[gpulse]

are lewis structural diagrams different from ionic bonding, covalent/molecular bonding? how to draw lewis s. d. for ionic, polar, non polar.

[Big-Daddy]

are lewis structural diagrams different from ionic bonding, covalent/molecular bonding? how to draw lewis s. d. for ionic, polar, non polar.

A Lewis structure makes no distinction between ionic and covalent: it rather assumes firstly that all molecules are covalent, and secondly that there are no differences in electronegativity. Differences in electronegativity will affect which atom in the molecule gains or loses the extra electrons in the case of an ion, but finally we are talking about covalent molecules with no consideration for ionic character when we refer to Lewis structures.

It's also interesting to note the difference between an "oxidation number" - the stock and trade of an ionic understanding - and the "formal charge", its covalent equivalent. You should look these phrases up if you are interested, but basically certain atoms follow certain rules and the oxidation states of the others are based around them. For instance, Group 1 metals always have an oxidation state of +1 and Group 2 of +2; F always has an oxidation state of 0 or -1; H usually has an oxidation state of +1, except with Group 1 or 2 metals where it has an oxidation state of -1, and in H2 where it is 0; O usually has an oxidation state of -2 (unless forced into +1 or higher with F, or kept to -1 with H or a Group 1 metal); halogens usually have -1 oxidation states; etc. Formal charge, meanwhile, is defined specifically by considering how many electrons are normally in the outer shell of the atom ("valence electrons") and then using your Lewis structure to check how any are there in the atom now (electrons = unbonded electrons + 1/2 * electrons in bonding pairs) and take away the valence number from this number of electrons to find the formal charge on the atom currently.

Hope this is of some help