Solutions for Chapter 2: Introductory Chemistry 5th Edition

A molecular orbital in which electron density is concentrated outside the region between the two nuclei of bonded atoms. Such orbitals, designated as s* or p*, are less stable (of higher energy) than bonding molecular orbitals. (Section 9.7)

An equation that relates the rate constant for a reaction to the frequency factor, A, the activation energy, Ea, and the temperature, T: k = Ae-Ea>RT. In its logarithmic form it is written ln k = -Ea>RT + ln A. (Section 14.5)

The pressure exerted by Earth’s atmosphere. (5.2)

Enantiomers that lack a chiral center and differ because of hindered rotation.

A substance that yields hydroxide ions (OH2) when dissolved in water. (2.7)

A reactive intermediate formed by b-elimination from adjacent carbon atoms of a benzene ring and having a triple bond in the benzene ring. The second p bond of the benzyne triple bond is formed by the weak overlap of coplanar 2p orbitals on adjacent carbons.

Organic material that bacteria are able to oxidize. (Section 18.4)

Tools that are used for drawing resonance structures and for showing the flow of electron density during each step of a reaction mechanism.

A force that becomes significant when polar molecules come in close contact with one another. The force is attractive when the positive end of one polar molecule approaches the negative end of another. (Section 11.2)

A type of secondary structure of DNA molecules in which two anti parallel polynucleotide strands are coiled in a right-handed manner about the same axis

A conformation that exhibits a gauche interaction.

The structure of the transition state for an exothermic step looks more like the reactants of that step than the products. Conversely, the structure of the transition state for an endothermic step looks more like the products of that step than the reactants.

The heat given off during a reaction.

A substance added to a solution that changes color when the added solute has reacted with all the solute present in solution. The most common type of indicator is an acid–base indicator whose color changes as a function of pH. (Section 4.6)

A chemical equation for a solution reaction in which soluble strong electrolytes are written as ions and spectator ions are omitted. (Section 4.2)

A compound that absorbs light and transfers the energy to another molecule.

The ease with which the electron cloud of an atom or a molecule is distorted by an outside influence, thereby inducing a dipole moment. (Section 11.2)

The most common isotope of hydrogen. (Section 22.2)

The total of (single bonds + lone pairs) for an atom in a compound.

Compounds with the following structure: R!C#C!H