Final answer:
The correct order of increasing first ionization energy for P, S, and Cl is option (a) P, S, Cl. First ionization energy increases across a period from left to right and decreases down a group from top to bottom on the periodic table.
Step-by-step explanation:
The correct order of increasing first ionization energy for the elements Phosphorus (P), Sulfur (S), and Chlorine (Cl) is determined by the general trend in the periodic table that ionization energy increases across a period (from left to right) and decreases down a group (from top to bottom).
Therefore, as P, S, and Cl are all in the same period with P being the furthest left and Cl being the furthest right, the correct order is P, S, Cl. So the correct answer would be (a) P, S, Cl or (b) P, S, Cl as they are the same.
We can apply this knowledge to other parts of the question. For instance, out of Na, Al, H, and He, Helium (d) would have the highest first ionization energy, being at the top right of its period. Conversely, Potassium (K) would have the smallest first ionization energy (a) as it is located on the far left and near the bottom of the periodic table. When predicting electron configuration, we know that Chlorine has the electron configuration of [Ne]3s²3p⁵ and Potassium has [Ar]4s¹.
For Exercise 3.4.1 and Exercise 4.7.2, among the elements listed (As, Bi, Ge, Pb, Sb, Sn), Arsenic (As) has the highest first ionization energy because it is farthest to the right and top among the listed elements on the periodic table. Similarly, for question 70, Fluorine (F) will have the smallest first ionization energy because it is furthest to the right and top of its group.