metallic bonding - positive ions in a sea of delocalised electrons, covalent network bonding - giant lattice with strong covalent bonds, monatomic bonding - individual atoms attracted by weak intermolecular forces, non-polar bonds - same / similar electronegativities gives equal sharing, polar bonds - differing electronegativities leads to unequal sharing (dipole), ionic bonds - very different electronegativities leads to transfer of electrons therefore ions, London dispersion forces - attractions between temporary dipoles caused by electron cloud wobble, pd-pd - attraction between permanent dipoles, hydrogen bonds - attraction between bonds of HF HO HN, electronegativity - measure of attraction for bonding electrons, atom size / covalent radius - half the distance between two covalently bonded nuclei, across a period - increasing nuclear charge pulls electrons in tight, down a group - increasing electron shells shield the nuclear charge meaning electrons held loose, first ionisation energy - energy to remove a mole of electrons from a mole of gaseous atoms, further ionisation energy - always increases but sharp spikes for a new shell (less shielding),

H 1.1 and 1.2 review

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