Question

which of the elements Na,Mg,Si and P would have greatest difference in their
1. first second ionisation enthalpy
2.second and third ionisation

Answer 1

HELLO FRIEND HERE IS YOUR ANSWER,,,,,,,,,,,


From the above given elements of sodium, magnesium and silicon, the element sodium is a metal belonging to alkali group. It's valence shell is containing only one electron, because of this it's $\triangle_i H_1$ is going to be lower than removing the electron.

After the removal of electron (one in number) it attains a configuration of a noble gas called Neon. That is, $\bf{Na^+ \: (1s^2 \: 2s^2 \: 2p^6)}$ accordingly it's $\triangle_i H_2$ supposedly goes higher. Accordingly this difference of first and second ionisation enthalpies the higher one would be Sodium or Na.

Point to be especially noted that the cases of Magnesium, silicon and phosphorus they might've a higher $\triangle_i H _1$ exception is about having a lower $\triangle_i H_2$.

Because of this the total difference between the two quantities $\triangle_i H_1$ and $\triangle_i H_2$ makes the value of difference go lower hence making Sodium element or Na as a emergent winner in this case.

HOPE THIS HELPS YOU AND CARS THE DOUBTS FOR DIFFERENCES IN IONISATION ENTHALPIES!!!!!!!!!

Answer 2

Among the elements Na, Mg, Si and P; Na would have the greatest difference between the first and second ionization enthalpies since after losing one electron it takes up the electronic configuration 1s2 2s2 2p6, so it becomes stable with completely filled p orbitals so it will be difficult to remove an electron from the stable configuration. But in case of the other elements, after removal of first electron the configuration obtained is not very stable and second electron can be easily removed so the difference between the first and second inoization enthalpy is less.

mark me brainliest