The ionization potential refers to the energy required to remove an electron from an atom or ion. It generally increases across a period (from left to right) in the periodic table and decreases down a group (from top to bottom).
Given the atomic numbers of the elements:
X (atomic number 19) corresponds to potassium (K)
Y (atomic number 37) corresponds to rubidium (Rb)
Z (atomic number 55) corresponds to cesium (Cs)
Based on their positions in the periodic table, we can make the following observations:
(1) Z would have the highest ionization potential: This statement is incorrect. In general, ionization potential tends to decrease down a group in the periodic table. Since cesium (Z) is at the bottom of Group 1, it would have a lower ionization potential compared to potassium (X) and rubidium (Y).
(2) Their ionization potential would increase with increasing atomic number: This statement is incorrect. As mentioned earlier, ionization potential generally increases across a period from left to right, not with increasing atomic number.
(3) Y would have the highest ionization potential: This statement is incorrect. Following the trend mentioned above, rubidium (Y) would have a lower ionization potential compared to cesium (Z) and potassium (X).
(4) Y would have an ionization potential between those of X and Z: This statement is correct. Considering the trend of increasing ionization potential across a period, we can conclude that rubidium (Y) would have an ionization potential higher than potassium (X) but lower than cesium (Z).
Therefore, the correct statement is (4) Y would have an ionization potential between those of X and Z.