Question

Law of multiple proportions is not applicable for the oxide(s) of (a) carbon (b) iron (c) nitrogen (d) aluminium

Short answer

Answer: Nitrogen

Step-by-step solution

Understanding the Law of Multiple Proportions

According to the Law of Multiple Proportions, when two elements form more than one compound, the masses of one element that combine with a fixed mass of the other element are in the ratio of small whole numbers.

Analyzing the oxides of each element

Now we will analyze the oxide compositions of each element given in the options. (a) Carbon Carbon forms two oxides: carbon monoxide (CO) and carbon dioxide (CO\(_2\)). The ratio of oxygen masses combining with a fixed mass of carbon in these two compounds is 1:2, which is a small whole number ratio. (b) Iron Iron forms two oxides: ferrous oxide (FeO) and ferric oxide (Fe\(_2\)O\(_3\)). For ferrous oxide, with a fixed mass of iron (1 mole), 1 mole of oxygen combines. In ferric oxide with fixed mass of iron (2 moles), 3 moles of oxygen combines. The ratio of oxygen masses combining with the fixed mass of iron in these two compounds is 3:4, which is a small whole number ratio. (c) Nitrogen Nitrogen forms several oxides: nitrous oxide (N\(_2\)O), nitric oxide (NO), nitrogen dioxide (NO\(_2\)), and nitrogen pentoxide (N\(_2\)O\(_5\)). The ratios of oxygen masses combining with a fixed mass of nitrogen in these compounds are not in small whole number ratios. (d) Aluminium Aluminium forms only one oxide: aluminium oxide (Al\(_2\)O\(_3\)). Since there is only one compound, the Law of Multiple Proportions does not apply.

Conclusion

From the analysis above, we can see that the Law of Multiple Proportions is not applicable for the oxide(s) of nitrogen (option (c)) as stated in Step 2.

Key concepts

Oxide Compositions

Understanding the oxide compositions of different elements is key to analyzing how they form compounds. For example, carbon can form two different oxides: carbon monoxide (CO) and carbon dioxide (CO\(_2\)). These compounds showcase how varying amounts of oxygen can combine with a fixed amount of carbon. The study of these oxide compositions helps us grasp the concept of how elements interact with oxygen to form distinctive compounds.

• Carbon Oxides: Carbon monoxide (CO) and carbon dioxide (CO\(_2\)) highlight a clear difference in oxygen proportion.
• Iron Oxides: Iron forms compounds like ferrous oxide (FeO) and ferric oxide (Fe\(_2\)O\(_3\)), each with varying oxygen quantities.
• Nitrogen Oxides: Nitrogen's multiple oxides including N\(_2\)O, NO, NO\(_2\), and N\(_2\)O\(_5\) showcase its complexity.
• Aluminium Oxide: Aluminium forms a single stable compound, Al\(_2\)O\(_3\).

Studying these compositions is essential for understanding more complex chemical concepts, such as the Law of Multiple Proportions.

Element Compound Analysis

When looking at the compounds that an element can form, it's important to examine how different elements react with oxygen to create various oxides. Element compound analysis involves studying the number and types of compounds formed by an element with oxygen.
By doing so, one can better identify the potential ratios of oxygen to the specific element itself. This analysis allows us to determine whether the mass ratios of oxygen to the element comply with certain chemical laws, like the Law of Multiple Proportions.
Iron, for example, forms distinct oxides at different proportions of iron and oxygen, highlighting the outcomes of detailed compound analysis. In comparison, aluminum yields only one oxide form. This limits the applicability of certain chemical laws in its case. Such analysis lays the groundwork for more in-depth chemical and scientific research, contributing to advancements in chemistry.

Chemical Laws

Chemical laws like the Law of Multiple Proportions provide scientists with a structured way to understand the complex behaviors of elements and compounds. This particular law states that if two elements can form more than one compound, the masses of one element that combine with a fixed mass of the other are in small whole number ratios.
In practice, for instance, this law is observed in carbon oxides:

• CO: Mass ratio of oxygen to carbon.
• CO\(_2\): Different mass ratio of oxygen to carbon.

These ratios exemplify small whole numbers as predicted by the law. However, for elements like aluminium which only form a single oxide, this law is not applicable. Understanding these chemical principles provides clarity on how different elements combine and form various compounds under established scientific guidelines.

Oxygen Ratios

The concept of oxygen ratios is integral to studying chemical reactions, particularly in how elements form oxides. By observing the ratios in which oxygen atoms bond with a fixed mass of another element, scientists can deduce significant information about the compound's structure.
The varying oxygen ratios are evident with elements such as iron and carbon, which each form multiple oxides. For iron:

• FeO: Iron and oxygen combine in a 1:1 ratio.
• Fe\(_2\)O\(_3\): A more complex 2:3 combination.

Carbon follows a 1:1 and 1:2 pattern in its oxides. On the other hand, nitrogen oxides do not always follow simple whole number ratios, demonstrating more chemical complexity. Understanding these ratios helps in identifying new compounds, predicting reactions, and exploring potential uses in various applications.