C5 Metallic Bonds Flashcards
(21 cards)
What are metal crystals
The atoms in metal are built up layer upon layer in a regular pattern
Metallic bonding
Metals are another example of giant structures. You can think of a metal as a lattice of positively charged ions. The metal ions are arranged in regular layers, one on top of another.
What are delocalized electrons
The electrons in the ‘sea’ of free-moving electrons are called delocalised electrons. They are no longer linked with any particular metal ion in the giant metallic structure. These delocalised electrons help to explain the properties of metals
Why are alloys in some metallic bonding
In alloys the layer cannot slide so wasily because atoms of other elements distort the layers
Why can metals be hammers into diffrent shapes
Metals can be hammered and bent into different shapes, and drawn out into wires. This is because the layers of atoms in a pure metal are able to slide easily over each other.
What is a metallic bond
the strong electrostatic attraction between sea of negative delocalised electrons and positive metal ions in a giant lattice structure.
How are atoms in a pure metal sturctured
The atoms in a pure metal, such as iron, are held together in a giant metallic structure. The atoms are arranged in closely packed layers. This regular arrangement allows the atoms to slide over one another quite easily. This is why pure iron is relatively soft and easily bent and shaped.
What are alloys formed of
Alloys are usually mixture of metals.
How can electrons move through the whole lattice structure
However, unlike glue, the electrons are able to move throughout the whole giant lattice. Because they can move around and hold the metal ions together at the same time,
Describe why metals can be bent, shaped, and pulled out
they consist of layers of ions that can slide over one another when the metal is bent, hammered or pressed.
What word is used to describe a material, such as a metal, that can be hammered into shapes
Malleability
Explain why metals are good conductors of thermal energy and electricity, in terms of their structure and bonding.
Structure: Metals have free-moving electrons.
Thermal conductivity: Free electrons carry heat quickly.
Electrical conductivity: Free electrons allow electricity to flow easily.
What can you deduce about the arrangement of the particles in a metal from the fact that metals form crystals?
Since metals form crystals, it means that they have an ordered structure
Why are the particles that make up a metal described as positively charged ions?
In a metal, atoms lose some of their electrons, leaving behind positively charged ions. These ions are held together by the deloclaised electrons around them.
What holds a metal lattice together?
A metal lattice is held together by the attraction between the positively charged ions and the free-moving electrons.
What are the general properties of metals?
Good conductors of heat and electricity
Malleable (can be hammered into shapes)
Ductile (can be drawn into wires)
Shiny (lustrous)
High melting and boiling points
Strong and dense
Metals facts
Metels are good conducter of hear and electricty
They have a high melting point
Malleable
Shiny
Non-metal
Poor conducters of heat
Low melting points
Brittle
Dull
Why do meatllic bond have a high melting point
Because the electrostatic attraction is strong
Is metallic bond a strong conducter
Electrons can flow freely througout the structure
what are delocalised electrons
The outer electrons from each atom are able to abandon the nucleus and move freely throughout the metal
