Write a balanced equation for the reaction that occurs in each of the following cases: (b) Strontium oxide is added to water. (c) A fresh surface of lithium metal is exposed to oxygen gas. (d) Sodium metal reacts with molten sulfur.

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Identify the reactants involved in the reaction. In this case, the reactants are lithium metal (Li) and oxygen gas (O2).

Determine the product of the reaction. When lithium reacts with oxygen, lithium oxide (Li2O) is formed.

Write the unbalanced chemical equation by placing the reactants on the left side and the product on the right side of the equation: \( \text{Li} + \text{O}_2 \rightarrow \text{Li}_2\text{O} \).

Balance the equation by adjusting the coefficients to ensure that the number of atoms for each element is the same on both sides of the equation. Start by balancing the lithium atoms and then the oxygen atoms.

Verify that the equation is balanced by counting the atoms of each element on both sides of the equation to ensure they are equal.

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Key Concepts

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

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms of 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. To balance an equation, coefficients are adjusted in front of the chemical formulas.

Combustion Reactions

Combustion reactions typically involve a substance reacting with oxygen to produce heat and light, often resulting in the formation of oxides. In the case of lithium, it reacts with oxygen to form lithium oxide. Understanding the general form of combustion reactions helps in predicting the products and balancing the equation.

Oxidation and Reduction

Oxidation and reduction (redox) reactions involve the transfer of electrons between substances. In the reaction between lithium and oxygen, lithium is oxidized as it loses electrons, while oxygen is reduced as it gains electrons. Recognizing the oxidation states of elements helps in identifying which species are oxidized and reduced in the reaction.

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(a) As described in Section 7.7, the alkali metals react with hydrogen to form hydrides and react with halogens to form halides. Compare the roles of hydrogen and halogens in these reactions. Write balanced equations for the reaction of fluorine with calcium and for the reaction of hydrogen with calcium. (b) What is the oxidation number and electron configuration of calcium in each product?