>>12565754read textbook/lecture notes. summary first then chapters.
atoms are not arranged randomly on a periodic table.
the organization reflects trends in an atom's behaviour.
bonding is an interaction between atoms.
the bonds are affected by things like electronegativity (willingness of a species to 'hold onto' electrons) which itself arises from an atom's structure (c.f. valence shells, #protons etc. )
the differences in electronegativity are a good rule-of-thumb for whether a bond is ionic or covalent.
ionic = large electronegativity difference.
covalent = not so much a gradient.
you also have partial charges (dipoles), which can be viewed as a key factor in intermolecular forces like hydrogen bonds.
intermolecular forces exist because no single bond or species exists in a vacuum. there's other shit around.
dipoles, i.e. partially positive/ partially negative underpin hydrogen bonding.
hydrogen has partial positive charge as it is not as electronegative (why? look at the structure of hydrogen and # of protons, # electrons)
oxygen is much more electronegative.
the resulting bond produces a gradient, and water molecules interact with eachother, all posessing a partial negative charge about the oxygen leading to an arrangment known as hydrogen 'bonding' -- think of each molecule like a little magnet.
