Lithium and magnesium exhibit a diagonal relationship in some chemical properties. How does lithium resemble magnesium in its reaction with oxygen and nitrogen? Consult a handbook of chemistry and compare the solubilities of carbonates, fluorides, and phosphates of these metals.

Lithium, the lightest metal in the periodic table, participates in several reactions due to its high reactivity. It reacts with oxygen to form lithium oxide ((Li_2O)), a white powdery solid. In a reaction with water, lithium produces lithium hydroxide ((LiOH)) and hydrogen gas, indicating its high reactivity even with moist air. Lithium similarly reacts with nitrogen, albeit less aggressively than with oxygen, to form lithium nitride ((Li_3N)), which is less common than its oxide.

When lithium encounters acids, it releases hydrogen gas and forms the respective lithium salt. Despite lithium's reactivity, it forms compounds that tend to be less soluble in water compared to those of alkaline earth metals, highlighting the unique aspects of its chemical behavior.

Magnesium shares some similarities with lithium in its chemical reactions, despite being positioned differently in the periodic table. Like lithium, magnesium readily reacts with oxygen to form magnesium oxide ((MgO)), which is a white solid possessing a high melting point and is commonly used as a refractory material. With nitrogen, magnesium forms magnesium nitride ((Mg_3N_2)), which, like lithium nitride, is less commonly encountered than the oxide.

Magnesium also reacts with acids, releasing hydrogen gas and forming magnesium salts. Unlike lithium, magnesium's compounds frequently exhibit higher solubility in water. The aforementioned differences in solubility patterns between lithium and magnesium compounds underscore the unique diagonal relationship these two elements share.

The solubility of ionic compounds varies with each metal and anion pair, influenced by factors such as the lattice energy of the solid and the hydration energy of the ions when dissolved. For example, lithium carbonate ((Li_2CO_3)) is only slightly soluble in water due to its high lattice energy, while lithium fluoride ((LiF)) is almost insoluble because of the strong ionic bond between lithium and fluoride ions.

Conversely, magnesium carbonate ((MgCO_3)) is insoluble, and magnesium fluoride ((MgF_2)) displays slight solubility. These solubility patterns reflect the ionic character and the balance of forces at play within these compounds, an essential consideration for understanding their behavior in different environments.

The formation of oxides is a common chemical process for both lithium and magnesium. Upon exposure to oxygen, lithium reacts to form lithium oxide, while magnesium forms magnesium oxide. These oxides are ionic compounds, featuring high melting points and stability due to the strong ionic bonds between the metal cations and oxide anions.

These oxides are important industrial materials; for instance, magnesium oxide is used in refractory linings for furnaces. The formation of these oxides is not only a simple reaction of metals with oxygen but also a demonstration of the trends in chemical properties across the periodic table.

Nitrides are compounds of nitrogen with a less electronegative element, such as lithium or magnesium. When these metals react with nitrogen, they form nitrides: lithium nitride ((Li_3N)) and magnesium nitride ((Mg_3N_2)). These reactions typically require high temperatures as nitrogen is relatively inert at room temperature.

While lithium nitride and magnesium nitride have different formulations due to their differing valencies, they both reveal the capabilities of lithium and magnesium to form compounds with nitrogen — an attribute not commonly seen with many other metals. Understanding the formation of nitrides helps in the study of high-temperature materials and the stoichiometry of chemical compounds.