Which property of the third-row nonmetallic elements might be the one depicted below:
a. first ionization energy,
b. atomic radius,
c. electronegativity,
d. melting point,
e. X―X single-bond enthalpy? [Find more in Sections 22.3, 22.4, 22.6, 22.8, and 22.10]

Verified step by step guidance

1. Identify the trend depicted in the data provided. Look for whether the property increases, decreases, or remains constant across the third-row nonmetallic elements.
2. Review the general trends for each property listed in the options across the periodic table, particularly focusing on the third-row nonmetallic elements. For example, first ionization energy generally increases across a period, atomic radius decreases, electronegativity increases, melting point varies depending on the type of element, and X―X single-bond enthalpy generally increases with the size of the atoms involved.
3. Match the trend you identified in step 1 with the expected trends for each property. For instance, if the property in the data increases from left to right across the third row, it could suggest a property like electronegativity or first ionization energy.
4. Consider any exceptions or special cases in the third row that might affect the trend, such as the presence of a metalloid or the transition from nonmetals to noble gases.
5. Select the property whose general trend best matches the trend depicted in the data. This will be your answer to which property might be depicted.

Key Concepts

First Ionization Energy

First ionization energy is the energy required to remove the outermost electron from a neutral atom in its gaseous state. This property generally increases across a period due to increasing nuclear charge, which holds electrons more tightly, and decreases down a group as the distance between the nucleus and outer electrons increases, reducing the effective nuclear charge felt by those electrons.

Atomic Radius

Atomic radius refers to the size of an atom, typically measured from the nucleus to the outer boundary of the surrounding cloud of electrons. Atomic radius decreases across a period due to increased nuclear charge pulling electrons closer to the nucleus, while it increases down a group as additional electron shells are added, increasing the distance between the nucleus and the outermost electrons.

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. It generally increases across a period as atoms become more effective at attracting electrons due to higher nuclear charge, and decreases down a group as the increased distance from the nucleus reduces the attraction between the nucleus and bonding electrons.