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- 1name the first period oxidesNa2O, MgO, AlO3, SiO2, P2O5, So2,Cl2O
- 2name the first period chloridesNaCl, MgCl2, AlCl3, SiCl4, PCl3, SCl2, Cl2
- 3IE patternsPeaks 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. - 4Pattern in atomic radius and whyDecreases left to right,
Peaks at group one dips at group 7 & 0
increase in proton number = increase in pulling electrons towards its centre. - 5When 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 3right side
P2- Oxygen, Fluorine are diatomic
P2 - Neon is Monoatomic
P3- Chlorine diatomic
P3- Argon is monoatomic - 6Are 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 - 7Why 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. - 8IN period 2 and three which molecules have the highest bp and mp? WhyP2 = Carbon, P3 = Silicon
Both form giant macro molecules with covalent bonding = makes them strong with lots of bonds which need breaking for melting/boiling.
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- A-Levels periodicity Flashcards on Untitled_2, created by Shell Wood on 28/05/2013.
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