- 11.2SE.1PE: Predicting Types and Relative Strengths of Intermolecular Attractio...
- 11.2SE.2PE: Predicting Types and Relative Strengths of Intermolecular Attractio...
Solutions for Chapter 11.2SE: Chemistry: The Central Science 13th Edition
Full solutions for Chemistry: The Central Science | 13th Edition
An OR group.
The distance between atoms in a covalent bond in picometers (pm; 1 pm 5 10212 m) or Å (1Å 5 10210 m).
bonding molecular orbital
A molecular orbital in which the electron density is concentrated in the internuclear region. The energy of a bonding molecular orbital is lower than the energy of the separate atomic orbitals from which it forms. (Section 9.7)
Processes in which one or more substances are converted into other substances; also called chemical changes. (Section 1.3)
In a crystal lattice it is defined as the number of atoms (or ions) surrounding an atom (or ion) (11.4). In coordination compounds it is defined as the number of donor atoms surrounding the central metal atom in a complex. (23.3)
A molecule containing an !OH group and a !CN group bonded to the same carbon.
An alkane whose structure contains a ring.
A reaction involving loss of CO2, characteristic of compounds containing a carbonyl group that is beta to a COOH group.
The angle created by two intersecting planes.
The process of separating compounds on the basis of their electric charge
Enantiomeric excess (ee)
The difference between the percentage of two enantiomers in a mixture
A conformation about a single bond of an alkane in which two groups on adjacent carbons lie at a dihedral angle of 60°
A protein, particularly rich in the basic amino acids lysine and arginine, that is found associated with DNA molecules
A polymer with identical confi gurations (either all R or all S) at all chiral centers along its chain, as, for example, isotactic polypropylene
molecular orbital (MO)
An allowed state for an electron in a molecule. According to molecular-orbital theory, a molecular orbital is entirely analogous to an atomic orbital, which is an allowed state for an electron in an atom. Most bonding molecular orbitals can be classified as s or p, depending on the disposition of electron density with respect to the internuclear axis. (Section 9.7)
In atomic and molecular orbitals, a location where the value of y is zero.
A mixture of equal amounts of two enantiomers.
Secondary structure of nucleic acids
The ordered arrangement of nucleic acid strands
A reaction that has a rate equation in which the sum of all exponents is three
A signal of an NMR spectrum that is shifted toward the right (smaller chemical shift) on the chart paper.
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