Shanxian Chemical
SUPPLEMENTS
Boiling Point of Hydrogen Halides
Hydrogen Halide Boiling Point Investigation
Hydrogen halide is a compound formed by hydrogen and halogens. The change of its boiling point is very interesting and is also an important item for chemical investigation.
The first word is hydrogen fluoride ($HF $), whose boiling point is quite different from the rest. Because of the hydrogen bond between hydrogen fluoride molecules, this bond force is strong, so that the molecules come together tightly. When heated to boil, more energy is required to break the hydrogen bond. The boiling point of hydrogen fluoride is higher, about 19.5 dollars ^ {\ circ} C $.
Subocular hydrogen chloride ($HCl $), its intermolecular only has van der Waals force. This force is much weaker than the hydrogen bond, so the boiling point of hydrogen chloride is lower, about $-85 ^ {\ circ} C $. Under normal conditions, hydrogen chloride is a gaseous state and escapes in the air. The same is true for
Hydrogen bromide ($HBr $) and hydrogen iodide ($HI $). With the increase of the atomic number of the halogen, the relative molecular weight of the hydrogen halide molecule increases. The larger the molecular weight, the stronger the van der Waals force. The boiling point of hydrogen bromide is about $-67 ^ {\ circ} C $, and the boiling point of hydrogen iodide is about $-35 ^ {\ circ} C $, both of which are gradually changing due to the change of Van der Waals force.
In summary, the boiling point of hydrogen halide, hydrogen fluoride is only higher with hydrogen bonds, and the rest increase gradually with the increase of relative molecular weight according to van der Waals force. This law has important guiding significance in many aspects such as chemical research and industrial preparation.
Hydrogen halide is a compound formed by hydrogen and halogens. The change of its boiling point is very interesting and is also an important item for chemical investigation.
The first word is hydrogen fluoride ($HF $), whose boiling point is quite different from the rest. Because of the hydrogen bond between hydrogen fluoride molecules, this bond force is strong, so that the molecules come together tightly. When heated to boil, more energy is required to break the hydrogen bond. The boiling point of hydrogen fluoride is higher, about 19.5 dollars ^ {\ circ} C $.
Subocular hydrogen chloride ($HCl $), its intermolecular only has van der Waals force. This force is much weaker than the hydrogen bond, so the boiling point of hydrogen chloride is lower, about $-85 ^ {\ circ} C $. Under normal conditions, hydrogen chloride is a gaseous state and escapes in the air. The same is true for
Hydrogen bromide ($HBr $) and hydrogen iodide ($HI $). With the increase of the atomic number of the halogen, the relative molecular weight of the hydrogen halide molecule increases. The larger the molecular weight, the stronger the van der Waals force. The boiling point of hydrogen bromide is about $-67 ^ {\ circ} C $, and the boiling point of hydrogen iodide is about $-35 ^ {\ circ} C $, both of which are gradually changing due to the change of Van der Waals force.
In summary, the boiling point of hydrogen halide, hydrogen fluoride is only higher with hydrogen bonds, and the rest increase gradually with the increase of relative molecular weight according to van der Waals force. This law has important guiding significance in many aspects such as chemical research and industrial preparation.
Scan to WhatsApp
