metallic, covalent and ionic Flashcards
what is a covalent bond
:A shared pair of electrons between two non-metals.
what is an ionic bond
the forming of ionic bonds is between metals and non metals
what is a metallic bond
The bonds present in metals between the positive metal ions and negatively charged electrons
between metals-positive metal ions, negative delocalised electrons
what are the 4 state symbols
aq
s
l
g
what force is in covalent bonding
intermolecular forces
what is the force in ionic bonding
electrostatic force
def. intermolecular
The forces which exist between molecules. The strength of the
intermolecular forces impact physical properties like boiling/melting point.
def. electrostatic force
The strong forces of attraction between oppositely charged ions.
what are the 3 covalent structures
simple molecules
large molecules
giant covalent
describe simple molecular (covalent)
has covalent bonds and has weak intermolecular forces of attraction
describe simple molecular (covalent)
has covalent bonds and has weak intermolecular forces of attraction
describe giant covalent
has strong covalent bonds
examples of giant covalent
graphite
diamond
silicon dioxide
graphene
examples of simple covalent
(normally gases)
halogens, cl2, I2
water, oxygen, methane, nitrogen
what is an alloy
a mixture of a metal with atoms of another element
mixture of 2 or more metals
why do metals have high boiling/melting points
electrostatic force of attraction between positive and negative metal ions and delocalised electrons is strong and requires a lot of energy to break.
giant structure
def. delocalised electrons
free moving electrons
what are covalent (simple molecules) melting and boiling points
low melting and boiling bonds arent strong like giant bonds
what are the 4 properties in a pure metal
malleable
high melting and boiling points
good conductors of electricity and thermal energy
what is an ion
A charged particle formed when when an atom gains or loses electrons
what is the structure of diamond
.giant covalent structure
.each CARBON atom is bonded to 4 other carbon atoms
.very strong covalent bonds
doesnt conduct electricity-no free electron in outer shel
hard
structure for metallic bonding
metals-malleable, ductile
giant structures
layers of ions slide
why are metallic bonds have good conductors
the delocalised electrons can move throughout the metal
metallic bonds characterists
high melting and boiling points
consist of metal ions an delocalised electrons
properties of giant covalent
very hard insoluble in water very string high melting+boiling doesnt conduct electricity(except graphite) solid
properties of small covalent bonding
low melting+boiling
doesnt conduct electricity-no charged particles
graphite properties
giant covalent structure bonded to three other carbon atoms very string slide past each other easily(Layers) spare electron becomes delocalised
what is a polymer
:Large long-chain molecules made up of lots of small monomers joined together
by covalent bonds(mononmer)
ionic bonding structure
giant lattice structure
ions attract each other
strong electrostatic forces
high melting add boiling
solid state dont conduct electricity
(only when molten/dissolved in water)
free moving
graphene properties
strong
conduct electricty
what bond is polymers in
covalent
polymers properties
Have very large molecules
properties of alloy
The different sized atoms distort the layers in the structure, making it
harder for them to slide over each other. So alloys are harder than pure
metals.
2 different metals
