MindMap Gallery Giant Covalent Bonding
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Giant Covalent Bonding
This mindmap is about giant covalent bonding. It has the following content: - allotrpoic forms of carbon - fun facts - silicon dioxide - comparing the different strcutures in matter You may find more mindmaps on EdrawMind.
Edited at 2022-07-10 05:18:57
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Giant Covalent Bonding
Allotropic forms of carbon
an element is said to exhibit allotropy if it occurs in 2 or more forms
Diamond
made up of only carbon atoms
every carbon atom is bonded to 4 other carbon atoms by strong covalent bonds
giant covalent structure
High melting point
large amount of energy required to break the strong covalent bonds between carbon atoms in the giant molecular structure
non - conductor of electricity
no delocalised electrons as all valence electrons of each carbon atoms are used for covalent tbonding
Graphite
found in sand
consists of seperate layers of carbon atoms
carbon atoms are arranged in regular hexagons in flat parallel layers
carbon forms strong covalent bonds with 3 other carbon atoms
forms rings of 6 carbon atoms which are joined together to form 2 - dimensional layers
no strong bonding in between layers
they are easily seperable from each other
held together by weak forces of attraction
so the layers slide over each other easily when a force is applied
accounts for softness and lubricating power of graphite
physical properties
high melting and boiling points
forces of attraction between layers are weak
but a lot of energy is still needed to break the strong covalent bonds between carbon atoms within layers
this can cause a change of state
Good conductor of electricity
each carbon atom has 1 valence electron that isn't used to form covalent bonds
delocalised electrons move freely along layers from one C.A. to another when graphite is connected to a circuit
this causes an electric current to flow, causing graphite to conduct electricity
Soft and slippery
when a force is applied
weak forces of attraction between the layers of carbon atoms are easily overcome
so layers can easily slide over one another
Silicon dioxide
giant covalent structure
structure similar to diamond
similar physical properties
used to produce glass
each silicon atom is bonded to 4 oxygen atoms
each oxygen atom is bonded to 2 oxygen atoms
atoms are held together by strong covalent bonds
high melting points
Fun facts
Fullerene
a molecule made up of carbon atoms
arranged in the form of a
hollow sphere
called 'buckyballs'
cylinder
called 'carbon nanotubes'
amorphous forms of carbon
most reactive form of carbon
does not have any crystalline structure
burns relatively easily in air
serving as a fuel
has structural features of graphite
has sheets and layers
atomic structure is irregular
Comparing the different structures in matter
covelent substances
simple molecular structure
hydrogen, nitrogen, carbon dioxide
exists as simple molecules
low melting and boiling points
soluble in organic solvents but not in water
doesn't conduct electricity in any state
giant covalent structure
diamond, graphite, silicond dioxide
exists as a giant network of covalently bonded atoms
high melting and boiling points
does not conduct electricity (except graphite)
giant structures
giant ionic
bonding
electrostatic attraction between oppositely charged ions
melting and boiling points
high
soulbility in water
usually soluble
solubility in organic solvents
insoluble
electrical conductivity
non - conductor in solid state, but conductor in molten and aqueous states
giant metallic
bonding
electrostatic attraction between metal cations and 'sea of mobile electrons'
melting and boiling points
high
solubility in water
insoluble
solubility in organic solvents
insoluble
electrical conductivity
conductor in solid and molten states
giant covalent
bonding
electrostatic attraction between shared electrons and positive nuclei of the atoms
melting and boiling points
high
solubility in water
insoluble
solubility in organic solvents
insoluble
summary of 4 structures in matter:
ionic
example
sodium chloride
particles present
cations, anions
bonding
ionic bond
electrostatic attraction between oppositely charged ions
melting and boiling points
high
physical state at r.t.p.
solid
solubility
in water
soluble
in organic solvents
insoluble
electrical conductivity
good conductor in molten and aqueous states
due to mobile ions
non conductor in solid states
due to ions in fixed positions
metallic
example
iron, nickel, steel
particles present
metal cations, sea of delocalised electrons
bonding
metallic bonding
electrostatic attraction between metal cations and sea of delocalised electrons
melting and boiling points
high
physical state at r.t.p
solid
solubility
in water
insoluble
in organic solvents
insoluble
electrical conductivity
good conductor in molten and solid states
simple molecular
example
carbon dioxide
particles present
simple molecules consisting of neutral atoms
bonding
covalent bonds within atoms of molecules
melting and boiling points
low
physical state at r.t.p
liquid or gas
solubility
in water
insoluble
in organic solvents
soluble
electrical conductivity
non - conductor
due to absence of mobile charge carriers
giant covalent
example
graphite
particles present
atoms
bonds between particles
covalent bonds between atoms within the layer
melting and boiling points
high
solubility
insoluble in any solvent
conduction of electricity
good conductor
due to mobile and declocalised electrons along the layers
diamond, silicon dioxide
particles present
atoms
bonds between particles
covalent bonds throughout the giant strcuture
melting and boiling points
high
solubility
insoluble in any solvent
conduction of electricity
non - conductor
due to absence of delocalised electrons