Metallic Bonding

Front

What is metallic bonding?

Back

Metallic bonding is the electrostatic attraction between positively charged metal ions and the delocalized electrons surrounding them, allowing metals to conduct electricity and heat.

Front

What are the characteristics of metals due to metallic bonding?

Back

Metals are typically malleable, ductile, good conductors of heat and electricity, and have a shiny appearance due to metallic bonding.

Front

What is the role of delocalized electrons in metallic bonding?

Back

Delocalized electrons are free-moving electrons that contribute to the conductivity and malleability of metals, allowing them to deform without breaking.

Front

How does metallic bonding differ from ionic and covalent bonding?

Back

Metallic bonding involves a sea of delocalized electrons, while ionic bonding involves the transfer of electrons between atoms, and covalent bonding involves the sharing of electrons.

Front

What is the significance of the 'sea of electrons' model in metallic bonding?

Back

The 'sea of electrons' model explains how metal atoms can lose their valence electrons, creating a pool of electrons that allows for conductivity and flexibility.

Front

What is the effect of temperature on metallic bonding?

Back

As temperature increases, metallic bonds can weaken, leading to increased malleability and ductility, but can also result in melting if the temperature is high enough.

Front

What is an example of a metal with strong metallic bonding?

Back

Tungsten (W) is an example of a metal with strong metallic bonding, which contributes to its high melting point and strength.

Front

What is the relationship between metallic bonding and electrical conductivity?

Back

The presence of delocalized electrons in metallic bonding allows metals to conduct electricity efficiently.

Front

What is the formula for copper(II) chloride?

Back

CuCl₂

Front

What is the formula for manganese(III) oxide?

Back

Mn₂O₃