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U Rapid Review
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Thermodynamics is the study of heat and its transformations Kinetic energy is energy of motion, while potential energy is stored energy
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136 U Step 4 Review the Knowledge You Need to Score High
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The common units of energy are the joule, J, and the calorie, cal A calorimeter is used to measure the heat released or absorbed during a chemical or physical change Know how a calorimeter works The specific heat capacity is the amount of heat needed to change the temperature of 1 gram of a substance by 1 K, while the molar heat capacity is the heat capacity per mole The heat lost by the system in calorimetry is equal to the heat gained by the surroundings The specific heat (c) of a solid can be calculated by: (csolid msolid Tsolid) = cwater mwater Twater or by g = cm T The First Law of Thermodynamics states that the total energy of the universe is constant (Energy is neither created nor destroyed) The Second Law of Thermodynamics states that all spontaneous processes move in a way that increases the entropy (disorder) of the universe The enthalpy change, H, is equal to the heat lost or gained by the system under constant pressure conditions H values are associated with a specific reaction If that reaction is reversed, the sign of H changes If one has to use a multiplier on the reaction, it must also be applied to the H value The standard enthalpy of formation of a compound, Hf , is the enthalpy change when 1 mol of the substance is formed from its elements and all substances are in their standard states The standard enthalpy of formation of an element in its standard state is zero H rxn = Hf products Hf reactants Know how to apply this equation H rxn is usually negative for a spontaneous reaction S = S products S reactants Know how to apply this equation S is usually positive for a spontaneous reaction The Gibbs free energy is a thermodynamic quantity that relates the enthalpy and entropy, and is the best indicator for whether or not a reaction is spontaneous If G > 0 the reaction is not spontaneous; if G < 0, the reaction is spontaneous; and if G = 0, the reaction is at equilibrium G = Gf products Gf reactants Know how to apply this equation G = H rxn T S rxn Know how to apply this equation For a system not at equilibrium: G = G + RT ln Q = G + 2303 RT log Q Know how to apply this equation For a system at equilibrium: G = RT ln K = 2303 RT log K Know how to apply this equation to calculate equilibrium constants
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CHAPTER
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Spectroscopy, Light, and Electrons
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IN THIS CHAPTER Summary: In developing the model of the atom it was thought initially that all subatomic particles obeyed the laws of classical physics that is, they were tiny bits of matter behaving like macroscopic pieces of matter Later, however, it was discovered that this particle view of the atom could not explain many of the observations being made About this time the dual particle/wave model of matter began to gain favor It was discovered that in many cases, especially when dealing with the behavior of electrons, describing some of their behavior in terms of waves explained the observations much better Thus, the quantum mechanical model of the atom was born
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Keywords and Equations
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KEY IDEA
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Speed of light, c = 30 108 ms 1 E = energy n = frequency p = momentum v = velocity
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m = mass En =
E = hn
c = ln
2178 10 joule n2 Planck s constant, h = 663 10 34 Js
l = wavelength n = principal quantum number h = p = mv mv
The Nature of Light
Light is a part of the electromagnetic spectrum radiant energy composed of gamma rays, X-rays, ultraviolet light, visible light, etc Figure 101 shows the electromagnetic spectrum
137
138 U STEP 4 Review the Knowledge You Need to Score High
Wavelength (m) 10 11 10 9 10 7 10 5 10 3 10 1 101 103
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