Question

Complete the following reactions: (a) \(\mathrm{XeF}_{4}+\mathrm{SF}_{4}\) (b) \(\mathrm{XeF}_{6}+\mathrm{H}_{2} \mathrm{O}\) (c) \(\mathrm{XeF}_{6}+\mathrm{NaF}\) (d) \(\mathrm{KrF}_{2}+\mathrm{SbF}_{5}\) (e) \(\mathrm{HXeO}_{4}^{-}+\mathrm{OH}^{-}\)

Short answer

The complete reactions are: (a) \(\mathrm{XeF}_{4}+\mathrm{SF}_{4} \rightarrow \mathrm{Xe}+\mathrm{SF}_{6}\), (b) \(\mathrm{XeF}_{6}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{XeO}_{3}+ 3\mathrm{HF}\),(c) \(\mathrm{XeF}_{6}+ \mathrm{NaF} \rightarrow \mathrm{Na}[\mathrm{XeF}_{7}]\),(d) \(\mathrm{KrF}_{2}+\mathrm{SbF}_{5} \rightarrow \mathrm{Kr}+2[\mathrm{SbF}_{6}^{-}]\),(e) \(\mathrm{HXeO}_{4}^{-}+\mathrm{OH}^{-} \rightarrow \mathrm{XeO}_{4}+ \mathrm{H}_{2}\mathrm{O}\).

Step-by-step solution

Identification of Reactants

First, identify the reactants. Noting the types of bonds they have, the types of reactions they usually undergo, and their general reactivity can be helpful. This applies to each reaction.

Predicting the Products

Based on the characteristics of the reactants, predict the possible products. Remember the laws of conservation of mass and charge - you have to balance all reactions. Here are the balanced equations for each part: (a) \(\mathrm{XeF}_{4}+\mathrm{SF}_{4} \rightarrow \mathrm{Xe}+\mathrm{SF}_{6}\), (b) \(\mathrm{XeF}_{6}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{XeO}_{3}+ 3\mathrm{HF}\), (c) \(\mathrm{XeF}_{6}+ \mathrm{NaF} \rightarrow \mathrm{Na}[\mathrm{XeF}_{7}]\),(d) \(\mathrm{KrF}_{2}+\mathrm{SbF}_{5} \rightarrow \mathrm{Kr}+2[\mathrm{SbF}_{6}^{-}]\),(e) \(\mathrm{HXeO}_{4}^{-}+\mathrm{OH}^{-} \rightarrow \mathrm{XeO}_{4}+ \mathrm{H}_{2}\mathrm{O}\)

Checking the Products

Check that the formulas of the products are correct and that the equations are balanced. The compound formulas must correspond to the established principles of chemical bonding and compound formation. Proper balancing ensures that the number and type of atoms in reactants equals the number and type in the products.

Key concepts

Balancing Chemical Equations

Balancing chemical equations is pivotal in chemistry to reflect the law of conservation of mass. This law states that in a chemical reaction, the mass of the products must equal the mass of the reactants. To balance an equation, we ensure that the number of atoms for each element is the same on both sides of the reaction.

For instance, consider the reaction where xenon hexafluoride (XeF6) reacts with sodium fluoride (NaF). The balanced chemical equation is \(\text{XeF6} + \text{NaF} \rightarrow \text{Na}[XeF7]\). Here, we have seven fluorine atoms on both sides, one xenon atom, and one sodium atom, adhering to the conservation of mass.

In balancing equations, there are simple rules to follow: start with compounds containing the most complex set of elements and end with the simplest substance, usually a pure element. Additionally, polyatomic ions that appear unchanged on both sides can be treated as a single unit. Practice is essential to master this skill, as it forms the foundation for understanding chemical reactions comprehensively.

Noble Gas Compounds

Noble gases are known for their lack of chemical reactivity due to their full valence electron shells, which make them quite stable. However, a few noble gases, particularly xenon (Xe) and krypton (Kr), can form compounds under certain conditions. These noble gas compounds are fascinating due to their rarity and unusual bonding.

Xenon, for example, forms compounds such as XeF4 and XeF6. These are powerful fluorinating agents and are used in various chemical reactions. The reaction of XeF4 with sulfur tetrafluoride (SF4) generating xenon and sulfur hexafluoride (SF6) is a classic example. The equation is \(\text{XeF4} + \text{SF4} \rightarrow \text{Xe} + \text{SF6}\).

It's important to understand that these compounds, while rare, are proof of the fact that even the most chemically inert elements can participate in reactions under the right conditions, revealing the nuanced complexity of chemical bonding and reactivity.

Chemical Reactivity

Chemical reactivity refers to the tendency of a substance to engage in chemical reactions. Reactivity is influenced by various factors, including the atom's electron configuration, bonding, structure, and the presence of catalysts. It governs how and why certain chemicals react with others and the speed or rate at which they do so.

In our example reactions involving noble gas compounds, we observe that the presence of highly electronegative fluorine (F) facilitates the formation of noble gas compounds and their subsequent reactions. For instance, krypton difluoride (KrF2) can react with antimony pentafluoride (SbF5), showing that Kr, under specific conditions, can be chemically reactive despite being a noble gas.

Understanding chemical reactivity is essential for predicting reactions, as seen in these exercises. Knowing how to balance chemical equations and being aware of the properties of noble gas compounds contribute to a holistic understanding of reactivity in chemistry.