Metallic Bonding Flashcards
What is metallic bonding.
The attraction between the positive metal ions and the sea of negative delocalised electrons which can move through the lattice.
Draw the arrangement of a metallic lattice.
In notes
How are electrons delocalised in a metallic structure.
When the atoms are close together, the valence electrons are delocalised and can move around the lattice.
What are the two factors that influence the strength of metallic bonding.
Charge of the ions
Size of the ions
(Metal)
How does charge of the metal ions affect the metallic bonding ?
The greater the charge of the ions, the greater the attraction between the actions and the sea of delocalised electrons. Therefore the stronger the lattice.
How does the size of metal ions affect the metallic bonding.
The smaller the metal ion, the closer the attraction between the metal ion nucleus and the sea of delocalised electrons therefore stronger lattice.
How would you get the maximum strength in a metallic structure ?
Small cations which are highly charged.
Draw a graph to show the meeting point of a metallic lattic across a period.
In notes
Draw a graph to show the trend of the melting points of metallic structures down a group.
In notes
What are the properties of metallic structures.
Malleable
Ductile
Conduct heat and electricity
Why are metallic structures malleable and ductile ?
If we beat a metal into another shape , the delocalised electron cloud continues to hold the shape together and the layers of cations can slide over eachother.
Why do metallic lattices conduct heat and electricity.
The electron cloud is mobile so electrons are free to move throughout the lattice. Electrons are attached to the positive current but are replaced by the negative current.
Explain why diamond can’t conduct electricity but graphite can
Diamond is a giant ionic lattice and is a solid - not enough movement of particles
Graphite has delocalised electrons which can travel through the substance to carry current.
