(a) At room temperature, $\mathrm{H}_{2} \mathrm{O}$ is a liquid and $\mathrm{KNO}_{3}$ is a solid. The student incorrectly claims that this is because potassium and nitrate ions experience stronger dispersion forces than $\mathrm{H}_{2} \mathrm{O}$ molecules. In terms of the types of aftractive forces, explain why the student is incorrect.

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∻Solution∻ ‖ 1 ⋮ **Identify the types of intermolecular forces in $\mathrm{H_2O}$ and $\mathrm{KNO_3}$**: $\mathrm{H_2O}$ molecules are polar and can form hydrogen bonds, which are a type of strong dipole-dipole interaction. $\mathrm{KNO_3}$ is an ionic compound, consisting of potassium ions ($\mathrm{K^+}$) and nitrate ions ($\mathrm{NO_3^-}$), which experience ionic bonding. ‖ ‖ 2 ⋮ **Explain the incorrect claim**: Dispersion forces, also known as London dispersion forces, are the weakest type of intermolecular force and are present in all molecules. However, they are not the primary force in either $\mathrm{H_2O}$ or $\mathrm{KNO_3}$. The student's claim is incorrect because the primary intermolecular force in $\mathrm{H_2O}$ is hydrogen bonding, not dispersion forces, and the primary force in $\mathrm{KNO_3}$ is ionic bonding, which is much stronger than dispersion forces. ‖ ‖ 3 ⋮ **Clarify the states of matter**: The state of matter (solid, liquid, or gas) at room temperature is determined by the strength of the intermolecular forces. The strong hydrogen bonds in $\mathrm{H_2O}$ allow it to be a liquid at room temperature, while the even stronger ionic bonds in $\mathrm{KNO_3}$ result in it being a solid. ‖ ∻Answer∻ ⚹ The student's claim is incorrect because $\mathrm{H_2O}$ molecules are held together by hydrogen bonds, not dispersion forces, and $\mathrm{KNO_3}$ is held together by ionic bonds, which are stronger than both dispersion forces and hydrogen bonds. This explains why $\mathrm{H_2O}$ is a liquid and $\mathrm{KNO_3}$ is a solid at room temperature. ⚹ ∻Key Concept∻ ⚹ Intermolecular forces determine the state of matter ⚹ ∻Explanation∻ ⚹ $\mathrm{H_2O}$ is a liquid at room temperature due to hydrogen bonding, while $\mathrm{KNO_3}$ is a solid due to ionic bonding. Dispersion forces are present in both but are not the determining factor for their states of matter. ⚹◊How do dispersion forces compare between potassium and nitrate ions compared to H2O molecules in terms of strength?⍭ Generate me a similar question◊

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