- 7.2SE.1PE: Predicting Relative Sizes of Atomic RadiiReferring to the periodic ...
- 7.2SE.2PE: Predicting Relative Sizes of Atomic RadiiReferring to the periodic ...
Solutions for Chapter 7.2SE: Chemistry: The Central Science 13th Edition
Full solutions for Chemistry: The Central Science | 13th Edition
Compounds of carbon and hydrogen containing only carbon–carbon single bonds. (Sections 2.9 and 24.2)
Any reaction in which a new carbon-carbon bond to an alkyl group is formed.
A carbocation in which the positive charge is adjacent to a carbon-carbon double bond.
Radical scavengers that prevent autooxidation by preventing radical chain reactions from beginning.
The light absorbed by a substance (A) equals the product of its extinction coefficient 1e2, the path length through which the light passes (b), and the molar concentration of the substance (c): A = ebc. (Section 14.2)
The pressure at which a gas at its critical temperature is converted to a liquid state. (Section 11.4)
delocalized molecular orbitals.
Molecular orbitals that are not confined between two adjacent bonding atoms but actually extend over three or more atoms. (10.8)
A reaction characterized by the addition of two hydroxyl groups (OH) across an alkene.
A compound containing a nitrogen atom directly connected to a carboncarbon p bond.
Members of group 7A in the periodic table. (Section 7.8)
heat of sublimation
The enthalpy change, ?H, for vaporization of a solid. (Section 11.4)
Hückel criteria for aromaticity
To be aromatic, a monocyclic compound must have one 2p orbital on each atom of the ring, be planar or nearly so, and have (4n 1 2) p electrons in the cyclic arrangement of 2p orbitals
A substance that exhibits one or more partially ordered liquid phases above the melting point of the solid form. By contrast, in nonliquid crystalline substances the liquid phase that forms upon melting is completely unordered. (Section 11.7)
A reagent used for allylic bromination to avoid a competing reaction in which bromine adds across the p bond.
An industrial process used to make nitric acid from ammonia. The NH3 is catalytically oxidized by O2 to form NO; NO in air is oxidized to NO2; HNO3 is formed in a disproportionation reaction when NO2 dissolves in water. (Section 22.7)
A method of electron book-keeping in which all bonds are treated as if they were purely ionic.
Addition of a reagent to a metal center causing it to add two substituents and to increase its oxidation state by two
A solvent that is a hydrogen-bond donor. Common protic solvents are water, low-molecular-weight alcohols, and low-molecular weight carboxylic acids.
A series of intermediates and curved arrows that show howthe reaction occurs in terms of the motion of electrons.
A conformation in which a hydrogen atom and a leaving group are separated by a dihedral angle of exactly 0°.