SnO can be prepared by: (1) Boiling a stannous chloride solution with \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) (2) Heating tin hydroxide in air (3) Heating tin oxalate \(\left(\mathrm{SnC}_{2} \mathrm{O}_{4}\right)\) in absence of air (a) 1 and 2 (b) 2 and 3 (c) 1,2 and 3 (d) 1 and 3

The reaction of stannous chloride (SnCl₂) with other chemical compounds is a fundamental procedure within inorganic chemistry, particularly in the synthesis of tin oxides. For example, when SnCl₂ is combined with sodium carbonate (Na₂CO₃), a chemical exchange takes place between the anions and cations of the reacting species.

Depending on the reaction conditions such as temperature, concentration, and the presence of oxygen, different products can be formed. Ideally, SnO could be one of the products when SnCl₂ is carefully reacted with Na₂CO₃. However, stannous chloride can also react to form stannic oxide (SnO₂), especially if there's excess oxygen. This demonstrates the importance of reaction conditions in the successful preparation of the desired tin oxide, in this case, SnO.

A controlled environment is critical to ensure that the product of the stannous chloride reaction is indeed stannous oxide and not stannic oxide or another unintended compound. This means that although stannous chloride has the potential to produce SnO, the reaction must be carefully managed to ensure its success. Thus, this method is not foolproof for exclusive SnO production.

Chemical synthesis of oxides involves various methods and principles to produce oxides from different precursor substances. In inorganic chemistry, oxides such as SnO can be synthesized through direct combination reactions, decomposition of complex compounds, or via exchange reactions.

Synthesis of tin(II) oxide, or SnO, can be approached by methods like boiling a stannous chloride solution with sodium carbonate or by heating tin hydroxide in the presence of air. The principle behind both methods involves a transformation from a compound with a different anion or functional group to the oxide form.

In the first method, the desired product SnO might be produced alongside other byproducts such as sodium chloride (NaCl), and the synthesis must be closely monitored to ensure the correct product is obtained. In the second method, the presence of air plays a crucial role. Normally, air would oxidize tin to a higher oxide, but with careful control over the reaction conditions, one can preferentially produce SnO instead of SnO₂. Each of these methods demonstrates the need for careful control of the reaction environment to obtain the desired oxide. This highlights the precise nature of oxide synthesis and the requirement for an understanding of how different conditions affect the outcome.

Inorganic chemistry reactions, like the preparation of oxides, showcase complex interactions between elements and compounds, resulting in a diversity of products based on the reactants and conditions employed. Reactions in inorganic chemistry are governed by principles such as redox reactions, precipitation, complexation, and decomposition, among others.

When heating tin oxalate (SnC₂O₄) in the absence of air, a decomposition reaction takes place. The oxalate decomposes, releasing gases like CO and CO₂, and leaving behind SnO. The absence of oxygen is vital to prevent further oxidation to SnO₂, thereby ensuring the production of SnO exclusively. This highlights how manipulating the reaction environment—in this case, the absence of air—can lead to the controlled synthesis of a specific oxide.

These inorganic reactions contribute crucially to the understanding of material synthesis and chemical transformation. Mastery of these reactions not only empowers chemists to design and create new materials but also equips them to predict and manage the outcomes of different chemical processes.