Question

Does the reaction of a main-group nonmetal oxide in water produce an acidic or a basic solution? Write a balanced equation for the reaction of a Group \(6 \mathrm{~A}(16)\) nonmetal oxide with water.

Short answer

Acidic; \(SO_3 + H_2O \rightarrow H_2SO_4\)

Step-by-step solution

Identify the Type of Oxide

Determine whether the main-group nonmetal oxide will form an acidic or basic solution when it reacts with water. Nonmetal oxides typically form acidic solutions.

Determine the Group 6A(16) Nonmetal Oxides

Identify a common nonmetal oxide from Group 6A(16). One of the well-known oxides for this group is Sulfur trioxide \((SO_3)\).

Write the Reaction Equation

Combine the identified oxide \(SO_3\) with water \(H_2O\) to form the acidic solution. The balanced equation is: \((SO_3 + H_2O \rightarrow H_2SO_4)\).

Balance the Equation Confirmation

Verify that the equation is balanced. Sulfur (S), oxygen (O), and hydrogen (H) atoms are balanced on both sides of the equation.

Key concepts

Group 6A Nonmetals

Group 6A elements, also known as the chalcogens, include oxygen, sulfur, selenium, tellurium, and polonium. These elements share similar chemical properties due to their position in the periodic table.
Nonmetals in this group, such as oxygen and sulfur, commonly form oxides when combined with oxygen. These oxides are usually acidic. For instance, sulfur can form sulfur dioxide \(SO_2\) and sulfur trioxide \(SO_3\).
When these oxides react with water, they typically produce acidic solutions.
This is because they yield acids, such as sulfurous acid \(H_2SO_3\) from \(SO_2\) and sulfuric acid \(H_2SO_4\) from \(SO_3\), upon reaction with water.
Here's a quick bullet point summary of Group 6A nonmetals:

• Oxygen (O)
• Sulfur (S)
• Selenium (Se)
• Tellurium (Te)
• Polonium (Po) - Metalloids and metals further down the group

Sulfur Trioxide and Water Reaction

One of the primary reactions involving Group 6A nonmetals is the reaction of sulfur trioxide \(SO_3\) with water.
This reaction is significant in both chemistry and environmental science.
When \(SO_3\) reacts with water \(H_2O\), it forms sulfuric acid \(H_2SO_4\).
This can be expressed as:
\[SO_3 + H_2O \rightarrow H_2SO_4\] Sulfuric acid is a strong acid and dissociates completely in water.
This reaction is highly exothermic, releasing a significant amount of heat.
It's important in industrial processes and environmental contexts since it contributes to acid rain formation.
Here's a brief summary of the reaction:

• Sulfur Trioxide: \(SO_3\)
• Reaction with Water: Forms sulfuric acid (\(H_2SO_4\))
• Type of Reaction: Exothermic

Writing Balanced Chemical Equations

Writing balanced chemical equations is an essential skill in chemistry.
It ensures that the same number of each type of atom appears on both sides of the equation.
Steps to balance a chemical equation:

• Write down the unbalanced equation.
• Count the number of atoms of each element on both sides.
• Add coefficients to balance the atoms, starting with the most complex molecule.
• Ensure all elements are balanced.
• Check your work by counting the atoms again.

For example, the balanced reaction of \(SO_3\) with water:
\[SO_3 + H_2O \rightarrow H_2SO_4\] In this equation:
Sulfur (S), oxygen (O), and hydrogen (H) atoms are balanced on both sides.
There is one sulfur atom, four oxygen atoms, and two hydrogen atoms on both sides.
Balancing chemical equations ensures the principle of conservation of mass is met and the stoichiometry of the reaction is correct.