- 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 reaction involving the addition of two groups to a conjugated p system in which one group is installed at the C1 position and the other group is installed at the C2 position.
Compounds of carbon and hydrogen containing only carbon–carbon single bonds. (Sections 2.9 and 24.2)
An array of closely spaced molecular orbitals occupying a discrete range of energy. (Section 12.4)
The heating of an ore to bring about its decomposition and the elimination of a volatile product. For example, a carbonate ore might be calcined to drive off CO2. (Section 23.2)
Compounds composed entirely of chlorine, fluorine, and carbon. (Section 18.3)
Reduction of the C"O group of an aldehyde or ketone to a CH2 group using Zn(Hg) and HCl
The most efficient arrangements for packing atoms, molecules, or ions in a crystal. (11.4)
A property of a solvent (vapor-pressure lowering, freezing-point lowering, boiling-point elevation, osmotic pressure) that depends on the total concentration of solute particles present. (Section 13.5)
The energy change that occurs when an electron is added to a gaseous atom or ion. (Section 7.5)
A derivative of a carboxylic acid in which H of the carboxyl group is replaced by a carbon.
For electromagnetic radiation, the number of wavelengths that pass a particular point in space per unit time.
An electrophilic aromatic substitution in which a hydrogen of an aromatic ring is replaced by an alkyl or acyl group.
A form of isomerism in which compounds with the same type and number of atoms and the same chemical bonds have different spatial arrangements of these atoms and bonds. (Sections 23.4 and 24.4)
For water, Kw is the product of the aquated hydrogen ion and hydroxide ion concentrations: 3H+43OH-4 = Kw = 1.0 * 10-14 at 25 °C. (Section 16.3)
The energy required to separate completely the ions in an ionic solid. (Section 8.2)
The difference between the mass of a nucleus and the total masses of the individual nucleons that it contains. (Section 21.6)
The row of elements that lie in a horizontal row in the periodic table. (Section 2.5)
A constant of proportionality between the reaction rate and the concentrations of reactants that appear in the rate law. (Section 14.3)
The SI unit for magnetic fi eld strength.
Valence Bond Theory
A model of bonding that places electron pairs between adjacent atoms to create bonds.