Table of Contents
- 1 Why does Br2 have a greater boiling point than BrCl?
- 2 Why does Br2 have a higher boiling point than Kr?
- 3 Why does Br2 have a higher boiling point than CH3Br?
- 4 Why does Br2 have a lower boiling point than ICl?
- 5 Why does Br2 have higher vapor pressure than I2?
- 6 Why does br2 have a lower boiling point than ICl?
- 7 Why do Br2 and ICL have the same dispersion forces?
- 8 Why does I2 have a higher boiling point than B2?
Why does Br2 have a greater boiling point than BrCl?
C) Br2 and Cl2 can react to form the compound BrCl. However, due to the greater polarizability of the electron cloud of Br2 compared to that of BrCl, the London forces in Br2 (l) are stronger than the combined intermolecular forces in BrCl (l). Thus, the boiling point of Br2 (l) is greater than that of BrCl (l).
Why is the boiling point of Br2 higher than that of Cl2?
Br2 molecules are larger than Cl2 molecules, so more electrons are present in Br2 molecules. Therefore there are stronger van der waals forces between Br2 molecules than Cl2 molecules, so more energy is needed to melt Br2.
Why does Br2 have a higher boiling point than Kr?
So it would be easier for the atom to develop an instantaneous dipole, strengthening the London forces between the atoms of the element, and increasing the boiling point of the substance. Krypton has a larger atomic radius than bromine.
Why is the boiling point of Br2 lower than that of iodine monochloride ICl even though they have nearly the same molar mass?
Explain why the boiling point of Br2 (59°C) is lower than that of iodine monochloride, ICl (97°C), even though they have nearly the same molar mass. ICl is polar while Br2 is nonpolar. The boiling point of a substance decreases with decreasing intermolecular force strength.
Why does Br2 have a higher boiling point than CH3Br?
Br2 has a larger molar mass, and therefore a larger electron cloud than CH3Br. Explains with reference to molecules and intermolecular forces why bromine has a higher boiling point than bromomethane. • Fully justifies differences in boiling points for ALL three compounds in terms of strength of attractive forces.
Why does CH3CH2OH have a higher boiling point than ch3och3?
(c) Both CH3OH and CH3CH2OH can H-bond but CH3CH2OH has more CH bonds for greater dispersion force interactions. Therefore, CH3CH2OH has the higher boiling point.
Why does Br2 have a lower boiling point than ICl?
ICl and Br2 have similar masses (~160 amu) and therefore experience similar London dispersion forces. ICl is polar and thus also exhibits dipole-dipole attractions; Br2 is nonpolar and does not. The relatively stronger dipole-dipole attractions require more energy to overcome, so ICl will have the higher boiling point.
What is the boiling point of Br2?
137.8°F (58.8°C)
Diatomic Bromine/Boiling point
Why does Br2 have higher vapor pressure than I2?
Since I2 has higher molecular weight, it has stronger London dispersion forces so it has a higher boiling point than Br2.
Why does iodine have a higher boiling point?
Iodine is always found in a compound. Its melting and boiling point are higher than fluorine, chlorine or bromine. This is because the instantaneous dipole-induced dipole bonds are stronger (it has more electrons).
Why does br2 have a lower boiling point than ICl?
Why does ICL have a higher boiling point than br2cl?
That means that ICl molecules are attracted to each other by dipole-dipole interactions as well as London dispersion forces, whereas Br₂ molecules are attracted to each other only by London dispersion forces. Dipole-dipole interactions are stronger, so it takes more energy to separate the molecules, so the boiling point is higher.
Why do Br2 and ICL have the same dispersion forces?
(Any connection to molecular weight is coincidental.) ICl and Br2 have the same number of electrons are are almost the same size, therefore, the strength of the London dispersion forces are essentially equal. That leaves the other two van der Waals forces as the distinguishing factors.
What is the boiling point of I-CL and bromine?
Explanation: The boiling point of bromine is 58.8 ∘C; the boiling point of I −Cl is 97.4 ∘C, so the difference is fairly dramatic. In the bromine molecule, however, only dispersion forces operate. Dispersion forces also operate in I −Cl, and these would be expected to be greater in that the iodine atom, has a larger more polarizable electron…
Why does I2 have a higher boiling point than B2?
Ok, answering my own question here: Upon further research online, I discovered that I2 has the higher boiling point because it has larger electron clouds, hence stronger London forces, which cause the boiling point to be higher than that of B2.