Final answer:
Element X is likely sulfur (S). It has a smaller atomic radius than Sr, a larger ionization energy than P, and a smaller electronegativity than Cl, placing it between P and Cl, to the right of Sr on the periodic table.
Step-by-step explanation:
The identity of element X can be deduced based on its properties in relation to other elements. Since the element has a smaller atomic radius than strontium (Sr), a larger ionization energy than phosphorus (P), and a smaller electronegativity than chlorine (Cl), we need to place it in the periodic table in such a way that it aligns with these properties.
Firstly, having a smaller atomic radius than strontium suggests the element is to the right of Sr in the periodic table, as atomic radius decreases from left to right across a period. Having a larger ionization energy than phosphorus places the element above P in the periodic table, since ionization energy increases going up a group. Lastly, having a smaller electronegativity than chlorine implies it is either to the left or below Cl in the periodic table. Considering all these constraints together, the likely identity of element X is between phosphorus and chlorine in the periodic table, and to the right of strontium, which points to the element sulfur (S).
It is essential to visualize the periodic table and consider the periodic trends of atomic radius, ionization energy, and electronegativity to identify the relative position and hence the identity of element X accurately.