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Complete the sentences to explain whether the polarity differences and hydrogen bond capacity explain the differences in the chart. Motoh tho word

Complete the sentences to explain whether the polarity differences and hydrogen bond capacity explain the differences in the chart. Motoh tho word

Chemistry
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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MReview I Constants I Periodic Table Intermolecular forces are attractions between molecules. They are weaker than chemical bonds, but they play an important role in associations between molecules, such as forming mixtures or complex structures found in biomolecules. Most intermolecular forces are due to the unequal distribution of electrons in a molecule, leading to partial charges. The degree to which an atom attracts electrons toward itself in a molecule is its electronegativity. Atoms with the same or similar electronegativities (with differences of <0.4) form covalent bonds, atoms with large differences in electronegativity (>2.0) form ionic bonds, and those with modest differences in electrnegatvities (between 0.4 and 2.0) form polar covalent bonds. Polar bonds are indicated with a +, where the + is on the atom with lower electronegativity (and a partial positive charge) while the is on the more electronegative, partially negative charged atom. Element Electronegativity H 2.1 C 2.5 3.0 3.5 F 4.0 For a molecule to be polar, not only must it have polar bonds but it must also be nonsymmetric. If the bonds are not polar, the molecule cannot be polar; if all the polar bonds cancel out, the molecule is also not polar. For example, CF4 contains all polar bonds, but because they are symmetrically arranged around the central atom, the dipoles cancel and the molecule is neutral. To determine whether the dipoles cancel, a correct Lewis structure is required. One special case of dipole interactions is hydrogen bonds. When a hydrogen is attached to N, O, or F, there is a strong dipole, with a positive partial charge on the hydrogen and a negative partial charge on the N, O, or F. Consequently, the negative partial charge on the N, O, or F is attracted to the H attached to an N, O, or F in another molecule. The N, O, or F is referred to as the hydrogen bond acceptor, while the molecule with the H attached to N, O, or F is the hydrogen bond donor. O H-O Forming intermolecular interactions releases energy. If the free energy released by the solvent-solute interactions is larger than the free energy required to break the solute-solute and solvent-solvent interactions, the solute will be soluble in the solvent.
Transcribed Image Text:MReview I Constants I Periodic Table Intermolecular forces are attractions between molecules. They are weaker than chemical bonds, but they play an important role in associations between molecules, such as forming mixtures or complex structures found in biomolecules. Most intermolecular forces are due to the unequal distribution of electrons in a molecule, leading to partial charges. The degree to which an atom attracts electrons toward itself in a molecule is its electronegativity. Atoms with the same or similar electronegativities (with differences of <0.4) form covalent bonds, atoms with large differences in electronegativity (>2.0) form ionic bonds, and those with modest differences in electrnegatvities (between 0.4 and 2.0) form polar covalent bonds. Polar bonds are indicated with a +, where the + is on the atom with lower electronegativity (and a partial positive charge) while the is on the more electronegative, partially negative charged atom. Element Electronegativity H 2.1 C 2.5 3.0 3.5 F 4.0 For a molecule to be polar, not only must it have polar bonds but it must also be nonsymmetric. If the bonds are not polar, the molecule cannot be polar; if all the polar bonds cancel out, the molecule is also not polar. For example, CF4 contains all polar bonds, but because they are symmetrically arranged around the central atom, the dipoles cancel and the molecule is neutral. To determine whether the dipoles cancel, a correct Lewis structure is required. One special case of dipole interactions is hydrogen bonds. When a hydrogen is attached to N, O, or F, there is a strong dipole, with a positive partial charge on the hydrogen and a negative partial charge on the N, O, or F. Consequently, the negative partial charge on the N, O, or F is attracted to the H attached to an N, O, or F in another molecule. The N, O, or F is referred to as the hydrogen bond acceptor, while the molecule with the H attached to N, O, or F is the hydrogen bond donor. O H-O Forming intermolecular interactions releases energy. If the free energy released by the solvent-solute interactions is larger than the free energy required to break the solute-solute and solvent-solvent interactions, the solute will be soluble in the solvent.
Part G Complete the sentences to explain whether the polarity differences and hydrogen bond capacity explain the differences in the chart. Match the words in the left column to the appropriate blanks in the sentences on the right. Reset Help do Given the four compounds in the chart, four is/are polar. do not Given the four compounds in the chart, three can participate in hydrogen bonding. one Given the four compounds in the chart, three has/have an available hydrogen bond donor. two three Given the four compounds in the chart, three has/have a hydrogen bond acceptor. four Therefore, the polarity differences and hydrogen bond capacity do explain the differences in the chart.
Transcribed Image Text:Part G Complete the sentences to explain whether the polarity differences and hydrogen bond capacity explain the differences in the chart. Match the words in the left column to the appropriate blanks in the sentences on the right. Reset Help do Given the four compounds in the chart, four is/are polar. do not Given the four compounds in the chart, three can participate in hydrogen bonding. one Given the four compounds in the chart, three has/have an available hydrogen bond donor. two three Given the four compounds in the chart, three has/have a hydrogen bond acceptor. four Therefore, the polarity differences and hydrogen bond capacity do explain the differences in the chart.
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