Few simple questions about atomic structure and properties

[mjolnir80]

Homework Statement

a)what property of graphite is the result of the presence of delocalized electrons?
b)what is the reason for the generally low melting point of group I A metals as compared with the high melting points of metals in the center of the transition series?

The Attempt at a Solution

a) is it the layers?
b)i thinks it the higher charge on the transition metals

thanks in advance

 

[Kushal]

well, in graphite each carbon atom is bonded to three other carbon atoms forming layers of hexagonal rings. one valence electron is left out, which acts as a charge carrier in the lattice.

in group 1 there is loosing packing and only 1 electron delocalised per atom. hence weak metallic bond. in transation metals d orbital electrons get delocalised as well, hence a stronger metallic bond.

 

[Blueshift5]

a) The property of graphite that is the result of the presence of delocalized electrons is its electrical conductivity. The delocalized electrons allow for the easy flow of electricity through the layers of graphite.

b) The reason for the generally low melting point of group I A metals is due to their low atomic mass and the presence of only one valence electron. This results in weaker metallic bonds, making it easier for the metal atoms to break apart and melt at lower temperatures. In contrast, the high melting points of metals in the center of the transition series are due to their higher atomic masses and the presence of multiple valence electrons. This results in stronger metallic bonds, making it more difficult for the metal atoms to break apart and melt at higher temperatures. Additionally, the presence of d-orbitals in the transition metals also contributes to their higher melting points.