Question

The dipole moment (μ) of HBr (a polar covalent molecule) is 0.838D (debye), and its percent ionic character is 12.4 % . Estimate the bond length of the H−Br bond in picometers.
Note that
1 D=3.34×10−30 C⋅m and
in a bond with 100% ionic character, Q=1.6×10−19 C.

Answer 1

Note: q = 1.6 × 10−19 C

       1D = 3.34 × 10−30Cm3.34 × 10−30 Cm

         μ = 0.838D

Asked: r?

Answer: 1. Using comparison 1.11.1 in the formula:

         μ = qr

          r = r = μ / q

          r = [0.838D (3.34 × 10−30 C⋅m / 1D)] / (1.6 × 10−19 C) * 0.124

          r = 1.41 x10 ^ -10 m.

Thus, the estimated bond length of the H bond BR bond in a picometer is 1.41 x10 ^ -10 m.

Further Explanation

Molecular geometry is the arrangement of atoms that make up molecules in three dimensions. Molecular geometry determines several properties of substances including reactivity, polarity, substance appearance, color, magnetism, and biological activity. The angle between the bonds that make up the atom depends only weakly on the molecule, that is, they can be understood as local and therefore transferable.

In molecular geometry, bond length or bond distance is the average distance between the nuclei of two atoms bound in a molecule. This is one of the properties that can be removed from bonds between atoms of a fixed type, which are relatively independent of the molecule. Bond length is related to bond order: when more electrons participate in bond formation, the bond becomes shorter. Bond length is also inversely proportional to bond strength and bond dissociation energy: all other factors being equal, stronger bonds will be shorter. In a bond between two identical atoms, half the bond distance is equal to the covalent radius.

Factors that affect the bond length

The factors that determine bond length are:

1. Covalent radius
2. Electronegativity
3. Order of ties

Learn more

definition of Molecular geometry brainly.com/question/2314942

definition of bond length brainly.com/question/2314942

Factors that affect the bond length brainly.com/question/2314942

Details

Grade: College

Subject: Chemistry

keywords: Molecular geometry, bond length

Answer 2

When two electrical charges, of opposite sign and equal magnitude, are separated by a distance, a dipole is established. The size of a dipole is measured by its dipole moment (μμ). Dipole moment is measured in Debye units, which is equal to the distance between the charges multiplied by the charge (1 Debye equals 3.34×10−30Cm3.34×10−30Cm). The dipole moment of a molecule can be calculated by Equation 1.11.1:

μ = qr

where

μ⃗ μ→ is the dipole moment vector qiqi is the magnitude of the ithith charge, and r⃗ ir→i is the vector representing the position of ithith charge.

 

r = μ/q

r = [0.838D(3.34×10−30 C⋅m/ 1D)]/ (1.6×10−19 C) *0.124
r = 1.41 x10^-10 m