- 184.108.40.206.7: Why are standards needed for measured quantities?
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- 18.104.22.168.9: Complete the following conversions. a. 10.5 g = ____ kg b. 1.57 km ...
- 22.214.171.124.10: Write conversion factors for each equality. a. 1 m3 = 1 000 000 cm3...
- 126.96.36.199.11: a. What is the density of an 84.7 g sample of an unknown substance ...
- 188.8.131.52.12: INFERRING CONCLUSIONS A student converts grams to milligrams by mul...
Solutions for Chapter 2.2: Units of Measurement
Full solutions for Modern Chemistry: Student Edition 2012 | 1st Edition
A basic nitrogen-containing compound of plant origin, many of which are physiologically active when administered to humans.
bonding molecular orbital.
A molecular orbital that is of lower energy and greater stability than the atomic orbitals from which it was formed. (10.6)
A rule that states that it is not possible for a bridgehead carbon of a bicyclic system to possess a carbon carbon double bond if it involves a trans p bond being incorporated in a ring comprised of fewer than eight atoms.
A class of substances formed from polyhydroxy aldehydes or ketones. (Section 24.8)
Any property of a substance that cannot be studied without converting the substance into some other substance. (1.6)
conservation of orbital symmetry
During a reaction, the requirement that the phases of the frontier MOs must be aligned.
Stereoisomers that are not mirror images of each other; refers to relationships among two or more objects
Hydrogens that have the same chemical environment
Homolytic bond cleavage
Cleavage of a bond so that each fragment retains one electron; formation of radicals.
A polymer constructed from a single type of monomer.
A reaction that involves the addition of H and X (either Br or Cl) across an alkene.
An equation of state for gases that embodies Boyle’s law, Charles’s law, and Avogadro’s hypothesis in the form PV = nRT. (Section 10.4)
A term that describes the position of equilibrium for a reaction: Keq = 3H3O+ 4 3A- 4 3HA4 3H2O4
Le Châtelier’s principle
A principle stating that when we disturb a system at chemical equilibrium, the relative concentrations of reactants and
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
In NMR spectroscopy, a technique in which only the one-bond couplings are observed. CH3 groups appear as quartets, CH2 groups appear as triplets, CH groups appear as doublets, and quaternary carbon atoms appear as singlets.
Plane of symmetry
An imaginary plane passing through an object dividing it so that one half is the mirror image of the other half
Primary (1°) amine
An amine in which nitrogen is bonded to one carbon and two hydrogens
Polymers that are hard at room temperature but soft when heated.
van der Waals forces
A group of intermolecular attractive forces including dipole-dipole, dipole-induced dipole, and induced dipole-induced dipole (dispersion) forces