Bonding In Metals STRUCTURE AND BONDING Flashcards
What is the arrangement of atoms in solids?
The atoms in metals are built up layer upon layer in a regular pattern. This allows them to move over each other easily.
What do metals form?
Crystals.
What is a metal?
A lattice of positively charged ions. The metal ions are arranged in regular layers, one on top of another.
What are the electrons like in a giant metal structure?
The outer electron of each atom can move freely throughout the giant structure. This forms a ‘sea’ of free-moving electrons surrounding the positively charged ions. There is a strong electrostatic attraction between the negatively charged electrons and the positively charged ions that binds the metals to each other.
The electrons in the ‘sea’ of free moving electron is called a delocalised electron.
What are the properties of giant metallic structures?
They can be hammered
Bent into different shapes
Drawn out into wires
This is all because the layers can slide easily over each other.
What is an alloy?
A mixture of two or more elements, at least one of which is a metal.
What are the properties of alloys?
Thy are harder because the carbon atoms are a different size to the iron atoms (in steels)
Why are metals malleable?
The delocalised electrons bind the positive ions together due to electrostatic forces of attraction. Although, as they can move throughout the whole structure , they allow the lattice to distort as they can move throughout the whole structure.
Why do metals have high melting and boiling points?
The electrostatic forces of attraction extend in all directions. Therefore, it takes a lot of energy to separate the metal ions from their fixed positions.
Why are metals good conductor of thermal energy?
The delocalised electrons can readily flow through the giant metallic lattice. The electrical charge and thermal energy are t and we’re quickly through the metal by the free-moving delocalised electrons.
