Period 3 chemistry
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The patterns the properties of the elements, oxides and chlorides of period 3 in the Periodic Table provide a good opportunity to test your understanding of chemical bonding, structure and the types of chemical change.
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Webguides
- Properties, structure and bonding of period 3 oxides
- Properties, structure and bonding of period 3 chlorides
- Bonding in aluminium chloride
Recently Asked Questions
- I am studying OCR AS Chemistry, and in my syllabus it tells me to appreciate that there is gradual transition from the extremes of ionic bonding to the extremes of covalent bonding. I have tried to find examples, or an explanation in my textbook, notes, and lots and lots of websites, but can't find anything. Can you help?
- How is it possible for the sulphur in sulphur trioxide to have 3 double bonds? If this were the case it would have an outer shell containing 12 electrons.
- The Nuffield Chemistry students’ book (on page 389) mentions that the introduction of some amount of covalency into an lattice is likely to make the lattice energy more negative than one might expect (in other words, it might make the lattice ‘stronger’). This, if I understand correctly, is because the deformation in electron clouds allow ions to attract each other more strongly. On page 391, the book states that Period 3 chlorides get less and less soluble as we go across period 3 - this makes sense to me, because the lattice energies get stronger, and the energy of hydration isn't likely to be able to overcome this large lattice energy. One page 390, however, the book states that as we go across period 3, the melting points of period 3 chlorides decrease - how is that possible if the lattice energies get more and more negative? Surely, melting involves breaking the lattice, and lattices with more covalent character (which are stronger) should be harder to melt...
Tests
updated: 09 July 2003
