HI has a higher boiling point because of the dipole-dipole Intermolecular forces as well as the dispersion forces, which become more evident with molecular weight, which will dominate over the dipole-dipole forces, so HCl has a lower boiloing point.
-84°C for HF -114.2°C for HCl So, HCl has a lower boiling point because the HF has hydrogen bonds attracting the molecules and so therefore has a higher heat of vaporization.
The boiling point of hydrogen flouride (HF) is the highest at 19.5oC. The boiling point of hydrogen bromide (HBr) -66.38oC and the boiling point of hydrogen chloride (HCl) is -85.1oC.
NaCl,HF,HCl,F2.
There is no hydrogen bonding in HBr and HI. The intermolecular forces are London dispersion forces- HI has more electrons, so more instantaneous induced dipole-dipole interaction- more intermolecular force- and therefore a higher boiling point.
HI is more stronger acid while H2Te is almost neutral.
HI has the lowest boiling point because it is covalent all other mentioned compounds rae ionic....
Strongest---------------> Weakest HI, HCl, H2S, H2O According to MasteringChemistry.com
Iodine is larger in size so makes weaker bond with hydrogen and HI easily ionizes in water and is strong acid while HCl bond is relatively strong and not broken down easily in water as compare to HI.
This is to do with the intermolecular forces in the two compounds. There are no hydrogen bonds between the molecules of either compound, since Br and I are not electronegative enough to polarise the molecules sufficiently. But since HI molecules contain more electrons than HBr, there are increased van der Waals forces in HI. For the same reason HBr has a higher boiling point than HCl, but HF has a higher boiling point than HCl, HBr or HI because of hydrogen bonding.
HF is electronegative compared to O2. HF has delta plus and delta minus creating a dipole moment, it is a polar molecule therefore it has a higher boiling point. O2 which is symmetrical and non polar (looks like O=O) and therefore has no dipole moment.
There is no hydrogen bonding in HBr and HI. The intermolecular forces are London dispersion forces- HI has more electrons, so more instantaneous induced dipole-dipole interaction- more intermolecular force- and therefore a higher boiling point.
HI is more stronger acid while H2Te is almost neutral.
HI has the lowest boiling point because it is covalent all other mentioned compounds rae ionic....
Strongest---------------> Weakest HI, HCl, H2S, H2O According to MasteringChemistry.com
O2, SO2, HF.. im positive, just did a webassign if you know what that is but its right...
Examples are: HCl, HNO3, HF, HI.
Hydrochloric acid.HClO4 >> HI >> HBr >> HCl >> H2SO4
HCl, HBr, HI, HNO3, H2SO4, HClO4
BaOH + HCl -> BaCl + H2O
The polarity of a bond increases with the increment of the difference of electronegativity between the corresponding two atoms. Therefore HCl is most polar whereas HI is the weakest among the given.