C2-bonding and structure

Created by

Elle Roberts

Cards (32)

what are ions?
charged particles
what happens when metals form ions?
lose electrons from the outer shell to form positive ions
what happens when non metals form ions?
gain electrons into the outer shell to form negative ions
what are cations?
positive ions
what are anions?
negative ions
what is ionic bonding?
between a metal and non metal
transfer of electrons
what is the structure of ionic compounds?
giant ionic lattice
properties of a regular lattice
ions are closely arranged
very strong electrostatic forces of attraction between oppositely charged ions
properties of ionic compounds
-high melting and boiling points as there are strong bonds between ions
-don't conduct electricity when solid
-when melted ions freely move to carry electric charge
-dissolve in water so ions separate and freely move carrying an electric charge
what is covalent bonding?
between non metals
sharing of electrons
what are simple molecular substances?
made up of molecules containing a few atoms joined together by covalent bonds
examples of simple molecular substances?
-hydrogen
-oxygen
-methane
-chlorine
-nitrogen
-water
-hydrogen chloride
properties of simple molecular substances
-atoms are held together by very strong covalent bonds but have weak forces of attraction between the molecules
-low melting and boiling points as there is low energy needed to break the forces
-gases or liquids at room temperature
-bigger molecules have stronger intermolecular forces so require more energy to melt
-don't conduct electricity as they are not charged so there are no free electrons
what are polymers?
long chains of repeating units
properties of polymers
-large intermolecular forces between molecules so more energy needed to break. solids at room temperature
-lower boiling points than ionic compounds
what are giant covalent structures?
all atoms bonded by strong covalent bonds
properties of giant covalent structures?
-very high melting and boiling points as lots of energy is needed to break covalent bonds between atoms
-don't conduct electricity as theres no charged particles
examples of giant covalent structures
-diamond made of carbon atoms
-graphite made from carbon atoms, layers of hexagons, delocalised electrons
-silicon dioxide made of silicon and oxygen
what are allotropes?
different structural forms of the same element in the same physical state
properties of diamond
-very hard as each carbon atom forms 4 covalent bonds
-high melting point as the covalent bonds need lots of energy to break
-doesn't conduct electricity as it has no free electrons
properties of graphite
-each carbon atom forms 3 covalent bonds creating sheets of carbon atoms arranged in hexagons
-no covalent bonds between layers so they're held together weakly so they can move over each other which makes it soft and slippery
-high melting points as covalent bonds need lots of energy to break
-conducts electricity as theres 1 delocalised electron in each carbon atom
properties of graphene
-one layer of graphite
-very strong
-light
-contains delocalised electrons so can conduct electricity
what are fullerenes?
molecules of carbon shaped like closed tubes or hollow balls
like the buckminsterfullerene
what can fullerenes be used for?
drug delivery
lubricants
industrial catalysts
what can nanotubes be used for?
nanotechnology
tennis racket frames
electronics
properties of metals
-solid at room temperature as the electrostatic forces between atoms and delocalised atoms are strong so need lots of energy to break so high melting and boiling points
-conductors of electricity and heat as delocalised electrons carry electrical charge and thermal energy
-malleable as layers of metal can slide over each other
why are alloys harder than pure metals?
alloys are mixtures of two or more metals or a metal and another element
when another element is mixed with a pure metal the new metal will distort the layers of metal atoms making it harder to slide over each other making alloys harder
properties of solids
-strong forces if attraction so particles are close together in a fixed arrangement
-definite shape and volume
-particles vibrate
properties of liquid
-weak force of attraction between particles
-randomly arranged and particle sized gaps
-definite volume, no definite shape
properties of gases
-very weak forces of attraction
-free to move and particles are far apart
-fill the container, no definite shape or volume
-constantly move in random motion
how does a solid change to a gas?
solid melts into liquid which boils into a gas
how does a gas turn into a solid?
gas condenses into a liquid which freezes into a solid