Question

Which of the following elements has the highest electronegativity? A. \(\mathrm{Mg}\) B. \(\mathrm{Cl}\) C. \(\mathrm{Zn}\) D. I

Short answer

The element with the highest electronegativity is \(\mathrm{Cl}\).

Step-by-step solution

Understand Electronegativity

Electronegativity is the tendency of an atom to attract electrons towards itself in a chemical bond. Higher electronegativity means a stronger attraction for electrons.

Recall the Trend in the Periodic Table

Electronegativity increases across a period from left to right and decreases down a group in the periodic table.

Identify Positions of Given Elements in the Periodic Table

Locate each element in the periodic table:- \(\mathrm{Mg}\) is in Group 2, Period 3- \(\mathrm{Cl}\) is in Group 17, Period 3- \(\mathrm{Zn}\) is in Group 12, Period 4- \(\mathrm{I}\) is in Group 17, Period 5

Determine Electronegativity Based on Position

\(\mathrm{Cl}\) and \(\mathrm{I}\) are both in Group 17 (halogens), which typically have high electronegativity. However, \(\mathrm{Cl}\) is higher in the periodic table (Period 3) compared to \(\mathrm{I}\) (Period 5), so \(\mathrm{Cl}\) has a higher electronegativity.

Compare Electronegativity Values and Conclude

Comparing all four elements' positions and knowing that electronegativity increases across periods and decreases down groups, \(\mathrm{Cl}\) has the highest electronegativity among the choices.

Key concepts

periodic table trends

The periodic table is more than just a chart of elements; it's a map of atomic properties that change in predictable ways. One crucial trend is electronegativity—how strongly an atom attracts electrons in a bond. As you move from left to right across a period, electronegativity increases due to increasing nuclear charge. This stronger pull from the nucleus attracts electrons more effectively. Conversely, as you move down a group, electronegativity decreases. This is because additional electron shells mean outer electrons are further from the nucleus and experience a weaker pull.

chemical bonding

Chemical bonding is the force that holds atoms together in compounds. Electronegativity plays a critical role here. When atoms with different electronegativities form bonds, the more electronegative atom attracts electron density towards itself, resulting in a polar bond. If the difference in electronegativity is significant enough, it can even lead to ionic bonding, where electrons are transferred from one atom to another. Understanding trends in electronegativity helps predict how atoms will bond, which is essential for understanding molecule behavior and properties.

atomic properties

Atomic properties like atomic radius, ionization energy, and electron affinity are interconnected. Electronegativity is a key property among these. Atoms with a small atomic radius usually have higher electronegativity because their protons can exert a strong attractive force on electrons. Similarly, high ionization energy (the energy required to remove an electron) often correlates with high electronegativity, as both indicate a strong attraction to electrons. By examining these properties, you can infer much about an element's chemical behavior and reactivity.