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Intermolecular Forces of Attraction - Coggle Diagram
Intermolecular Forces
of Attraction
Van der Waals Forces
Dipole Dipole forces
London dispersion forces
Responsible for
the physical properties
• Melting and Boiling point
• Solubility
Dipole-dipole forces
Polar molecules
The more polar a molecule is
The stronger the dipole-dipole moment
HCl > HBr
because Cl is more electronegative
than Br
weaker than hydrogen bonds
The (+) end of the dipole of one molecule
will attract the (-) end of the dipole of another
molecule
London Dispersed forces
all atoms and non polar
atoms when they're close
Random movement of electrons
At any given instant,
electron distribution are
asymmetrical
giving the atom
temporary
dipole moment
Next, the electrons in
neighboring atom produced
dipole
.
Induction
- process where new
dipole is formed
forces attraction between
temporary dipole
and
induced
dipole
Factors which Influence
Van der Waals forces
SIZE
SHAPE
Polarity
•
Polarizability
is a measure of how easily an electron cloud is distorted by an electric field.
• Increases with size
•Linear unbranced - stronger temporary dipole
• Larger surface area
• Boiling point : Butane > 2-methylpropane
• electron higher
• more distance
• greater temporary dipole
• greater boiling point
Hydrogen bond
A strong permanent dipole
A hydrogen atom is covalently bonded with:
an electronegative atom (F,O,N)
the lone pair of another electronegative atom
H-F > H-O > H-N
Effects on Physical properties
Solubility of simple
covalent molecules
Boiling point
H20 > HF > NH3
Density water and ice
Metallic bond
Formes when atoms give up their
valence electron and forms positive ions
result from the electrostatic attraction between metal cations and delocalized electrons.
Attraction between the
free-floating valence electrons
and positively charged metal ions
Metallic properties
• malleable
• ductile
•can conduct electricity in solid
Melting points and boiling points
indicates the metal's strength
