Part AWhat is the predominant intermolecular force in the liquid state of each of these compounds: methanol (CH3OH), carbon tetrachloride (CCL,), and hydrogen chloride (HCl)?Drag the appropriate items to their respective bins.> View Available Hint(s)ResetHelpCCL,CH,OHHCIDipole-dipole forcesHydrogen bondingDispersion forcesB.WordMasteri.P Type here to search I Review| Constants| PemLearning Goal:Chemists use the term intermolecular forces to describe the attractions between two or more moleculesDipole-dipole forces result from the attraction of the positive end of one polar molecule to the negative end of another polar molecule. Compounds consisting of atoms with different electronegativities may have a dipole moment,caused by an asymmetry of electrons.partial chargeHydrogen bonding is a particularly strong type of dipole-dipole force that occurs when hydrogen is attached to nitrogen, oxygen, or fluorine. Water is an example of a substance in which hydrogen bonding occurs. Because of oxygen's highelectronegativity and the electron deficiency of the hydrogen atom, the hydrogen atoms are attracted to the lone pairs of electrons on the oxygen of another water molecule.All substances have dispersion forces, also known as London forces. These forces are very weak and are only important in the absence of any other intermolecular force. Nonpolar covalent molecules and single-atom molecules are examples ofsubstances that lack all other intermolecular forces except for dispersion. Dispersion forces result from shifting electron clouds, which can cause a weak, temporary dipole.

The attraction forces between the different molecules are known as intermolecular forces.

What is the predominant intermolecular force in the liquid state of each of these compounds: methanol (CH3OH), carbon tetrachloride (CCL,), and hydrogen chloride (HCl)? Drag the appropriate items to their respective bins. > View Available Hint(s) Reset Help CCL, CH,OH HCI Dipole-dipole forces Hydrogen bonding Dispersion forces

What is the predominant intermolecular force in the liquid state of each of these compounds: methanol (CH3OH), carbon tetrachloride (CCL,), and hydrogen chloride (HCl)? Drag the appropriate items to their respective bins. > View Available Hint(s) Reset Help CCL, CH,OH HCI Dipole-dipole forces Hydrogen bonding Dispersion forces

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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