Problem 109 - A Complete Resource Book in Chemistry for JEE Main

Question

Which of the following is an explosive compound? (a) \(\mathrm{XeOF}_{2}\) (b) \(\mathrm{XeF}_{2}\) (c) \(\mathrm{XeO}_{3}\) (d) \(\mathrm{XeOF}_{4}\)

Step-by-Step Solution

Answer

\( \mathrm{XeO}_{3} \) is the explosive compound.

Step 1: Understand the Nature of Xenon Compounds

Xenon is a noble gas that can form several compounds, particularly with oxygen and fluorine, due to its ability to expand its octet. Among these, some xenon compounds are known to be highly explosive, especially those with higher oxidizing potential.

Step 2: Evaluate the Structure and Oxidation States

Evaluate the oxidation states of xenon in each compound:(a) In \( \mathrm{XeOF}_{2} \), xenon has an oxidation state of +4.(b) In \( \mathrm{XeF}_{2} \), xenon has an oxidation state of +2.(c) In \( \mathrm{XeO}_{3} \), xenon has an oxidation state of +6.(d) In \( \mathrm{XeOF}_{4} \), xenon has an oxidation state of +6.

Step 3: Identify Explosive Xenon Compound

Explosive xenon compounds are often those with higher oxidation states as they are strong oxidizers, which makes them unstable and prone to explosive reactions. From the options, \( \mathrm{XeO}_{3} \) is known to be highly explosive due to xenon’s +6 oxidation state and its strong oxidizing properties.

Key Concepts

Oxidation States in Xenon Compounds

Xenon's ability to form compounds is largely dictated by its oxidation states. Typically viewed as inert, this noble gas surprises many with its chemistry. It can reach oxidation states as high as +8. In xenon compounds, the oxidation state of xenon depends on the other atoms it is bonded with—usually fluorine or oxygen. For example, in the compound \( \mathrm{XeO}_{3} \), xenon exhibits an oxidation state of +6 because oxygen is a highly electronegative element, pulling electrons away and allowing xenon to assume a larger positive oxidation state. Understanding oxidation states helps us predict the reactivity and potential explosiveness of a compound. The higher the oxidation state, the stronger the oxidizing potential, and the more likely it is for the compound to exhibit explosive characteristics.

Properties of Explosive Compounds

Explosive compounds often have very high oxidizing capacities. This means they can quickly release oxygen atoms in a reaction, producing energy explosively. Xenon trioxide \( \mathrm{XeO}_{3} \) is an exemplary explosive compound due to xenon's ability to take on a +6 oxidation state. This gives it strong oxidizing properties. A few key attributes that contribute to the explosiveness of a compound are:

• High oxidation states, providing excess oxidation potential.
• Instability in the molecular structure, which can easily collapse.
• Presence of elements that can undergo rapid oxidation-reduction reactions.

The instability and high energy release, especially when triggered by external factors such as heat or shock, are why \( \mathrm{XeO}_{3} \) and similar compounds are considered dangerous.

Chemistry of Noble Gases

Noble gases, including xenon, are traditionally known for their lack of reactivity due to fully filled valence shells. Yet, xenon's chemistry challenges this stereotype, thanks to its capacity to form several compounds, particularly oxides and fluorides. The chemistry of noble gases involves some fascinating concepts:

• Formation of compounds usually require extreme conditions, like high pressure or the presence of highly electronegative elements.
• The compounds are often extremely reactive or unstable, especially those involving higher oxidation states.
• The ability of xenon to expand its octet—going beyond the typical eight electrons in the valence shell—enables it to participate in diverse bonding scenarios.

Despite being labeled as inert, noble gases like xenon offer a playground of chemical exploration, emphasizing the versatility and depth of chemical behavior across the periodic table.