Chapter 7

Question 1

A molecular orbital that is higher in energy than the atomic orbitals that combined to produce it. (7.7)

Answer 1

Antibonding Molecular Orbital

Question 2

Describes the two bonds that form an axis perpendicular to the trigonal plane in trigonal bipyramidal geometry. (7.1)

Answer 2

Axial

Question 3

A molecular orbital that is lower in energy than the atomic orbitals that combined to produce it. (7.7)

Answer 3

Bonding Molecular Orbital

Question 4

A number based on the number of electrons in bonding and antibonding molecular orbitals that indicates, qualitatively, how stable a bond is. (7.7)

Answer 4

Bond Order

Question 5

Describes bonding electron density that is spread out over the molecule or part of the molecule, rather than confined between two specific atoms. (7.8)

Answer 5

Delocalized

Question 6

Attractive forces that act between polar molecules. (7.3)

Answer 6

Dipole-Dipole Interactions

Question 7

A lone pair or a bond, regardless of whether the bond is single, double, or triple. (7.1)

Answer 7

Electron Domain

Question 8

The arrangement of electron domains (bonds and lone pairs) around a central atom. (7.1)

Answer 8

Electron-Domain Geometry

Question 9

Describes the three bonds that are arranged in a trigonal plane in a trigonal bipyramidal geometry. (7.1)

Answer 9

Equatorial

Question 10

The mixing of atomic orbitals. (7.5)

Answer 10

Hybridization

Question 11

Orbitals formed by hybridization of some combination of s, p, or d atomic orbitals. (7.5)

Answer 11

Hybrid Orbitals

Question 12

A special type of dipoledipole interaction that occurs only in molecules that contain H bonded to a small, highly electronegative atom, such as N, O, or F. (7.3)

Answer 12

Hydrogen Bonding

Question 13

A fleeting nonuniform distribution of electron density in a molecule without a permanent dipole. (7.3)

Answer 13

Instantaneous Dipole

Question 14

The attractive forces that hold particles together in the condensed phases. (7.3)

Answer 14

Intermolecular Forces

Question 15

Coulombic attractions between ions and polar molecules. (7.3)

Answer 15

Ion-Dipole Interactions

Question 16

Describes electrons that are shared between two specific atoms and that cannot be repositioned to generate additional resonance structures. (7.8)

Answer 16

Localized

Question 17

Attractive forces that act between all molecules, including nonpolar molecules, resulting from the formation of instantaneous dipoles and induced dipoles.

Answer 17

Dispersion Forces (London Dispersion Forces)

Question 18

The arrangement of bonded atoms. (7.1)

Answer 18

Molecular Geometry

Question 19

Orbitals that result from the interaction of atomic orbitals of bonding atoms. (7.7)

Answer 19

Molecular Orbitals

Question 20

A theory that describes the orbitals in a molecule as bonding and antibonding combinations of atomic orbitals. (7.7)

Answer 20

Molecular Orbital Theory

Question 21

The sign of a wave’s amplitude. (7.7)

Answer 21

Phase

Question 22

A bond that forms from the interaction of parallel p orbitals. (7.6)

Answer 22

Pi(π) Bond

Question 23

Describes a molecule in which a dipole moment has been induced. (7.3)

Answer 23

Polarized

Question 24

A bond in which the shared electron density is concentrated directly along the internuclear axis. (7.6)

Answer 24

Sigma(σ) Bond

Question 25

Molecules that have the same chemical formula but different arrangements of atoms. (7.2)

Answer 25

Structural Isomer

Question 26

Atoms share electrons when an atomic orbital on one atom overlaps with an atomic orbital on the other. (7.4)

Answer 26

Valence Bond Theory

Question 27

A model that accounts for electron pairs in the valence shell of an atom repelling one another. (7.1)

Answer 27

Valence-Shell Electron-Pair Repulsion (VSEPR)

Question 28

The attractive forces that hold particles together in the condensed phases that include dipole-dipole interactions (including hydrogen bonding) and dispersion forces. (7.3)

Answer 28

van der Waals Forces

Question 29

How many electron groups exist in a double bond?

Answer 29

1

Same as lone pair and a single bond.

Question 30

benzene resonance

Answer 30

resonance

Question 31

Electron geometry of 3 electron groups around a central atom.

Answer 31

Triagonal Planar Electron Geometry

Question 32

Electron geometry of 4 electron groups around a central atom.

Answer 32

Tetrahedral Electron Geometry

Question 33

Electron geometry of 2 electron groups around a central atom.

Answer 33

Linear Electron Geometry

Question 34

Electron geometry of 5 electron groups around a central atom.

Answer 34

Bipyramidal Electron Geometry

Question 35

Electron geometry of 5 electron groups around a central atom.

Answer 35

Octahedral Electron Geometry

Question 36

Which occupies more space? Lone pair electrons or bonding pair?

Answer 36

Lone Pair Electrons

Question 37

Molecular geometry of four electron groups around the central atom and one is a lone pair.

Answer 37

Pyramidal Shape

Question 38

Molecular geometry of four electron groups around the central atom and two are lone pairs.

Answer 38

Bent or Tetrahedral-bent

Question 39

Molecular geometry of five electron groups around the central atom with one lone pair.

Answer 39

seesaw shape or distorted thtraheron

Question 40

Molecular geometry of five electron groups around the central atom with two lone pairs.

Answer 40

T-shaped