Studied by 0 people
Looks like no one added any tags here yet for you.
What is a metallic bond?
The strong electrostatic attraction between positive metal ions and negative delocalised electrons in a metal lattice
Why to metals bond like this?
Metal elements cannot transfer electrons unless there is a non-metal present therefore, in metal element outer main levels of atoms merge so they are no longer associated with a specific atom.
What structure do metals have?
A fixed lattice of positive ions with a delocalised sea of electrons
What are the three properties of metals?
- Good electrical conductivity
- High melting and boiling point
- High malleability and ductility
Why can metals conduct electricity?
Delocalised electrons free to move throughout lattice and carry current
What do metals have high melting and boiling points?
Lots of energy required to break strong metallic bonds
What two factors influence the melting point of metals?
- Charge
- Size of metal ion
How does charge influence the melting point of metals?
Greater charge contributes more electrons to delocalised sea = more electrostatic forces of attraction between ions and electrons = more energy to break
How does the size of the metal ion influence the melting point of metals?
Positive nuclei of smaller cations are closer to delocalised electrons = stronger metallic bond = more energy to break
Why are metals malleable and ductile?
No bonds holding specific ions together = ions can slide past each other = relocation of metal ions doesn't charge their environment = lattice structure retained
