Period 3 oxides and chlorides (Periodicity of chemical properties - Part 4)

Periodicity of chemical properties (Chapter 10 - Part 4):
Going across a period the elements get more electronegative as electrons are more strongly attracted by the increasing positive nuclear charge.
2- The electronegativity and acidic/basic nature of the Period 3 oxides:
a.  Na, Mg, and Al form an ionic bond with oxygen in their oxides forming a large lattice.
b. Silicon bond covalently with oxygen to form SiO2 that has large molecular lattice.
3- The high melting points of ionic oxides make them suitable to be used in:
a. magnesium oxide to line the inside of furnaces.
b.  aluminum oxide and silicon dioxide are used to make ceramics, with giant covalent structures designed to withstand high temperatures and provide electrical insulation.
c. P, S and chlorine bond covalently with oxygen forming small molecules.
 4- Chlorides of Period 3 elements:
Chlorine has electronegativity equal to -1 where the rest of period three elements form positive ions with chlorine because of lower electronegativity comparing to chlorine.
a. The first three elements chlorides dissolve in water forming hydrate ions.
b. AlCl3 dimerize into Al2Cl6 solid hydrate that breaks down releasing hydrogen ions that react with chlorine atoms forming white fumes.
c. Sulfur and phosphorus both form chlorides that hydrolyze forming hydrogen chloride fumes.
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