A hypothetical molecule, X–Y, has a dipole moment of 1.76 D and a bond length of 151 pm. Calculate the percent ionic character of this molecule.
To calculate the percent ionic character of a molecule, we can use the concept of electronegativity difference and apply it to the dipole moment.
1. Start by finding the electronegativities of elements X and Y. You can refer to the periodic table or any reliable source to determine these values.
2. Next, calculate the electronegativity difference (Δχ) between X and Y by subtracting the smaller electronegativity value from the larger one.
3. Now, use the formula:
Percent ionic character = [(1 - e^(-Δχ))/ (1 + e^(-Δχ))]^2 × 100
In this case, we also need to convert the dipole moment (μ) from Debye (D) units to Coulomb-meter (C·m) by using the conversion factor: 1 D = 3.336 × 10^(-30) C·m.
Let's calculate the percent ionic character step by step:
1. Determine the electronegativities of elements X and Y.
For example, assume element X has an electronegativity of 2.5 and element Y has an electronegativity of 3.0.
2. Calculate the electronegativity difference (Δχ).
In this case, Δχ = 3.0 - 2.5 = 0.5.
3. Convert the dipole moment (μ) from Debye units to Coulomb-meter (C·m).
Given μ = 1.76 D, the conversion factor is 1 D = 3.336 × 10^(-30) C·m.
So, μ = 1.76 × 3.336 × 10^(-30) C·m.
4. Calculate the percent ionic character.
Using the equation:
Percent ionic character = [(1 - e^(-Δχ))/ (1 + e^(-Δχ))]^2 × 100
Plug in the values:
Percent ionic character = [(1 - e^(-0.5))/ (1 + e^(-0.5))]^2 × 100.
Now, evaluate the expression and calculate the percent ionic character.
Note: The value of Δχ and the actual electronegativity values for elements X and Y would vary depending on the hypothetical molecule being referred to.