Question

Give an example of a simple chemical reaction that involves the transfer of electrons from a metallic element to a nonmetallic element.

Short answer

An example of a simple chemical reaction that involves the transfer of electrons from a metallic element to a nonmetallic element is the reaction between sodium (Na) and chlorine (Cl) to form sodium chloride (NaCl). In this reaction, sodium loses its one valence electron (forming Na⁺) and chlorine gains one electron (forming Cl⁻), creating an ionic bond between the two ions in the compound NaCl. The overall reaction is: Na(s) + Cl₂(g) -> 2NaCl(s)

Step-by-step solution

Choose a metallic element and a nonmetallic element

For this example, we'll select sodium (Na), a metallic element, and chlorine (Cl), a nonmetallic element. Both of these elements can undergo a simple chemical reaction, resulting in an ionic bond.

Write the electron configuration

First, let's write the electron configuration for sodium (Na) and chlorine (Cl). Sodium (Na) has 11 electrons and its electron configuration is: \(1s^2 2s^2 2p^6 3s^1\) Chlorine (Cl) has 17 electrons and its electron configuration is: \(1s^2 2s^2 2p^6 3s^2 3p^5\) Notice that sodium has one electron in its outermost shell (3s^1), while chlorine has five electrons in its 3p orbital (and seven in the outermost shell in total: 3s^2 3p^5).

Understand the electron transfer process

In order to achieve a stable electron configuration, sodium can lose its one electron in the outermost shell (3s^1), becoming a positively charged ion (cation) and chlorine can gain one electron, filling its 3p orbital, becoming a negatively charged ion (anion).

Write the ionic bond formation equation

Considering the electron transfer process, let's write the chemical equation for the reaction between sodium (Na) and chlorine (Cl), which leads to the formation of sodium chloride (NaCl): Na(s) + Cl_2(g) -> 2NaCl(s) Since the sodium loses an electron, its charge becomes +1, and since chlorine gains an electron, its charge becomes -1. Therefore, the ionic compound sodium chloride (NaCl) has a balanced charge, Na^+ and Cl^- ions attract and form the ionic bond. Our example of a simple chemical reaction involving the transfer of electrons from a metallic element (sodium) to a nonmetallic element (chlorine) is the formation of sodium chloride (NaCl) from sodium and chlorine.

Key concepts

Chemical Reaction

A chemical reaction is a transformative process where the initial substances, known as reactants, change to form new substances called products. During this process, bonds are broken and formed, resulting in distinct properties for the reactants and products.
A classic example of a chemical reaction is one that involves electron transfer between a metallic and a nonmetallic element.

• Reactants: These are the substances you start with, such as sodium (Na) and chlorine (Cl) in our example.
• Products: The new substances formed from the reaction; in this case, sodium chloride (NaCl).

Specifically, the reaction between sodium and chlorine is characterized by the movement of electrons from sodium to chlorine, leading to the formation of ions and an ionic compound. This is a key aspect of chemical reactions involving metals and nonmetals. Such transformations involve energy changes, often observed as heat, light, or other forms of energy being absorbed or released.

Ionic Bond

An ionic bond is a type of chemical bond characterized by the transfer of electrons from one atom to another. It typically occurs between atoms with significant differences in electronegativity, such as metals and nonmetals. In our example, sodium and chlorine engage in electron transfer to form an ionic bond.

• Formation: Sodium (Na), being a metal, tends to lose its valence electron, while chlorine (Cl), a nonmetal, gains an electron to fill its valence shell.
• Resulting Ions: The sodium atom, upon losing an electron, becomes a positively charged ion ( ext{Na}^+), and the chlorine atom, upon gaining that electron, becomes a negatively charged ion ( ext{Cl}^-).

The attraction between these oppositely charged ions constitutes the ionic bond. The resulting compound, sodium chloride (NaCl), is neutral overall, due to the equal number of positive and negative charges. Ionic bonds are strong and typically result in the formation of a crystal lattice structure, lending to the high melting and boiling points of ionic compounds.

Electron Configuration

Electron configuration is a description of the arrangement of electrons in an atom’s orbitals. It reveals how electrons are distributed among different energy levels and sublevels (s, p, d, and f). Understanding electron configuration is crucial to predicting how atoms will interact and bond with one another.

• Sodium (Na): The electron configuration for sodium is \(1s^2 \, 2s^2 \, 2p^6 \, 3s^1\). Sodium has one electron in its outermost shell (3s). This lone electron is easily lost in chemical reactions, making sodium highly reactive.
• Chlorine (Cl): The electron configuration for chlorine is \(1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^5\). With seven electrons in its outer shell, chlorine needs just one more electron to achieve a stable octet configuration.

In the reaction between sodium and chlorine, sodium transfers its single valence electron to chlorine. As a result, sodium achieves a stable electron configuration resembling that of neon ( ext{Na}^+), while chlorine achieves a stable electron configuration similar to argon ( ext{Cl}^-). This electron exchange is the basis for ionic bond formation and demonstrates how electron configuration governs chemical reactivity and bonding.