Atoms with same number of protons and different number of neutrons.
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Define: Relative Isotopic Mass
Mass of one atom of an isotope compared to 1/12th of mass of one atom of carbon-12.
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Define: Relative Atomic Mass
The average mass of one atom compared to 1/12th of mass of one atom of carbon-12.
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Define: Relative Molecular Mass
Average mass of a molecule compared to 1/12th of mass of one atom of carbon-12.
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Equation: Relative Atomic Mass (Ar)
Isotopic mass x abundance / 100 or Isotopic mass x relative abundance / total abundance.
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What does Mass spectrometer measure for each Isotope?
Mass/charge ratio and an abundance.
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What are the 4 stages is Mass spectrometry?
Vaporization , Acceleration, Deflection and Detection.
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Vapourisation
Chemicals injected into the instrument knock electrons off and form ions.
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Acceleration
Positive Ions are accelerated into the instrument.
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Deflection
Positive ions are deflected with a magnetic field. Lighter ions are deflected more than heavier ions with same charge.
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Detection
Charged ions are detected as a tiny current and signal is fed into a computer.
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Define: First Ionisation Energy
The energy needed to remove one electron from each atom in one mole of gaseous atom to form one mole of gaseous 1+ ion.
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Define: Second Ionisation Energy
Energy needed to remove 1 electron from each ion in 1 mole of gaseous 1+ ions to form 1 mole of gaseous 2+ ions.
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What are the Factors affecting Ionisation Energy?
Nucleus charge, Distance from nucleus, Shielding.
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How does attraction from nucleus affect ionisation energy?
There are more protons equating to atom having higher nuclear charge therefore there is a greater attraction.
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How does sheilding of attraction of the nucleus affect ionisation energy?
An electron in outermost shell is repelled by electrons in complete inner shells, weakening attraction from nucleus.
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How does distance of electrons from nucleus affect ionisation energy?
Bigger the atom the further the outermost shell (valence shell) are from nucleus therefore weaker the attraction.
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What are electron shells made up of?
Sub-shells and Orbitals.
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What are numbers given to each energy level called?
Principal Quantum Number.
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Name the first 4 sub-shells.
s , p , d , f
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How many electrons are in each orbital
2 electrons of oppositely spin.
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why does 4s become before 3d?
4s has a lower state of energy than the 3d sub-shell so 4s fills up first.
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Define: atomic radius
Atomic radius refers size of atoms in an element by looking at the distance from the center of the nucleus to the boundary of the surrounding.
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What is the relationship between atomic radius and the periodic table?
Atomic radii decreases as you move from left to right as the increased number of protons create more positive charge attraction for electrons which are in same shell with similar shielding.
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Other cards in this set
Card 2
Front
Mass of one atom of an isotope compared to 1/12th of mass of one atom of carbon-12.
Back
Define: Relative Isotopic Mass
Card 3
Front
The average mass of one atom compared to 1/12th of mass of one atom of carbon-12.
Back
Card 4
Front
Average mass of a molecule compared to 1/12th of mass of one atom of carbon-12.
Back
Card 5
Front
Isotopic mass x abundance / 100 or Isotopic mass x relative abundance / total abundance.
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