Please enable JavaScript.
Coggle requires JavaScript to display documents.
structure and characteristics of the three diff bonding - Coggle Diagram
structure and characteristics of the three diff bonding
IONIC BONDING
forms giant ionic structure
arranged in giant ionic crystal lattice structure
consist of ions held by strong electrostatic forces of attraction between positive and negative charged ions
physical properties of ionic compounds
high melting and boiling points
ins held tgt by strong electrostatic attraction between oppositely charged which REQUIRES a lot of energy to break down the structure
conduct electricity in the molten or aqueous state : ions are MOBILE and electrical conduction is possible
cannot conduct electricity in solid state ions are held in FIXED POSITIONS in the crystal lattice structure , with no free-moving charged carriers
dissolves in INORGANIC solvents (water)
COVALENT BONDING
have simple molecular structure OR giant molecular structure
simple molecular : (water , methane , carbon dioxide)
giant molecular structures ( diamond , graphite)
simple molecular structure
have LOW melting and boiling points thus is volatile (vaporise easily)
(low mp and bp due to ) weak intermolecular forces between simple molecule
REQUIRES very LITTLE heat to overcome the intermolecular forces
do not conduct electricity in all states as there is NO. free-moving ions or electrons to conduct electricity
soluble in organic solvents , insoluble in water (exceot alcohol and sugar )
macromolecules or giant molecular structues
Diamond
bonding : consists of only carbon atoms , each carbon atoms uses all four valence electrons to form four strong covalent bonds with other four carbon atoms in TETRAHEDRAL arrangement
all carbon atoms bonded tgt by STRONG COVALENT COVALENT BONDS in three dimensional lattice
properties
HARD - carbon atoms unable to slide over each other as all carbon atoms are bonded by strong covalent bonds between carbon atoms in a giant ionic crystal lattice structure which requires large amount of energy to overcome to break
CANNOT CONDUCT ELECTRICITY - there are no free moving electrons to carry electric current through the structure as all valence electrons are used for bonding
HIGH MP AND BP - a lot of energy is needed to break the MANY strong covalent bonds between carbon atoms
USE- jewellery , cutting tools , used on hard surfaces
Graphite
consist of only carbon atoms, allotropes
consists of hexagonal layers of carbon atoms , layers are held by WEAK INTERMOLECULAR FORCES - two dimension flat layers
properties
HIGH MP , BP - a lot of energy is needed to overcome numerous strong covalent bonds between carbon atoms
SOFT - hexagonal layers are able to slide over each other because the weak intermolecular forces of attraction between the layers of carbon can be EASILY overcome with LITTLE energy
CONDUCTS ELECTRICITY BETWEEN LAYERS - since each carbon atoms used only 3 valence electron , hence with the freely moving , delocalised electrons , electric current is able to be carried between the layers
silicon
GMS similar to diamond l silicon
PROPERTIES : not as hard as diamond , high mp , bp , only conduct electricity when they are impurities
silicon dioxide (silica)
GMS similar to diamond
each silicon atom is bonded to four other oxygen atoms, in aa tetrahedral arrangement ( 4 covalent bonds formed)
PROPERTIES : not as hard as diamond , high mp and bp , poor conductor of electricity