Here's a breakdown:
* Nature of the force: It's an attractive force due to the opposite charges of the electron (negative) and the proton in the nucleus (positive).
* Formula: The force (F) is calculated using Coulomb's Law:
F = k * (q1 * q2) / r²
Where:
* k is Coulomb's constant (approximately 8.98755 × 10⁹ N·m²/C²)
* q1 and q2 are the magnitudes of the charges (in Coulombs)
* r is the distance between the charges (in meters)
* In the case of a hydrogen atom:
* q1 = charge of the electron = -1.602 × 10⁻¹⁹ C
* q2 = charge of the proton = +1.602 × 10⁻¹⁹ C
* r = the average distance between the electron and the proton (the Bohr radius, approximately 5.29 × 10⁻¹¹ m)
* Note: The force is constantly changing due to the electron's movement around the nucleus. The formula above calculates the average force.
In summary, the force between the electron and nucleus in a hydrogen atom is a fundamental electrostatic force that keeps the atom together.
