Electrostatic Forces Definition

Chemistry Glossary Definition of Electrostatic Forces

Electrostatic forces
Electrostatic forces are forces caused by electric charge. PM Images/Getty Images

There are several types of forces in science. Physicists deal with the four fundamental forces, which are the gravitational force, weak nuclear force, strong nuclear force, and electromagnetic force. The electrostatic force is associated with the electromagnetic force. Here is the definition of electrostatic force, its history, and a look at how it's calculated.

Key Takeaways: Electrostatic Force

  • The electrostatic force is also known as the Coulomb force or Coulomb interaction.
  • It is the attractive or repulsive force between two electrically charged objects.
  • Like charges repel each other while unlike charges attract each other.
  • Coulomb's law is used to calculation the strength of the force between two charges.

Electrostatic Forces Definition 

Electrostatic forces are attractive or repulsive forces between particles that are caused by their electric charges. This force is also called the Coulomb force or Coulomb interaction. It is named for the French physicist Charles-Augustin de Coulomb, who described the force in 1795.

How the Electrostatic Force Works

The electrostatic force acts over a distance of about one-tenth the diameter of an atomic nucleus or 10-16 m. Like charges repel, while unlike charges attract. So, two positively charged protons repel each other as do two cations, two negatively charged electrons, or two anions. Protons and electrons are attracted to each other. So are cation and anions.

Why Protons Don't Stick to Electrons

While protons and electrons are attracted by electrostatic forces, protons don't leave the nucleus to get together with electrons because they are bound to each other and to neutrons by the strong nuclear force. The strong nuclear force is much more powerful than the electromagnetic force, but it acts over a much shorter distance. In a sense, protons and electrons are touching in an atom because electrons have properties of both particles and waves. The wavelength of an electron is comparable in size to an atom, so electrons can't get closer than they already are.

Calculating the Electrostatic Force Using Coulomb's Law

The strength or force of the attraction or repulsion between two charged bodies can be calculated using Coulomb's law:

F = kq1q2/r2

Here, F is the force, k is proportionality factor, q1 and q2 are the two electric charges, and r is the distance between the centers of the two charges. In the centimeter-gram-second system of units, k is set to equal 1 in a vacuum. In the meter-kilogram-second (SI) system of units, k in a vacuum is 8.98 × 109 newton square meter per square coulomb. While protons and ions have measurable sizes, Coulomb's law treats them as point charges.

It is important to note the force between two charges is directly proportional to the magnitude of each charge and inversely proportional to the square of the distance between them.

Verify Coulomb's Law

You can set up a very simple experiment to verify Coulomb's law. Suspend two small balls with the same mass and charge from a string of negligible mass. Three forces will act upon the balls: the weight (mg), the tension on the string (T), and the electric force (F). Because the balls carry the same charge, they will repel each other. At equilibrium:

T sin θ = F and T cos θ = mg

If Coulomb's law is correct:

F = mg tan θ

The Importance of Coulomb's Law

Coulomb's law is extremely important in chemistry and physics because it describes the force between parts of an atom and between atoms, ions, molecules, and parts of molecules. As the distance between charged particles or ions increases, the force of attraction or repulsion between them decreases and the formation of an ionic bond becomes less favorable. When charged particles move closer to each other, energy increases and ionic bonding is more favorable.


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  • Coulomb, Charles Augustin (1788) [1785]. "Second mémoire sur l'électricité et le magnétisme". Histoire de l’Académie Royale des Sciences. Imprimerie Royale. pp. 578–611.
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