BONDING + STRUCTURE
type
examples
particles at
lattice point
metallic
ionic compound
GIANT METALLIC STRUCTURE
GIANT IONIC STRUCTURE
metal
metal + non-metal
Na, Fe, Cu, …
NaCl, CaCl2, …
positive metal ions
positive + negative ions
metalic bond: strong electostatic
attraction between positive metal ions +
mobile (delocalized) electrons
ionic bond: strong electrostatic
covalent compound
GIANT COVALENT
SIMPLE MOLECULAR
STRUCTURE
STRUCTURE
mainly Group IV non-metals + its
compounds
diamond, graphite, silicon (Si), silicon
dioxide (SiO2)
atoms
non-metal
I2, HCl, H2O, CH3OH, …
simple discrete molecules
covalent bonds: strong electrostatic
attraction between the positive ions +
atoms held by strong covalent
negative ions
bonds in molecules
molecules held by weak
intermolecular forces
diamond + carbon = allotropes: same
element, diff molecular structure
no. of valence electrons increases 
bonding
diamond + silicon dioxide: tetrahedral
charge of positive metal ions increases
no. of delocalised electrons increases 
strength of metallic bond increases
metal ions smaller  positive nuclei
closer to delocalised electrons 
every Na+ particle is surrounded by 6
Cl- particles, every Cl- particle is
surrounded by 6 Na+ particles (Cl- : Na+
ratio = 1:1)
greater electrostatic attraction between
positive nuclei + delocalised electrons
 stronger metallic bonds
giant crystal lattices formed from 3-D
regular packing of positive + negative
arrangement (each carbon/silicon atom
joined to 4 other carbon/oxygen atoms)
van der Waals forces
graphite: carbon atoms hexagonally
hydrogen bonds found between
arranged (each C atom bonds with 3
molecules that contain H directly
other C atoms) in flat, parallel layers
bonded to N, O or F, stronger than van
held tgt by weak van der Waals forces
der Waals forces (give higher b.p. +
(4th unpaired valence electron of each
m.p.)
C atom = delocalised along layers)
ions
high m.p. + b.p.
m.p. + b.p.
strong electrostatic forces of attraction
high m.p. + b.p.
high m.p. + b.p.
low m.p. + b.p.
between positive ions + ‘sea’ of
strong electrostatic forces of attraction
strong covalent bonds between atoms
weak intermolecular forces of attraction
negative delocalized electrons require a
between oppositely charge ions require
in molecules require a large amt of heat
between molecules require small amt
large amt of heat energy to break
a large amt of heat energy to overcome
energy to overcome
of heat energy to overcome
up/overcome
soluble in water, insoluble in organic
(non-polar) solvents
organic: e.g. hexane, benzene,
insoluble in all solvents
except reaction w/ water to form alloys
(may be observed as “dissolving” but
solubility
not physically dissolving; chemical
change as new substances form)
reactive metals e.g. sodium, potassium
react w/ water  potassium gas
methylbenzene
generally: insoluble in water, soluble
water molecules = polar molecules
in organic (non-polar) solvents
which form electrostatic forces of
HCl in organic non-polar solvents 
attraction w/ ions  cause ions to
insoluble in all solvents
exist as simple discrete molecules
separate  dissolves compound
strong covalent bonds between atoms
HCl in water  ionises to form H+ + Cl-
organic molecules = non polar
in molecules require a large amt of
molecules  cannot attract ions 
energy to overcome
unable to dissolve compound
polar moleculars  more soluble in
polar solvents (water)
non-polar molecules  more soluble in
non-polar solvents
good in solid + molten states
not in solid state, good in molten
poor in any state
poor in any state
delocalised electrons rapidly carry
(liquid) / aqueous state
substances made of neutral atoms + do
no mobile charged particles to carry
electrical
charges through metal lattice, greater
solid state  ions fixed within crystall
not contain mobile charge particles
charges + conduct electricity
conductivity
no. of valence electrons  electrical
lattice, can only vibrate about lattice
(delocalised electrons / mobile ions) to
conductivity increases
points
carry charges + conduct electricity
molten/aqueous state  ions free to
EXCEPT polar molecules which form
ions in water e.g. HCl
(heat: delocalised electrons gain kinetic
move  act as charge carries to
EXCEPT graphite
ionises in water  form acidic solutions
energy, move faster to transfer gained
conduct electricity
graphite = presence of delocalised
w/ mobile H+ + Cl- ions  conducts
energy throughout metal 
electrons along layers  good
electricity
rapid movement of delocalised
conductor of electricity
electrons)
hard yet malleable + ductile
malleable: can be hammered into
different shapes
ductile: drawn into wires w/o breaking
layers of atoms can slide over one
hardness
another w/o breaking strong metallic
bonds
hard + brittle
shatter when hit
very hard
large amt of energy required to break +
when lattice is hit  layer of ions is
deform strong covalent bonds between
shifted  ions w/ same charges are
atoms
lined up together
like charges repel each other  split
EXCEPT graphite
ionic lattice  causes it to shatter
graphite layers held by weak van der
Waals forces  soft
generally soft
small amt of energy required to break +
deform weak intermolecular forces
between molecules