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Quantum physics
Uni of Notts, fundamentals of inorganic & organic chemistry, first year
| Term | Definition |
|---|---|
| Electromagnetic (EM) radiation | Wide variety of travelling waves of packets of energy called photons which vary in intensity & frequency |
| Relationship between wavelength & frequency | Since EM radiation is made of photons which travel at the speed of light (3 x 10^18), the wavelength times the frequency will always equal the speed of light since they're inversely proportional |
| Formula showing relationship between wavelength & frequency | λv = c λ = wavelength v = frequency c = speed of light |
| Why metals in the vapour phase show certain colours: Electron excitation | In the vapour phase metal ions are isolated & no longer delocalised which allows them to absorb external energy sources & enter a higher energy excited state |
| Why metals in the vapour phase show certain colours: Electron relaxation | Metal atoms are unstable in an excited state so the electrons radiate stored energy as visible light corresponding to the difference in energy between the excited & ground state |
| What Planck meant by "radiation is quantised" | Radiation is only emitted or absorbed in packets of energy called quanta which can't be split. Radiation can only have energy values in multiples of quanta & no intermediate values |
| Energy of a quantum reaction | E = hv E = energy of a quantum h = Planck's constant (6.63 x 10^-34J) v = frequency of quantum |
| Photoelectric effect | When electrons are ejected from a surface (usually metal) when excited by a high enough EM frequency regardless of intensity & excess energy is converted into kinetic energy |
| Photoelectric experiment | Electrons are ejected from the irradiated surface which are then detected by a wire anode which registers a current proportional to the kinetic energy of the electron |
| de Broglie's theory | If light is something that everyone knows is a wave that behaves like particles, then electrons can be something that everyone knows is a particle but behaves like waves |
| The de Broglie relationship | λ = h/p λ = wavelength p = momentum of particles h = Planck's constant (6.63 x 10^-34J) |
| Electron position & momentum | Electrons have positions in space relative to dimensional coordinates x, y, & z but they're always moving with a momentum (p) parallel to each axis which can be shown as px, py, & pz |
| Heisenberg's uncertainty principle | The more accurately we know either the position or the momentum of an electron, the less accurately we can know the other. This is a physical property applying to all matter as small as a Planck constant |
| Heisenberg uncertainty equation | Δx.Δpx > h/4π Δx = Change of position of electron Δpx = Change of momentum of electron h = Planck's constant (6.63 x 10^-34J) π = pi (3.14...) |
Created by:
Beech47
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