Complete the exercises below. Consider the elements Li, K, Cl, C, Ne, and Ar. From this list, select the element that a. is most electronegative, b. has the greatest metallic character, c. most readily forms a positive ion, d. has the smallest atomic radius, e. forms π bonds most readily, f. has multiple allotropes.

Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. It varies across the periodic table, generally increasing from left to right and decreasing from top to bottom. Elements like fluorine are highly electronegative, while metals tend to have lower values. Understanding electronegativity helps predict bond types and molecular behavior.

Metallic character refers to the set of properties associated with metals, including conductivity, malleability, ductility, and the tendency to lose electrons and form positive ions. This character increases down a group in the periodic table and decreases across a period. Recognizing metallic character is essential for understanding reactivity and bonding in elements.

Atomic radius is the distance from the nucleus of an atom to the outermost shell of electrons. It generally decreases across a period due to increased nuclear charge pulling electrons closer, and increases down a group as additional electron shells are added. The atomic radius is crucial for understanding trends in reactivity, ionization energy, and the formation of bonds.