Solution Found!
Solved: Explain the observed trend in the boiling points of the compounds listed. Why is
Chapter 12, Problem 102P(choose chapter or problem)
Explain the observed trend in the boiling points of the compounds listed. Why is \(\mathrm{H}_{2} \mathrm{O}\) atypical?
Equation Transcription:
Text Transcription:
H_2 O
Questions & Answers
QUESTION:
Explain the observed trend in the boiling points of the compounds listed. Why is \(\mathrm{H}_{2} \mathrm{O}\) atypical?
Equation Transcription:
Text Transcription:
H_2 O
ANSWER:
Solution 102P
Find:
Here we have to explain the trend of boiling points of the following compounds, H2Te, H2Se, H2S and H2O.
Explanation:
Step 1:
Higher the boiling point, higher will be the forces because more thermal energy needed to separate the molecules in liquid state. Even though Sulfur is more electronegative than Se or Te , the size of the molecules is a bigger factor in their interactions. As we move down a group, the atomic size increases hence more energy will be required to break a molecule. Hence the boiling point also increases as we go down a group.
H2S< H2Se<H2Te
H2S = 212 K
H2Se = 232 K
H2Te = 271 K