Light as a particle
· apply the quantised energy of photons: E=hf=hc/wavelength
· analyse the photoelectric effect with reference to:
- evidence for the particle-like nature of light
- experimental data in the form of graphs of photocurrent versus electrode potential, and of kinetic energy of electrons versus frequency
- kinetic energy of emitted photoelectrons: KEmax=hf-W, using energy units of joule and electron-volt
- effects of intensity of incident irradiation on the emission of photoelectrons
· describe the limitation of the wave model of light in explaining experimental results related to the photoelectric effect
Matter as particles or waves
· interpret electron diffraction patterns as evidence for the wave-like nature of matter
· distinguish between the diffraction patterns produced by photons and electrons
· calculate the de Broglie wavelength of matter: wavelength=h/p
Similarities between light and matter
· discuss the importance of the idea of quantisation in the development of knowledge about light and in explaining the nature of atoms
· compare the momentum of photons and of matter of the same wavelength including calculations using: p=h/wavelength
· explain the production of atomic absorption and emission line spectra, including those from metal vapour lamps
· interpret spectra and calculate the energy of absorbed or emitted photons: E = hf
· analyse the emission or absorption of a photon by an atom in terms of a change in the electron energy state of the atom, with the difference in the states’ energies being equal to the photon energy: E = hf=hc/wavelength
· describe the quantised states of the atom with reference to electrons forming standing waves, and explain this as evidence for the dual nature of matter
· interpret the single photon and the electron double slit experiment as evidence for the dual nature of light and matter
· apply the quantised energy of photons: E=hf=hc/wavelength
· analyse the photoelectric effect with reference to:
- evidence for the particle-like nature of light
- experimental data in the form of graphs of photocurrent versus electrode potential, and of kinetic energy of electrons versus frequency
- kinetic energy of emitted photoelectrons: KEmax=hf-W, using energy units of joule and electron-volt
- effects of intensity of incident irradiation on the emission of photoelectrons
· describe the limitation of the wave model of light in explaining experimental results related to the photoelectric effect
Matter as particles or waves
· interpret electron diffraction patterns as evidence for the wave-like nature of matter
· distinguish between the diffraction patterns produced by photons and electrons
· calculate the de Broglie wavelength of matter: wavelength=h/p
Similarities between light and matter
· discuss the importance of the idea of quantisation in the development of knowledge about light and in explaining the nature of atoms
· compare the momentum of photons and of matter of the same wavelength including calculations using: p=h/wavelength
· explain the production of atomic absorption and emission line spectra, including those from metal vapour lamps
· interpret spectra and calculate the energy of absorbed or emitted photons: E = hf
· analyse the emission or absorption of a photon by an atom in terms of a change in the electron energy state of the atom, with the difference in the states’ energies being equal to the photon energy: E = hf=hc/wavelength
· describe the quantised states of the atom with reference to electrons forming standing waves, and explain this as evidence for the dual nature of matter
· interpret the single photon and the electron double slit experiment as evidence for the dual nature of light and matter
