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Chapter 8: Problem 33

Describe the difference between a binary acid and an oxyacid.

Short Answer

Expert verified
The main differences between binary acids and oxyacids include composition, bonding, and properties. Binary acids consist of hydrogen and a non-metal element and are formed through a single covalent bond between the hydrogen and the non-metal atom. Oxyacids, on the other hand, contain hydrogen, oxygen, and a non-metal element and are formed when hydrogen is bonded to a polyatomic ion containing the non-metal atom and oxygen atoms. Oxyacids generally exhibit stronger acidic properties due to the presence of an electronegative oxygen atom in their structure.

Step by step solution

01

Definition of Binary Acids

A binary acid is a type of acid that contains only two elements: hydrogen (H) and a second, more electronegative element (usually a non-metal). These acids are formed when hydrogen is bonded to the non-metal atom through a single covalent bond. Examples of some common binary acids include hydrochloric acid \( (HCl) \), hydrobromic acid \( (HBr) \), and hydroiodic acid \( (HI) \).
02

Definition of Oxyacids

An oxyacid is an acid that contains hydrogen, oxygen, and another element (usually a non-metal). It is formed when hydrogen is bonded to a polyatomic ion containing the non-metal atom and oxygen atoms through a single covalent bond. Examples of some common oxyacids include sulfuric acid \( (H_2SO_4) \), nitric acid \( (HNO_3) \), and phosphoric acid \( (H_3PO_4) \).
03

Main Differences between Binary Acids and Oxyacids

1. Composition: Binary acids consist of hydrogen and a non-metal element, while oxyacids contain hydrogen, oxygen, and a non-metal element. 2. Bonding: In binary acids, hydrogen is bonded directly to the non-metal atom, while in oxyacids hydrogen is bonded to a polyatomic ion containing the non-metal atom and oxygen atoms. 3. Properties: Compared to binary acids, oxyacids generally exhibit stronger acidic properties due to the presence of an electronegative oxygen atom in their structure. The oxygen atom enhances the acidity of the acid by stabilizing the negative charge on the conjugate base when the proton is donated. In summary, binary acids and oxyacids differ in their composition, bonding structure, and some of their chemical properties. Binary acids are simpler in composition, containing only two elements, while oxyacids contain three elements, including oxygen, which generally results in stronger acidity.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Binary Acids
Binary acids are one of the simpler forms of acids in chemistry, consisting solely of two distinct elements. They are composed primarily of hydrogen and some other non-metallic element. This simple composition gives them unique characteristics that are important to understand.

A hallmark example of a binary acid is hydrochloric acid, represented chemically as \( HCl \). Similarly, hydrobromic acid and hydroiodic acid, \( HBr \) and \( HI \) respectively, are also common binary acids encountered in chemistry.

  • Structure: The key structural feature of binary acids is the single covalent bond formed between the hydrogen atom and the more electronegative non-metal atom.
  • Properties: Binary acids tend to form solutions that are acidic when dissolved in water, and they display distinct properties according to the identity of the non-metal they are bonded with.
Understanding these properties helps provide insights into how binary acids behave in various chemical reactions.
Oxyacids
Oxyacids introduce additional complexity into the world of acids by incorporating oxygen into their structure. These acids are comprised of hydrogen, oxygen, and a third non-metal element. This combination results in notable differences from binary acids, especially in terms of their acidic strength.

Common examples of oxyacids include sulfuric acid \( H_2SO_4 \), nitric acid \( HNO_3 \), and phosphoric acid \( H_3PO_4 \). These compounds are well-known for their industrial and laboratory applications due to their potent acidic nature.

  • Structure: Oxyacids feature hydrogen atoms bonded to a polyatomic ion, which includes the non-metal atom and oxygen atoms. The presence of these additional oxygen atoms plays a critical role.
  • Acidic Strength: The presence of oxygen contributes to enhanced acidity. Oxygen is highly electronegative, which assists in stabilizing the negative charge on the ion when the acid releases a proton (\( H^+ \)).
These structural aspects make oxyacids generally stronger than binary acids. This makes them crucial in a variety of chemical processes.
Chemistry Education
In the study of chemistry, understanding the differences between various types of acids, such as binary acids and oxyacids, is essential for grasping broader chemical principles. Acids are a fundamental part of chemistry education due to their ubiquitous presence in both natural and industrial processes.

  • Conceptual Understanding: Gaining knowledge about the composition and bonding of acids not only helps in identifying them in chemical reactions but also assists in predicting their behavior in different environments.
  • Practical Applications: Many processes, ranging from biological systems to industrial manufacturing, involve reactions with acids. Understanding how binary acids and oxyacids function is crucial in fields like medicine, material science, and environmental science.
Learning about acids isn't just about memorization; it's about applying this knowledge to solve real-world problems. With the right educational resources, students can appreciate the elegance and logic of chemistry, preparing them for a future in science.

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Most popular questions from this chapter

Describe electronegativity trends in the periodic table.

Predict the molecular shape of each molecule. a. \(\mathrm{COS} \quad\) b. \(\mathrm{CF}_{2} \mathrm{Cl}_{2}\)

Name each of the binary covalent compounds listed below. \(\mathrm{CCl}_{4}\)

How could you predict the presence of a sigma or pi bond in a molecule?

Rank each of the molecules below in order of the shortest to the longest sulfur-oxygen bond length. a. \(\mathrm{SO}_{2} \quad\) b. SO_ \(_{3}^{2-} \quad\) c. \(\mathrm{SO}_{4}^{2-}\)
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