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Question	Answer
When looking at the structure of elements is it more likely that they will be diatomic or monoatomic on the left or right side of the period? Name examples from period 2 and 3	right side P2- Oxygen, Fluorine are diatomic P2 - Neon is Monoatomic P3- Chlorine diatomic P3- Argon is monoatomic
Are chemicals in periods 2 and 3 more likely to bond via metallic bonding if they are on the left or right side of the period? Examples?	Left side Sodium, lithium
Why do noble gases take the most energy for them to be Ionised?	Because they are stable with full outer shells and so to remove an electron a lot of energy is needed. Also NG are generally smaller in diameter and so the protons have a greater hold on the electron.
IN period 2 and three which molecules have the highest bp and mp? Why	P2 = Carbon, P3 = Silicon Both form giant macro molecules with covalent bonding = makes them strong with lots of bonds which need breaking for melting/boiling.
name the first period oxides	Na2O, MgO, AlO3, SiO2, P2O5, So2,Cl2O
name the first period chlorides	NaCl, MgCl2, AlCl3, SiCl4, PCl3, SCl2, Cl2
IE patterns	Peaks in IE for noble gases. Lowest values are group 1 Alkali Metals. As you go across the period the IE increases as the proton number increases.
Pattern in atomic radius and why	Decreases left to right, Peaks at group one dips at group 7 & 0 increase in proton number = increase in pulling electrons towards its centre.

Resource summary

	Created by Shell Wood over 11 years ago