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8 Cards in this Set
- Front
- Back
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Define Atomic number, Mass number, RAM, RIM and RMM |
Atomic number is the number of protons. Mass number is the number of nucleons (protons and neutrons). RAM is the average mass of an atom of an element compared to 1/12th the mass of a Carbon-12 atom. RIM is the average mass of an atom of an isotope... RMM is the average mass of a molecule compared to... |
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Describe the 5 stages of ionisation? |
A substance is heated by an electric heater so it is vapourised. It then enters the ionisation chamber where high energy electrons bombard the atoms at high speed, knocking off electrons and forming cations. These cations are then accelerated by an electric field and attracted to a negatively charged plate which forms a beam of ions. Ions with a low m/z value are deflected more by the magnetic field which deflects ions towards the detector. The detector is a metal plate. The greater the current produced the more abundant. |
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How do you work out the RAM of an element and the RMM of a molecule? |
For the RAM, you find the sum of the abundance multiplied by the mass number, and average that. For the RMM, fragmentation occurs. The RMM will be the furthest peak to the right with the largest m/z value |
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What rules are there to remember when working out electronic configuration? |
The s sublevel is filled before the d sublevel from 3d onwards. Copper and Chromium each donate one electron to the 3d sublevel from the 4s sublevel so they either have 5 or 10 (more stable). Transition metals lose an electron from their 4s sublevel before their 3d sublevel when forming ions. |
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Why do isotopes have similar chemical properties? |
Isotopes have the same number of electrons and the same electronic configuration. Electrons determine chemical properties so the chemical properties are the same. |
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What is first ionisation energy? |
The energy required to remove 1 mole of electrons from 1 mole of gaseous atoms to form 1 mole of ions with a single positive charge. Lower ionisation energy means it is easier to form an ion. |
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What is the first ionisation energy equation? |
Mg -> Mg+ + e- |
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Why do successive ionisation energies increase? |
The more electrons removed, the fewer remain. There is less repulsion between electrons and more stable, so harder to remove. |
