5 Questions
What is the relationship between the size of the halogen atom and the carbon–halogen bond length?
The carbon–halogen bond length increases as the halogen atom size increases.
Which of the following is a characteristic of fluoromethane?
It has a strong C–X bond and a short C–X bond length.
What is the trend in the polarity of the methyl halides as one progresses from fluorine to iodine substitution?
The polarity decreases as one progresses from fluorine to iodine substitution.
What is the relationship between the size of the halogen atom and the carbon–halogen bond strength?
The carbon–halogen bond strength decreases as the halogen atom size increases.
Which of the following is a characteristic of iodomethane?
It has a weak C–X bond and a long C–X bond length.
Study Notes
Halogen Atom Size and Carbon-Halogen Bond Properties
- Halogen atom size increases as you go down the periodic table, with fluorine being the smallest and iodine being the largest.
- As you go down the periodic table, the carbon-halogen bond length increases, and the carbon-halogen bond strength decreases.
- The electrostatic potential maps at the van der Waals surface illustrate the trend in polarity, C–X bond length, and halogen atom size for the four methyl halides.
- Fluoromethane has the highest polarity, shortest C–X bond length, and strongest C–X bond.
- Iodomethane has the lowest polarity, longest C–X bond length, and weakest C–X bond.
- The trend in carbon-halogen bond properties can be observed in the methyl halides, with fluorine substitution resulting in the strongest and shortest bond, and iodine substitution resulting in the weakest and longest bond.
This quiz explores the relationship between halogen atom size, carbon-halogen bond length, and bond strength as you move down the periodic table. It also examines the polarity of methyl halides.
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