[ironhorse777]

Hi,
I have a couple of questions regarding few statements in my textbook regarding metallic bonding. Please help.

1)...the fewer valence electrons per atom involved in metallic bonding, the more metallic the bonding is. How?

2)As the number of bonding electrons increases the bonding energies and melting points of metals increase. How?

3)when the 3d and 4s orbitals are filled, the outer electrons become more loosely bound and the bonding energies and melting points of the metals decrease -How?

4)With the introduction of 3d electrons in transition metals the melting point and and bonding energies increase much higher-how?

From Materials Science and Engineering by Smith.

Thank you

[billnotgatez]

Forum rules require that you are a participant in the process of learning.
What are your thoughts on the questions?
Please read forum rules.

[ironhorse777]

Forum rules require that you are a participant in the process of learning.
What are your thoughts on the questions?
Please read forum rules.

Sorry my bad.
1)fewer valence electrons means they get attracted by numerous positive ion cores hence they move about freely but how does this make the bond more metallic?
2)As the number of bonding electrons increase it gets more tightly packed and hence both melting point and bonding energy increase? I want to how why this increase in MP and bonding energies with close packing-Due to stronger forces of attraction?
3) opposite of 2 right?
4) sorry I have no clue

[ironhorse777]

Anyone?

w.r.t Question 4. In transition elements the MP increases because it has larger number of unpaired electrons in d-orbital right?