Question

Which element is more likely to form chemical bonds: xenon (Xe) or sodium (Na)? Explain why.

Short answer

Sodium (Na) is more likely to form chemical bonds because it has one electron to lose for stability, unlike xenon (Xe), which is already stable.

Step-by-step solution

Understanding Chemical Bonds

Chemical bonds occur when atoms interact to achieve a stable electronic configuration. Elements form bonds to achieve a full outer shell of electrons, often following the octet rule, which means having eight electrons in their outer shell.

Analyzing Xenon's Properties

Xenon (Xe) is part of the noble gases, which have complete outer electron shells. Xenon has an atomic number of 54 with a full outer shell (8 electrons in the outer shell), making it very stable and largely unreactive under normal conditions.

Analyzing Sodium's Properties

Sodium (Na) is an alkali metal with an atomic number of 11. It has one electron in its outer shell and desires to lose this electron to achieve the stable electronic configuration of the noble gas neon, which means it is highly reactive and eager to form bonds.

Comparing Reactivity Based on Electronic Configuration

Elements with incomplete outer electron shells, like sodium, are more likely to form bonds to fulfill the octet rule. Xenon has a complete set of outer electrons, making it stable and unlikely to form bonds under normal conditions.

Final Conclusion

Due to the difference in electron configuration, sodium, with its single electron in the outer shell, is much more likely to form chemical bonds compared to xenon, which has a full outer shell and is stable on its own.

Key concepts

Xenon Chemistry

Xenon is a fascinating element among the noble gases. As a noble gas, it is known for its stability and reluctance to react. Xenon's atomic number is 54, which means it has 54 protons and 54 electrons.
The electrons are arranged in shells around the nucleus, and xenon's outer shell is fully occupied with eight electrons. This full outer shell makes xenon a stable element, and under normal conditions, it does not need to form chemical bonds to achieve stability.
● Xenon's stability makes it unreactive, but under extreme conditions, such as high pressure or the presence of strong electronegative elements, xenon can form compounds.
● A well-known example of xenon's chemical activity is the formation of xenon hexafluoroplatinate, which requires specific conditions for xenon to bond with fluorine and platinum.
Though xenon does not form bonds easily, its ability to do so under certain circumstances makes it an exciting subject of study in chemistry.

Sodium Reactivity

Sodium is an essential element situated among the alkali metals in the periodic table. With an atomic number of 11, sodium has 11 electrons with only one electron in its outermost shell, which plays a critical role in its chemical behavior.
Alkali metals, including sodium, are characterized by their extreme reactivity. Sodium readily loses its lone valence electron to achieve a stable electron configuration resembling that of neon, a noble gas.
● When sodium reacts, it often forms ionic bonds by transferring its outer electron to another element, completing its outer shell.
● A common example of sodium's reactivity is its reaction with water, where it forms sodium hydroxide and releases hydrogen gas.
This intense reactivity makes sodium highly valuable in various chemical processes and industrial applications. Sodium's eager formation of bonds ensures that it is frequently involved in chemical reactions.

Noble Gases

Noble gases, including helium, neon, argon, krypton, xenon, and radon, are known for their lack of reactivity. This group of elements is located in the far-right column of the periodic table.
The defining characteristic of noble gases is their complete outer electron shells. Having a full set of electrons in their valence shell means they have little tendency to gain, lose, or share electrons.
● This stability makes noble gases, under normal circumstances, largely nonreactive.
● They exist as monatomic gases, meaning each atom retains its independence.
However, noble gases can participate in chemical reactions under specific conditions, such as high pressures or with strong reactants, leading to the formation of some interesting and rare compounds.

Alkali Metals

Alkali metals comprise elements like lithium, sodium, potassium, rubidium, cesium, and francium. These elements occupy the first column of the periodic table and share several notable characteristics, primarily due to their single valence electron.
This lone valence electron influences alkali metals' desire to achieve stability by shedding that electron, thus readily participating in chemical reactions.
● They are extremely reactive, particularly with water and halogens, and must be stored under oil or an inert atmosphere to prevent unwanted reactions.
● Their reactions are often vigorous and may be explosive, as seen when sodium or potassium comes into contact with water.
The high reactivity of alkali metals makes them crucial in a diverse range of applications, from making powerful batteries to playing essential roles in biological systems.