Metallic Bonds Flashcards

What is the name of the model of metallic bonding that is illustrated?

Why are the electrons in a metallic solid described as delocalized?

Which electrons from the metal make up the delocalized electrons?

Are the metal atoms that are shown cations or anions?

How do the metallic ions differ from the ions that exist in ionic solids?

Explain what holds the metal atoms together in the solid.

Malleability indicates that delocalized electrons move.

Brittle materials can be easily deformed without breaking.

Lustrous metals absorb and release light.

Metals have high melting points due to strong bonds.

Metals generally have low boiling points.

Metals are ductile because the sea allows this.

Metals have poor conduction of heat.

Metals have good conduction of electricity.

In what form do elements such as hydrogen, nitrogen, and oxygen normally occur?

How many electrons are shared in a double covalent bond?

Metallic Bonds and Properties of Metals

The sea of electrons model illustrates metallic bonding, depicting how electrons are distributed among metal atoms.
Delocalized electrons in metallic solids are loosely held and can move freely around the positively charged ions (cations).
Valence electrons from metal atoms contribute to the delocalized electron cloud, allowing for conductivity and malleability.
Metal atoms in a metallic solid are considered cations (positively charged) due to the loss of valence electrons.
Unlike ionic bonds, in metallic bonding, electrons are not completely transferred between atoms; they are shared in a cloud-like arrangement.
Metal atoms are held together by the sea of electrons, which creates a strong bond in the solid structure.
Metals exhibit malleability due to the movement of delocalized electrons, which allows the metal to deform without breaking.
Metals are not brittle, maintaining structural integrity when force is applied.
Metals appear lustrous, as they can absorb and reflect light, giving them a shiny appearance.
Metals have high melting points due to strong metallic bonds requiring significant energy to break.
Metals generally have low boiling points, differentiating them from the high melting points caused by strong bond interactions.
Ductility is a characteristic of metals, allowing them to be drawn into wires thanks to the flexibility of the electron sea.
Metals exhibit good conductivity of electricity due to the presence of delocalized electrons that can move freely.
Elements like hydrogen, nitrogen, and oxygen usually exist as diatomic molecules, occurring in pairs rather than as metals.
In a double covalent bond, a total of four electrons are shared between two atoms, allowing for strong bonding.

Explore the fundamentals of metallic bonding with these flashcards. Learn about the sea of electrons model, the nature of delocalized electrons, and the role of valence electrons in metals. Perfect for quick revision and understanding of metallic bond properties.