Task 1 and 2
First ionisation energy – The first ionisation energy is the energy required to remove the most loosely held electron from one mole of gaseous atoms to produce one mole of gaseous ions each with a charge of +1.
The first ionisation decreases as you go down a group. This is because the electrons are getting further away from the nucleus meaning it is easier to remove the outer electron. There is also less shielding thus allowing the outer electron to be removed much more easily. As you go down the group the number of inner shells increases therefore the distance of the outer electrons from the nucleus also increases thus showing there is a weaker force of attraction on the outer electrons. There are also more shells meaning the shielding on the outer electrons from the nucleus would increase thus would mean there is less attraction. …show more content…
The atomic radius also decreases as the increased nuclear charge pulls the electrons towards it and the atom also gets smaller. As you go across a period, the number of protons added to the nucleus increases thus causing the nuclear charge to also increase. The outer electrons are much closer to the nucleus and therefore the attraction between the electrons and the nucleus is much stronger. This therefore shows that it is very difficult to remove the outer electron. Also, the electrons are added to the same shell thus meaning shielding would stay the same.
Aluminium has a lower ionisation energy than magnesium. This is because of the electronic configuration. The electronic configuration for aluminium is 1s2 2s2 2p6 3s2 3p1 and the electronic configuration for magnesium is 1s2 2s2 2p6 3s2. The outer electron for aluminium is in the p sub shell and the outer electron for magnesium is in the s sub shell. The energy in the p sub shell for aluminium is higher than that of the s sub shell for aluminium so less energy is needed to remove
First ionisation energy – The first ionisation energy is the energy required to remove the most loosely held electron from one mole of gaseous atoms to produce one mole of gaseous ions each with a charge of +1.
The first ionisation decreases as you go down a group. This is because the electrons are getting further away from the nucleus meaning it is easier to remove the outer electron. There is also less shielding thus allowing the outer electron to be removed much more easily. As you go down the group the number of inner shells increases therefore the distance of the outer electrons from the nucleus also increases thus showing there is a weaker force of attraction on the outer electrons. There are also more shells meaning the shielding on the outer electrons from the nucleus would increase thus would mean there is less attraction. …show more content…
The atomic radius also decreases as the increased nuclear charge pulls the electrons towards it and the atom also gets smaller. As you go across a period, the number of protons added to the nucleus increases thus causing the nuclear charge to also increase. The outer electrons are much closer to the nucleus and therefore the attraction between the electrons and the nucleus is much stronger. This therefore shows that it is very difficult to remove the outer electron. Also, the electrons are added to the same shell thus meaning shielding would stay the same.
Aluminium has a lower ionisation energy than magnesium. This is because of the electronic configuration. The electronic configuration for aluminium is 1s2 2s2 2p6 3s2 3p1 and the electronic configuration for magnesium is 1s2 2s2 2p6 3s2. The outer electron for aluminium is in the p sub shell and the outer electron for magnesium is in the s sub shell. The energy in the p sub shell for aluminium is higher than that of the s sub shell for aluminium so less energy is needed to remove