19.10: Vibrational Raman spectra of diatomic molecules
19.11: The vibrations of polyatomic molecules
Box 19.1 Climate change
19.12: Vibration–rotation spectra
19.13: Vibrational Raman spectra of polyatomic molecules
CHECKLIST OF KEY IDEAS
TABLE OF KEY EQUATIONS
FURTHER INFORMATION 19.1 THE ROTATIONAL ENERGY LEVELS OF MOLECULES
QUESTIONS AND EXERCISES
Chapter 20: Spectroscopy: electronic transitions and photochemistry
Ultraviolet and visible spectra
20.1: Practical considerations
20.2: Absorption intensities
20.3: The Franck–Condon principle
20.4: Specific types of transitions
Box 20.1 Vision
Radiative and nonradiative decay
20.5: Fluorescence
20.6: Phosphorescence
20.7: Lasers
20.8: Applications of lasers in chemistry
Photoelectron spectroscopy
Photochemistry
20.9: Quantum yield
Box 20.2 Photosynthesis
20.10: Mechanisms of photochemical reactions
20.11: The kinetics of decay of excited states
20.12: Fluorescence quenching
CHECKLIST OF KEY IDEAS
TABLE OF KEY EQUATIONS
FURTHER INFORMATION 20.1 THE BEER–LAMBERT LAW
FURTHER INFORMATION 20.2 THE EINSTEIN TRANSITION PROBABILITIES
QUESTIONS AND EXERCISES
Chapter 21: Spectroscopy: magnetic resonance
Principles of magnetic resonance
21.1: Electrons and nuclei in magnetic fields
21.2: The technique
The information in NMR spectra
21.3: The chemical shift
Box 21.1 Magnetic resonance imaging
21.4: The fine structure
21.5: Spin relaxation
21.6: Proton decoupling
21.7: Conformational conversion and chemical exchange
21.8: The nuclear Overhauser effect
21.9: Two-dimensional NMR
21.10: Solid-state NMR
The information in EPR spectra
21.11: The g-value
21.12: Hyperfine structure
CHECKLIST OF KEY IDEAS
TABLE OF KEY EQUATIONS
QUESTIONS AND EXERCISES
Chapter 22: Statistical thermodynamics
The partition function
22.1: The Boltzmann distribution
22.2: The interpretation of the partition function
22.3: Examples of partition functions
22.4: The molecular partition function
Thermodynamic properties
22.5: The internal energy and the heat capacity
22.6: The entropy and the Gibbs energy
22.7: The statistical basis of chemical equilibrium
22.8: The calculation of the equilibrium constant
CHECKLIST OF KEY IDEAS
TABLE OF KEY EQUATIONS
FURTHER INFORMATION 22.1 THE CALCULATION OF PARTITION FUNCTIONS
FURTHER INFORMATION 22.2 THE EQUILIBRIUM CONSTANT FROM THE PARTITION FUNCTION
QUESTIONS AND EXERCISES
Appendix 1: Quantities and units
Appendix 2: Mathematical techniques
Basic procedures
A2.1 Algebraic equations and graphs
A2.3 Vectors
Calculus
A2.4 Differentiation
A2.6 Integration
A2.6 Differential equations
Appendix 3: Concepts of physics
Classical mechanics
A3.1 Energy
A3.2 Force
Electrostatics
A3.3 The Coulomb interaction
A3.4 The Coulomb potential
A3.5 Current, resistance, and Ohm’s law
Electromagnetic radiation
A3.6 The electromagnetic field
A3.7 Features of electromagnetic radiation
Appendix 4: Review of chemical principles
A4.1 Oxidation numbers
A4.2 The Lewis theory of covalent bonding
A4.3 The VSEPR model
Data section
Index
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[...]... International Union of Pure and Applied Chemistry and was a member of IUPAC’s Physical and Biophysical Chemistry Division Julio de Paula is Professor of Chemistry and Dean of the College of Arts & Sciences at Lewis & Clark College A native of Brazil, Professor de Paula received a B.A degree in chemistry from Rutgers, The State University of New Jersey, and a Ph.D in biophysical chemistry from Yale... concentration 0.10 Reaction stoichiometry CHECKLIST OF KEY IDEAS TABLE OF KEY EQUATIONS QUESTIONS AND EXERCISES Chemistry is the science of matter and the changes it can undergo The branch of the subject called physicalchemistry is concerned with the physical principles that underlie chemistryPhysicalchemistry seeks to account for the properties of matter in terms of fundamental concepts such as atoms, electrons,... framework for all other branches ofchemistry for inorganic chemistry, organic chemistry, biochemistry, geochemistry, and chemical engineering It also provides the basis of modern methods of analysis, the determination of structure, and the elucidation of the manner in which chemical reactions occur To do all this, it draws on two of the great foundations of modern physical science, thermodynamics... INTRODUCTION One of the roles of physical chemistry is to establish the link between the properties of bulk matter and the behaviour of the particles—atoms, ions, or molecules of which it is composed A physical chemist formulates a model, a simplified description, of each physical state and then shows how the state’s properties can be understood in terms of this model The existence of different states of matter... numerical value of the molar mass of an element or compound, respectively More precisely (but equivalently), the RAM of an element or the RMM of a compound is its average atomic or molecular mass relative to the mass of an atom of carbon-12 set equal to 12 The atomic weight (or RAM) of a natural sample of carbon is 12.01 and the molecular weight (or RMM) of water is 18.02 The molar mass of an element is... The molar mass of H2O is 18.02 g mol−1, so the mass of water produced is (2 × 1.38 mol) × (18.02 g mol−1) = 49.7 g Checklist of key ideas You should now be familiar with the following concepts 1 Physicalchemistry is the branch ofchemistry that establishes and develops the principles ofchemistry in terms of the underlying concepts of physics and the language of mathematics 2 The states of matter are... 100 cm3 of solution: 2.11 g Molar mass of B: 234.01 g mol−1 Density of solution in water: 1.01 g cm−3 Density of solution in benzene: 0.881 g cm−3 0.30 Calculate the mole fractions of the molecules of a mixture that contains 56 g of benzene and 120 g of methylbenzene (toluene) 0.31 A simple model of dry air at sea level is that it consists of 75.53 per cent (by mass) of nitrogen, 23.14 per cent of oxygen,... University of Keele Anthony Meijer, University of Sheffield Marcelo de Miranda, University of Leeds Damien Murphy, University of Cardiff Gavin Reid, University of Leeds Stephen Roser, University of Bath Karl Ryder, University of Leicester Sven Schroeder, University of Manchester David Steytler, University of East Anglia Michael Stockenhuber, University of Newcastle, New South Wales Svein Stolen, University of. .. measurement of the mass of its atoms and then multiplication of the mass of one atom by Avogadro’s constant (the number of atoms per mole) Care has to be taken to allow for the isotopic composition of an element, so we must use a suitably weighted mean of the masses of the isotopes present The values obtained in this way are printed on the periodic table inside the back cover The molar mass of a compound of. .. follows: 1 mol of specified particles is equal to the number of atoms in exactly 12 g of carbon-12 (12C) This number is determined experimentally by dividing 12 g by the mass of one atom of carbon-12 Because the mass of one carbon-12 atom is measured by using a mass spectrometer as 1.992 65 × 10−23 g, the number of atoms in exactly 12 g of carbon-12 is Number of atoms = total mass of sample mass of one atom