C3 structure and bonding Flashcards
what are the 3 types of bonding
covalent ionic and metallic
what is ionic bonding
compounds formed from metals combined
with non-metals.
what is covalent bonding
two non-metal atoms share a pair of electrons
what is metallic bonding
the electrostatic attraction between positive metal ions and delocalised electrons
what happens in ionic bonding
transfer of electron to the outer shell
both atoms become ions because they have full outer shells
the ions are oppositely charges which attract each other by electrostatic forces to form an ionic compound
what is an ionic compound
a giant structure of ions
how are ionic compounds held together
strong electrostatic forces of attraction between
oppositely charged ions these forces act in all directions in the
lattice and this is called ionic bonding
what are some of the properties of ionic compounds
high melting and boiling points
do not conduct electricity when solid because the ions cannot move
do not conduct electricity when molten
what structures have giant covalent bonding
diamond graphite and silicon
what is an intermolecular force
forces of attraction between the molecules
what are the 3 states of matter
solid liquid and gas
how much energy is needed to change state
The amount of energy needed to change state from solid to liquid and from liquid to gas depends on the strength of the forces between the particles of the substance
state the 3 limitations of the particle model
the forces between the particles
the volume of the particles
the space between the particles
what does aqueous mean
dissolved in water
what happens when a substance changes state
the particle stay the same
how do solid particles move
they vibrate around fixed proportions
how do liquid particles move
flow around each other
how do gas particles move
very quickly in all directions
name 2 things a pure substance will do
melt and freeze at 1 specific temperature the melting point
boil and condense at 1 specific temperature the boiling point
what is a polymer
large molecule made up of repeating subunits known as monomers
how are atoms arranged in pure metals
atoms are arranged in layers, which allows metals
to be bent and shaped.
why are alloys harder than pure metals
in an alloy, there are atoms of different sizes.
The smaller or bigger atoms distort the layers of atoms in the pure metal.
This means that a greater force is required for the layers to slide over each other
why are metals good conductors of electricity
the delocalized electrons in the metal carry electrical charge through the metal.
why are metals good conductors of thermal energy
the delocalized electrons transfer the energy
what are the properties of diamond
diamond is very hard,
very high melting point
does not conduct electricity ( no charged particles)
what are the properties of graphite
each carbon atom forms three covalent bonds with
three other carbon atoms, forming layers of hexagonal rings which have no covalent bonds between the layers.
layers are held together by weak intermolecular forces
In graphite, one electron from each carbon atom is delocalised
conducts heat and electricity
very high melting point
what is graphene
a form of carbon and a single layer of graphite
what are the properties of graphite
arranged in a hexagonal structure (1 atom thick)
very strong
good thermal and electrical conductor
nearly transparent
what are fullerenes
Fullerenes are molecules of carbon atoms with hollow shapes
describe the structure of fullerenes
hexagonal rings of carbon atoms but they may also contain rings with five or seven carbon atoms.
what was the first fullerene to be discovered
The first fullerene to be discovered was Buckminsterfullerene (C60) which has a spherical shape. joined together in a series of pentagons and hexagons
what are carbon nanotubes
cylindrical fullerenes
what can fullerenes be used for
deliver drugs in the body
lubricants
catalysts
reinforcing materials
