- Chapter 1: Chemical Foundations
- Chapter 10: Liquids and Solids
- Chapter 11: Properties of Solutions
- Chapter 12: Chemical Kinetics
- Chapter 13: Chemical Equilibrium
- Chapter 14: Acids and Bases
- Chapter 15: Applications of Aqueous Equilibria
- Chapter 16: Spontaneity, Entropy, and Free Energy
- Chapter 17: Electrochemistry
- Chapter 18: The Nucleus: A Chemists View
- Chapter 19: The Representative Elements: Groups 1A Through 4A
- Chapter 2: Atoms, Molecules, and Ions
- Chapter 20: The Representative Elements: Groups 5A Through 8A
- Chapter 21: Transition Metals and Coordination Chemistry
- Chapter 22: Organic and Biological Molecules
- Chapter 3: Stoichiometry
- Chapter 4: Types of Chemical Reactions and Solution Stoichiometry
- Chapter 5: Gases
- Chapter 6: Thermochemistry
- Chapter 7: Atomic Structure and Periodicity
- Chapter 8: Bonding: General Concepts
- Chapter 9: Covalent Bonding: Orbitals
Chemistry 7th Edition - Solutions by Chapter
Full solutions for Chemistry | 7th Edition
A compound that reacts with a diene in a Diels-Alder reaction.
In electrocyclicreactions, a type of rotation in which the orbitalsbeing used to form the new s bond must rotate in opposite directions (one rotates clockwise while the other rotates counterclockwise).
A reaction that occurs between chlorobenzene and either NaOH (at high temperature) or NaNH2.
A vacancy in the valence band of a semiconductor, created by doping. (Section 12.7)
Thedetermining factor by which ions are separatedfrom each other in mass spectrometry.
A combination of two or more substances in which each substance retains its own chemical identity. (Section 1.2)
nucleophilic acyl substitution
A reaction in which a nucleophile attacks a carboxylic acid derivative.
An allowed energy state of an electron in the quantum mechanical model of the atom; the term orbital is also used to describe the spatial distribution of the electron. An orbital is defined by the values of three quantum numbers: n, l, and ml (Section 6.5)
Part per million (ppm)
Units used on NMR spectra to record chemical shift relative to the TMS standard.
Pauli exclusion principle
A rule stating that no two electrons in an atom may have the same four quantum numbers (n, l, ml, and ms). As a reflection of this principle, there can be no more than two electrons in any one atomic orbital. (Section 6.7)
A conformation in which a hydrogen atom and a leaving group are approximately coplanar.
plane of symmetry
A plane that bisects a compound into two halves that are mirror images of each other.
A polymer that can be molded when hot and retains its shape when cooled
The determination of the amount of a given substance that is present in a sample. (Section 17.7)
The gain of electrons. Alternatively, either the gain of hydrogen, loss of oxygen, or both
The difference in energy between a resonance hybrid and the most stable of its hypothetical contributing structures in which electrons are localized on particular atoms and in particular bonds.
Secondary (2°) amine
An amine in which nitrogen is bonded to two carbons and one hydrogen
The preferred metric units for use in science. (Section 1.4)
A homogeneous alloy, where two or more elements are distributed randomly and uniformly throughout the solid. (Section 12.3)
Constitutional isomers in equilibrium with each other that differ in the location of a hydrogen atom and a double bond relative to a heteroatom, most commonly O, N, or S.
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