please explain how hydrogen ion and flouride are isosteres using the given paragraph
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Generally isosteres means species having same number of atoms and electrons . but which electrons are same , this is related to molecular bonding .
here Hydrogen ion ( H+ )
configuration , 1s^0
Fluoride ions ( F-)
configuration , 1s² , 2s² , 2p^6
here you see both are fullfill outer subshell , then these are similar according to configuration . hence ,combination for other atom both have similar subshell 's electrons require , hence no of electrons indirectly same . no of atoms always same , you can see this
H+ ( 1 atom)
F- ( 1 atoms )
hence , this is classical isosteres
here Hydrogen ion ( H+ )
configuration , 1s^0
Fluoride ions ( F-)
configuration , 1s² , 2s² , 2p^6
here you see both are fullfill outer subshell , then these are similar according to configuration . hence ,combination for other atom both have similar subshell 's electrons require , hence no of electrons indirectly same . no of atoms always same , you can see this
H+ ( 1 atom)
F- ( 1 atoms )
hence , this is classical isosteres
abhi178:
actually this is an higher class , questions , but i think you read ncert
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Well classical isosters are the molecules or ions having same number of atoms and same number of valence shell electrons.
Later the definition was revised to include compounds having similar reactive electron shells.
Here Hydrogen ion : H ^+ion = 0 = 1s0 electrons
Fluoride Ion F ^- ion = 10= 1s2 2s2 2p6
So valence shell electrons are zero in hydrogen ion and Fluoride Ion 8 - octet configuration which is stable.
conclusion:
Both have small atomic nuclei and outer shell electrons are full or almost empty in Hydrogen ion. ( reactivity will be same for both)
Hence Hydrogen and Fluoride form Classical isosters when ionized.
Later the definition was revised to include compounds having similar reactive electron shells.
Here Hydrogen ion : H ^+ion = 0 = 1s0 electrons
Fluoride Ion F ^- ion = 10= 1s2 2s2 2p6
So valence shell electrons are zero in hydrogen ion and Fluoride Ion 8 - octet configuration which is stable.
conclusion:
Both have small atomic nuclei and outer shell electrons are full or almost empty in Hydrogen ion. ( reactivity will be same for both)
Hence Hydrogen and Fluoride form Classical isosters when ionized.
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