Chem C Flashcards
DIMOND
-how does is bond
-melting point?
-electrical conductivity
-strong and hard
How it bonds - Each carbon bonds with 4 other carbons in a covalent bond
Melting point - Very high melting point as a lot of energy is required to break the millions of strong covalent bonds in the giant structure.
Electrical conductivity - Does not conduct electricity as no free electrons.
Strong and hard - Millions of strong covalent bonds held together in the giant structure
What is Silicon dioxide made from
SiOz - (Silicon and Oxygen) forms the same structure and has the exact same properties as diamond
GRAPHITE
-How does it bond?
-Melting point
-Electrical conductivity
-Slippery
-How does it bond? - Each carbon bonds with 3 other carbons in a covalent bond. The 4th electron is delocalised to form layers of carbons and layers of electrons
-Melting point - High melting point as lots of energy needed to break the strong covalent bonds in the giant structure
- Electrical conductivity - Does conduct electricity as delocalised electrons are able to move and carry the electrical current
- slippery - The layers of carbon can slide over each other
GRAPHENE
-how does it bond
-Melting point
-Electrical conductivity
-how does it bond - A single layer of graphite
-Melting point - High melting point as lots of energy needed to break the strong covalent bonds
-Electrical conductivity - Conducts electricity as has delocalised electrons carry the electrical current through the material
NANOSCIENCE
-How big?
-Why do they have different properties?
-Order of particle size (largest first)
-Use
-How big? - 1-100nm in size (a few hundred atoms)
- Why do they have different properties? - Due to a large surface area to volume ratio
-Order of particle size (largest first) - Nano - fine - coarse (dust)
-use - Medicine, electronics, cosmetics, sun creams
FULLERENES
-how does it bond?
-buckminsterfullerene?
-Use?
-how does it bond? - Molecules of carbon atoms with hollow spaces. Made up of hexagonal rings of carbon
-buckminsterfullerene - The first fullerene to be discovered. A spherical sphere
Use - drug delivery
POLYMERS
-bonding?
-state at room temp?
-use ?
- bondings - Very large molecules of lots of small molecules joined together by covalent bonds
-state at room temp - Solid at room temperature as strong intermolecular forces between the polymers
-Use - plastics
State symbols
Solid - (s)
Liquid - (l)
Gas - (g)
Aqueous (in solution) - (aq)
IONIC BONDING
- happens between?
- how does it form?
-ion
-metals form… - non-metals form…
-melting points? - electrical conductivity solid?
- electrical conductivity molten or in solution?
- happens between - a metal and a non metal
- how does it form - the metal transfers electrons to the non- metal forming ions
- ion- a charged particle form an atom gaining or losing electrons
- metals form… - positive ions
- non - metals form… - negative ions
-melting points - high me,ting points as a lot energy needed to break the ionic bond and the electrostatic force in the giant ionic lattice
-electrical conductivity solid - as a solid it does not conduct electricity because the ions can’t move
-electrical conductivity molten or in solution - can conduct electricity as the ions are free to move and carry the electrical current through the material
What is a giant ionic lattice
The giant structure formed when millions of of ions come together
COVALENT BONDING
- happens between…
- how does it form?
- molecule?
-melting point?
- electrical conductivity?
- Happens between - two non - metals
-how does it form - non metals share a pair of electrons - molecules- two or more atoms bonded together
-melting points - low melting point as little energy is required to break the weak intermolecular force
-electrical conductivity - does not conduct electricity as no free electrons that can move and carry an electrical current
