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 cloud.
This list contains the 118 elements of chemistry. 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.Choose one: A. Br2 is larger than ICl. click on any element's name for further chemical properties, environmental data or health effects.. 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.
Cl2, Br2, and I2 also follow a pretty clear trend. Bromine has higher boiling point than Fluorine, in halogens family boiling point increases down the group due to molecular nature and increase in Vander waal's forces. Which compound, Br_2 or I_2, has the higher boiling point and why? In this trend HCl/Cl2 is actually the odd one out, as it’s the only pair where the acid has a higher boiling point than the diatomic molecule. Br_2 because it is smaller and has fewer dispersion forces than I_2. If the intermolecular forces between molecules are relatively strong, the boiling point will be relatively high and if it is relatively weak, the boiling point … Among Br2 and I2 , Bromine has lower boiling point as compared to iodine ( … At room temperature, Cl2 is a gas, Br2 is a liquid, and KBr is a solid

Chlorine has the lowest boiling point as compared to other two (bromine and iodine) because Br and I is larger than Cl, therefore Br2 AND I2 has stronger intermolecular foces (Van der Waals) compared to Cl2. Bromine is a chemical element with symbol Br and atomic number 35. I_2 because it is larger and has more dispersion forces than Br_2. Both trends are driven by dispersion forces, where the higher amount of dispersion forces (due to more electrons) results in a higher boiling point. The molar mass is not identical: the molar mass of Br2 is only 159.80 g/mol compared to 162.35 g/mol for ICl. Br_2 because it has more dispersion forces than O_2. KBr will have by far the highest boiling point. The most important factor in determining the boiling point (without knowing the boiling point), is the intermolecular forces involved. Boiling Point: 58.8±9.0 °C at 760 mmHg Vapour Pressure: 190.2±0.1 mmHg at 25°C Enthalpy of Vaporization: 30.0±0.0 kJ/mol Flash Point: Index of Refraction: 1.551 Molar Refractivity: 17.5±0.3 cm 3 Note that, these points are associated with the standard atmospheric pressure.. Boiling Point – Saturation. In thermodynamics, the term saturation defines a condition in which a mixture of vapor and liquid can exist together at a given temperature and pressure. Property Name Property Value Reference; Molecular Weight: 84.16 g/mol: Computed by PubChem 2.1 (PubChem release 2019.06.18) XLogP3-AA: 2.6: Computed by … Since Cl2 is smaller than Br2, Cl2 will have a lower boiling point. B. The larger the molecule, the higher the boiling point, because larger molecule = more polarizable = strong London dispersion forces = stronger intermolecular forces = … Chemical elements listed by boiling point The elemenents of the periodic table sorted by boiling point. D. I_2 because it is more polar than Br_2. C. ICl is ionic. It is the third-lightest halogen, and is a fuming red-brown liquid at room temperature that evaporates readily to form a similarly coloured gas.


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