Electrostatic Attraction
Summary: Electrostatic attraction is the force of attraction between oppositely charged objects or particles; it is the force that holds ions together in ionic bonding, binds metal ions to delocalised electrons in metallic bonding, and holds electrons around the nucleus in every atom. Tags: igcse chemistry Created: 2026-07-18
Electrostatic attraction is the force of attraction between oppositely charged objects or particles — positive attracts negative, while like charges repel. In chemistry it is the fundamental “glue” behind chemical bonding: it is the force named explicitly in the definition of the Ionic Bond (“the strong electrostatic attraction between oppositely charged ions”) and in the definition of Metallic Bonding (the attraction between positive metal ions and the sea of delocalised electrons). It also operates inside every atom, where the positively charged nucleus attracts the negatively charged electrons in their shells (see Atomic Structure), and between the nuclei and shared electron pairs in Covalent Bonding. The strength of an electrostatic attraction increases with larger charges and with smaller distances between them, which is why small, highly charged ions form particularly strong bonds. This page covers electrostatic attraction in the chemistry bonding context; the physics treatment of charge, fields and Coulomb’s law lives in the Concepts page Electrostatic force.
The Force Between Opposite Charges
Two simple rules govern electrostatic forces:
| Charges | Interaction |
|---|---|
| Positive and negative (opposite) | Attract |
| Positive and positive, or negative and negative (like) | Repel |
The force is stronger when:
- the charges are larger (e.g. a 2+ ion attracts a 2− ion more strongly than a 1+ ion attracts a 1− ion), and
- the charged particles are closer together (smaller ions can approach more closely, giving stronger attraction).
Role in Ionic Bonding
When a metal atom transfers electrons to a non-metal atom, Positive Ions (Cations) and Negative Ions (Anions) are produced. The electrostatic attraction between these oppositely charged ions is the Ionic Bond:
- The attraction is strong — large amounts of energy are needed to overcome it, giving Ionic Compounds their high melting and boiling points.
- The attraction is non-directional — each ion attracts every oppositely charged neighbour, so the ions pack into a giant ionic lattice of alternating charges rather than forming molecules.
- Repulsion matters too: if layers of the lattice are forced to slide so that like charges align, the ions repel and the crystal shatters — the reason ionic compounds are brittle (see Ions and Ionic Bonds).
Role in Metallic Bonding
In a metal, each atom releases its outer electrons into a shared “sea”, leaving a lattice of positive metal ions. The metallic bond is the electrostatic attraction between the positive metal ions and the delocalised electrons moving among them (see Metallic Bonding and Delocalised Electron):
- More delocalised electrons per atom and smaller ions give a stronger attraction, and so a higher melting point.
- Because the attraction is between the ions and the mobile electron sea rather than between specific pairs of particles, layers of ions can slide without breaking the bonding — metals are malleable where ionic compounds are brittle.
Role Within the Atom
Electrostatic attraction also holds every atom together:
- The nucleus contains positively charged protons; the negatively charged electrons in their shells are attracted to it (see Atomic Structure and Electron Shell).
- Electrons in shells closer to the nucleus are attracted more strongly; outer electrons are further away and partly shielded by inner shells, which is why they are the electrons lost or shared in bonding (see Valence Electron).
- This attraction underlies Periodic Table Trends: across a period the nuclear charge increases, pulling the outer shell in more strongly; down a group the outer electrons are further from the nucleus and lost more easily.
In Covalent Bonding the same force appears in a different arrangement: both nuclei are electrostatically attracted to the shared pair of electrons between them, and this attraction holds the two atoms together.
Summary of Bonding Contexts
| Context | Attraction between | Result |
|---|---|---|
| Ionic Bond | Oppositely charged ions | Giant ionic lattice |
| Metallic Bonding | Positive metal ions and delocalised electrons | Giant metallic lattice |
| Covalent Bonding | Nuclei and shared electron pair(s) | Molecules or giant covalent structures |
| Within an atom | Nucleus (protons) and electrons | Electrons held in shells |
Sources
- Cambridge IGCSE Chemistry 0620 Syllabus (2023-2025) — Sections 2.4–2.6 (Ions and ionic bonds; covalent bonds; metallic bonding), Cambridge Assessment International Education
Common Misconceptions
| Misconception | Reality |
|---|---|
| ”Electrostatic attraction is a weak force” | In bonding it is strong — it is the force behind ionic and metallic bonds, both of which need high temperatures to overcome |
| ”Only ionic compounds involve electrostatic attraction” | It operates in all bonding: ionic, metallic, covalent, and within every atom between nucleus and electrons |
| ”The attraction in an ionic lattice is between one pair of ions” | It acts in all directions — each ion attracts all oppositely charged neighbours throughout the lattice |
| ”Like charges can attract if the bond is strong enough” | Like charges always repel; only opposite charges attract — this repulsion is why ionic crystals are brittle |
| ”Electrostatic attraction and gravity hold electrons in the atom” | Gravity is negligible at atomic scales; it is the electrostatic attraction to the nucleus that holds electrons in their shells |