- Chapter 1: THE PROPERTIES OF GASES
- Chapter 10: Atomic structure and atomic spectra
- Chapter 11: Molecular structure
- Chapter 12: Molecular symmetry
- Chapter 13: Molecular spectroscopy 1: rotational and vibrational spectra
- Chapter 14: Molecular spectroscopy 2: electronic transitions
- Chapter 15: Molecular spectroscopy 3: magnetic resonance
- Chapter 16: Statistical thermodynamics 1: the concepts
- Chapter 17: Statistical thermodynamics 2: applications
- Chapter 18: Molecular interactions
- Chapter 19: Materials 1: macromolecules and aggregates
- Chapter 2: The First Law
- Chapter 20: Materials 2: the solid state
- Chapter 21: Molecules in motion
- Chapter 22: The rates of chemical reactions
- Chapter 23: The kinetics of complex reactions
- Chapter 24: Molecular reaction dynamics
- Chapter 25: Processes at solid surfaces
- Chapter 3: The Second Law
- Chapter 4: Physical transformations of pure substances
- Chapter 5: Simple mixtures
- Chapter 6: Phase diagrams
- Chapter 7: Chemical equilibrium
- Chapter 8: Quantum theory: introduction and principles
- Chapter 9: Quantum theory: techniques and applications
Physical Chemistry 8th Edition - Solutions by Chapter
Full solutions for Physical Chemistry | 8th Edition
Theoretically the lowest attainable temperature. (5.3)
Rainwater that has become excessively acidic because of absorption of pollutant oxides, notably SO3, produced by human activities. (Section 18.2)
addition to p bond
One of the six kinds of arrow-pushing patterns used in drawing mechanisms for radical reactions. A radical adds to a p bond, destroying the p bond and generating a new radical.
In UV-Vis spectroscopy, an equation describing the relationship between molar absorptivity (e), absorbance (A), concentration (C), and path length (l): e = A (C Ž l)
A reaction (generally involving radicals) in which one chemical entity can ultimately cause a chemical transformation for thousands of molecules.
Chemical shift (d)
The shift in parts per million of an NMR signal relative to the signal of TMS
A voltaic cell containing the same electrolyte and the same electrode materials in both the anode and cathode compartments. The emf of the cell is derived from a difference in the concentrations of the same electrolyte solutions in the compartments. (Section 20.6)
A drawing style in which none of the bonds are drawn. Groups of atoms are clustered together when possible. For example, isopropanol has two CH3 groups, both of which are connected to the central carbon atom, shown like this: (CH3)2CHOH.
The highest temperature at which it is possible to convert the gaseous form of a substance to a liquid. The critical temperature increases with an increase in the magnitude of intermolecular forces. (Section 11.4)
The angle by which two groups are separated in a Newman projection.
A chemical formula that shows the kinds of atoms and their relative numbers in a substance in the smallest possible whole-number ratios. (Section 2.6)
Members of group 7A in the periodic table. (Section 7.8)
A polymer constructed from a single type of monomer.
A kinetic property measured by the rate at which a nucleophile causes nucleophilic substitution on a reference compound under a standardized set of experimental conditions.
A compound that rotates plane-polarized light.
A species formed when a neutral molecule loses one electron; it contains both an odd number of electrons and a positive charge.
The combination of a Michael addition followed by an aldol condensation to form a ring.
A substance dissolved in a solvent to form a solution; it is normally the component of a solution present in the smaller amount. (Section 4.1)
A compound that contains a sulfur atom that has double bonds with two oxygen atoms and is flanked on both sides by R groups.
An excellent leaving group (OTs). transition state (Sect. 6.6): A state through which a reaction passes. On an energy diagram, a transition state corresponds with a local maximum.