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Bonding
Atoms want to achieve noble gas electronic configuration
Ionic Bonding: Non-directional electrostatic attraction between
oppositely charged (positive and negative) ions
...

Structure: Giant Metallic Structure - regular arrangement of
positive ions surrounded by delocalised electrons
Covalent Bonds
Giant Covalent: Directional electrostatic attraction between
shared pairs of electrons and positively charged nuclei
• Non-metal combine to form stable electrostatic configuration
(overlapping of orbitals)
Structure: Giant Network Structure - atoms are connected by
covalent bond
Intermolecular Force: Molecules are attracted by a weak

intermolecular force (three types: Van der Waal’s force, Dipoledipole force and hydrogen Bond)
Structure: Covalent Bond holding atoms in a molecule, but weak
intermolecular force attracting molecules
Van der Waal’s Force - All molecules and noble gas atoms
• One end of atom having excess electron / proton over the other
(random fluctuation of electron - instantaneous) - temporary
dipole
• Electrons in the neighbouring molecules/atom are
Attracted to positive end of the temporary dipole
Repelled by negative end of the temporary dipole
• Form induced dipole
• Van der Wasl’s Force = attraction between induced dipole and
temporary dipole
• The molecular Mass - Larger molecules have more electron, more
chance of getting partically charged
Dipole-Dipole Attraction - Polar Molecule/ Atom ONLY
• Attraction between positive and negative end of polar molecule
• Determine: Difference in Electronegativity
Hydrogen Bonding - Molecules that have hydrogen bonded
• Hydrogen Atom is bonded to highly electronegative atoms
• The high electronegative atoms form sigma Properties
Bonding Ionic Bond

Structur
e

Giant Lattice
- regular
arrangement
between
oppositely
charged ions

Metallic
Bond

Giant
Covalent
Bond
Giant
Giant
Metallic Network regular
all atoms
arrangement are held by
of positive
covalent
ions
bond

Intermolecul
ar Force
Covalent
Bond holding
atoms in a
molecule, but
weak
intermolecular

Melting/
Boiling
point

High - every
ions are
strongly held
together by
electrostatic
attraction
...


Volatility No - strong
ionic bond
need to be
broken
Solubilit
y

Dissolve in
polar solvent,
as they move
between the
ions

Strength Brittle (can
split to
smaller
crystal with

surrounded
by
delocalised
electrons
High positive ions
are strongly
held by
electrostatic
attraction
...


force
attracting
molecules

High every
atoms are
strongly
held by
covalent
bond
...

No - strong
No metallic
Strong
bond need
Covalent
to be broken bond need
to be
broken
N/A
Solvent
cannot
move
between
the
covalent
bonded
atoms

Low - only
weak
intermolecular
force
between
molecules
...


Melleable
(layer of
metal ion
can slide

N/A

Very Hard
(Except
Graphite)

Yes - Weak
intermolecular
force can be
broken easily
Polar
molecules
dissolve in
polar solvent
Non-polar
molecules
dissolve in
non-polar
solvent

smooth
surface) or
Crushed Rearrangeme
nt of ions
...

Because
they have
the ability to
slide over
each other
without
breaking the
metallic
bond
Only in
Conduct Only in
molten or
molten or
ivity
aqueous
aqueous
state state mobile ions
mobile ions
(free to move) (free to
move)

Cannot except
graphite has
mobile
decolonize
electrons

Cannot - no
free electrons
or charged
particle

Bond Order (Number of bonds/Number of Domains): Number of
electron pairs shared between two atoms
Bond Length: Distance between the nuclei of the two bonded atoms
Bond Strength: Strength of electrostatic attraction between the
shared pair electron and positive nuclei - energy required to break
the bond
Valence Shell Electron Pair Repulsion Model
Bond pair and lone pair do not like to be close together
...
Note
that the repulsion of lone pair is greater than bond pair
...
5)
Trigonal Pyramid (107)
V shape (104)

3
4

 



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