Question

The more reactive an atom, the higher its potential energy. Which atom has higher potential energy, neon or fluorine? Explain.

Short answer

Fluorine has a higher potential energy than neon, as it is more reactive due to its incomplete outer electron shell (2s²2p⁵), whereas neon's stable, completely filled outer electron shell (1s²2s²2p⁶) makes it less reactive and gives it lower potential energy.

Step-by-step solution

Understanding Atomic Reactivity and Potential Energy

Atomic reactivity depends on the electron configuration of an atom. More reactive atoms tend to have electron configurations that are not stable, with incompletely filled outer electron shells. These atoms have a higher potential energy because they are more likely to undergo chemical reactions and have a higher tendency to bond with other atoms or gain/lose electrons. Conversely, atoms with stable electron configurations have completely filled outer electron shells, making them less likely to react. These atoms are less reactive and have lower potential energy.

Electron Configurations of Neon and Fluorine

Let's look at the electron configurations of neon and fluorine to understand their reactivity. Neon (Ne) has an atomic number of 10. Its electron configuration is: 1s²2s²2p⁶ Fluorine (F) has an atomic number of 9. Its electron configuration is: 1s²2s²2p⁵ Neon has a completely filled outer electron shell (2s²2p⁶), while fluorine has an incomplete outer electron shell (2s²2p⁵).

Assessing Reactivity and Potential Energy

Since neon has a completely filled outer electron shell, it is stable and less likely to react with other atoms. This makes neon less reactive and suggests it has lower potential energy. On the other hand, fluorine has an incomplete outer electron shell, making it more likely to react with other atoms in order to complete its outer electron shell. This means that fluorine is more reactive and has a higher potential energy than neon.

Conclusion

In conclusion, fluorine has a higher potential energy than neon, because it is more reactive due to its incomplete outer electron shell (2s²2p⁵) compared to neon's stable, completely filled outer electron shell (1s²2s²2p⁶).

Key concepts

Atomic Reactivity

Exploring the concept of atomic reactivity is foundational to understanding the energy dynamics within an atom. Atoms are more than tiny particles; they are the basic units of matter with electrons buzzing around their nucleus in specific layers or 'shells.' These layers are vital when we talk about atomic reactivity. Elements with incomplete outer shells tend to be like guests at a party avidly seeking companions to interact with—this searching is actually atoms trying to achieve stability by filling their outer shell, making them more reactive.

On the flip side, atoms that lounge around with full outer shells are the ones enjoying the peace. Neon is one such element with a full dance card, so to speak. Its outer shell is complete, so it's less likely to boogie with other elements. This makes neon's reactivity and potential energy significantly lower than an atom like fluorine, which has an available seat in its outer shell and is eagerly looking to fill it.

Electron Configuration

Consider electron configuration as the address of electrons within an atom. It tells us where electrons live and how they're spread out across different shells and subshells. Picture a block of apartments—the configuration tells you which levels are fully occupied and which ones still have vacancies.

Each atom strives for the most stable arrangement, which usually mirrors the noble gases confetti—full and satisfied. This is precisely what's happening with neon: a perfect electron count in its outer shell makes it content and stable (1s²2s²2p⁶). But for fluorine, there's that one pesky vacancy (1s²2s²2p⁵) that makes it a bit like that one guy actively searching for a roommate. Thus, electron configuration helps us understand why certain atoms are more reactive: they want to reach their nirvana of full occupancy.

Chemical Reactions

Chemical reactions are like the universe's dating scene, with atoms meeting and deciding whether to form bonds based on their electron configurations. An atom with a lonely seat in its outer shell, like fluorine, will react more enthusiastically when it encounters another atom that can offer an electron to fill that gap. This reaction is not just a matter of preference but of reaching a lower, more stable energy level.

In contrast, atoms like neon are the hermits of the elemental world—they are already in their comfort zone, with no desire to change or react. This stability means that their potential energy remains unaffected while the eager fluorine, anxiously awaiting interactions, displays high atomic potential energy. We can say that the reactivity of an atom significantly influences the type and number of chemical reactions it can engage in, making its potential energy an important player in the predictability and outcomes of such encounters.