Covalent Bonding
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.
These pages cover electronegativity, ionic bonding and giant ionic lattices, metallic bonding, and covalent bonding with sigma and pi bonds, dative bonds and giant covalent structures.
They then cover the shapes and bond angles of molecules, polar molecules, and intermolecular forces with hydrogen bonding and the anomalous properties of water.
Revision Notes
6 revision notes, in the order the specification teaches them.
Nature of Covalent Bonding
Revise how atoms share electron pairs, including dot-and-cross diagrams and simple molecular substances.
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Dative Covalent Bonding
Learn how a dative covalent bond forms when both electrons in the shared pair are donated by the same atom.
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Giant Covalent Structures
Compare diamond, graphite and graphene: how each is bonded, and why the structure explains hardness, melting point and electrical conductivity.
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Sigma 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).
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Bond 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).
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Electronegativity
Connect electronegativity differences with polar bonds, uneven electron density and partial charges in covalent molecules.
Start revisingSummary Map
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Summary map
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Covalent Bonding Map
Cambridge International AS & A Level Chemistry · Topic 3 Chemical bonding · Covalent bonding
The whole section on one A4 page: covalent and coordinate bonds, expanded octets, σ and π bonds, hybridisation, bond energy and length, and electronegativity.
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Revision Game
Match reagents to products, with your board's reagents and conditions.
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Specification
Every specification point in this topic, in the exam board's own words. Rate how confident you are with each one.
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Self-assessment · 27 points
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3.4.1
- 3.4.1
define covalent bonding as electrostatic attraction between the nuclei of two atoms and a shared pair of electrons
Revise - b i
understand that elements in period 3 can expand their octet including in the compound sulfur dioxide, SO2
Revise - b ii
understand that elements in period 3 can expand their octet including in the compound phosphorus pentachloride, PCl5
Revise - b iii
understand that elements in period 3 can expand their octet including in the compound sulfur hexafluoride, SF6
Revise
3.4.2
- a iii
describe that π bonds are formed by the sideways overlap of adjacent p orbitals above and below the σ bond
Revise
3.4.3
3.6.2
3.7.1
- b
use dot-and-cross diagrams to illustrate covalent bonding including the representation of any compounds stated in 3.4 and 3.5 (dot-and-cross diagrams may include species with atoms which have an expanded octet or species with an odd number of electrons)
Revise - c
use dot-and-cross diagrams to illustrate coordinate bonding including the representation of any compounds stated in 3.4 and 3.5
Revise
4.2.1
- c i
describe, in simple terms, the lattice structure of a crystalline solid which is giant molecular, including silicon(IV) oxide
Revise - c ii
describe, in simple terms, the lattice structure of a crystalline solid which is giant molecular, including graphite
Revise - c iii
describe, in simple terms, the lattice structure of a crystalline solid which is giant molecular, including diamond
Revise
4.2.2
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