Question

The oxides of the selenium(IV) and tellurium(IV) are \(\mathrm{SeO}_{2}\) and \(\mathrm{TeO}_{2} .\) One of these oxides is amphoteric and one is acidic. Which is which?

Short answer

Selenium(IV) oxide (SeO2) is acidic, while tellurium(IV) oxide (TeO2) is amphoteric.

Step-by-step solution

Determine the location on the periodic table

Check the position of selenium and tellurium in the periodic table. Both selenium and tellurium are in the same group (Group 16 - the oxygen group) of the periodic table. Tellurium is below selenium in the group.

Correlate position to basicity

Understand that as we go down the group, elements' tendency to behave as a base increases. It means, the cations of the elements which are below in the group have more tendency to hydrolyze water and behave like a base. Therefore, tellurium(IV) oxide (TeO2) is more likely to behave as a base.

Classify the oxides

Because TeO2 shows both acidic and basic behavior, it is amphoteric. SeO2, being above in the group, is less likely to behave as a base and hence is acidic.

Key concepts

Periodic Table Groups

The periodic table is arranged in rows called periods and columns called groups or families. Group 16, often referred to as the oxygen group, includes elements such as oxygen, sulfur, selenium, tellurium, and polonium.
These elements share certain chemical properties due to having six valence electrons. As you move down the group from oxygen to polonium, several trends appear. For instance, elements increase in atomic size and mass.
A notable trend is the increasing metallic character. Oxygen and sulfur are nonmetals, selenium and tellurium are metalloids, while polonium is metallic. This change affects their chemical behavior, particularly when forming compounds like oxides.
Understanding periodic table groups helps predict the types of reactions and the properties of compounds that each element will form. It provides a basis for expecting interactions these elements might have with others, particularly in oxide formation.

Selenium and Tellurium Chemistry

Selenium and tellurium are fascinating elements with properties that are beneficial in both chemistry and industry.
Found in Group 16 of the periodic table, selenium is a non-metal, whereas tellurium is classified as a metalloid. This difference impacts their chemical properties and behavior.
Selenium often exhibits similar properties to sulfur but has a greater tendency to show metallic characteristics compared to oxygen and sulfur. This results in selenium forming a variety of oxidation states, commonly \ \( +4 \) and \( +6 \).
In contrast, tellurium, being further down the group, exhibits stronger metallic properties and readily forms metalloids with varying oxidation states. Tellurium's chemistry is dominated by the \ \( +4 \) oxidation state due to its tendency to stabilize before fully oxidizing.
Knowing the chemistry of selenium and tellurium helps discern their behavior, especially when predicting the amphoteric nature of \( \text{TeO}_2 \) and the acidic nature of \( \text{SeO}_2 \). Their positioning in the periodic table influences their oxidation states and chemical reactions extensively.

Oxide Classification

Oxides are compounds that form between an element and oxygen. These can be classified based on their chemical behavior as acidic, basic, or amphoteric.
Acidic oxides typically form from nonmetals. These oxides, when reacting with water, produce acids. For instance, \( \text{SeO}_2 \) is an acidic oxide.
In contrast, basic oxides usually form from metals. They typically react with acids to form salts and water. As one moves down any group containing nonmetals, the elements may transition from forming primarily acidic oxides to forming basic or amphoteric oxides.
Amphoteric oxides are unique as they exhibit both acidic and basic properties, allowing them to react with both acids and bases to form salt and water. \( \text{TeO}_2 \), being an amphoteric oxide, demonstrates this dual behavior.
Understanding the oxide classification is crucial for predicting an element's reaction based on the type of oxide it forms, with \( \text{TeO}_2 \) highlighted for its remarkable versatility.