Covalent Bonding
Use this landing page to move quickly between the main covalent bonding revision pages for Topic 3. Each card links to a focused page covering covalent bond formation, dative covalent bonding and electronegativity.
Choose a Covalent Bonding Page
Covalent bonding forms when atoms share pairs of electrons. These pages separate the key ideas so that students can revise ordinary covalent bonds, dative covalent bonds and how electronegativity affects bond polarity.
Key idea: A covalent bond is a shared pair of electrons attracted to the nuclei of both bonded atoms. Differences in electronegativity can make that shared pair unevenly distributed.
Nature of Covalent Bonding
Revise how atoms share electron pairs, including dot-and-cross diagrams and simple molecular substances.
Start revisingDative Covalent Bonding
Learn how a dative covalent bond forms when both electrons in the shared pair are donated by the same atom.
Start revisingGiant Covalent Structures
Compare diamond, graphite and graphene: how each is bonded, and why the structure explains hardness, melting point and electrical conductivity.
Start revisingSigma and Pi Bonds and Hybridisation
How σ and π bonds form by orbital overlap, the bonding in N₂ and HCN, and sp, sp² and sp³ hybridisation (3.4.2).
Start revisingBond Energy and Bond Length
Defining bond energy and bond length, how they are linked, and using them to compare the reactivity of covalent molecules (3.4.3).
Start revisingElectronegativity
Connect electronegativity differences with polar bonds, uneven electron density and partial charges in covalent molecules.
Start revisingHow to Use These Pages
Start with the nature of covalent bonding to secure electron-pair sharing and dot-and-cross diagrams. Then move to dative covalent bonding to understand how one atom can provide both electrons in the shared pair. Finally, use electronegativity to explain bond polarity and uneven electron density.
Exam focus: For covalent bonding, distinguish clearly between shared electron pairs, lone pairs, dative covalent bonds and polar bonds. Use precise language about electron density rather than vague statements such as “the atom pulls harder”.
Copyright notice: This revision page, including its written explanations, layout and teaching sequence, is produced for Online Learning System by Dr. Mohammed Al-Fatah. It is intended for student revision and may not be copied, redistributed or republished without permission.
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