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The metals of group 2 from top to bottom these metals will form ions most readily and why?...Question no.1...
2.Which elements in period 2 have higher ionisation energies than their immediate successors?
3.What is the electronic configuration of theelement in the third period, which gains one electrons to change into an anion?
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Answers
and we know , ionisation energy is inversely proportional to size of atom.
hence, down the group ionisation energy decrease.
we also Know ,
Less ionisation energy means high tendency to accept electrons , hence high tendency form ions .
hence, groupII down the group , metals form ions most radily.
2. highest ionisation energy in period II = Ne ( Neon ) becoz it has stable configuration . higher energy will require to remove first electron from complete shell.
3. in third period " Cl " has higher tendency to accept electrons and form anoin .
hence, configuration of " Cl " :
1s² , 2s² , 2P^6 , 3s² , 3P^5
1. from top to bottom ionisation energy decrease due to down the group size of atom increases .
and we know , ionisation energy is inversely proportional to size of atom.
hence, down the group ionisation energy decrease.
we also Know ,
Less ionisation energy means high tendency to accept electrons , hence high tendency form ions .
hence, groupII down the group , metals form ions most radily.
2. highest ionisation energy in period II = Ne ( Neon ) becoz it has stable configuration . higher energy will require to remove first electron from complete shell.
3. in third period " Cl " has higher tendency to accept electrons and form anoin .
hence, configuration of " Cl " :
1s² , 2s² , 2P^6 , 3s² , 3P^5
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