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Chapter 7: Problem 12

Distinguish between binary acids and oxyacids, and give two examples of each.

Short Answer

Expert verified
Binary acids: HCl, HBr. Oxyacids: H_2SO_4, HNO_3.

Step by step solution

01

- Understand Binary Acids

Binary acids are composed of hydrogen and one other nonmetal element. They usually form when hydrogen combines with a halogen or another nonmetal.
02

- Examples of Binary Acids

Examples of binary acids include hydrochloric acid (HCl) and hydrobromic acid (HBr).
03

- Understand Oxyacids

Oxyacids contain hydrogen, oxygen, and another element (usually a nonmetal). These acids have hydrogen bonded to a polyatomic ion that includes oxygen.
04

- Examples of Oxyacids

Examples of oxyacids include sulfuric acid (H_2SO_4) and nitric acid (HNO_3).

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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 type of acid that consists of only two elements: hydrogen and one other nonmetal element. They form when a hydrogen atom bonds with another nonmetal atom, usually a halogen. The general formula for binary acids is HX, where 'H' stands for hydrogen and 'X' represents a nonmetal. Common nonmetals that bond with hydrogen to form binary acids include halogens such as chlorine and bromine.

For example:
  • Hydrochloric acid (HCl) - This is a common binary acid where hydrogen is bonded to chlorine, a halogen.
  • Hydrobromic acid (HBr) - In this case, hydrogen is bonded to bromine, another halogen.
Binary acids are often strong acids and are highly corrosive. They are widely used in various industrial processes and laboratory settings.
Oxyacids
Oxyacids are another category of acids that contain hydrogen, oxygen, and another element, typically a nonmetal. These acids are more complex and have a general structure where hydrogen is bonded to a polyatomic ion that includes oxygen. The presence of oxygen in these acids is what distinguishes them from binary acids. Oxyacids usually have a central atom, which is surrounded by oxygen atoms and bonded to hydrogen.

Oxyacids include:
  • Sulfuric acid (H₂SO₄) - This is a strong acid with hydrogen ions bonded to the sulfate ion (SO₄²⁻).
  • Nitric acid (HNO₃) - Hydrogen in this acid is bonded to the nitrate ion (NO₃⁻).
Oxyacids play a crucial role in many chemical reactions and are essential in various industries including fertilizers, explosives, and in the production of chemicals.
Examples of Acids
Understanding the differences between binary acids and oxyacids is fundamental in chemistry. Here are some key examples to illustrate these differences.

  • Hydrochloric acid (HCl): A binary acid composed of hydrogen and chlorine. It is a strong acid, commonly used in laboratory settings.
  • Hydrobromic acid (HBr): Another binary acid, where hydrogen is bonded to bromine. It is known for its strong acidic properties.
  • Sulfuric acid (H₂SO₄): An oxyacid containing hydrogen, oxygen, and sulfur. It is one of the most widely used industrial chemicals due to its strong acidic nature.
  • Nitric acid (HNO₃): This oxyacid consists of hydrogen, oxygen, and nitrogen. It is a strong acid used extensively in the production of fertilizers and explosives.
Each type of acid has its specific applications and properties, making them essential for various scientific and industrial processes.

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Most popular questions from this chapter

What is the relationship between the empirical formula and the molecular formula of a compound?

Write the formula for and indicate the charge on each of the following ions: a. sodium ion b. aluminum ion c. chloride ion d. nitride ion e. iron(II) ion f. iron(III) ion

Write formulas for each of the following compounds: a. sodium fluoride b. calcium oxide c. potassium sulfide d. magnesium chloride e. aluminum bromide f. lithium nitride g. iron(II) oxide

Determine the number of moles of each type of monatomic or polyatomic ion in one mole of the following compounds. For each polyatomic ion, determine the number of moles of each atom present in one mole of the ion. a. \({KNO}_{3}\) b. \({Na}_{2} {SO}_{4}\) c. \({Ca}({OH})_{2}\) d. \(({NH}_{4})_{2} {SO}_{3}\) e. \({Ca}_{3}({PO}_{4})_{2}\) f. \({Al}_{2}({CrO}_{4})_{3}\)

Assign oxidation numbers to each atom in the following molecules and ions: a) \({CO}_{2}\) e. \({H}_{2} {O}_{2}\) b) \({NH}_{4}^{+}\) t. \({P}_{4} {O}_{10}\) c) \({MnO}_{4}^{-}\) g. \({OF}_{2}\) d) \({S}_{2} {O}_{3}^{2-}\)
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