This introduction covers The Art of Sharing within Covalent Bonding for GCSE Chemistry. Revise Covalent Bonding in Bonding & Structure for GCSE Chemistry with 25 exam-style questions and 20 flashcards. This is a high-frequency topic, so it is worth revising until the explanation feels precise and repeatable. It is section 1 of 12 in this topic. Use this introduction to connect the idea to the wider topic before moving on to questions and flashcards.
Topic position
Section 1 of 12
Practice
25 questions
Recall
20 flashcards
📖 The Art of Sharing
What actually holds a covalent bond together is simultaneous attraction from two nuclei. When two non-metal atoms are close enough, both positive nuclei attract the same pair of electrons at the same time. The shared electron pair sits between both nuclei, pulled toward each simultaneously. Neither atom "owns" the electrons outright — both nuclei exert a continuous pull on them. This dual attraction is what creates the bond. The stronger each nucleus's pull on electrons (electronegativity), the more the shared pair tilts toward that atom.
We've seen how metals give electrons to non-metals in ionic bonding. But what happens when TWO non-metals meet? Both nuclei have a strong pull on electrons. Neither will donate electrons to the other, because both are attracted to electrons strongly enough to hold onto them.
The result is not a compromise between competing desires — it is simultaneous attraction. Both nuclei can hold onto the same shared pair of electrons at the same time. The shared electrons sit between the two nuclei and are attracted to both of them at once. This bilateral attraction — two nuclei pulling on the same electron pair — is what holds the atoms together and constitutes the covalent bond.
Take hydrogen (H₂) as the simplest example. Each hydrogen atom has just 1 electron, but needs 2 to fill its outer shell. When two hydrogen atoms approach each other, they each contribute their single electron to a shared pair. Now both atoms can "claim" 2 electrons — the shared pair belongs to both of them. This shared pair of electrons IS the covalent bond.
The key insight: In covalent bonding, electrons are SHARED, not transferred. Neither atom becomes an ion — they stay neutral. They form a MOLECULE — a distinct particle with a fixed number of atoms held together by covalent bonds.
And here's something crucial for understanding properties: the covalent bonds within a molecule are incredibly strong. But the forces BETWEEN different molecules are very weak. This is why water (covalent molecules) boils at just 100°C, while salt (ionic lattice) needs 801°C to melt!