S2.3 The metallic model SL

Question 1

Delocalised electrons

Answer 1

An electron that is not associated with one specific atom and is free to move within the molecular structure.

Question 2

Metallic bond

Answer 2

The electrostatic attraction between a lattice of positive metal ions and a sea of delocalised electrons.

Question 3

What happens to the electrons in a metallic lattice?

Answer 3

In a metallic lattice, the outer valence electrons are delocalized, meaning they are free to move throughout the lattice and are shared among all metal atoms, leading to the formation of a “sea of electrons.

Question 4

What is the charge of the metal atoms within a metallic lattice, and why?

Answer 4

The remaining metal atoms in a metallic lattice become positively charged cations because their outer valence electrons are delocalized and shared among the lattice, leaving the core atoms positively charged.

Question 5

What maintains the lattice structure in metals?

Answer 5

The lattice structure in metals is maintained by the electrostatic forces between the positively charged cations and the delocalized electrons.

Question 6

Why are metals conductive?

Answer 6

Metals are conductive because the delocalized electrons in the metallic lattice can move freely throughout the lattice, allowing electricity to flow easily through the metal.

Question 7

Why are metals malleable?

Answer 7

Metals are malleable due to the presence of delocalized electrons in the metallic lattice, which allows the metal atoms to slide over each other when force is applied without breaking the metallic bond, thus enabling metals to be hammered or rolled into thin sheets.

Question 8

How do metals conduct heat?

Answer 8

Metals conduct heat through thermal conductivity, a property facilitated by the movement of delocalized electrons transferring thermal energy across the material.

Question 9

What factors predict metallic bond strength?

Answer 9

Smaller ion radius and higher ionic charge enhance metallic bond strength through increased electron density and electrostatic attraction.

Question 10

How do melting points of s and p block metals change with group and period?

Answer 10

Decrease down a group due to larger ion radius. Increase across a period due to higher ionic charge, enhancing metallic bond.

Question 11

Electron density

Answer 11

The relative amount of electrons in a region of space.