Bonding, Structure, And The Properties Of Matter Flashcards
Ions
An atom or group of atoms with an electrical charge, either positive (+) or negative (-)
Ionic bonding
Between metals and non-metals
High melting and boiling points
Giant ionic structures
High melting and boiling points
Strong electrostatic forces in all directions
Can dissolve through H2O
Can conduct electricity when molten or dissolved in H2O as ions become free to move
Ionic lattice
When ions are closely packed with very strong electrostatic forces, between oppositely charged ions
Limitations of a dot-and-cross diagram
Is 2 dimensional
Does not show how ions are arranged in space
Limitations of a 2 dimensional diagram
Does not show where ions are located on other layers
Limitations of a 3 dimensional diagram
Not to scale
No information on forces of attraction
Covalent bonding
Sharing of electrons between non-metals
Low melting and boiling points
Giant covalent structures
Bonded through strong covalent bonds
High melting and boiling points
Do not conduct electricity - not even when molten (except graphite)
Graphite
Each carbon atom forms three covalent bonds with three other carbon atoms
One electron from each carbon atom is delocalised
Weak intermolecular forces between layers
Conducts heat and electricity because each carbon atom has one delocalised electron
Graphene
A single layer of graphite
Diamond
Each carbon atom forms four covalent bonds with other carbon atoms
High melting point and does not conduct electricity
Hardest natural substance
Nanoscience
The study of objects on the nanometre scale
Nanoparticles
Used in cosmetics, sun creams, deodorants and as catalysts
Fullerenes
3 bonds for each carbon - leaving 1 electron free to conduct electricity
They can be used to deliver drugs as they are hollow
Used as lubricants as they reduce friction
Used as catalysts
Metallic bonding
It occurs in metallic elements and alloys
Conduct electricity due to the sea of delocalised electrons
Strong electrostatic forces holding the atoms in a regular structure
Layers of atoms can slide over each other, allowing metals to be bent and shaped
Alloys
A mixture of 2 or more metals
Harder than pure metals as atoms cannot slide past each other as layers are distorted
Pure metals
Chemical elements that consist of only one type of atom
Polymers
The atoms in the polymer molecules are linked to other atoms by strong covalent bonds
Solids at room temperature due to strong intermolecular forces
Limitations of the states of matter model
There are no forces
All particles are represented as spheres
All spheres are solid
Limitations of the particle theory in relation to changes in state
Particles represented by solid inelastic spheres which have no forces between them
