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Lithium, represented as Li, is a fascinating element when it comes to forming ions. It belongs to Group 1 of the periodic table, also known as the alkali metals. The defining characteristic of these metals is their ability to lose one electron to achieve a stable electron arrangement. In the case of lithium, losing one electron leads to a positively charged ion, known as a lithium ion, denoted as \( \text{Li}^{+} \). This charge of +1 is crucial for forming ionic compounds, as it allows lithium to bond with negatively charged ions, aiding in the creation of stable structures like \( \text{Li}_3\text{N} \).

When lithium atoms form ions, they do so by shedding their single valence electron. By losing this electron, lithium achieves the same electronic configuration as the noble gas helium, thereby gaining stability. This ionization process is why the lithium ion has a charge of +1.

Nitrogen is a standout element from Group 15 of the periodic table. Unlike lithium, which loses electrons, nitrogen tends to gain electrons when forming ions. Normally, a nitrogen atom has five valence electrons. By gaining three additional electrons, nitrogen achieves a complete set of eight valence electrons, fulfilling the stable electron configuration reminiscent of noble gases like neon.

The gain of three electrons bestows upon the nitrogen ion a negative charge of -3, symbolized as \( \text{N}^{3-} \). This need for three additional electrons highlights nitrogen's role in forming ionic bonds with elements like lithium. The negatively charged nitrogen ion balances out the positive charges of lithium ions, culminating in the electrically neutral compound \( \text{Li}_3\text{N} \).

Valence electrons are the outermost electrons in an atom and play a pivotal role in chemical bonding. For lithium, which has an atomic number of 3, there is only one valence electron. This one electron is easily lost in the quest for a stable electron configuration, resulting in a \( \text{Li}^{+} \) ion. With three lithium atoms in \( \text{Li}_3\text{N} \), each contributing one electron, a total of three electrons are earmarked for bonding.

Nitrogen, with an atomic number of 7, naturally possesses five valence electrons. To achieve a stable octet, nitrogen tends to accept three electrons, culminating in a \( \text{N}^{3-} \) ion. Hence, in the compound \( \text{Li}_3\text{N} \), nitrogen's original five valence electrons, combined with the three additional electrons it gains from lithium, amount to eight valence electrons, showcasing a stable electronic environment.

One of the essential properties of ionic compounds is their electrical neutrality. This means that the sum of positive and negative charges within the compound must equal zero. For the compound \( \text{Li}_3\text{N} \), we see this principle in action. Here, three lithium ions, each with a charge of +1, contribute a total positive charge of +3. On the other hand, the single nitrogen ion bears a charge of -3.

The combination of these charges results in the equation \(+3 + (-3) = 0\). This balance indicates that the compound is electrically neutral. The neutrality confirms stable bonds between lithium and nitrogen in the compound \( \text{Li}_3\text{N} \), illustrating the elegance and predictability of ionic compounds based on the interplay of charged ions.