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1 month ago

Arrange the bromine-containing compounds CaBr2, Br2, NBr3, CBr4 in order of increasing predicted boiling point.

Chemistry

1 answer:

VMariaS [2.9K]1 month ago

3 0

Explanation:

In an ionic compound, powerful attractive forces act between the atoms involved due to their opposing electrical charges.

For instance, $CaBr_{2}$ represents an ionic compound where calcium has a +2 charge, and each bromine atom has a -1 charge.

As a result, to break these bonds, additional heat is required, which explains the elevated boiling point of calcium bromide.

On the other hand, $NBr_{3}$ is a covalent compound and since nitrogen exhibits greater electronegativity and a lone electron pair, a net dipole moment is created.

Furthermore, $CBr_{4}$ is also covalent and because bromine has higher electronegativity than carbon, the dipole moment is directed outward, so in $CBr_{4}$ , the dipole moment is effectively zero.

Consequently, its boiling point is lower than that of $NBr_{3}$ .

$Br_{2}$ is a covalent compound and does not possess a dipole moment.

Therefore, we can summarize that the given bromine-containing compounds can be ranked in order of increasing boiling point as follows.

$Br_{2}$ < $CBr_{4}$ < $NBr_{3}$ < $CaBr_{2}$

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