Mr. Fady Hany Chemistry Platform Secondary Stage

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States of matter

Solid, liquid, vapour or gas

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Solid

Small interspaces and incompressible (Fixed volume)

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Liquid

Larger interspaces and incompressible (Fixed Volume)

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Gas / Vapour

Very large interspaces and compressible (P inc. lead to V dec.)

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Fusion (or Melting)

Process that absorb heat due to increase in temperature

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Evaporation

Process that absorb heat due to increase in temperature

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Process that release heat due to decrease in temperature

Condensation, freezing and deposition

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Turning from solid to gas WITHOUT passing through liquid state

Sublimation

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Turning from gas to solid WITHOUT passing through liquid state

Deposition

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Average kinetic energy of molecules increase means

Temperature increases

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Heat

Form of energy measured by joule that transfer from hot to cold due to difference in temperature

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Temperature conversions

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When temperature change by

1℃ = 1K = 1.8F

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Process that absorb heat

Endothermic

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Process that release heat

Exothermic

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Low specific heat

Get hot and cold fast

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Large specific heat

Get hot and cold slow like water

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Specific Heat measured by

kJ/kg.K or J/g.℃

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Quantity of heat absorbed or released when temperature doesn't change

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Quantity of heat absorbed or released that lead to change in temperature

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Number of moles

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Water has high latent heat of vapourization

due to presence of hydrogen bond BETWEEN WATER MOLECULES

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Intermolecular forces

Van Der Waals forces, Hydrogen bonds

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Intramolecular forces

Ionic Bond, Covalent Bond, Metallic Bond

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Number of hydrogen bonds increases

Boiling Point increases