Rucete ✏ Chemistry In a Nutshell
1 Cation's radius is smaller than the radius of atoms.
1. When metal lose their electron and be converted cation.
2. When atom lose their electron, their mutual repulsion among the electrons will be smaller.
2 Anion's radius is bigger than the covalent radius of the atoms.
1. Increased electron can increase mutual repulsion among the electrons, and cause expansion of the electron orbital.
Repulsion among the electrons and ionic radius : The static reaction force between electron and electron weakens the attraction between the nucleus and the electron of the atom.
For example, when a neutron atom accepts an electron and becomes an anion, it tries to keep the distance between electrons apart because of the rebound between the electron and the increased electrons. As a result, the radius of Anion becomes larger than the radius of the atom.
3 Non-spherical ions : The concept of ionic radii is based on the assumption of a spherical ion shape. On the other hand, from a group theoretical point of view the assume is only justified for ions that reside on high symmetry crystal lattice sites like Na and Cl in halite or Zn and S in sphalerite.
Ionic Radius | In a nutshell
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1. When metal lose their electron and be converted cation.
2. When atom lose their electron, their mutual repulsion among the electrons will be smaller.
2 Anion's radius is bigger than the covalent radius of the atoms.
1. Increased electron can increase mutual repulsion among the electrons, and cause expansion of the electron orbital.
Repulsion among the electrons and ionic radius : The static reaction force between electron and electron weakens the attraction between the nucleus and the electron of the atom.
For example, when a neutron atom accepts an electron and becomes an anion, it tries to keep the distance between electrons apart because of the rebound between the electron and the increased electrons. As a result, the radius of Anion becomes larger than the radius of the atom.
3 Non-spherical ions : The concept of ionic radii is based on the assumption of a spherical ion shape. On the other hand, from a group theoretical point of view the assume is only justified for ions that reside on high symmetry crystal lattice sites like Na and Cl in halite or Zn and S in sphalerite.
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Chemistry in a nutshell