C2-bonding structure of atom

Created by

osama bin laden

Cards (40)

features of solids
fixed shape in regular pattern
vibrate not move
features of liquid
can move
particles close together but flow around
features of gas
widely spread
particles move quickly and randomly
what are the limitations of the simple particle model
assumes all particles are solid spheres
assumed there are no forces between particles
how to turn gas int liquid
condensation
why do elements do ionic bonding
to achieve full outer shell to become a stable element
which elements does ionic boding take place
metal and non metal
what happens during ionic bonding between group 1 and 7
group 1 metals lose electron
group 7 non metal gains one electron
so both ions have a full outer shell
what happens during ionic boning between group 2 and 6
group 2 metal lose 2 electrons
group 6 non metal gains 2 electrons
so both ions have full outer shell to be stable
why do ionic compounds have a high melting and boiling point
strong electrostatic forces of attraction require lost of heat energy to break
why can't ionic compounds conduct electricity when a solid
ions locked in place by strong electrostatic forces so ions can vibrate but cannot move
which elements does covelant bonding happened between
non metals
what happens in a covalent bond
non metals share electron to become stable - bonded together
why do small covenant molecules have a low melting and boiling point
it has weak intermolecular forces which don't require a lot of energy to break
why can't small covenant molecules conduct electricity
they don't have an overall electric charge
why are giant covalent substances solids at room temperature
they have high melting and boiling points
why do giant covenant bonds have high melting and boiling points
they have millions of covelant bonds that require lots of energy to break
why can't diamond conduct electricity
all outer electrons are in covalent bonds so it has no free electrons to carry electrical charge
features o silicon dioxide
high melting and boiling points
can't conduct electricity
features of graphite
soft
high melting and boiling points
good conductor of electricity and heat
why is graphite soft
hexagonal rings of layers slide over each other because it have no covelant bonds
why does graphite have a high melting and boiling point
has strong covenant bonds which require lost of energy to break
how is graphite a good conductor of heat and electricity
delocalise electrons (electrons not in a bond ) can move
what element if graphite formed from
carbon
properties of graphene
good conductor of heat
very strong
high melting and boiling points
uses of fullerenes
deliver drug into body
lubricants in machines
catalyst
properties of carbon nanotubes
high tensile strength
good conductors of electricity and heat
uses of carbon nanotubes
reinforce materials- tennis rackets
what is the bonding in polymers
strong covenant bonds
what is the structure of polymers
large molecule made up of identical monomers
why are polymers solids at room temperature
intermolecular forces are strong which requires lots of energy to break so it has a high melting point
what happens during metallic bonding
force between delocalised electrons and positive metal ions cause a strong electrostatic attraction
which elements does metallic bonding occur
metals
properties of metals
bent and shaped
good conductors of heat and electricity
high melting and boiling points
why can metals be bent and shaped
layers of atoms can slide over each other
how are metals good at conducting heat and electricity
delocalised electrons can move which can carry thermal energy or electrical charge
what is an alloy
mixture of metals to make pure metals harder
limitations go ball and stick model
ions shown as widely space but are packed together
only shows tiny part of giant crystal lattice
limitations of dot and cross model
doesn't tell us shape of molecule
limitations of space filling diagram
difficult to see 3D packing
only shows tiny part of giant crystal lattice