- Chapter 1: A Review of General Chemistry
- Chapter 10: Alkynes
- Chapter 11: Radical Reactions
- Chapter 12: Synthesis
- Chapter 13: Alcohols and Phenols
- Chapter 14: Ethers and Epoxides; Thiols and Sulfides
- Chapter 15: Infrared Spectroscopy and Mass Spectrometry
- Chapter 16: Nuclear Magnetic Resonance Spectroscopy
- Chapter 17: Conjugated Pi Systems and Pericyclic Reactions
- Chapter 18: Aromatic Compounds
- Chapter 19: Aromatic Substitution Reactions
- Chapter 2: Molecular Representations
- Chapter 20: Aldehydes and Ketones
- Chapter 21: Carboxylic Acids and Their Derivatives
- Chapter 22: Alpha Carbon Chemistry: Enols and Enolates
- Chapter 23: Amines
- Chapter 24: Carbohydrates
- Chapter 25: Amino Acids, Peptides, and Proteins
- Chapter 26: Lipids
- Chapter 27: Synthetic Polymers
- Chapter 3: Acids and Bases
- Chapter 4: Alkanes and Cycloalkanes
- Chapter 5: Stereoisomerism
- Chapter 6: Chemical Reactivity and Mechanisms
- Chapter 7: Substitution Reactions
- Chapter 8: Alkenes: Structure and Preparation via Elimination Reactions
- Chapter 9: Addition Reactions of Alkenes
Organic Chemistry, - Standalone Book 2nd Edition - Solutions by Chapter
Full solutions for Organic Chemistry, - Standalone Book | 2nd Edition
The Group 1A elements (Li, Na, K, Rb, Cs, and Fr). (2.4)
A bond to a chair conformation of cyclohexane that extends from the ring parallel to the imaginary axis through the center of the ring; a bond that lies roughly perpendicular to the equator of the ring.
An ion in which carbon has an unshared pair of electrons and bears a negative charge.
A substance that increases the rate of a chemical reaction without itself being consumed. (13.6)
A reaction in which a carbonyl group is completely reduced and replaced with two hydrogen atoms.
The mass of a substance divided by its volume. (1.6)
The use of electrolysis to reduce or refine metals. (Section 20.9)
heat of combustion
The heat given off during a reaction in which an alkane reacts with oxygen to produce CO2 and water.
When considering electrons in atomic orbitals, a rule that states that one electron is placed in each degenerate orbital first, before electrons are paired up.
A reaction with water. When a cation or anion reacts with water, it changes the pH. (Sections 16.9 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)
Numbers of protons and neutrons that result in very stable nuclei. (Section 21.2)
melt transition temperature (Tm)
The temperature at which the crystallineregions of a polymer become amorphous.
A solid, inorganic substance occurring in nature, such as calcium carbonate, which occurs as calcite. (Section 23.1)
Points in an atom at which the electron density is zero. For example, the node in a 2s orbital is a spherical surface. (Section 6.6)
An organic compound containing at least one halogen.
Addition of a reagent to a metal center causing it to add two substituents and to increase its oxidation state by two
parts per million (ppm)
The concentration of a solution in grams of solute per 106 (million) grams of solution; equals milligrams of solute per liter of solution for aqueous solutions. (Section 13.4)
A compound that is similar in structure to pyridine but contains one extra nitrogen atom at the 3 position.
A molecule, ion, or radical described as a composite of a number of contributing structures