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Chemistry
Topic 2: bonding
intermolecular forces
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london forces are
temporary
london forces act between all
atoms
and
molecules
london forces
Electrons keep moving within the atom
Where there is a
high
amount of electrons it becomes partially
negative
Areas with less electrons become partially
positive
This means atom can become temporarily
attracted
to another atom
hydrogen bonding
strongest
intermolecular
Can only occur between F H O
permanent dipole dipole
attractive
forces between two neighbouring molecules with a
permanent dipole
intramolecular
forces are stronger than intermolecular forces e.g.
hydrogen
is weaker than covalent bond
Describe how
London forces
form between
halogen
molecules.
the uneven distribution of electrons causes a
temporary dipole
in the first molecule which causes a second dipole in another molecule
Methanol
,
CH3OH
, is miscible with water in all proportions. Sodium chloride is much less soluble in methanol than in water.
Explain these statements using your knowledge of the interactions between solutes and solvents.
there is
hydrogen
bonding between methanol and water
the
strength
of all intermolecular forces between methanol and water is approximately the
same
as those in water and methanol
in sodium chloride the
hydration
of Na+ and Cl- happens
the ionic bonding is
stronger
than the bonding between sodium chloride ions and water
Explain why
hydrogen bonding
causes ice to be less dense than liquid water
there us more space between molecules duet to
3D lattice
hydrogen bonds are longer than
covalent
bonds
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