- 22.2SE.1PE: Predicting the Products of Chemical ReactionsPredict the products f...
- 22.2SE.2PE: Predicting the Products of Chemical ReactionsPredict the products f...
Solutions for Chapter 22.2SE: Chemistry: The Central Science 13th Edition
Full solutions for Chemistry: The Central Science | 13th Edition
The product obtainedfrom 1,2-addition across a conjugated p system.
An alloy of mercury with another metal or metals. (21.2)
Instability that arises when a planar ring of continuously overlapping p orbitals contains 4n p electrons.
atomic mass unit (amu)
A unit of measure equivalent to 1 g divided by Avogadro’s number.
A means of protecting a metal against corrosion by making it the cathode in a voltaic cell. This can be achieved by attaching a more easily oxidized metal, which serves as an anode, to the metal to be protected. (Section 20.8)
A substance formed by addition of a proton to a Brønsted–Lowry base. (Section 16.2)
A substance formed by the loss of a proton from a Brønsted–Lowry acid. (Section 16.2)
In NMR spectroscopy,protons or carbon atoms whose surrounding electron density is poor.
The term used to express the concept of less shielding in NMR
A long, unbranched-chain carboxylic acid, most commonly of 12 to 20 carbons, derived from the hydrolysis of animal fats, vegetable oils, or the phospholipids of biological membranes.
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)
For substituted cycloalkanes, a drawing style used to clearly identify which groups are above the ring and which groups are below the ring. (See also Sect. 4.14.)
An effect thatprevents the use of bases stronger than hydroxidewhen the solvent is water.
The mass of one mole of a substance in grams; it is numerically equal to the formula weight in atomic mass units. (Section 3.4)
A collection of Avogadro’s number 16.022 * 10232 of objects; for example, a mole of H2O is 6.022 * 1023 H2O molecules. (Section 3.4)
Solids that are composed of molecules. (Sections 12.1 and 12.6)
The conversion of a substance from one state of matter to another. The phase changes we consider are melting and freezing 1solid ? liquid2, sublimation and deposition, and vaporization and condensation 1liquid ? gas2. (Section 11.4)
Polar covalent bond
A covalent bond between atoms whose difference in electronegativity is between approximately 0.5 and 1.9.
Primary structure of nucleic acids
The sequence of bases along the pentose-phosphodiester backbone of a DNA or RNA molecule read from the 5’ end to the 3’ end
A solution prepared by dissolving Ag2O in aqueous ammonia; used for selective oxidation of an aldehyde to a carboxylic acid.
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