T3+Brendan

Brendan Halse Task 3

Question 1
 * Element || Proton Number Z || First Ionisation Energy (kJ/mol) ||
 * Li || 3 || 520 ||
 * Na || 11 || 496 ||
 * K || 19 || 419 ||
 * Rb || 37 || 403 ||
 * Cs || 55 || 376 ||

Question 2/4

Question 3 As you move down the group ionisation energy decreases, which on the graph is shown by the blue line as it goes from Li to Cs the line decreases in height or it could be said it has a negative gradient.

Question 5 As you move down the group the atomic radius increases as you go down the group, on the graph it is shown by the red line and it has a positive gradient as it goes from Li to Cs.

Question 6 As you go down the group reactivity increases because first ionisation energy decreases therefore it is easier to remove the electrons thus it reacts with other elements more easily. 2Na + 2H2O --> 2NaOH + H2 is a reaction that results in a small fire from the Na. however 2Cs + 2H2O --> 2CsOH + H2 is a reaction that results in a violent explosion, a small amount, only a couple of grams, can blow up a bathtub.

Question 7 Group 2 does show a similar trend to group 1 because as you go down the group there are more electron shells thus atomic radius increases and because atomic radius has increased the attraction of the outer electrons to the nucleus is less therefore first ionisation energy has also decreased.

Question 8 Question 9
 * Element || Proton Number Z || First Ionisation Energy (kJ/mol) ||
 * Li || 3 || 520 ||
 * Be || 4 || 900 ||
 * B || 5 || 801 ||
 * C || 6 || 1806 ||
 * N || 7 || 1402 ||
 * O || 8 || 1314 ||
 * F || 9 || 1681 ||
 * Ne || 10 || 2081 ||

Question 10 In general as you move across the period the first ionisation energy increases. I would say this because even thoguh there is great fluctuation it shows a general trend towards increasing.

Question 11 Question 12
 * Element || Proton Number Z || Electronegativity (Pauling) ||
 * Li || 3 || 0.98 ||
 * Be || 4 || 1.57 ||
 * B || 5 || 2.04 ||
 * C || 6 || 2.55 ||
 * N || 7 || 3.04 ||
 * O || 8 || 3.44 ||
 * F || 9 || 3.98 ||
 * Ne || 10 || 0 ||

Question 13 In general as you move across the period electronegativity increases. Looking at the graph it is obvious that as you go from Li to F the graph has a very positive gradient.

Question 14 As you go across the period reactivity does something similar to a parabola in that in the centre it is at its lowest point and is increasing as you go outward form there. This is because electronegativity is very high at one end and very low at the other so at one end electrons are given away very easily but at the other electrons are taken or accepted very easily.

Question 15 Neon doesn't follow the trend because it has a full shell of outer electrons therefore it does not have a charge that wants to gain an electron.