Question

1. based on the concept of periodic trends, answer the following questions for these atoms: p, s, cl, f. be prepared to defend your answers.

d which element has the highest electronegativity?
f
e which element has the least metallic character?
f which element has the largest ion?
phosphorus

Explanation:

Part d: Which element has the highest electronegativity?

Electronegativity generally increases across a period (from left to right) and decreases down a group (from top to bottom) in the periodic table. Among P (Phosphorus), S (Sulfur), Cl (Chlorine), and F (Fluorine), F is in the upper - rightmost position relative to the others. It is in period 2 and group 17, while P is in period 3, group 15; S is in period 3, group 16; Cl is in period 3, group 17. So, following the trend of electronegativity, F has the highest electronegativity.

Part e: Which element has the least metallic character?

Metallic character decreases as we move from left to right across a period and increases as we move down a group. Metallic character is associated with the ability to lose electrons. Non - metals have less metallic character than metals, and among non - metals, elements on the right - hand side of the periodic table have less metallic character. F is a non - metal, and among P, S, Cl, and F, F is the most non - metallic (has the least tendency to lose electrons) as it is the furthest to the right and highest up in the periodic table among these elements. P is a metalloid - like non - metal with more metallic character than F, S is also a non - metal but less non - metallic than F, and Cl is a non - metal but F is more electronegative and less metallic in character than Cl.

Part f: Which element has the largest ion?

When atoms form ions, for non - metal atoms (P, S, Cl, F are non - metals or metalloids), they generally gain electrons to form anions. The size of an ion depends on the number of electron shells and the effective nuclear charge. Phosphorus (P) when forming an anion (\(P^{3 - }\)) has 3 electron shells. Sulfur (\(S^{2 - }\)) also has 3 electron shells, Chlorine (\(Cl^{-}\)) has 3 electron shells, and Fluorine (\(F^{-}\)) has 2 electron shells. Among the ions with 3 electron shells, the effective nuclear charge is in the order \(P^{3 - }

Answer:

F (Fluorine)