basically chem q:
explain why the 2nd ionisation energy of sodium is greater than the second ionisation energy of magnesium?
My answer-
na+ has full outer shell (noble gas E.c) stable, so doesnt want lose/gain electrons- difficult to ionize, whereas mg+ will readily lose another electron-to gain full outer shell, so more energy needed to ionize sodium
Checked on internet-
someone wrote this-
Once sodium loses one electron it satisfies the octet rule because it now has 8 electrons in it's outermost shell. So it is stable. More stable than if it lost another electron (which would result in it having only 7 in the outermost shell). So you require more energy to pull out that second electron.
Magnesium on the other hand, needs to lose 2 electrons to satisfy the octet rule. So pulling out the second electron will be easy (coz it would rather be in a state with 8 electrons in the outermost shell). Hence .. second ionisation energy (energy required to lose the second electron) is greater in sodium than in magnesium
But mark scheme?!:
doesnt give any marks for above^!!!
Question- are ions with noble gas configs stable? why wont mark scheme let this?