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A sodium ion is represented as Na鈦�. Sodium atoms naturally have 11 protons and 11 electrons, but when they form an ion, they lose one electron. This results in a positively charged ion, as now there is one more proton than electrons. The original electron configuration of a neutral sodium (Na) atom is \(1s^2 2s^2 2p^6 3s^1\), with the last electron residing in the 3s shell. To become a sodium ion, the atom loses this outermost electron in the 3s orbital.

This means the sodium ion has the electron configuration of \(1s^2 2s^2 2p^6\), akin to that of a neon atom, a stable noble gas. These stable noble gas configurations are particularly sought after in nature due to their full outer electron shells.

The noble gas configuration refers to the particularly stable electron arrangements found in inert or noble gases. Noble gases, such as helium, neon, and argon, have fully filled outer electron shells. This full valence shell makes them highly stable and largely non-reactive with other elements. Elements in the periodic table naturally strive to revert to this state of stability.

For sodium, the loss of one electron to become Na鈦� results in the electron configuration \(1s^2 2s^2 2p^6\), matching that of neon, the closest noble gas. Achieving the noble gas configuration is often the driving force behind ion formation as atoms seek stability through the simplest path possible, which often involves gaining or losing electrons to have a completely filled outer energy level.

Electron arrangement is the distribution of electrons in an atom's electron shells and subshells. In the orderly filling of these shells, electrons first fill the lowest energy levels available before moving to higher ones. This is governed by several principles, such as the Aufbau principle and Hund's Rule.

For sodium, its electron arrangement starts with the filling of the 1s, 2s, and 2p subshells, resulting in \(1s^2 2s^2 2p^6\), before moving up to the 3s orbital where one electron is added, yielding \(3s^1\). However, upon ion formation, sodium gives away the 3s electron, reverting back to a noble gas-like stable arrangement. This electron redistribution mirrors the natural tendency of elements to reach the most stable electron configuration possible.

Ion formation involves the gain or loss of electrons in an atom, resulting in a charged particle called an ion. For an element like sodium, which readily loses electrons, this process occurs easily due to its electron configuration.

When sodium loses an electron during ion formation, it becomes a positively charged ion (cation). This process leads sodium to lose the single electron in its outermost 3s orbital, transforming the electron configuration from \(1s^2 2s^2 2p^6 3s^1\) to \(1s^2 2s^2 2p^6\). This loss is energetically favorable because it allows sodium to reach the stable electron configuration of the nearest noble gas, neon.

• Electrons are lost or gained to achieve stability.
• Cations form when electrons are lost, leading to positive charge.
• Anions form when electrons are gained, leading to negative charge.

Understanding ion formation is critical to predicting the behavior of elements in chemical reactions, as ions are essential participants in the formation of ionic compounds.