CHEM101 Lecture Notes - Lecture 3: Principal Quantum Number, Bohr Model, Matter Wave
Document Summary
Evidence that light and matter have both wave-like and particle-like properties. Understand how to use quantum numbers to describe the energy and position of electrons. Problems with the wave theory of light. Einstein used planck"s quantum theory to explain the photoelectric effect. Electrons ar eonly emitted from a metal"s surface if the incident light supplies enough energy to reach the threshold value for emission. High voltage to gas produces distinctive coloured striations of colour, depending on the gas. The emitted light can be passed through a prism, or spectrometer which creates a line spectrum unique to that gaseous element. 1885 balmer showed that the line spectrum for h2 fit a simple equation. Quantised energies of orbits and the electrons. Only certain orbits are allowed for the electron for energies. Lowest state closest to the nucleus is the ground state. Energy is emitted (as light) or absorbed to change states which corresponds to the difference to change.
