please answer to my questions also

Dear Suchita,

3.1 - Periodic trends NaAr (the third period)

Characteristic	Trend (left to right)	Reason
Atomic radius	decreases in size from left to right	increased attractive force (acting on the same energy shell) from the nucleus as the number of protons (and hence the nuclear charge) increases
Ionic radius	decreases across the period until formation of the negative ions then there is a sudden increase followed by a steady decrease to the end	In general as above. The sudden increase on formation of negative ions is due to the new (larger) outer shell
Electronegativity	Increases	More electron attracting power of the larger nuclear charge as we move to the right
Metallic character	Decreases - Na, Mg, Al metals; Si metalloid; P, S, Cl, Ar non-metals	Metallic character is a measure of the ease of loss of electrons from the outer shell. This decreases with increasing nuclear charge.
Oxides	Na, Mg - alkaline Al - amphoteric Si, P, S, Cl -acidic
Chloride character	NaCl - ionic MgCl2 - some covalent character AlCl3 - covalent The remainder covalent	Increasing charge density of the positive ion polarises the chloride ion as we move to the right hand side
Melting point	NaAl steady increase	Increasing availability of electrons in the metallic bonding associated with greater charge density of the metal ion
	Si massive increase	Si giant macromolecular structure
	P large decrease	P4 molecules
	S small increase	S8 molecules
	Cl  Ar decrease	Cl2 molecules and Ar atoms

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