Consider the elements N, Si, Al, S, and F. Identify which of these elements: (a) Has the highest ionization energy; (b) Has the most metallic character; (d) Forms a 2- anion.

Verified step by step guidance

1. Step 1: Understand the concept of ionization energy, which is the energy required to remove an electron from an atom in the gaseous state. Generally, ionization energy increases across a period from left to right and decreases down a group in the periodic table.
2. Step 2: Identify the position of each element (N, Si, Al, S, and F) in the periodic table. Note that N (Nitrogen) and F (Fluorine) are in the same period, while Si (Silicon) and Al (Aluminum) are in the same group.
3. Step 3: Determine which element has the highest ionization energy by comparing their positions. Since ionization energy increases across a period, Fluorine (F) is expected to have the highest ionization energy among the given elements.
4. Step 4: Understand the concept of metallic character, which refers to how easily an element can lose electrons to form positive ions. Metallic character increases down a group and decreases across a period.
5. Step 5: Identify the element with the most metallic character by considering their positions. Aluminum (Al), being further left and down in the periodic table compared to the others, is expected to have the most metallic character.

Key Concepts

Ionization Energy

Ionization energy is the energy required to remove an electron from an atom in its gaseous state. It generally increases across a period from left to right due to increasing nuclear charge, which holds electrons more tightly. Conversely, it decreases down a group as the outer electrons are further from the nucleus and experience more shielding from inner electrons.

Metallic Character

Metallic character refers to the tendency of an element to exhibit properties typical of metals, such as conductivity, malleability, and ductility. It increases down a group in the periodic table and decreases across a period from left to right. This trend is due to the increasing ability of elements to lose electrons and form positive ions.

Anions and Their Formation

Anions are negatively charged ions formed when an atom gains one or more electrons. Nonmetals, particularly those in groups 15, 16, and 17 of the periodic table, commonly form anions. For example, sulfur (S) can gain two electrons to form a 2- anion (S^2-), which is essential for understanding the reactivity and bonding behavior of elements.