AS Level Chemistry - Unit 3.4 Covalent bonding and coordinate (dative covalent) bonding

**This Powerpoint specifically uses the Cambridge AS Level Chemistry Syllabus (9701) and covers all criteria for – Unit 3.4 Covalent bonding and coordinate (dative covalent) bonding
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Students will be able to -

1 define covalent bonding as electrostatic attraction between the nuclei of two atoms and a shared pair of
electrons
(a) describe covalent bonding in molecules including:
• hydrogen, H2
• oxygen, O2
• nitrogen, N2
• chlorine, Cl 2
• hydrogen chloride, HCl
• carbon dioxide, CO2
• ammonia, NH3
• methane, CH4
• ethane, C2H6
• ethene, C2H4
(b) understand that elements in period 3 can expand their octet including in the compounds sulfur dioxide, SO2, phosphorus pentachloride, PCl 5, and sulfur hexafluoride, SF6
© describe coordinate (dative covalent) bonding, including in the reaction between ammonia and
hydrogen chloride gases to form the ammonium ion, NH4+, and in the Al 2Cl 6 molecule

2 (a) describe covalent bonds in terms of orbital overlap giving σ and π bonds:
• σ bonds are formed by direct overlap of orbitals between the bonding atoms
• π bonds are formed by the sideways overlap of adjacent p orbitals above and below the σ bond
(b) describe how the σ and π bonds form in molecules including H₂, C₂H₆, C₂H₄, HCN and N₂
© use the concept of hybridisation to describe sp, sp² and sp³ orbitals

3 (a) define the terms:
• bond energy as the energy required to break one mole of a particular covalent bond in the gaseous state
• bond length as the internuclear distance of two covalently bonded atoms
(b) use bond energy values and the concept of bond length to compare the reactivity of covalent molecules

**Every Powerpoint includes learning objectives, a starter and plenary, suitable activities and review questions with mark scheme. We also provide a free pdf version of the file so it can easily be printed for students as a handout or uploaded to the school VLE system
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