Atom Model Flashcards
Rutherford’s Model - Gold Foil Experiment
- The atom is a mostly empty space with a tiny, very dense (about 10-15) positively charged nucleus in the centre surrounded by tinier, much lighter negatively charged electrons
(No proton or neutron yet)
Rutherford’s Model - Gold Foil Experiment
- Nearly 100% of mass is contained within the nucleus
- Number of electrons equal number of positive charges in the nucleus
- An atoms nucleus in the order of 10-15m in diameter
- A atom is in the order of 10-10 m in diameter
- A nucleus is 100,000 smaller than the atom
Limitations of Rutherford Model
- Electrons dont spiral in
- Electrons can have any amount of enegry
Bohr Model
- Electrons move in circular orbits
- A number of allowable orbits of different radii exist for each atom, name n = 1,2,3 etc.
- An electron occupies the lowest energy orbit available
Bohr Model #2
- Electrons can ‘jump’ to higher obrits by absorbing quantised energy
- EM radiation is emitted when electrons ‘relax’ to a lower energy level
Hydrogen Energy Levels
Hydrogen has photons named according to what energy level they are relaxing to
Only 4 of these are in the visible spectrum, these are in the Balmer Series
Hydrogen Wavelengths
The Rydberg equation specifically calculates the wavelengths of photons being emitted from electron relaxations in hydrogens
1/wavelength = R(1/n (final energy)2 - 1/n(initial energy)2
De-Broglie’s Hypothesis
Matter as a Wave - supported electrons have wave like properties
If light can act like a wave and particle , the matter, which is made up of particles, might act like a wave
Einstein = mc2
Planck = E = hc/wavelength
wavelength = hc/mv
Light with Momentum
wavelength = h/p
Electron Orbitals
Flower pattern around electron with each petal distance being wavelength
equation is n(wavelength) = 2pir
