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Bonding

AQA AS-level ChemistryTopic 3 of 1630 lessons

Revision notes for Bonding in AQA Chemistry (7404). Every lesson in BrainCake comes with R.E.C.I.P.E. recall steps, a quick check and spaced reviews.

  1. Ionic BondingIonic bonding is the electrostatic attraction between oppositely charged ions.
  2. Sodium ChlorideSodium chloride has ionic bonding.
  3. Magnesium OxideMagnesium oxide has ionic bonding.
  4. Ionic LatticesIn an ionic compound each ion attracts oppositely charged ions in all directions.
  5. Properties of Ionic CompoundsThese strong electrostatic forces of attraction mean that ionic compounds have a high melting and boiling point.
  6. Covalent bonds and Small MoleculesA covalent bond is a localised bond formed as a strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.
  7. Single and Double Covalent BondsPairs of electrons that are not involved in covalent bonding are called lone pairs.
  8. Co-ordinate BondingA dative covalent bond or a co-ordinate bond is a covalent bond in which the shared pair of electrons has been supplied by only one of the bonding…
  9. Metallic BondingAll metals are solid at room temperature with the exception of mercury.
  10. Properties of MetalsMost metals have strong metallic bonds, high electrical conductivity in the solid and liquid states and high melting and boiling points.
  11. ElectronegativityElectronegativity is the attraction of a bonded atom for the pair of electrons in a covalent bond.
  12. Trends in ElectronegativityElectronegativity is the power of an atom to attract the pair of electrons in a covalent bond.
  13. Polar Covalent BondsIn a non-polar bond, the bonded electron pair is shared equally between the two bonded atoms because either the atoms have the same or similar…
  14. Dipole-Dipole ForcesIf you compare fluorine molecules F-F with H-Cl molecules, the molecules have the same shape and number of electrons.
  15. Van der Waals forcesIntermolecular forces are weak interactions between the dipoles of molecules.
  16. Hydrogen BondingHydrogen bonds are permanent dipole-dipole interactions between the hydrogen in a H-F, H-N or H-O bond and an electronegative atom containing a lone…
  17. Boiling Point of HydridesThe boiling points of hydrides generally increase across a period from groups 4 to 7.
  18. The Importance of Hydrogen BondingHydrogen bonds are about 10% the strength of covalent bonds, but when there are a lot of them, their effect can be significant.
  19. Electron Pair Repulsion TheoryThe electron pair repulsion theory can be used to predict the shape and bond angles of covalent molecules and polyatomic ions.
  20. Two Pairs of ElectronsIf there are two pairs of electrons around the atom the molecule is linear with a bond angle of 180°.
  21. Three Pairs of ElectronsThe maximum number of covalent bonds that can be formed by each atom sharing one of its electrons is equal to the number of outer shell electrons.
  22. Four Pairs of ElectronsCarbon is in group 4 so methane CH4 has four C-H bonds.
  23. Five Pairs of ElectronsPCl5 has three chlorine atoms around a central phosphorus atom arranged in a plane 120° apart and two atoms above and below the plane with a bond…
  24. Six Pairs of ElectronsThe octet rule and expanded octet rule determines how many valence electrons there are.
  25. Bonding-Pair Lone-Pair RepulsionLone pairs affect the bond angle.
  26. Heating a Solid, Liquid or GasThe three states of matter are solid, liquid and gas.
  27. CrystalsCrystals are solid with regularly arranged particles held together by electrostatic forces of attraction.
  28. DiamondMost non-metals exist as simple covalent molecules.
  29. Graphite and GrapheneGraphite is a giant covalent structure.
  30. FullerenesCarbon atoms can join together to form hollow cages of various shapes called fullerenes.

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