- Chapter 1: Matter and Change
- Chapter 10: States of Matter
- Chapter 11: Gases
- Chapter 12: Solutions
- Chapter 13: Ions in Aqueous Solutions and Coiigative Properties
- Chapter 14: Acids and Bases
- Chapter 15: Acid-Base Titration andpH
- Chapter 16: Reaction Energy
- Chapter 17: Reaction Kinetics
- Chapter 18: Chemical Equilibrium
- Chapter 19: Oxidation-Reduction Reactions
- Chapter 2: Measurements and Calculations
- Chapter 20: Electrochemistry
- Chapter 21: Nuclear Chemistry
- Chapter 22: Organic Chemistry
- Chapter 23: Biological Chemistry
- Chapter 3: Atoms: The Building Blocks ofMatter
- Chapter 4: Arrangement of Electrons in Atoms
- Chapter 5: The Periodic Law
- Chapter 6: Chemical Bonding
- Chapter 7: Chemical Formulas and Chemical Compounds
- Chapter 8: Chemical Equations andReactions
- Chapter 9: Stoichiometry
Modern Chemistry 1st Edition - Solutions by Chapter
Full solutions for Modern Chemistry | 1st Edition
A group derived by removing a hydrogen from an alkane; given the symbol R!
A radical reaction that achieves installation of a bromine atom at an allylic position.
A high-energy intermediate formed during the elimination-addition reaction that occurs between chlorobenzene and either NaOH (at high temperature) or NaNH2.
A compound containing a Br group and a hydroxyl group (OH) on adjacent carbon atoms.
An intermediate containing a positively charged carbon atom.
A molecule containing an !S!S! group
electromotive force (emf)
A measure of the driving force, or electrical pressure, for the completion of an electrochemical reaction. Electromotive force is measured in volts: 1 V = 1 J>C. Also called the cell potential. (Section 20.4)
The region of an IR spectrum that contains signals resulting from the vibrational excitation of most single bonds (stretching and bending).
Liquids that do not dissolve in one another to a significant extent. (Section 13.3)
A substance added to a solution that changes color when the added solute has reacted with all the solute present in solution. The most common type of indicator is an acid–base indicator whose color changes as a function of pH. (Section 4.6)
The total energy possessed by a system. When a system undergoes a change, the change in internal energy, ?E, is defined as the heat, q, added to the system, plus the work, w, done on the system by its surroundings: ?E = q + w. (Section 5.2)
Any molecule or ion that can form a new covalent bond by accepting a pair of electrons.
The intermediateformed during oxymercuration.
A rule stating that the molecular ion of a compound with an odd number of nitrogen atoms has an odd m/z ratio; if zero or an even number of nitrogen atoms, the molecular ion has an even m/z ratio
In mass spectrometry,the ion that is generated when the compound is ionized.
A graphic representation of the equilibria among the solid, liquid, and gaseous phases of a substance as a function of temperature and pressure. (Section 11.6)
A polyester in which the carboxyl groups are derived from carbonic acid
A compound with a weak bond that undergoes homolytic bond cleavage with great ease, producing radicals that can initiate a radical chain process.
A covalent bond involving one electron pair. (Section 8.3)
A list of ligands arranged in order of their abilities to split the d-orbital energies (using the terminology of the crystal-field model). (Section 23.6)