principles of chemistry - metallic bonding

These flashcards cover key concepts related to metallic bonding as outlined in IGCSE Chemistry.

What is a characteristic of metallic lattices?

Metals consist of giant structures of atoms arranged in a regular pattern.

What role do outer shell electrons play in metallic bonding?

The electrons in the outer shell of metal atoms are delocalised and free to move through the structure.

What gives rise to strong metallic bonds?

The sharing of delocalised electrons among metal atoms.

What does metallic bonding involve in terms of electrostatics?

It involves strong electrostatic attraction between negatively charged electrons and positive metal ions.

How do metals typically conduct heat and electricity?

Metals can conduct heat and electricity due to the presence of delocalised electrons.

What is a typical property of metals related to melting and boiling points?

Most metals have high melting and boiling points due to strong metallic bonding.

What allows metals to be malleable?

The layers of atoms in metals can slide over each other, allowing them to be bent and shaped.

Describe the structure of metals.

Metals have giant structures of atoms with strong metallic bonding.

Why are metals good conductors of electricity?

Because of the delocalised electrons that can move freely through the metal.

What effect does metallic bonding have on the physical properties of metals?

It leads to their high melting and boiling points, electrical conductivity, and malleability.

What is the significance of delocalised electrons in metallic structures?

They create strong metallic bonds and enable electrical conductivity.

How does the arrangement of atoms in metals influence their physical properties?

The regular arrangement allows for strong bonding and movement, affecting conductivity and malleability.

What happens to the layers of metal atoms during deformation?

The layers can slide over each other without breaking the metallic bond.

What is a defining feature of metallic structures in terms of bonding?

The presence of strong metallic bonds due to delocalised electrons.

Explain why metals have good thermal conductivity.

Due to delocalised electrons that can transfer energy through the metal.

What are the characteristics of the electrostatic attractions in metallic bonding?

They are strong due to the attraction between negatively charged electrons and positively charged metal ions.

Define malleability in the context of metals.

The ability of metals to be bent and shaped due to the sliding of atomic layers.

What types of ions are present in metallic bonding?

Positive metal ions surrounded by a sea of delocalised electrons.

What does a 2-D diagram of a metallic lattice typically represent?

The arranged pattern of metal atoms and delocalised electrons.

How do metallic bonds compare to other types of bonds?

Metallic bonds are characterized by delocalised electrons, which distinguishes them from ionic and covalent bonds.

What is the relationship between metallic bonding and the physical state of metals?

Strong metallic bonding contributes to metals being solid at room temperature.