Course review
Review each learning objective in this topic, then open its concept explanation or question set.
Learning objective
• Electrostatic attraction between shared electron pair and nuclei • Octet rule: tendency to achieve 8 valence electrons • Lewis formulas (up to 4 electron pairs per atom)
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Learning objective
• Single, double, triple bonds (1, 2, 3 shared pairs) • More bonds → shorter length, stronger bond
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Learning objective
• Both electrons from same atom • Identify coordination bonds; include transition element complexes at HL
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Learning objective
• Predict molecular shapes from electron domain repulsion • Electron domain and molecular geometry (up to 4 domains) • Include bond angles and lone-pair effects for common shapes
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Learning objective
• Results from electronegativity differences • Deduce polar bonds from electronegativity values and show bond dipoles
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Learning objective
• Depends on bond polarity + molecular geometry • Net dipole moment • Identify when bond dipoles cancel or produce a polar molecule/ion
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Learning objective
• Carbon allotropes: diamond, graphite, fullerenes, graphene • Silicon and silicon dioxide
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Learning objective
• London dispersion forces • Dipole-induced dipole • Dipole-dipole • Hydrogen bonding • Deduce IMF types from molecular size and polarity
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Learning objective
• Relative strength: London < dipole-dipole < hydrogen bonding • Effects on volatility, conductivity, solubility • Explain properties of covalent substances using IMF strength and molar mass
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Learning objective
• Separates components based on IMF attractions • Calculate and interpret RF values • Link mobile/stationary phase attraction to separation; operational details are not assessed
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Learning objective
• Multiple possible positions for double bonds • Deduce resonance structures and use the term delocalization
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Learning objective
• Important resonance example
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Learning objective
• Atoms with 5 or 6 electron domains • VSEPR for these species • Draw Lewis formulas and geometries for five- and six-domain species
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Learning objective
• Determine preferred Lewis formula • Use formal charge to compare valid Lewis structures
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Learning objective
• σ bonds: head-on orbital combination, electron density along bond axis • π bonds: lateral p-orbital combination, electron density on opposite sides
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Learning objective
• Mixing atomic orbitals to form hybrid orbitals • Relationships: Lewis formulas → electron domains → geometry → hybridization • Analyse hybridization and bond formation in molecules and ions
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