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Chemistry Unit 1
- Mass Number = Number of Protons +
Neutrons (in the nucleus/atom)
- Relative Atomic Mass = The mean mass of
an atom of an element compared to one
twelfth the mass of a 12C atom.
- The first ionisation energy is the enthalpy change when one mole of
gaseous atoms forms one mole of gaseous ions with a single positive
charge
- The second ionisation energy is the enthalpy change
when one mole of gaseous ions with a single positive
charge forms one mole of gaseous ions with a double
positive charge
- Ti+ (g) --> Ti2+ (g) + e-
- Ti+ (g) --> Ti2+ (g) + e-
- X(g) --> X+ (g) + e-
- 1.The attraction of the nucleus (The more protons in the nucleus the
greater the attraction)
- 2. The distance of the electrons from the nucleus (The bigger the atom
the further the outer electrons are from the nucleus and the weaker the
attraction to the nucleus)
- 3. Shielding of the attraction of the nucleus (An electron in an outer shell is repelled by electrons in
complete inner shells, weakening the attraction of the nucleus)
- The second ionisation energy is the enthalpy change
when one mole of gaseous ions with a single positive
charge forms one mole of gaseous ions with a double
positive charge
- Emperical Formula: the simplest whole number ratio of atoms
of each element in a compound
- Covalent Bond: a shared pair of electrons
- Dative Covalent Bond: A covalent bond in which the shared pair of electrons are
provided by just one of the bonded atoms
- Electronegativity: The power of an atom to withdraw electron density from a
covalent bond
- Structural Isomerism: Compounds which have the same
molecular formula but a different structural
formula/displayed formula
- Cracking: A process used by the petroleum industry to produce shorter
alkanes and alkenes from longer alkanes
- Ideal Gas Equation: pV=nRT
- No. of moles = Mass/Mr
- Concentration = No. of moles/Volume
- Atom Economy = (mass desired product /
mass all reactants)x100
- % Yield = (Actual yield / Theoretical yield)x100
- Mass Spectrometry:
- Step 1) Ionisation •Sample is
dissolved in a polar solvent •A
high voltage is applied to
sample •The particles lose an
electron ( or more) •Forming
positive ions with different
charges E.g. Ti Ti+ + e–
- Step 2) Acceleration •Positive ions are
accelerated by an electric field •To a
constant kinetic energy
- Step 3) Deflection •The positive ions with smaller m/z values will
have the same kinetic energy as those with larger m/z and will
move faster. •The heavier particles take longer to move through
the drift area. •The ions are distinguished by different flight times
- Step 4) Detection •The ions reach the detector and generate a small current,
which is fed to a computer for analysis. The current is produced by electrons
transferring from the detector to the positive ions. The size of the current is
proportional to the abundance of the species
- Step 4) Detection •The ions reach the detector and generate a small current,
which is fed to a computer for analysis. The current is produced by electrons
transferring from the detector to the positive ions. The size of the current is
proportional to the abundance of the species
- Step 3) Deflection •The positive ions with smaller m/z values will
have the same kinetic energy as those with larger m/z and will
move faster. •The heavier particles take longer to move through
the drift area. •The ions are distinguished by different flight times
- Step 2) Acceleration •Positive ions are
accelerated by an electric field •To a
constant kinetic energy
- Step 1) Ionisation •Sample is
dissolved in a polar solvent •A
high voltage is applied to
sample •The particles lose an
electron ( or more) •Forming
positive ions with different
charges E.g. Ti Ti+ + e–
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