The dipole moment (μ) of hbr (a polar covalent molecule) is 0.851d (debye), and its percent ionic character is 12.6 % . estimate the bond length of the h−br bond in picometers. note that 1 d=3.34×10−30 c⋅m and

Bond length of HBr = 141 pm

Explanation:

measured dipole moment of HBr = 0.851 D

therefore,

dipole moment of HBr in C.m is,

dipole moment is related with charge and bond length as follows:

Here Q is charge and r is interatomic distance or bond length

In case of HBr, Q is 1.6×10^-19 C.

Calculate diople moment HBr, as follows:

Bond length of HBr is 141 pm

h let me think

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.