- Chapter 1: Introduction to Chemistry
- Chapter 10: The Mole
- Chapter 11: Stoichiometry
- Chapter 12: States of Matter
- Chapter 13: Gases
- Chapter 14: Mixtures and Solutions
- Chapter 15: Energy and Chemical Change
- Chapter 16: Reaction Rates
- Chapter 17: Chemical Equilibrium
- Chapter 18: Acids and Bases
- Chapter 19: Redox Reactions
- Chapter 2: Analyzing Data
- Chapter 20: Electrochemistry
- Chapter 21: Hydrocarbons
- Chapter 22: Substituted Hydrocarbons and Their Reactions
- Chapter 23: The Chemistry of Life
- Chapter 24: Nuclear Chemistry
- Chapter 3: Matter Properties and Changes
- Chapter 4: The Structure of the Atom
- Chapter 5: Electrons in Atoms
- Chapter 6: The Periodic Table and Periodic Law
- Chapter 7: Ionic Compounds and Metals
- Chapter 8: Covalent Bonding
- Chapter 9: Chemical Reactions
Chemistry: Matter & Change 1st Edition - Solutions by Chapter
Full solutions for Chemistry: Matter & Change | 1st Edition
Compounds containing a nitrogen atom that is connected to one, two, or three alkyl or aryl groups.
A conformation of cyclohexane in which all bond angles are fairly close to 109.5° and many hydrogen atoms are eclipsing each other.
The temperature at which the vapor pressure of a liquid is equal to the external atmospheric pressure. (11.8)
The generally larger formation constants for polydentate ligands as compared with the corresponding monodentate ligands. (Section 23.3)
An equation that uses chemical symbols to show what happens during a chemical reaction. (3.7)
The quantity of solute present in a given quantity of solvent or solution. (Section 4.5)
For alkenes, a stereodescriptorthat indicates that the two priority groups are on opposite sides of the p bond.
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)
heat of combustion
The heat given off during a reaction in which an alkane reacts with oxygen to produce CO2 and water.
Cleavage of a single bond by H2, most commonly accomplished by treating a compound with H2 in the presence of a transition metal catalyst.
A compound with the structure R!C#C!R, where each R group is not a hydrogen atom.
inversion of configuration
During a reaction, when the configuration of a chirality center is changed.
Compounds formed when hydrogen reacts with nonmetals and metalloids. (Section 22.2)
Nonpolar covalent bond
A covalent bond between atoms whose difference in electronegativity is less than approximately 0.5.
From the Greek meaning nucleus-loving. Any species that can donate a pair of electrons to form a new covalent bond; alternatively, a Lewis base
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)
Polypeptide chains comprised of more than 40 or 50 amino acids.
A starting substance in a chemical reaction; it appears to the left of the arrow in a chemical equation. (Section 3.1)
A compound containing an !SH (sulfhydryl) group bonded to an sp3 -hybridized carbon.
Groups that weakly activate an aromatic ring toward electrophilic aromatic substitution, thereby enhancing the rate of the reaction.