Write a balanced equation for the reaction that occurs in each of the following cases: (d) Fluorine reacts with water.

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Identify the reactants and products in the reaction. Fluorine (F_2) reacts with water (H_2O).

Determine the products of the reaction. Fluorine is a strong oxidizing agent and will react with water to form oxygen difluoride (OF_2) and hydrogen fluoride (HF).

Write the unbalanced chemical equation: F_2 + H_2O \(\rightarrow\) OF_2 + HF.

Balance the equation by adjusting coefficients to ensure the same number of each type of atom on both sides of the equation.

Check the balanced equation to confirm that the number of atoms for each element is equal on both sides.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Chemical Reactions

A chemical reaction involves the transformation of reactants into products through the breaking and forming of chemical bonds. Understanding the types of reactions, such as synthesis, decomposition, and redox reactions, is essential for predicting the products formed. In this case, recognizing that fluorine is a highly reactive halogen helps anticipate its behavior when reacting with water.

Balancing Chemical Equations

Balancing chemical equations is the process of ensuring that the number of atoms for each element is the same on both sides of the equation. This is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. Proper balancing is crucial for accurately representing the stoichiometry of the reaction.

Fluorine and Water Reaction

When fluorine reacts with water, it undergoes a highly exothermic reaction, producing hydrofluoric acid and oxygen. This reaction is significant due to fluorine's strong oxidizing properties and the potential hazards associated with hydrofluoric acid. Understanding the products formed and their implications is vital for safely handling such reactions.

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