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Solutions for Chapter 5.1: History of the Periodic Table
Full solutions for Modern Chemistry: Student Edition 2012 | 1st Edition
The conjugate base of an alcohol.
The scientific discipline that studies the composition, properties, and transformations of matter. (Chapter 1: Introduction)
The species formed when a base accepts a proton from an acid
The group that is formed when two cysteine residues of a polypeptide or protein are joined together.
The transition of an electron in a transition-metal compound from a lower-energy d orbital to a higher-energy d orbital. (Section 23.6)
A material that can undergo a substantial change in shape via stretching, bending, or compression and return to its original shape upon release of the distorting force. (Section 12.6)
gas constant (R)
The constant of proportionality in the ideal-gas equation. (Section 10.4)
An equation that is often employed to calculate the pH of buffered solutions: pH = pKa + log 3conjugated base4 3acid4
A series of atoms, ions, or molecules having the same number of electrons. (Section 7.3)
The nucleophile in a Michael reaction.
A solid, inorganic substance occurring in nature, such as calcium carbonate, which occurs as calcite. (Section 23.1)
Two liquids that can be mixed with each other in any proportion.
A kinetic property measured by the rate at which a nucleophile causes nucleophilic substitution on a reference compound under a standardized set of experimental conditions.
An intermediate with a positively charged oxygen atom.
In mass spectrometry,the ion that is generated when the compound is ionized.
The negative log in base 10 of the aquated hydrogen ion concentration: pH = -log3H+4. (Section 16.4)
polar covalent bond
A covalent bond in which the electrons are not shared equally. (Section 8.4)
A polymer containing the !NHCO2! group as a repeating unit
Any chemical species that contains one or more unpaired electrons.
redox (oxidation–reduction) reaction
A reaction in which certain atoms undergo changes in oxidation states. The substance increasing in oxidation state is oxidized; the substance decreasing in oxidation state is reduced. (Section 4.4; Chapter 20: Introduction)