C2 - Metallic Bonding Flashcards
What does metallic bonding involve?
Delocalised electrons
What do metals also consist of? (In terms of structure?)
A giant structure
What do the electrons in the outer shell of a metal like?
As they are delocalised(free to move around), there are strong forces of electrostatic attraction between the positive metal ions and shared negative electrons
What does strong electrostatic attraction give metals?
It holds the atoms together in a regular structure known as metallic bonding. This makes metallic bonding very strong
When substances are held together by metallic bonding,what do they include?
Elements and alloys
In metallic bonds,what produces ALL the properties of metals
Delocalised electrons
What state are metals in at room temperature?
Solid
What properties do compounds with metallic bonds have?
Very high melting and boiling points
Are metals good at conducting electricity and heat?
Yes as the delocalised electrons carry an electrical charge and thermal (heat) energy through the whole structure
Are metals malleable and if so why?
Yes as the layers of atoms in a metal can slide over each other, making metals malleable - this means that they can be bent,hammered or rolled into flat sheets
What is harder than pure metals?
Alloys
Why are alloys often used instead of pure metals?
As pure metals are often too soft when they are pure so they are mixed with other metals to make them harder. Alloys are harder than pure metals which makes it more useful
What is an alloy?
A mixture of two or more metals or a metal and another element
What do different elements have in terms of atoms?
Different elements have different sized atoms. So when another element is mixed with a pure metal, the new metal atoms will distort the layers of metal atoms, making it more difficult for them to slide over each other. This makes alloys harder than pure metals
