Final answer:
To rank the elements from lowest to highest ionization energy (Cl, Si, Mg, Na, P, Ar, Al, S), we look at the periodic trend that ionization energy generally increases across a period and decreases down a group. The correct order is Na, Mg, Al, Si, P, S, Cl, Ar, starting with Na as it has the lowest ionization energy being farthest left and lowest on the period, to Ar with the highest ionization energy as a noble gas on the right.
Step-by-step explanation:
The student has asked to rank several elements in order from the lowest to the highest ionization energy, specifically: Cl, Si, Mg, Na, P, Ar, Al, S. Ionization energy is the energy required to remove an electron from a gaseous atom or ion. In general, ionization energy increases across a period (from left to right) and decreases down a group (from top to bottom) on the periodic table.
Given this trend, the order from lowest to highest ionization energy typically starts with the element on the left and bottom of the period and ends with the element on the right and top. In this case, we would expect the alkali metal (Na) to have the lowest ionization energy and the noble gas (Ar) to have the highest. The expected order will then often follow the atomic numbers of the elements as you move across the period.
Considering the elements provided, the order from lowest to highest ionization energy would be: Na, Mg, Al, Si, P, S, Cl, Ar. Sodium (Na) has the lowest ionization energy because it is a Group 1 element and is farthest to the left and lowest down within this group of elements. Argon (Ar) has the highest ionization energy as it is a noble gas and is placed at the far right of the period. The other elements increase in ionization energy as their atomic numbers increase and the number of protons in the nucleus, which attracts the electrons more strongly, also increases.