Analyze the properties of a sodium atom and a sodium ion. What are the differences in mass, stability, and reactivity that are caused due to the differences between the sodium atom and sodium ion?

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To analyze the properties of a sodium atom and a sodium ion, we need to understand their structures and the changes that occur when sodium atoms lose or gain electrons.

1. Sodium Atom:
A sodium atom has an atomic number of 11 and consists of 11 protons and 11 electrons. The protons are located in the nucleus, while the electrons orbit around the nucleus in energy levels or shells. In its ground state, the electron configuration of a sodium atom is 2-8-1, where the outermost energy level (valence shell) contains a single electron.

2. Sodium Ion:
A sodium ion is formed when a sodium atom loses an electron. Since sodium atoms tend to lose electrons easily, they form a sodium ion with a charge of +1. When a sodium atom loses an electron, it still retains the 11 protons in its nucleus but now has only 10 electrons. The electron configuration of a sodium ion becomes 2-8.

Differences in Mass:
The mass of a sodium atom is determined by the combined mass of its protons, neutrons, and electrons. With 11 protons and 11 electrons, the sodium atom has an equal number of protons and electrons, resulting in a net charge of zero. The mass of a sodium atom is therefore the sum of the masses of its 11 protons, 11 neutrons (in most cases), and 11 electrons.

On the other hand, the mass of a sodium ion is slightly smaller than that of a sodium atom due to the loss of one electron. Since electrons have a negligible mass compared to protons and neutrons, the loss of one electron has a minimal effect on the overall mass of the ion. So, sodium ions have slightly less mass than sodium atoms.

Stability:
Sodium atoms are relatively stable because their electron configuration follows the octet rule. However, due to the presence of a single electron in their outermost shell, sodium atoms are prone to losing this electron to achieve a stable configuration. By doing so, they form a sodium ion with a complete outer shell, which is energetically favorable and increases their stability.

Sodium ions (Na+), being positively charged, have a high degree of stability due to the electron configuration resembling a noble gas configuration. By losing an electron, sodium ions attain a stable electron configuration similar to that of neon (2-8). This increases their stability by reducing the potential for electron-electron repulsion.

Reactivity:
Sodium atoms are highly reactive because the single electron in their outermost shell is relatively loosely bound compared to the inner electrons. This makes it easier for sodium atoms to lose this outer electron to achieve a stable electron configuration. Sodium has a strong tendency to donate its outer electron, leading to its high reactivity in various chemical reactions.

On the other hand, sodium ions (Na+) are less reactive than sodium atoms because they have already lost their outermost electron. Since sodium ions have a stable, complete outer electron shell, they are less likely to undergo reactions that involve gaining or losing additional electrons.

In summary, the differences in mass, stability, and reactivity between sodium atoms and sodium ions are primarily due to the loss of an electron by sodium atoms to form sodium ions. The loss of an electron reduces the mass of the ion slightly, increases its stability, and decreases its reactivity compared to the highly reactive sodium atoms.