Multiple Choice
Which of the following best describes the molecular polarity of xenon tetrafluoride (XeF_4)?
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13. Liquids, Solids & Intermolecular Forces
Molecular Polarity
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Given the following bonds: (i) H–F, (ii) H–Cl, (iii) H–Br, rank them from most polar to least polar.
A
H–F > H–Cl > H–Br
B
H–Cl > H–F > H–Br
C
H–F > H–Br > H–Cl
D
H–Br > H–Cl > H–F
Verified step by step guidance1
Understand that bond polarity depends on the difference in electronegativity between the two atoms forming the bond. The greater the difference, the more polar the bond.
Identify the electronegativity values of the atoms involved: Hydrogen (H), Fluorine (F), Chlorine (Cl), and Bromine (Br). These values can be found on the Pauling scale.
Calculate the electronegativity difference for each bond: $\Delta \chi = |\chi_{\text{H}} - \chi_{\text{X}}|$, where X is F, Cl, or Br.
Compare the calculated differences: the bond with the largest $\Delta \chi$ is the most polar, and the one with the smallest $\Delta \chi$ is the least polar.
Rank the bonds from most polar to least polar based on the differences found: $\text{H–F} > \text{H–Cl} > \text{H–Br}$.
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