Sodium reacts vigorously with water to produce

Analysis

The question asks for the products formed when a Group 1 metal (Sodium) reacts with water. This is a classic displacement reaction involving an alkali metal.

Concept

Group 1 metals (the alkali metals) are highly reactive. When they react with water, they displace hydrogen from the water molecule. The general equation for this reaction is: Metal + Water → Metal Hydroxide + Hydrogen Gas

Because sodium is very reactive, this reaction is exothermic (releases heat), which is why it is described as "vigorous."

Solution

1. Identify the reactants: Sodium (Na) and Water ($H_2O$).
2. Write the chemical equation: $2Na(s) + 2H_2O(l) \rightarrow 2NaOH(aq) + H_2(g)$
3. Break down the products: • $NaOH$ (Sodium Hydroxide): This is an alkaline solution, which is why Group 1 metals are called "alkali metals." • $H_2$ (Hydrogen gas): This is released as a gas, often causing the sodium to fizz and move rapidly across the surface of the water.

Comparing this to your options:

• Option A is incorrect because chlorine is not present in the reactants.
• Option B is incorrect because nitrogen is not present in the reactants.
• Option C matches our chemical equation perfectly.
• Option D is incorrect because the primary product in water is the hydroxide, not the oxide.

Conclusion

The reaction between sodium and water produces sodium hydroxide and hydrogen gas. This matches option C.

Exam Tip

Remember the acronym "MAHO" for Group 1 metals reacting with water: Metal + Aqua (water) → Hydroxide + Oxygen (wait, no—Hydrogen!). Just remember: Metal + Water → Hydroxide + Hydrogen. Also, always remember that alkali metals are stored in oil to prevent them from reacting with moisture in the air!