Magnesium metal burns in oxygen to form magnesium oxide, MgO. (a) Write a balanced equation for the reaction.

Verified step by step guidance

1. Identify the reactants and products: Magnesium (Mg) and oxygen (O₂) are the reactants, and magnesium oxide (MgO) is the product.
2. Write the unbalanced chemical equation: Mg + O₂ → MgO.
3. Balance the equation by adjusting coefficients: Start by balancing the number of oxygen atoms. Since O₂ has 2 oxygen atoms, you need 2 MgO to balance the oxygen atoms, resulting in Mg + O₂ → 2 MgO.
4. Balance the magnesium atoms: Since there are 2 MgO molecules, you need 2 Mg atoms on the reactant side, resulting in 2 Mg + O₂ → 2 MgO.
5. Verify the balance: Ensure that there are equal numbers of each type of atom on both sides of the equation. There are 2 Mg atoms and 2 O atoms on each side, confirming the equation is balanced.

Key Concepts

Balancing Chemical Equations

Balancing chemical equations is essential to ensure that the law of conservation of mass is upheld, meaning the number of atoms of each element must be the same on both sides of the equation. This involves adjusting coefficients in front of the chemical formulas to achieve balance, reflecting the actual stoichiometry of the reaction.

Combustion Reactions

Combustion reactions involve a substance (usually a hydrocarbon or metal) reacting with oxygen to produce heat and light, often resulting in the formation of oxides. In the case of magnesium, it reacts with oxygen to form magnesium oxide, illustrating a typical combustion reaction where a metal burns in the presence of oxygen.

Stoichiometry

Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It allows chemists to predict the amounts of substances consumed and produced in a reaction, which is crucial for writing balanced equations and understanding the proportions in which elements combine.