Define the following and give an example of each. (a) dispersion force Dispersion forces are -Select- : electrostatic attractions that occur due to the random electronic motion within all substances, -Select- : those that are nonpolar. When the electrons within a molecule or atom are distributed asymmetrically about the nucleus, that molecule or atom will adopt a --Select- :).-Select- : dipole. The presence of this dipole can then distort the electrons of a neighboring atom or molecule, producing an -Select-- : dipole. These two rapidly fluctuating dipoles thus result in a brief electrostatic -Select- :) between the two species. These forces are stronger in-Select- atoms and molecules. For example, dispersion forces between -Select- :) molecules will be stronger than dispersion forces between -Select- : molecules. (b) dipole-dipole attraction A dipole-dipole force is the electrostatic attraction between two -Select- A dipoles. The attraction occurs between the partial positive end of one polar molecule and the partial -Select-- A end of another polar molecule, For example, -Select- A molecules will exhibit dipole-dipole forces on each other. (c) hydrogen bond Hydrogen bonding is a particularly -Select-- :) type of dipole-dipole attraction that occurs when a hydrogen atom is bonded to a small, -Select- :) electronegative atom (including F, O, and N). The attraction is between the hydrogen atom and the F, O, or N atom on the neighboring molecule. For example, -Select- e molecules will exhibit hydrogen bonding.
Define the following and give an example of each. (a) dispersion force Dispersion forces are -Select- : electrostatic attractions that occur due to the random electronic motion within all substances, -Select- : those that are nonpolar. When the electrons within a molecule or atom are distributed asymmetrically about the nucleus, that molecule or atom will adopt a --Select- :).-Select- : dipole. The presence of this dipole can then distort the electrons of a neighboring atom or molecule, producing an -Select-- : dipole. These two rapidly fluctuating dipoles thus result in a brief electrostatic -Select- :) between the two species. These forces are stronger in-Select- atoms and molecules. For example, dispersion forces between -Select- :) molecules will be stronger than dispersion forces between -Select- : molecules. (b) dipole-dipole attraction A dipole-dipole force is the electrostatic attraction between two -Select- A dipoles. The attraction occurs between the partial positive end of one polar molecule and the partial -Select-- A end of another polar molecule, For example, -Select- A molecules will exhibit dipole-dipole forces on each other. (c) hydrogen bond Hydrogen bonding is a particularly -Select-- :) type of dipole-dipole attraction that occurs when a hydrogen atom is bonded to a small, -Select- :) electronegative atom (including F, O, and N). The attraction is between the hydrogen atom and the F, O, or N atom on the neighboring molecule. For example, -Select- e molecules will exhibit hydrogen bonding.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Concept explainers
Bond Parameters
Many factors decide the covalent bonding between atoms. Some of the bond parameters are bond angle, bond order, enthalpy, bond length, etc. These parameters decide what kind of bond will form in atoms. Hence it is crucial to understand these parameters in detail and understand how changing these parameters affects the kind of bonding or various characteristics.
Bond Dissociation Energy
The tendency of an atom to attract an electron is known as its electronegativity.
Question
(a)
dispersion force
Dispersion forces are (Very weak),(Very strong) electrostatic attractions that occur due to the random electronic motion within all substances,(excluding),(including) those that are nonpolar. When the electrons within a molecule or atom are distributed asymmetrically about the nucleus, that molecule or atom will adopt a (temporary),(permanent), (induced),(instantaneous) dipole. The presence of this dipole can then distort the electrons of a neighboring atom or molecule, producing an (induced),(instantaneous) dipole. These two rapidly fluctuating dipoles thus result in a brief electrostatic (attraction),(Repulsion) between the two species. These forces are stronger in (Larger and heavier),(Smaller and lighter) atoms and molecules. For example, dispersion forces between (Fluorine),(iodine) molecules will be stronger than dispersion forces between (Fluorine),(iodine) molecules.
(b)
dipole-dipole attraction
A dipole-dipole force is the electrostatic attraction between two (temporary),(permanent) dipoles. The attraction occurs between the partial positive end of one polar molecule and the partial (Positive),(Negative) end of another polar molecule. For example, (Nitrogen),(oxygen),(carbon monoxide),(chlorine)molecules will exhibit dipole-dipole forces on each other.
(c)
hydrogen bond
Hydrogen bonding is a particularly (weak),(strong) type of dipole-dipole attraction that occurs when a hydrogen atom is bonded to a small, (weakly),(highly) electronegative atom (including F, O, and N). The attraction is between the hydrogen atom and the F, O, or N atom on the neighboring molecule. For example, (acetone),(Carbon dioxide),(water),(Nitrogen dioxide) molecules will exhibit hydrogen bonding.
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