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3 of 3 objectives have lessons · 0 studied · 0 secure
What Cambridge says you should be able to do, in our words. Codes are the topic number plus the objective’s position.
Define covalent bonding as the electrostatic attraction between the nuclei of two atoms and a shared pair of electrons, and: (a) describe covalent bonding in molecules including hydrogen, H₂, oxygen, O₂, nitrogen, N₂, chlorine, Cl₂, hydrogen chloride, HCl, carbon dioxide, CO₂, ammonia, NH₃, methane, CH₄, ethane, C₂H₆, and ethene, C₂H₄; (b) understand that elements in Period 3 can expand their octet, including in sulfur dioxide, SO₂, phosphorus pentachloride, PCl₅, and sulfur hexafluoride, SF₆; (c) describe coordinate (dative covalent) bonding, including in the reaction of ammonia and hydrogen chloride gases to form the ammonium ion, NH₄⁺, and in the Al₂Cl₆ molecule.
Taught in: Coordinate (dative) bonds: one atom brings both electrons, Double and triple bonds: O₂, N₂, CO₂ and C₂H₄, Breaking the octet rule: SO₂, PCl₅ and SF₆, Covalent bonds: sharing a pair of electrons · 24 questions
(a) Describe covalent bonds in terms of orbital overlap giving σ and π bonds: σ bonds form by direct overlap of orbitals between the bonding atoms, and π bonds form by sideways overlap of adjacent p orbitals above and below the σ bond; (b) describe how σ and π bonds form in molecules including H₂, C₂H₆, C₂H₄, HCN and N₂; (c) use the concept of hybridisation to describe sp, sp² and sp³ orbitals.
Taught in: Hybridisation: sp³, sp² and sp orbitals, σ and π bonds: head-on versus sideways overlap · 12 questions
(a) Define bond energy as the energy required to break one mole of a particular covalent bond in the gaseous state, and 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.
Taught in: Bond energy and bond length, Using bond energies to compare reactivity · 13 questions