Why do the first and the second ionization energies of Group 14 elements decrease from carbon to tin whereas, the third and the fourth ionization energies vary irregularly.
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Answered by
19
It is bcuz as we move down a group atomic size increases..hence. .I.P decreases
Secondly as we move from left to right the nuclear charge increases so I. P increases..
When the atomic size is more the attractive force between the no clues and shells is less and wen n.c is mire the attractive frce is more..
Hope this helped
Secondly as we move from left to right the nuclear charge increases so I. P increases..
When the atomic size is more the attractive force between the no clues and shells is less and wen n.c is mire the attractive frce is more..
Hope this helped
Anonymous:
For atomic radius the force is less and for nuclear charge it is more..
Hope this helped
When the atomic size is more the attractive force between the no clues and shells is less and wen n.c is mire the attractive frce is more..? is it more or less?
can u write that line again
Sorry I didn't mean to add the words 'no clues'I clicked it by mistake..I think that is causing the confusion..
yes please write that line again
When the atomic radius is more the attractive force is less between the nucleus and the shells so I.P decreases .When the nuclear charge is more the attractive force between the nucleus and the shell is more..so I.P increases..
I hope this helped u..and pls mark ad brainliest if u r satisfied with the ans..
thanks
Ur welcome
Answered by
11
Because its easy to remove first and second electrons of these elements but we require more energy to release third and next electrons. After exit of two electrons the atomic radius decreases and electrons held more close to the nucleus so more energy is needed to remove further electrons.
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