Coulomb's Law & Attractive Forces
- Coulomb's law describes the electrostatic force between two charged particles
- The formula for Coulomb's law is , where:
- Fcoulombic is the force between the charges
- k is Coulomb's constant
- q1 and q2 are the value of the charges
- r is the distance between the charges
- For a cation and anion in an ionic bond, Fcoulombic
- increases with increasing charge of each ion
- decreases with increasing ionic radius
Coulombic force between cations and anions
Diagram showing that the Coulombic force between a cation and anion decreases with increasing ionic radius and increases with increasing charge
- The greater the force between the charges
- the stronger the interaction between the ions
- the greater the bond energy (also known as lattice energy)
- the more negative the minimum potential energy of a stable ionic bond between the two ions
Worked example
The graph shows the potential energy of three potassium salts, X, Y, and Z, as a function of internuclear distance. Based on the data, what are the most likely identities of compounds X, Y, and Z?
|
X |
Y |
Z |
A. |
KI |
KBr |
KCl |
B. |
KBr |
KCl |
KI |
C. |
KCl |
KI |
KBr |
D. |
KCl |
KBr |
KI |
Answer:
- Each potassium salt contains a K+ ion and a halide ion with a 1- charge
- So, we do not need to consider the effect that charge has on internuclear distance or potential energy
- The ionic radius of the halide ions increases down the group, thus Cl- < Br- < I-
- As ionic radius increases
- the internuclear distance between the potassium and halide ions increases
- Fcoulombic between the ions decreases
- the lattice energy decreases
- the potential energy minimum becomes less negative
- So, KCl with the smallest halide ion will have the smallest internuclear distance and the most negative minimum potential energy
- KI with the largest halide ion will have the largest internuclear distance and the least negative minimum potential energy
- Therefore, the answer is D