Metallic Bonding Flashcards
what is Metallic Bonding
Strong electrostatic attraction between metal ions and the sea of delocalised electrons that surround them.
What’s the difference between metallic bonds and covalent bonds?
Metallic bonds are delocalised ; whereas covalent bonds are localised
What are the properties of metals?
They have: high melting points, they’re ductile, they’re malleable, they’re conductors of heat, they’re conductors of electricity
What is the strength of a metallic bond dependant on?
- the number of electrons on the metal’s outer shell(it’s charge)
- the size of the metal/ion
What is the electron configuration of sodium?
1s2 2s2 2p6 3s1
Are the delocalised electrons in a metal restricted to one atom?
No, they’re shared between all the atoms in the metal
Why are metals good at conducting electricity?
Because the delocalised electrons are free to move through out the metal’s lattice and they carry a current which allows metals to conduct electricity
Why do metals have high melting points?
Because there’s a strong electrostatic attraction between the positive metal ions and the negative electrons. This electrostatic attraction requires a lot of energy and high temperatures in order to be broken
Why are metals malleable and ductile?
Because layers of positive ions can slide over each other into new positions without breaking more metallic bonds than are made
Overall the charges in a metal are what?
Balanced
In a metal, can you tell which electron comes from which atom?
No
What does it mean to say that metals are soronous?
That they produce a deep ringing sound
The electrons in metal atoms overlap, making it easier for electrons to do what?
To move between energy levels/electron shells
Are metals soluble or insoluble?
Insoluble because of their strong metallic bonds
