Why does oxygen exit as a diatom molecule while the other elements in the Group 16 exist as polyatomic molecules? Calculate the number of unpaired electrons in O2+ and O2`2- ions by drawing molecular orbital diagram
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Oxygen has 2s 2p orbitals only with a valency of -2. So it forms O2 molecule with each atom contributing 2 electrons for sharing.
Other atoms in the group have d and f orbitals which also participate in bonding. Further they are bigger atoms. So electrons are not so tightly bonded to the nucleus. Each atom can expose itself to a larger number of other atoms around it. So they form polyatomic molecules.
O2 + : O2 molecule with one positive charge... : one unpaired electron.
or O^2- ?
O2^2- : two unpaired electrons.
Other atoms in the group have d and f orbitals which also participate in bonding. Further they are bigger atoms. So electrons are not so tightly bonded to the nucleus. Each atom can expose itself to a larger number of other atoms around it. So they form polyatomic molecules.
O2 + : O2 molecule with one positive charge... : one unpaired electron.
or O^2- ?
O2^2- : two unpaired electrons.
Shizuka294:
Thnk you!
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