mg occupies s orbital whereas al occupies p orbital. distance between p orbital and nucleus is more than that of s orbital due to which atomic radius of al is more than that of mg..........................................................................contd..........................................
by BIPIN SHARMA.
Electron configurations indicate that from Be to B there are electrons in the 2p subshell, which has more energy than 2s. These 2p electrons are not as strongly attached to the nucleus as they contain more energy, therefore they are more easily removed.
In moving from Mg to Al there are electrons in 3p - the same logic as above applies.
Fluorine is more electronegative than Mg. It is easier to remove the first electron from a Mg atom that it is to remove one from a F atom.
Electronegativity is the ability of an atom to attract electrons towards itself. That means that the electrons in Fluorine are held tighter than in Mg. And this is why the first ionization of Mg is lower that that of Fluorine :)
Hope it helps.
Ionization energy of Na is less than that of Mg because Na gives only one electron but Mg gives two electrons as valency of magnesium is 2 and that of sodium is 1. And the I.E successor after 1st electron is always greater than the predecessor.i.e, 1st I.E < 2nd I.E <3rd I.E OR
3rd I.E > 2nd I.E > 1st I.E
Mg looses 2 electrons Al looses 3.
ionization energies of mg is less than chlorine because chlorine requires only one electron to complete its octet so it will not prefer to loose its electron morover its electronegativity is also higher and it is of smaller size than mg so electtron removal is difficult
Sr Mg B N Ne Apex, Draikman
Yes it is.
My answer: The 3p electron in aluminum is slightly more distant from the nucleus than the 3s, and partially screened by the 3s2 electrons as well as the inner electrons. Both of these factors offset the effect of the extra proton.
Mg 2+ This cation has already donated it's valence shell and would require that core electrons be pulled by a large ionization energy.
Chlorine is Cl, C is carbon. The first ionization energy of magnesium is less than that of chlorine.
Ne (Highest First Ionization Energy) C Be Mg Sr (Lowest First Ionization Energy)
ionization energies of mg is less than chlorine because chlorine requires only one electron to complete its octet so it will not prefer to loose its electron morover its electronegativity is also higher and it is of smaller size than mg so electtron removal is difficult
Because Be contains more protons and thus has greater nuclear positivity which exerts a stronger attraction for its electrons which requires more energy to remove one of the electrons leading to a higher ionization potential.
Sr Mg B N Ne Apex, Draikman
Mg + Ionization energy ----> Mg2+ + 2e
mg+ 2e
First ionization energy of magnesium = 870/ kj/mol First ionization energy of phosphorous = 589 kj/mol So, magnesium has the larger ionization energy required to pull the first valance electron. Do you know why?
Yes.
1000 mg=1g
less than
Yes (40% of it)