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1.1.2 the kinetic molecular theory
kinetic energy
kinetic energy = ½ mass times velocity squared
1.1.3 kinetic energy and temperature
kelvin to celsius
temperature in kelvin = temperature in celsius + 273.15
1.3.1 and 1.3.2 emission spectra
photon energy
where
speed of light frequency wavelength
where
1.4.1 the mole as the unit of amount
Avogadro’s constant, Avogadro number, the mole
1.4.2 relative atomic mass and relative formula mass
relative atomic mass
1.4.3 molar mass
molar mass
1.4.5 molar concentration
molar concentration
number of moles = concentration in mol times volume of solution in litres
dilution and concentration
where
1.5.3 and 1.5.4 the ideal gas laws
ideal gas equation
- P: pressure in Pa (
) - V: volume in
- n: number of moles
- R: universal gas constant,
or - T: temperature in kelvin
combined gas equation
- units should be the same on both sides for the same quantity
- P: pressure in Pa (
) - V: volume in
- T: temperature in kelvin
van der Waal’s equation
corrects for intermolecular forces and the volume that gas particles occupy
2.1.3 ionic structures and properties
lattice enthalpy
- where K is a constant for a structure that takes account of the many ion interactions and depends on the geometry of the lattice
- n and m are magnitude of charges on the ions
and are the ionic radii
ionic character of a bond
- where
is the difference in electronegativity between the atoms in a given bond
2.2.10 intermolecular forces and chromatography
retardation factor
- units for nominator and denominator need to be the same (typically
)
2.2.14 formal charge (HL)
formal charge
1.1.4 measuring enthalpy changes
transfer of thermal energy, specific heat
- Q is the heat added
- m is the mass of the object
- c is the specific heat capacity
is the temperature change
enthalpy change of combustion of a liquid
1.2.4 calculating enthalpy changes (HL)
standard enthalpy change of combustion
standard enthalpy change of formation
1.2.5 Born-Haber cycles (HL)
lattice enthalpy in born-haber cycle
1.4.1 entropy (HL)
entropy change
1.4.2 Gibbs energy (HL)
change in Gibbs energy
standard Gibbs energy change of formation
1.4.4 ∆G and equilibrium (HL)and 2.3.5 the reaction quotient, Q
reaction quotient Q
2.1.4 percentage yield
percentage yield
2.1.5 atom economy
atom economy
2.2.1 rate of reaction
rate of reaction
units are
2.2.9 and 2.2.10 rate equations
rate equation
2.2.11 the rate constant, k
units of k
2.2.12 and 2.2.13 the Arrhenius equation
Arrhenius equation
2.3.2 and 2.3.3 equilibrium law
equilibrium constant, K
for a balanced equation:
2.3.7 measuring position of equilibrium
relating the equilibrium constant and Gibbs energy change
3.1.4 the pH scale
pH
3.1.5 the ionic product constant of water
the ionic product constant of water
3.1.9 the pOH scale (HL)
3.1.10 and 3.1.11 acid and base dissociation constants (HL)
acid dissociation constant
base dissociation constant
logarithm of above
relationship between the two
3.1.17 buffer composition (HL) and pH
pH of an acidic buffer
pOH of a basic buffer
3.2.12 the standard hydrogen electrode (HL)
standard electrode potential
arbitrarily assigned
- all solutions at concentration of
- gases at pressure of
- all substances pure
- temperature
- if the half-cell does not include a solid metal, platinum is used as the electrode
3.2.13 standard electrode potentials
standard cell potential
3.2.14 electrode potentials and Gibbs energy changes (HL)
relating electrode potential and Gibbs energy changes
Faraday constant