- 6.2.2: a. How many s bond orbitals are available for overlap with the vaca...
- 6.2.3: a. How many s bond orbitals are available for overlap with the vaca...
- 6.2.4: Rank the following carbocations in each set from most stable to lea...
Solutions for Chapter 6.2: Carbocation Stability Depends on the Number of Alkyl Groups Attached to the Positively Charged Carbon
Full solutions for Organic Chemistry | 8th Edition
Solutions for Chapter 6.2: Carbocation Stability Depends on the Number of Alkyl Groups Attached to the Positively Charged CarbonGet Full Solutions
A peroxide for which each oxygen atom is connected to an acyl group. Acyl peroxides are often used as radical initiators, because the O!O bond is especially weak.
The mass of an atom in atomic mass units. (3.1)
The dipole moment that is due to unequal electron sharing between two atoms in a covalent bond. (Section 9.3)
A polymer that contains a large number of branches connected to the main chain of the polymer.
Carboxyl group (Section 1.3D)
A !COOH group.
A process in which a substance (or substances) is changed into one or more new substances. (3.7)
crossed aldol reaction
An aldol reaction that occurs between different partners.
Alkanes whose carbon atoms are joined in rings. (24.2)
The use of electrolysis to reduce or refine metals. (Section 20.9)
The measure of disorder associated with a system.
Important biological molecules that catalyze virtually all cellular processes.
Gibbs free energy
A thermodynamic state function that combines enthalpy and entropy, in the form G = H - TS. For a change occurring at constant temperature and pressure, the change in free energy is ?G = ?H - T?S. (Section 19.5)
An amorphous solid formed by fusion of SiO2, CaO, and Na2O. Other oxides may also be used to form glasses with differing characteristics. (Section 22.10)
A compound containing a CRN bond.
In 1H NMR spectroscopy, the area under a signal indicates the number of protons giving rise to the signal.
Elements in the s and p blocks of the periodic table. (Section 6.9)
Molecular orbital (MO) theory
A theory of chemical bonding in which electrons in molecules occupy molecular orbitals that extend over the entire molecule and are formed by the combination of the atomic orbitals that make up the molecule
oxidation number (oxidation state)
A positive or negative whole number assigned to an element in a molecule or ion on the basis of a set of formal rules; to some degree it reflects the positive or negative character of that atom. (Section 4.4)
An equation thatdescribes the relationship between the rate of a reactionand the concentration of reactants.
A triester formed from glycerol and three long-chain carboxylic acids.
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