From elements Arsenic to Antimony, which has the smallest Ionic Radius and why.
Your question is unclear. Are you asking for the ionic radius of As vs that of Sb or for the ionic vadius of elements beginning with As and ending with Sb. And which ion (+3, +5, or some other) are you asking about. Here is a site that explains about covalent and ionic radii (the ionic radii is near the end but it will help to read all of it).
http://www.chemguide.co.uk/atoms/properties/atradius.html
To determine which element, arsenic (As) or antimony (Sb), has the smallest ionic radius, we need to compare their respective ionic radii.
1. Start by finding the electron configuration of each element and identifying the number of valence electrons:
- Arsenic (As): [Ar] 4s2 3d10 4p3 (5 valence electrons)
- Antimony (Sb): [Kr] 5s2 4d10 5p3 (5 valence electrons)
2. Next, consider that both arsenic and antimony are nonmetals belonging to Group 15 (Group VA) of the periodic table. Nonmetals tend to gain electrons to achieve a stable electron configuration, forming negative ions (anions).
3. In this case, both arsenic and antimony will tend to gain three electrons to achieve a stable 8-electron configuration in their valence shell (by attaining the electron configuration of a noble gas). As a result, both elements are expected to form ions with a 3- charge (As3- and Sb3-).
4. The ionic radius is the size of an ion. As a general trend, the ionic radius increases as we move down a group in the periodic table. Therefore, antimony (Sb) should have a larger ionic radius than arsenic (As) since it is located below arsenic in Group 15.
So, to answer your question, arsenic (As) has the smallest ionic radius among these two elements (arsenic and antimony) because it is located higher up in Group 15 of the periodic table.