Covalent Bond vs. Electrovalent Bond

Attribute	Covalent Bond	Electrovalent Bond
Nature	Sharing of electrons between atoms	Transfer of electrons from one atom to another
Formation	Occurs between non-metal atoms	Occurs between metal and non-metal atoms
Electronegativity	Atoms have similar electronegativity	Atoms have different electronegativity
Bond Strength	Relatively weaker	Relatively stronger
Physical State	Can exist as solids, liquids, or gases	Often exist as solids
Examples	Oxygen molecule (O2), Water molecule (H2O)	Sodium chloride (NaCl), Calcium oxide (CaO)

Introduction

Chemical bonds are the forces that hold atoms together in a molecule or compound. Two common types of chemical bonds are covalent bonds and electrovalent bonds. While both types involve the sharing or transfer of electrons between atoms, they differ in terms of their formation, strength, properties, and applications. In this article, we will explore the attributes of covalent bonds and electrovalent bonds, highlighting their similarities and differences.

Covalent Bond

A covalent bond is formed when two atoms share one or more pairs of electrons. This type of bond typically occurs between nonmetal atoms, as they have a higher tendency to gain electrons and form negative ions. In a covalent bond, the shared electrons are attracted to the nuclei of both atoms, resulting in a stable molecule. The strength of a covalent bond depends on the number of shared electrons and the distance between the nuclei of the bonded atoms.

Covalent bonds can be further classified into two types: polar covalent bonds and nonpolar covalent bonds. In a polar covalent bond, the shared electrons are not equally shared between the atoms, leading to a partial positive charge on one atom and a partial negative charge on the other. This occurs when there is a significant difference in electronegativity between the atoms involved. On the other hand, in a nonpolar covalent bond, the shared electrons are equally distributed between the atoms, resulting in a balanced charge distribution.

Covalent bonds have several important properties. They are generally stronger than electrovalent bonds, requiring more energy to break. Covalent compounds often have lower melting and boiling points compared to electrovalent compounds. Additionally, covalent compounds tend to have lower solubility in water and are often insoluble in nonpolar solvents. Covalent bonds also allow for the formation of complex molecular structures, enabling the existence of a wide range of organic and inorganic compounds.

Electrovalent Bond

An electrovalent bond, also known as an ionic bond, is formed when there is a complete transfer of electrons from one atom to another. This type of bond typically occurs between a metal and a nonmetal atom, as metals have a lower tendency to gain electrons and form positive ions. In an electrovalent bond, the metal atom loses one or more electrons to form a positive ion (cation), while the nonmetal atom gains those electrons to form a negative ion (anion). The resulting electrostatic attraction between the oppositely charged ions forms the electrovalent bond.

Electrovalent bonds are characterized by their high strength and stability. The strength of an electrovalent bond depends on the magnitude of the charges on the ions and the distance between them. Electrovalent compounds typically have high melting and boiling points due to the strong electrostatic forces between the ions. They are also often soluble in water and other polar solvents, as the polar nature of water molecules allows them to surround and separate the ions.

Electrovalent compounds exhibit several properties that distinguish them from covalent compounds. They are usually crystalline solids at room temperature and have a tendency to form regular, repeating patterns called crystal lattices. Electrovalent compounds are good conductors of electricity in the molten or aqueous state, as the movement of ions allows for the flow of electric current. They also often exhibit high hardness and brittleness, making them suitable for applications such as construction materials and ceramics.

Comparison

Now that we have explored the attributes of covalent bonds and electrovalent bonds individually, let's compare them side by side:

Formation

• Covalent Bond: Formed by the sharing of electrons between nonmetal atoms.
• Electrovalent Bond: Formed by the complete transfer of electrons from a metal atom to a nonmetal atom.

Strength

• Covalent Bond: Generally stronger than electrovalent bonds.
• Electrovalent Bond: High strength due to the strong electrostatic forces between ions.

Melting and Boiling Points

• Covalent Bond: Covalent compounds often have lower melting and boiling points compared to electrovalent compounds.
• Electrovalent Bond: Electrovalent compounds typically have high melting and boiling points.

Solubility

• Covalent Bond: Covalent compounds generally have lower solubility in water and are often insoluble in nonpolar solvents.
• Electrovalent Bond: Electrovalent compounds are often soluble in water and other polar solvents.

Conductivity

• Covalent Bond: Covalent compounds are generally poor conductors of electricity.
• Electrovalent Bond: Electrovalent compounds are good conductors of electricity in the molten or aqueous state.

Structure

• Covalent Bond: Allows for the formation of complex molecular structures.
• Electrovalent Bond: Electrovalent compounds tend to form regular, repeating crystal lattices.

Conclusion

Covalent bonds and electrovalent bonds are two fundamental types of chemical bonds with distinct attributes. Covalent bonds involve the sharing of electrons between nonmetal atoms, resulting in the formation of stable molecules. On the other hand, electrovalent bonds occur through the complete transfer of electrons from a metal atom to a nonmetal atom, leading to the formation of oppositely charged ions. While covalent bonds are generally stronger, electrovalent bonds exhibit higher melting and boiling points. Covalent compounds have lower solubility and conductivity compared to electrovalent compounds. Understanding the differences between these two types of bonds is crucial in comprehending the properties and behavior of various substances in the field of chemistry.