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25 Cards in this Set
- Front
- Back
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What is an isotope?
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An atom of the same element but with a different number of neutrons.
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What is Relative atomic mass?
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The Average mass of an atom compared to the mass of a carbon-12 atom( compared to 1/12 of a carbon-12 atom)
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What are the five staged is mass spectrometry?
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Vapourisation
Ionisation Acceleration Deflection Detection |
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Vapourisation
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The sample is heated to turn it into a gas.
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Ionisation
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The gas is passed under an electron gun where an electron will be knocked off the atom leaving it with a 1+ charge.
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Acceleration
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-vely charged plates are used to direct the +ve ions and increase there speed.
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Deflection
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An electromagnet created a magnetic field to deflect the ions.
Heavy= small deflection Light= large deflection |
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Detection
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The magnetic field is increased to ions hit the detector in order of increasing mass.
The ions hit the detector, gain and electron and induce a current proportional to the abundance of that ion. |
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What is mass spectrometry used for?
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To identify the different isotopes that make up an element. Different isotopes are detected separately because they have different masses.
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What is the order of the sub levels in electron shells?
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S
P D F |
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S can hold...?
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2 electrons.
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P can hold...?
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2 Electrons each but always come in groups of three in an energy level therefore...
6 in total. |
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D can hold...?
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2 electrons each but always come in groups of five in an energy level so therefore...
10 in total. |
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Which is easiest to fill 3D or 4S?
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4S
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Three rules for allocating electrons to atomic orbitals?
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- Atomic orbitals with lower energy are filled first
- Atomic orbitals of the same energy fill singly before pairing starts - No atomic orbital can hold more that 2 electrons |
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Ionisation
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The process by which atoms lose or gain electrons.
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The first ionisation energy is...
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the energy needed to remove one electron from each atom in one mole of gaseous atoms to produce one mole of gaseous 1+ions.
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What are the three factors affection ionisation energy?
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Nuclear charge
Distance from nucleus Shielding |
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Explain Nuclear charge in terms of affecting ionisation energy?
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The more protons in the nucleus the stronger the attraction for the electrons therefore the harder to lose an electron.
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Explain distance from the nucleus in terms of affecting ionisation energy?
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Attraction falls with distance. The further away an atom from the nucleus the easier it is to lose.
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Explain shielding in terms of affecting ionisation energy?
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As the number of electrons between the outer electrons and the nucleus increases the attraction between the outer electrons and the nucleus decreases.
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A high ionisation energy means...?
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there is a high attraction between the nucleus and the electron.
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Down a group the ionisation energy...?
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decreases. (ie electrons are easier to remove)
This is because the atoms get bigger meaning that there is a farther distance between the electrons and the nucleus. also there are more electrons down a group so outer electrons are more shielded. |
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Across a period ionisation energy...?
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increases. (ie electrons are harder to remove)
This is because the number of protons is increasing therefore there is stronger nuclear attraction between the nucleus and the electrons. |
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Explain the drops between groups 2 and 3, and groups 5 and 6?
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Groups 2 and 3
Aluminium's outer electron shell is a 3P orbital which means it is further from the nucleus and there is also extra shielding meaning it is easier to lose. Groups 5 and 6 Sulphur has 2 electrons in its outer orbital whereas phosphors has one. It is easier for sulphur to lose its electron because of the repulsion between the two. |
