Using only the periodic table as your guide, select the most electronegative atom in each of the following sets: (d) Zn, Ge, Ga, As.

Verified step by step guidance

1. Identify the location of each element (Zn, Ge, Ga, As) on the periodic table to understand their properties better.
2. Recall that electronegativity generally increases as you move from left to right across a period and decreases as you move down a group.
3. Compare the positions of Zn, Ge, Ga, and As in the periodic table. Note that they are all in the same period (Period 4).
4. Since they are in the same period, focus on their positions from left to right to determine which has the highest electronegativity.
5. Identify the element that is furthest to the right in Period 4 among the given elements, as this element will have the highest electronegativity.

Key Concepts

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons in a chemical bond. It is a key factor in determining how atoms interact with each other, influencing bond polarity and molecular structure. The Pauling scale is commonly used to quantify electronegativity, with higher values indicating a stronger tendency to attract electrons.

Periodic Trends

Periodic trends refer to the predictable patterns observed in the properties of elements as you move across or down the periodic table. Electronegativity generally increases from left to right across a period and decreases from top to bottom within a group. Understanding these trends helps in predicting the behavior of elements in chemical reactions.

Element Classification

Elements can be classified into categories such as metals, nonmetals, and metalloids based on their properties. In the given set, Zn (zinc) is a metal, Ge (germanium) and Ga (gallium) are metalloids, and As (arsenic) is a nonmetal. This classification is important as it influences the electronegativity values and the reactivity of the elements.