(1) atomic structure Flashcards
Dalton’s model
- 19th cent.
- Atoms = solid spheres
- Different spheres made up different elements
Thompson’s model
- 1897
- Plum pudding
- Electrons embedded in positive mass
Rutherford’s model
- 1909
- Gold foil experiment
- Tiny + nucleus (most alpha particles went straight through)
- Cloud of - electrons (some alpha particles deflected backwards)
- Most of atom is empty space
Bohr’s model
- Electrons in fixed shells
- Shells have fixed energy
- EMR is emitted/absorbed when electron jumps between shells (has a fixed frequency)
Modern model
- Subshells
Relative Atomic Mass
-The average mass of an atom of an element compared to 1/12th the mass of a carbon 12 atom
Relative isotopic Mass
-The mass of an atom of an isotope of an element compared to 1/12th the mass of a carbon 12 atom
Ar formula
Sum of the product of isotopic masses and relative abundance / 100
Relative Molecular Mass
-The average mass of a molecule compared to 1/12th the mass of a carbon 12 atom
Relative Formula Mass
-Average mass of a formula unit compared to 1/12th the mass of a carbon 12 atom
Electrospray ionisation
- Sample dissolved in polar solvent (water/ethanol)
- Pushed through nozzle at high pressure
- High voltage applied
- Particles gain H+ ion
-(m/z value 1 unit greater on spectrum due to proton)
X(g) + H+(g) -> XH+(g)
Electron impact ionization
- Sampled is vaporized
- High energy electrons fired with electron gun
- Knocks 1* electron off
- *Sometimes more
X(g)-> X+(g) + e-
Acceleration stage
- Ions accelerated by electric field
- All ions have same kinetic energy
- Lighter ions accelerate faster than heavier ones
Ion drift stage
- No electric field
- Lighter ions drift faster
Detection stage
- Lighter ions reach detector first
- Detector records the current created when ion arrives and time taken to travel through spectrometer
- Mass/charge value calculated