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Explanation of Trends in Boiling Points of Hydrogen Halides

Explore the varying boiling points of hydrogen halides (HCl, HBr, HI) based on electronegativity differences, number of electrons, and London forces. Understand intermolecular forces between NH2OH, CBr4, H2SeO4, SO2. Determine melting points for substances like HCl vs. NaCl. Predict liquid properties based on intermolecular forces.

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Explanation of Trends in Boiling Points of Hydrogen Halides

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  1. Chapter 10 Worked Example 1 Explain the trend in the boiling points of the hydrogen halides: HCl, -85 oC; HBr, -67 oC; HI, -35 oC. - Electronegativity differences: HCl > HBr > HI - Number of electrons and London forces: HCl < HBr < HI → not by dipole-dipole forces, but by London forces

  2. Chapter 10 Worked Example 2

  3. Chapter 10 Worked Example 3

  4. Chapter 10 Worked Example 4 Identify the kinds of intermolecular forces that might arise between molecules of each of the following substances: (a) NH2OH; (b) CBr4; (c) H2SeO4; (d) SO2 • Solution • London forces, dipole-dipole forces, hydrogen bonding • London forces • London forces, dipole-dipole forces, hydrogen bonding • London forces, dipole-dipole forces

  5. Chapter 10 Worked Example 5 Suggest, giving reasons, which substance in each of the following pairs is likely to have the higher normal melting point (Lewis structures may help your arguments): • HCl or NaCl; (b) C2H5OC2H5 (diethyl ether) or C4H9OH (butanol); • (c) CHI3 or CHF3; (d) C2H4 or CH3OH. Solution

  6. Chapter 10 Worked Example 6

  7. Chapter 10 Worked Example 7 Predict how each of the following properties of a liquid varies as the strength of intermolecular forces increases and explain your reasoning: (a) boiling point; (b) viscosity; (c) surface tension. Solution

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