Final answer:
The correct answer is option d, 'More than one response', because both Cl- and Si2- have their valence electrons listed correctly as they achieve a stable electron configuration resembling the noble gases. Al3+ has no valence electrons as it has lost them to form the ion.
Step-by-step explanation:
The question is looking for the correct representation of valence electrons for the given elements or ions. It is crucial to understand the electron configuration of elements to deduce the correct number of valence electrons. Let's consider the given options:
- a. Al3+ would have lost three electrons, which are the valence electrons of aluminum (3s23p1). Aluminum normally has three valence electrons but as an Al3+ ion, it has none.
- b. Cl typically has seven valence electrons (3s23p5). Changing its charge does not change the number of valence electrons. Cl- gains one electron to fill its valence shell, ending with eight valence electrons.
- c. Si typically has four valence electrons (3s23p2). Changing its charge to Si2- means it gains two additional electrons to fill its valence shell, leading to a pseudo-noble gas configuration.
Option e states 'No correct response', which would be incorrect because we can determine that Cl- and Si2- indeed have their valence electrons represented correctly in the context of their ionic forms. Therefore, the correct answer is d. More than one response, which encompasses both (b) and (c).