- 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
An addition reaction in which two groups are installed on opposite sides of a p bond.
See beta rays.
Cis, trans isomers
Stereoisomers that have the same connectivity but a different arrangement of their atoms in space as a result of the presence of either a ring or a carboncarbon double bond.
Addition of a nucleophile to the b-carbon of an a,b-unsaturated carbonyl compound. (Section 20.2A) Addition to carbons 1 and 4 of a conjugated diene.
A solid that possesses rigid and long-range order; its atoms, molecules, or ions occupy specific positions. (11.4)
A cyclohexene resulting from the cycloaddition reaction of a diene and a dienophile.
The escape of a gas through an orifice or hole. (Section 10.8)
Coal, oil, and natural gas, which are presently our major sources of energy. (Section 5.8)
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)
An equation of state for gases that embodies Boyle’s law, Charles’s law, and Avogadro’s hypothesis in the form PV = nRT. (Section 10.4)
Infrared (IR) spectroscopy
A spectroscopic technique in which a compound is irradiated with infrared radiation, absorption of which causes covalent bonds to change from a lower vibration state to a higher one. Infrared spectroscopy is particularly valuable for determining the kinds of functional groups present in a molecule.
law of constant composition
A law that states that the elemental composition of a pure compound is always the same, regardless of its source; also called the law of definite proportions. (Section 1.2)
The sum of the number of protons and neutrons in the nucleus of a particular atom. (Section 2.3)
Melt transition (Tm)
The temperature at which crystalline regions of a polymer melt.
The state of a system at a particular instant; one of many possible energetically equivalent ways to arrange the components of a system to achieve a particular state. (Section 19.3)
A solid, inorganic substance occurring in nature, such as calcium carbonate, which occurs as calcite. (Section 23.1)
net ionic equation
A chemical equation for a solution reaction in which soluble strong electrolytes are written as ions and spectator ions are omitted. (Section 4.2)
An electrically charged group of two or more atoms. (Section 2.7)
Lipids that are based on a tetracyclic ring system involving three six-membered rings and one five-membered ring. Cholesterol is an example.
Compounds containing a mercapto group (SH).