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c3 - Structure and bonding (giant ionic structures (ions free to move…
c3 - Structure and bonding
atoms into ions
a compound contains two or more elements that are chemically combined
sharing electrons = covalent
transferring electrons = ionic
lose/gain electrons to form charges particle
ionic bonding
ions formed are held next to each other by very strong forces of attraction between oppositely charged ions - electrostatic force of attraction in all directions is called ionic bonding
ionic compound are neutral
giant ionic structures
ions free to move anywhere in liquid, attracted to oppositely charged electrodes held in molten compound - carry their electric charge through liquid
many ionic compounds dissolve in water - lattice splits up by water molecules, ions free to move in solution formed
ionic compound in solution
- H2o molecules separate ions from attic - free to move,
does conduct electricity
solutions of an ionic compound conduct electricity
solid ions dont conduct electricity, ions in fixed position
ionic solid
- fixed position, can't move,
doesnt conduct electricity
ionic compounds have a high melting and boiling point
takes a lot of energy to break up a giant lattice, lots of strong bonds to break
ionic compounds consist of a giant structure of ions arrogated in a lattice
ionic solid melts and becomes liquid
molten ionic compound
- high temp,overome strong attractive forces between ions, free to move,
does conduct electricity
states of matter
covalent
neither atom can give away atom
diamond has a giant covalent structure
non metals react together, atom share pair of electrons and form molecules -covalent bonding
structure of a simple molecules
covalent bonds re very strong
compounds make of simple molecules don't conduct electricity, no overall charge on simple molecule, neutral molecule cant carry electrical charge
intermolecular force increase with size of molecule, larger molecule have a high melting and boiling point
weak intermolecular forces between molecules
giant covalent structures
diamond - no delocalised electron
giant covalent structures
1) diamond - carbon
2) graphite
3) silicon dioxide
high melting and boiling point
insoluble in water
each carbon atom forms 4 strong covalent bonds in giant lattice
apart from graphite, hard, doesn't conduct electricity
graphite
soft, feels slippery
layers can slide over each other
no covalent bonds between layers, only weak intermolecular forces
forms hexagons
carbon atoms only bonded with 3 atoms
good conductor of electricity
forms 3 strong covalent bonds, one spare outer
electron on each carbon atom in graphite
electron can move freely about the layers of
carbon atoms -
sea of delocalised electrons
can conduct electricity
fullerenes and graphene
graphene
incredibly strong
single sheet of carbon atoms from graphite
piece of sticky tape, pull of graphene, under microscope, thinnest material ever made
excellent conductor of thermal energy and electricity
low density
most reactive form of carbon
fullerene
trying to create carbon atom behaviour in outer space in lab, created carbon 60 atom
structure of hexagon and pentagons arranges in sphere
hollow shaped molecules of carbon fullerene
high ensile strength - tennis racket
high electrical and thermal conductivity, delocalised electrons
could be used for drug delivery in body to treat cancer in specific parts of body, used as lubricants and catalysts - large surface area
bonding in metals
metals from crystals
metallic bonding
outer electron from each metals atom can easily move throughout giant structure
delocalised electron - no loner linked with particular metal ion
strong electrostatic attraction between -ve charges electron and +ve charged ion bonds metal ions to each other
giant metallic structure
-ve charge between +ve charge ion hold metal ions positions by electrostatic forces of attraction
delocalised electron can flow through giant metallic structure
when struck, metal atoms slip past one another without breaking metals structure
atoms arranged in closely packed layers allow atoms to slide over each other
atoms usually mixture of metals
metals are ductile - drawn out into wires
an alloy is a mixture of two or more elements, at least one is metal
takes a lot of energy to separate metal ion from fixed position
electrons able to move throughout whole lattice
delocalised electron enables lattice to distort
