1 of 34 © Boardworks Ltd 2009 2 of 34 © Boardworks Ltd 2009 Photon energy In 1905, Albert Einstein published a paper that described his photon theory of light. This explained experimental evidence, such as the photoelectric effect, that did not fit with the classical wave model of light. Einstein proposed that, although light exhibited wave-like properties, it travelled in particles called photons. He explained that photons contain discrete ‘energy packets’ called quanta, and that the energy of an individual quantum depends on the frequency of the light. 3 of 34 © Boardworks Ltd 2009 Thermal radiation All objects with a temperature above absolute zero emit thermal radiation. Why do objects emit this radiation? All charged particles emit radiation when they accelerate. If an object has a temperature above absolute zero, then its electrons and protons will vibrate and emit radiation. Absolute zero is the temperature (-273°C, 0K) at which particles theoretically lose all their energy and stop vibrating. 4 of 34 © Boardworks Ltd 2009 Incandescence 5 of 34 © Boardworks Ltd 2009 The incandescent light bulb How could you use incandescence to explain how a conventional light bulb works? 1. A current flows through the filament. 2. The filament heats up. 3. The thermal emission of the filament moves into the visible spectrum. Why is the incandescent light bulb not an efficient device for producing light? The filament’s emission spectrum remains mostly in the infrared, even when it is at its hottest. Most of the bulb’s energy input is therefore wasted as heat. 6 of 34 © Boardworks Ltd 2009 Emission spectra 7 of 34 © Boardworks Ltd 2009 Explaining the origin of line spectra 8 of 34 © Boardworks Ltd 2009 Dropping energy levels Each possible drop between atomic energy levels in an atom corresponds to the emission of one specific frequency of photon. n=4 n=3 n=2 n=1 This results in one line in an element’s emission spectrum. Three lines in hydrogen’s spectrum are shown here, along with the energy jumps that they correspond to. ground hydrogen 9 of 34 © Boardworks Ltd 2009 The fluorescent lamp The incandescent light bulb is an inefficient device for producing light (typically 1–2%). The fluorescent lamp is an alternative, with an efficiency of around 10%. Fluorescent lamps use electricity to cause excitation of mercury vapour. When the mercury atoms relax, they emit ultraviolet photons. Ultraviolet light is not visible, but can be converted into visible light using a phosphor. This coats the inside of the bulb and fluoresces when bombarded with the ultraviolet light from the mercury vapour. 10 of 34 © Boardworks Ltd 2009 Understanding thermal emission 11 of 34 © Boardworks Ltd 2009 12 of 34 © Boardworks Ltd 2009 Quantised absorption Just as an electron can drop between energy levels in an atom, releasing a single photon, it can also jump up one or more energy levels if it absorbs a photon of the right energy. Only a single photon of the relevant energy can cause this. It is not possible for an electron to ‘store up’ energy from smaller quanta until it has enough to make the jump. One result of this is that shining a continuous spectrum of light at a transparent material leads to a few discrete frequencies being absorbed, while the rest are transmitted. This forms an absorption spectrum. 13 of 34 H emission spectrum H absorption spectrum © Boardworks Ltd 2009 Analysing light from a source 14 of 34 © Boardworks Ltd 2009 Energy of photons in light 15 of 34 © Boardworks Ltd 2009 The electronvolt A joule (J) is a large unit of energy when dealing with tiny atoms. Scientists often use an alternative unit for small amounts of energy, called an electronvolt (eV). An electronvolt is equal to the amount of energy transferred to a single electron if it is accelerated through a potential difference of 1 V: 1 eV = 1.6 × 10-19 J How many electronvolts to one joule? 1 J = 1/(1.6 × 10-19) eV = 6.25 × 1018 eV Use these two conversion rates to change between the two. Be careful to use joules in calculations with other SI units. 16 of 34 © Boardworks Ltd 2009 Wave speed, wavelength and frequency The speed, wavelength and frequency of a wave are related by the following equation: wave speed = frequency × wavelength c = fλ What is the photon energy, in electronvolts, of red light of wavelength 685 nm? E = hf = hc/λ = 6.63 × 10-34 × 3 × 108 / (685 × 10-9) = 2.9 × 10-19 J = 2.9 × 10-19 × 6.25 × 1018 eV = 1.8 eV 17 of 34 © Boardworks Ltd 2009 Wave and photon calculations 18 of 34 © Boardworks Ltd 2009 Wavelength of emitted radiation Given a set of values for atomic energy levels in a particular element, it is possible to calculate the wavelengths of radiation it can emit or absorb. 1 2 3 4 5 6 The difference between two -0.85 eV energy levels gives the -1.5 eV energy of the photon corresponding to that jump, and this can be used to find -3.4 eV frequency and wavelength: hf = E1 – E2 hc/λ = E1 – E2 -13.6 eV What wavelengths of light are emitted in transitions 1–6? 19 of 34 © Boardworks Ltd 2009 20 of 34 © Boardworks Ltd 2009 The discovery of photoelectricity Photoelectricity was first discovered in 1887 by Heinrich Hertz during investigations into radio waves using a ‘spark gap’. Radio waves are produced when a high voltage is supplied across two electrodes causing a spark in the gap. Hertz found that if ultraviolet light was shone on the electrodes, the sparks were much stronger and thicker. 21 of 34 © Boardworks Ltd 2009 Measuring photoelectricity In the late 19th century, scientists used apparatus like this photocell to analyse and measure photoelectricity. photocell When light is shone on the cathode of the photocell, electrons are released. They are attracted to the anode, causing a current to flow. anode cathode vacuum 22 of 34 © Boardworks Ltd 2009 The gold leaf electroscope 23 of 34 © Boardworks Ltd 2009 Einstein’s photoelectric equation 24 of 34 © Boardworks Ltd 2009 The photoelectric effect equation 25 of 34 © Boardworks Ltd 2009 26 of 34 © Boardworks Ltd 2009 Wave–particle duality 27 of 34 © Boardworks Ltd 2009 Wave properties of particles In 1924, Lois De Broglie came up with a radical new way of looking at the relationship between waves and particles. He suggested that all particles could behave as waves. De Broglie deduced that a particle had a wavelength, and it was dependent on only one thing – the momentum of that particle: λ=h/p Three years later, this hypothesis was confirmed for electrons with the first observations of electron diffraction. 28 of 34 © Boardworks Ltd 2009 De Broglie wavelength calculations 29 of 34 © Boardworks Ltd 2009 Waves and particles 30 of 34 © Boardworks Ltd 2009 31 of 34 © Boardworks Ltd 2009 Glossary 32 of 34 © Boardworks Ltd 2009 What’s the keyword? 33 of 34 © Boardworks Ltd 2009 Multiple-choice quiz 34 of 34 © Boardworks Ltd 2009
