2.1.1: Atomic structure Flashcards
Ion
A charged particle; an atom that has gained/lost electrons.
Relative formula mass (not required)
The number of times the mean mass of one molecule of the molecular compound is heavier than 1/12.0, the mass of one atom of carbon-12.
Relative atomic mass (Aᵣ)
The weighted mean mass of an atom of an element relative to 1/12th the mass of an atom of carbon-12.
Relative isotopic mass
The mass of an isotope relative to 1/12th the mass of an atom of carbon-12.
Degenerate
having the same energy
Orbital
A probability region for an electron.
First ionisation energy
The energy required to remove 1 mole of electrons from 1 mole of gaseous atoms to form 1 mole of gaseous unipositive cations.
Positive ion
Cation
Negative ion
Anion
Electron relative mass
1/1840
Neutron relative mass
1
Proton relative mass
1
Uses of Mass Spectrometry
- Determination of (relative masses/abundances of) isotopes
- Determination of successive ionisation energies
- Determination of molecular structure
Mass Spectrometry steps
1) Vaporise sample
2) Ionise sample
3) Accelerate sample
4) Deflect through magnetic field according to mass/charge ratio
5) Detect the ions
Why is the ‘charge’ in the mass-charge ratio always the same?
- Electron gun knocks out outermost electron
- Therefore the charge is always +1
- So the mass determines the deflection