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Chapter 14: Problem 2

a. Distinguish between binary acids and oxyacids in terms of their component elements and the systems used in naming them. b. Give three examples of each type of acid.

Short Answer

Expert verified
Binary acids are hydrogen and one nonmetal, named with 'hydro-' and '-ic'. Oxyacids are hydrogen, oxygen, and another element, named with '-ic' or '-ous'. Examples: HCl, HBr, HI (binary); H鈧係O鈧�, HNO鈧�, H鈧働O鈧� (oxyacids).

Step by step solution

01

- Understand Binary Acids

Binary acids are composed of hydrogen and one other nonmetal element. Their names typically begin with the prefix 'hydro-', followed by the root name of the nonmetal, and end with the suffix '-ic acid'. For example, HCl is named hydrochloric acid.
02

- Understand Oxyacids

Oxyacids contain hydrogen, oxygen, and another element (usually a nonmetal). They are often derived from polyatomic ions. The naming system for oxyacids depends on the suffix of the polyatomic ion: if the ion ends in '-ate', the acid name will end in '-ic acid'; if the ion ends in '-ite', the acid name will end in '-ous acid'. For example, H鈧係O鈧� (from the sulfate ion) is named sulfuric acid.
03

- Examples of Binary Acids

Three examples of binary acids are: 1. Hydrochloric acid (HCl) 2. Hydrobromic acid (HBr) 3. Hydroiodic acid (HI)
04

- Examples of Oxyacids

Three examples of oxyacids are: 1. Sulfuric acid (H鈧係O鈧�) 2. Nitric acid (HNO鈧�) 3. Phosphoric acid (H鈧働O鈧�)

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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 a class of acids composed of only two elements: hydrogen and a nonmetal. These acids are simple in structure but play an important role in chemistry.
  • They typically contain hydrogen and one other nonmetal element.
  • Common nonmetals include chlorine, bromine, and iodine.
  • Their names follow a specific convention: starting with the prefix 'hydro-', followed by the root of the nonmetal's name, and ending with '-ic acid'.
For instance, when hydrogen combines with chlorine to form HCl, it is named hydrochloric acid. Similarly, hydrogen with bromine (HBr) is called hydrobromic acid, and hydrogen with iodine (HI) is called hydroiodic acid. Understanding these naming conventions is essential for mastering the identification and use of binary acids in various chemical reactions.
Oxyacids
Oxyacids are a different type of acid that consist of hydrogen, oxygen, and another element, usually a nonmetal. These acids are more complex than binary acids.
  • They contain at least one oxygen atom in addition to hydrogen and another nonmetal.
  • These are often derived from polyatomic ions.
  • Named based on the polyatomic ions they contain.
The naming system for oxyacids varies slightly depending on the suffix of the polyatomic ion they are derived from:
  • If the polyatomic ion ends with '-ate,' the acid name will end with '-ic acid.'
  • If the polyatomic ion ends with '-ite,' the acid name will end with '-ous acid.'
For example: H鈧係O鈧� (derived from the sulfate ion SO鈧劼测伝) is named sulfuric acid, HNO鈧� (from the nitrate ion NO鈧冣伝) is called nitric acid, and H鈧働O鈧� (from the phosphate ion PO鈧劼斥伝) is known as phosphoric acid. Recognizing these naming patterns helps in understanding the characteristics and reactions of oxyacids.
Acid Naming Conventions
Naming conventions for acids are crucial for clear communication in the field of chemistry.
  • Binary acids typically follow the 'hydro + root name of the nonmetal + ic acid' pattern.
  • Oxyacids are named based on the ending of their corresponding polyatomic ions.
Here are a few examples for clarity:
  • Binary acid: HCl -> Hydrochloric Acid
  • Binary acid: HBr -> Hydrobromic Acid
  • Oxyacid: H鈧係O鈧� (sulfate) -> Sulfuric Acid
  • Oxyacid: HNO鈧� (nitrite) -> Nitrous Acid
Understanding these naming conventions allows for accurate identification and usage of acids in both laboratory and industrial settings. This fundamental knowledge is essential for students as they progress in their chemistry studies.

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Most popular questions from this chapter

Write the balanced chemical equation for each of the following reactions between water and the non-metallic oxide to form an acid. $$ \begin{array}{l}{\text { a. } \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow} \\ {\text { b. } \mathrm{SO}_{3}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow} \\ {\text { c. } \mathrm{N}_{2} \mathrm{O}_{5}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow}\end{array} $$

Complete the following neutralization reactions. Balance each reaction, and then write the overall ionic and net ionic equation for each. $$ \begin{array}{l}{\text { a. } \mathrm{HCl}(a q)+\mathrm{NaOH}(a q) \longrightarrow} \\ {\text { b. } \mathrm{HNO}_{3}(a q)+\mathrm{KOH}(a q) \longrightarrow} \\ {\text { c. } \mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{HNO}_{3}(a q) \longrightarrow} \\ {\text { d. } \mathrm{Mg}(\mathrm{OH})_{2}(a q)+\mathrm{HCl}(a q) \longrightarrow}\end{array} $$

Distinguish between a monoprotic, a diprotic, and a triprotic acid. Give an example of each.

Compare the general properties of acids with the general properties of bases.

Name each of the following oxyacids: $$ \begin{array}{ll}{\text { a. HNO }_{3}} & {\text { c. } \mathrm{HClO}_{3}} \\\ {\text { b. } \mathrm{H}_{2} \mathrm{SO}_{3}} & {\text { d. HNO }_{2}}\end{array} $$
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