Question

Fill in the blanks. "ous" acid of a nonmetal "X" has 2 "'O" atoms. Per acid of the same nonmetal has the formula ___

Short answer

Answer: The formula for the per acid of the nonmetal X is XO_3.

Step-by-step solution

Understanding "ous" and "per" acids

An "ous" acid is a lower oxidation state acid, which means it has fewer oxygen atoms in the formula compared to the corresponding "per" acid. On the other hand, a "per" acid is a higher oxidation state acid, which means it has more oxygen atoms in the formula than the corresponding "ous" acid.

Find the formula for the "ous" acid of nonmetal X

The given information states that the "ous" acid of the nonmetal X has 2 oxygen atoms. Based on this information, the formula for the "ous" acid of nonmetal X is: XO_2(ous)

Determine the formula for the corresponding "per" acid

Since per acids have one more oxygen atom than their corresponding "ous" acids, we can add another oxygen atom to the formula of the ous acid to find the per acid's formula. Therefore, the per acid of X is: XO_3(per) So, the answer to fill in the blank for the per acid of the nonmetal X is XO_3.

Key concepts

Oxyacids

Oxyacids are a type of acid that contain hydrogen, oxygen, and another element often referred to as the central atom, typically a nonmetal. These acids are named based on the number of oxygen atoms bonded to the central atom, which influences their acidity and oxidation state. The more oxygen atoms present, the stronger the oxyacid is, typically. Oxyacids are common in chemistry due to their role in various chemical reactions and processes. Examples of oxyacids include sulfuric acid (\(\text{H}_2\text{SO}_4\)) and nitric acid (\(\text{HNO}_3\)).

The naming of oxyacids can vary, but typically they are categorized by prefixes such as "per-" and suffixes like "-ous" and "-ic". These prefixes and suffixes indicate the number of oxygen atoms relative to a base "ic" acid. Understanding these naming conventions is crucial for identifying the composition and properties of oxyacids.

Oxidation States

The concept of oxidation states is fundamental in understanding oxyacids and their properties. An oxidation state refers to the degree of oxidation of an atom within a molecule. It is a hypothetical charge that an atom would have if all bonds to atoms of different elements were 100% ionic. In oxyacids, the central element usually contributes positive oxidation states, while oxygen contributes negative oxidation states.

In oxyacids like sulfuric acid or phosphoric acid, the central atom's oxidation state raises as more oxygen atoms are added. For instance, in sulfuric acid (\(\text{H}_2\text{SO}_4\)), sulfur has a higher oxidation state than in sulfurous acid (\(\text{H}_2\text{SO}_3\)). Recognizing these oxidation levels helps to predict properties such as reactivity and acidity. More oxygen atoms usually mean a higher oxidation state, leading to stronger acids.

Acid Formulas

Forming acid formulas requires understanding how the oxidation state and the number of oxygen atoms are related. This directly affects the naming and the structure of the acid in question. To derive an acid formula:

• Identify the central atom and its typical valence.
• Determine the oxidation state of this atom within the molecule.
• Adjust the number of oxygen atoms to match the expected oxidation state for a specific acid type ("ous" or "per").

These steps help determine whether you should add more oxygen atoms or remove some to achieve the correct oxidation state for defining the acid. For example, a nonmetal "X" with an "ous" acid formula like XO₂ can be adjusted to form the "per" acid formula XO₃ simply by increasing the oxygen atoms by one.

By following these guidelines, any acid formula can be accurately constructed to reflect its chemical properties correctly.