than the diameter of molecules volume is negligible No forces of attraction/ repulsion between molecules All collisions between particles are elastic EKEK conserved Temperature of gas related to average EKEK of molecules Conditions at which gases behave ideally: High temperature • Low pressure
  3. OF GAS LAWS: Real gases do not obey kinetic theory in two ways: • There is not zero attraction between molecules • We cannot ignore the volume of molecules themselves Deviations visible at low temp. and high pressure Molecules are close to each other The volume of molecules is not negligible relative to the container VDW forces present, pulling molecules to each other Pressure is lower than expected from ideal gas The effective volume is less than expected from the ideal gas
  4. CAS EQUATAONS uantityUnitConver sionPressurePascal 1 KPa = 1000PaVolumem31 m3 = 1000dm3 - 1 xl 06cm3Temperat ureOKOC + 273 uantity Pressure Volume Temperatu re Unit Pascal 3 m OK Con vers ion 1000 1m3 1000 dm3 6cm3 OC + 273
  5. STATE Particles touching but may have gaps Have EKEK slide past each other in random motion Enthalpy of Fusion: heat energy required to change 1 mole of solid into a liquid at its melting point Heating a Solid (melting): • Energy transferred makes solid particles vibrate faster • Forces of attraction weaken & solid changes to liquid Enthalpy of Vaporisation: heat energy required to change 1 mole of liquid into a gas at its boiling point Heating a Liquid (vaporisation): • • • Energy transferred makes liquid particles move faster Forces of attraction weaken The highest energy particles escape first Liquid starts to evaporate - temp. Below b.p. Forces weaken further - particles move faster & Spread Liquid boils - temp. At b.p.
  6. EVAPORATAON OF A A Constant evaporation from the surface Particles continue to break away from the surface but are trapped in space above the liquid. As gaseous particles collide, some of them hit the surface of the liquid again and become trapped there. An equilibrium is set up in which the number of particles leaving the surface is balanced by the number rejoining it. Liquid water molecules Vapor water molecules A fixed number of gaseous particles will be in the space above the liquid in this equilibrium. Vapour Pressure: pressure exerted by a vapour in equilibrium with a liquid.
  7. CRYSTALLASATQON Anhydrous Salt containing no water molecules. Hydrous Salt containing water molecules. Water of Crystallisation The number of water molecules present in the Hydrous salt. For example, has 5 water of crystalisation.
  8. RECYCLANG Finite resource: resource which doesn't get replaced at the same rate that it is used up. Examples of finite resources: copper, aluminium, glass Advantage of Recycling: o Saves energy o Reduces environmental issues o Conserves ore supplies o Less wastage o Cheaper than extracting
  9. STATES OF ANO Solubility For solids, generally, solubility increases with increasing temperature as the increase in temperature facilitates the overcoming of intermolecular bonds, making it easier for the solid to dissolve. For gases, generally, solubility decreases with increasing temperature as the pressure of the gas increases (pressure only affects the solubility of gases) Conductivity Solids (metals) are generally the best conductors of electricity, while gases are the worst. Solids (metals) are generally better conductors of heat than liquids, while liquids are better thermal conductors than gases. This is because of the proximity of molecules in solids, allowing heat to be transferred rapidly through vibrations of neighbouring molecules.
  10. SOuO STATE Diamond: • High m.p./b.p. - each carbon forms four covalent bonds • Hard-tetrahedral structure • Doesn't conduct heat or electricity - no free e- • Used for cutting as is the strongest known substance and has sharp edges Macromolecular Lattice Graphite: Three strong (sp2) covalent bonds • Fourth e- in p orbital forms a pi bond, forming a cloud of delocalised electrons above and below the planes Layers kept together by weak Van der Waal 's forces High m.p./b.p. - strong covalent bonds throughout Soft - forces between layers are weak • Conducts electricity - has delocalized electrons Macromolecular Lattice
  11. kFFkCT OF ON Relatively high m.p./b.p.: many strong H- bonds High viscosity: hydrogen bonding reduces the ability of water molecules to slide over each other High surface tension: hydrogen bonds in water exert a downward force on the surface of the liquid @ Ice is less dense than water: larger spaces between molecules in a hexagonal structure
  12. HYDROGEN-BONOEO In ice form, water molecules slow down and come closer together Due to polarity, molecules form hydrogen bonds between lone pairs of oxygen & ö+ö+charge of hydrogens Each water molecule has 2 H-bonds They arrange themselves into an open crystalline, hexagonal structure Due to large spaces, ice is less dense than water
  13. @ Iodine: • Dark grey crystalline solid; vaporizes into purple gas • m.p./b.p. are slightly higher than room temp • Slightly soluble in water; dissolves in organic solvents • Diatomic molecules formed due to covalent bonds between individual atoms • Molecules have weak Van der Waals forces of attraction between them
  14. C atoms in pentagonal and hexagonal rings Spherical C60 molecules held together by Van der Waals forces Can conduct heat and electricity Very strong and tough Insoluble in water Low m.p./b.p.
  15. NANOTlJBkS C atoms in hexagonal rings only Cylindrical The structure is rod-like due to continuing rings Conducts heat and electricity 4. Very strong and tough 6 Insoluble in water High m.p./b.p. 7.

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