Question

Magnesium metal is very malleable and is able to be pounded and stretched into long, thin, narrow “ribbons” that are often used in the introductory chemistry lab as a source of the metal. If a strip of magnesium ribbon is ignited in a Bunsen burner flame, the magnesium burns brightly and produces a quantity of white magnesium oxide powder. From the information given above, indicate one chemical property of magnesium metal.

Short answer

One chemical property of magnesium metal is its reactivity with oxygen, which allows it to form compounds such as magnesium oxide (MgO).

Step-by-step solution

Observe the reaction

When magnesium ribbon is ignited in a Bunsen burner flame, it burns brightly and produces a white magnesium oxide powder. This reaction can be represented by a chemical equation: Magnesium (Mg) + Oxygen (O2) -> Magnesium Oxide (MgO)

Identify the chemical property

As magnesium combines and reacts with oxygen to form magnesium oxide, this tells us that magnesium has the ability to form compounds by reacting with other elements, which in this case is oxygen. This key aspect denotes the chemical property being exhibited.

Conclusion

From the given information, one chemical property of magnesium metal is its ability to react with oxygen to form magnesium oxide. This illustrates magnesium's reactivity with oxygen and its capability to form compounds.

Key concepts

Magnesium Combustion

Magnesium is a versatile metal that is widely used for its physical and chemical properties. One of its most captivating chemical behaviors is combustion. When you ignite a magnesium ribbon using a Bunsen burner, it burns with an intense white flame. This brilliant brightness occurs because magnesium reacts exothermically when ignited. The term 'exothermic' means that the reaction releases energy in the form of light and heat. This property makes magnesium an interesting subject in many chemistry experiments, especially those focusing on thermal and combustion processes.

• Magnesium ignites at a relatively high temperature of around 3102°F (1710°C).
• It produces a bright white flame, due to the energy being released.
• The reaction is a showcase of magnesium's oxidative ability when combined with suitable elements like oxygen.

Overall, the combustion of magnesium not only highlights its reactive nature but also provides a visual representation of chemical reactions involving metals.

Reactivity with Oxygen

A key component in understanding magnesium's chemical properties is its reactivity with oxygen. This reactivity is crucial as it reveals magnesium's ability to participate in chemical reactions to form new substances.Magnesium, when exposed to air, reacts readily with oxygen to form magnesium oxide. This chemical reaction can be expressed by the equation: \[ \text{Mg} + \text{O}_2 \rightarrow \text{MgO} \]

• The reaction between magnesium and oxygen is a redox reaction, involving the transfer of electrons.
• Magnesium loses electrons to become Magnesium ions \( \text{Mg}^{2+} \).
• Oxygen gains electrons to form oxide ions \( \text{O}^{2-} \).

This readiness to react with oxygen makes magnesium an excellent material for demonstrations in introductory chemistry classes, helping to illustrate fundamental redox reactions.

Magnesium Oxide Formation

When magnesium burns in the presence of oxygen, it forms magnesium oxide. This compound is a white powdery substance that is very different in properties from elemental magnesium. Understanding this transformation helps in grasping the changes materials undergo during chemical reactions.

Significance of Magnesium Oxide

Magnesium oxide (MgO) is not only a product of magnesium combustion but is also widely used in various applications.

• It serves as a refractory material, able to withstand high temperatures.
• Is utilized in medicine as a component in some antacids and laxatives.
• Acts as a flame retardant in various materials owing to its stability at high temperatures.

This transformation from a solid metal to a white powdered compound illustrates the principles of chemical change: altering structures and forming new materials with distinct properties. Such experiments are foundational to learning how compounds are formed and understanding the broader concept of chemical reactions.