Which is a stronger base, S^2– or Se^2–? Explain.

Verified step by step guidance

Step 1: Understand the concept of basicity. Basicity refers to the ability of a species to accept protons (H+ ions). A stronger base is more willing to accept protons.

Step 2: Consider the periodic trend. As you move down a group in the periodic table, the size of the atoms increases. Sulfur (S) is above Selenium (Se) in the periodic table.

Step 3: Analyze the charge density. Smaller ions have higher charge density, which generally makes them stronger bases because they can attract protons more effectively.

Step 4: Compare the sizes of S2- and Se2-. Since S2- is smaller than Se2-, it has a higher charge density.

Step 5: Conclude that S2- is a stronger base than Se2- because it has a higher charge density and can attract protons more effectively.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Acidity and Basicity

Acidity and basicity are fundamental concepts in chemistry that describe the ability of a substance to donate protons (acids) or accept protons (bases). The strength of a base is often determined by its ability to accept protons and the stability of the resulting conjugate acid. In this context, comparing the basicity of S2- and Se2- involves understanding how these anions interact with protons and their respective stability.

Periodic Trends

Periodic trends refer to the predictable patterns in the properties of elements as you move across or down the periodic table. For example, basicity generally increases down a group due to the increasing size and decreasing electronegativity of the elements. In comparing S2- and Se2-, one must consider their positions in the periodic table and how these trends affect their basicity.

Conjugate Acids

The concept of conjugate acids is essential for understanding basicity. When a base accepts a proton, it forms its conjugate acid. The stability of this conjugate acid influences the strength of the base; a more stable conjugate acid corresponds to a stronger base. In the case of S2- and Se2-, analyzing the stability of their conjugate acids (H2S and H2Se) helps determine which anion is the stronger base.