Question

The electrostatic forces of attraction between the metallic ions and free electrons is called

Short answer

Answer: The term is "Metallic Bond," which is the electrostatic attraction between positively charged metallic ions and negatively charged delocalized electrons in a crystal lattice. This interaction occurs due to the "sea of electrons" that surrounds the metal ions, holding the metal lattice together and resulting in unique properties of metals, such as conductivity and high melting points.

Step-by-step solution

Define the term

The electrostatic forces of attraction between the metallic ions and free electrons is called "Metallic Bond." Metallic bonding is a type of chemical bonding that holds together metals in solid-state structures, allowing them to conduct electricity and heat, and exhibit unique mechanical properties like malleability and ductility.

Explain the forces involved

In metallic bonds, the valence electrons of metal atoms are delocalized, meaning they are not associated with any particular atom but are distributed throughout the entire crystal lattice. These delocalized electrons create a "sea of electrons" that surrounds the positively charged metal ions. This sea of electrons attracts the metallic ions and acts as a glue that holds the metal lattice together. The electrostatic forces of attraction between the positively charged metal ions and negatively charged delocalized electrons are what create the metallic bond. This results in the unique properties of metals, such as their ability to conduct electricity and their high melting and boiling points. To reiterate, the term that describes the electrostatic forces of attraction between metallic ions and free electrons is called "Metallic Bond."

Key concepts

Electrostatic Forces

Electrostatic forces are fundamental forces that occur due to electric charges. In the context of metallic bonding, these forces play a crucial role in holding the entire metal structure together.

In metals, the valence electrons become delocalized. That means instead of orbiting a single nucleus, they roam freely around several ions. The positive metallic ions stay fixed in a lattice.

While the electrons are negatively charged, the metal ions are positively charged. An attractive force, called an electrostatic force, forms between the two. This force holds the whole metal structure together and enables many of its properties, like conductivity and malleability.

• Electrostatic force works like a glue for metal structures.
• It exists between positively charged ions and delocalized electrons.
• These forces result in unique properties of metals.

Metallic Ions

In a metal, atoms lose their outer electrons easily, becoming positively charged ions. These are known as metallic ions. Unlike in ionic or covalent bonds where electrons are shared or exchanged specifically, in metallic bonds, electrons are delocalized.

Metallic ions arrange themselves in a structured pattern called a lattice. This structured arrangement is crucial for giving metals their strength and durability. In pure metals, this regular lattice arrangement allows layers to slide over each other. This is why metals can be bent and shaped without breaking.

• Metal atoms lose electrons to become metallic ions.
• Metallic ions form a regular lattice structure.
• This lattice is essential for metal's strength.

Delocalized Electrons

The term 'delocalized electrons' refers to electrons in a metal that do not belong to any single atom. Instead, they move freely across the entire metal structure. This movement forms a "sea of electrons" around the array of metallic ions.

Delocalized electrons are key to understanding the special characteristics of metals. They allow electrical currents to pass through effortlessly. This free-flowing sea of electrons also helps metals conduct heat efficiently.

Another important aspect is how these electrons give metals their shiny appearance, as they reflect light efficiently.

• Delocalized electrons are not tied to one atom.
• They create a 'sea of electrons' that enhances conductivity.
• They contribute to metal's reflectivity and shine.

Conductivity in Metals

Conductivity is one of the most renowned properties of metals. It is largely due to the presence of delocalized electrons. These electrons can move through the metal, carrying electric current and heat.

When an electric field is applied to a metal, the delocalized electrons flow from a region of negative charge to a region of positive charge. This movement or flow of electrons is what carries electric current through the material.

Similarly, when metals are heated at one end, these free-flowing electrons readily conduct energy to cooler parts, transferring heat effectively.

• Conductivity for electricity stems from electron flow.
• The same principle applies to heat conduction.
• High conductivity is a defining characteristic of metals.