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Recent Activity Show 0 new item s Loading…. The remaining elements in period 3 do not conduct electricity. They have no free electrons that can move around and carry charge from place to place. Metallic bonding is often incorrectly described as the attraction between positive metal ions and delocalised electrons. However, metals still consist of atoms, but the outer electrons are not associated with any particular atom.
In a similar way, graphite a non-metal also has delocalised electrons. However, you don't see the idea that it consists of carbon ions.
The giant lattice structure of silicon is similar to that of diamond. This allows it to carry more charge per unit time, leading to a higher rate of conductivity.
Similarly with regards to ionic lattices, a greater charge means there will be more ions formed per molecule that is made molten. So one mol of NaCl will have 2 x 6. So, MgCl2 has more ions to conduct electricity and thus shows greater conductivity. I'm not sure if it has much to do with the actual 'ease' of breaking bonds. Both NaCl and MgCl2 would have to be in a molten state to be able to conduct electricity anyway, so I don't think it plays a role for ionic compounds.
For metallic compounds, again, as they are simply ions surrounded by electrons there isn't any bond-breaking to be done. Sign up to join this community. The best answers are voted up and rise to the top. Stack Overflow for Teams — Collaborate and share knowledge with a private group. Create a free Team What is Teams? Well I think it generally goes down because the energy separation between S and P bands increase as principal quantum number n increases.
But I'm not sure what factor overrides this to cause Na to have a significantly higher conductivity than Li. Any ideas will be helpful! Enthalpy Chemist Sr. Conductivity has no direct link with orbital separation. It is linked with the electron's "effective" mass in the solid, which heavy software can compute but is a very indirect result of the crystal form and the underlying orbitals, and in pure metals, with the temperature and allegedly the dispersion relation of phonons, again an indirect consequence of the crystal form and the underlying orbitals.
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