HCL has a higher boiling point compared to HBr
This is due to difference in electronegativity.
H - 2.1
Cl - 3.0
Br - 2.8
The difference for HCl is 0.9, the difference for HBr is 0.7.
The larger the difference in electronegavity means the stronger the bond. Large difference means greater attraction hence more energy is needed to overcome this bond.
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∙ 15y agoWiki User
∙ 13y agoHBr and HCl are both polar have similar dipole-dipople forces. This can be determined by looking at their electronegativities.
Now, you need to determine their London Dispersion Forces- HBr is bigger than HCl (it is lower on the Periodic Table), so it has much more dispersion force.
Br2 has a higher boiling point than Cl2 because bromine is a larger atom than chlorine, leading to stronger van der Waals forces between the Br2 molecules.
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∙ 11y agoBr2 because it is a larger atom than Cl making the Intermolecular forces larger for Br2.
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∙ 11y agoHCl has a higher boiling point.
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∙ 12y agoHCl has a lower boiling point than HBr.
Bromine (Br2) is a liquid at room temperature and pressure. It can be converted to a gas by heating it above its boiling point of 58.8°C.
Among the given molecules, bromine (Br2) has the highest vapor pressure due to its relatively low boiling point and weak intermolecular forces between its molecules. Water (H2O) has a lower vapor pressure compared to bromine because of its stronger hydrogen bonding. Nitrogen trichloride (NCl3) has the lowest vapor pressure since it is a polar molecule with stronger intermolecular forces compared to the other two molecules.
Bromine (Br2) is a liquid at room temperature. It has a boiling point of 58.8°C and a melting point of -7.2°C.
The distance between nuclei of a bromine molecule (Br2) is approximately 228 picometers (pm). This distance is based on experimental measurements of the bond length in the Br2 molecule.
The oxidation number of Br2 is 0. Each bromine atom in the Br2 molecule has an oxidation number of 0 because the molecule is in its elemental form.
Yes, because BrBr2 is ionically bonded, while the Br2O is covalently (molecularly) bonded. Ionic bonds are stronger than covalent (molecular) bonds. This means that BeBr2 has stronger attraction between molecules and it will take more energy (heat) to "unstick them" into the gas phase. Because there is more heat needed to get BeBr2 boiling, it has a higher boiling point.
Bromine (Br2) is a liquid at room temperature and pressure. It can be converted to a gas by heating it above its boiling point of 58.8°C.
Bromine (Br2) is a liquid at room temperature. It has a boiling point of 58.8°C and a melting point of -7.2°C.
Among the given molecules, bromine (Br2) has the highest vapor pressure due to its relatively low boiling point and weak intermolecular forces between its molecules. Water (H2O) has a lower vapor pressure compared to bromine because of its stronger hydrogen bonding. Nitrogen trichloride (NCl3) has the lowest vapor pressure since it is a polar molecule with stronger intermolecular forces compared to the other two molecules.
The distance between nuclei of a bromine molecule (Br2) is approximately 228 picometers (pm). This distance is based on experimental measurements of the bond length in the Br2 molecule.
a molecule of bromine
Bromine (Br2) is liquid at room temperature, because it boiling point at normal pressure is 58.8 °C (higher) and its freezing point is -7.2 °C (which is lower than room temperature).
The oxidation number of Br2 is 0. Each bromine atom in the Br2 molecule has an oxidation number of 0 because the molecule is in its elemental form.
Br2 is a molecule consisting of two bromine atoms bonded together.
The bonding order of bromine molecule is one.
2Br is two separate bromine atoms. Br2 is a bromine molecule, consisting of two bromine atoms bonded together.
No, only Br2 is a diatomic molecule from the list provided. Diatomic molecules consist of two atoms of the same element bonded together, such as Br2 which is made of two bromine atoms. HNO1, H2O, and CO2 have more than two atoms in their molecules.