To calculate the dipole moment assuming one elementary charge of opposite kinds located at each nucleus, and to determine the percentage ionic character of KCl, we will use the concepts of charge and distance in the dipole moment equation, and understand the measure of ionic character compared to a hypothetical purely ionic bond.

Step 1: Calculating theoretical dipole moment
The elementary charge (e) is $$ 1.602 \times 10^{-19} $$ Coulombs. If KCl were purely ionic, the potassium and chlorine atoms would carry charges of +e and -e respectively. The dipole moment $$ \mu $$ is calculated by the formula:

where: - $$ q $$ is the charge in Coulombs (+e for K⁺ and -e for Cl^-) - $$ d $$ is the separation distance between the charges, which is 2.6 $$ \times 10^{-10} $$ meters. Thus, using the values: $$ \mu = 1.602 \times 10^{-19} \, \text{Coulombs} \times 2.6 \times 10^{-10} \, \text{meters} = 4.1652 \times 10^{-29} \, \text{Coulomb meters} $$

Step 2: Actual dipole moment of KCl
The actual measured dipole moment of KCl is given as 3.336 $$ \times $$ 10^-29 Coulomb meters. This is due to the actual electron distribution in the bond being not purely ionic.

Step 3: Percentage ionic character
The percentage ionic character can be calculated by comparing the actual dipole moment to the theoretical dipole moment for fully ionic charges, using the formula:

Substituting the values we have:

This calculation shows that while KCl is primarily ionic, it has less than 100% ionic character, indicating some degree of covalent character in its bonding, where the electron distribution is not completely transferred but shared to a certain extent.