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Inorganic Chemistry Lecture 6 (Intermolecular forces (The attractive and…
Inorganic Chemistry Lecture 6
Intermolecular forces
The attractive and repulsive forces between atoms and electrons can be used to explain molecular structure (VSEPR)
These forces are less than 1/10 as strong as a covalent bond, but are significant enough to answer questions such as why is H2O a liquid?
However, there are also forces between molecules which can be used to explain the many properties of matter
Intermolecular forces: The weak attractions/repulsions between molecules
Electrostatic Forces
These forces are between full charges (+) and (-) and are the strongest force
There is a repulsive force when two particles with the same charge both positive or negative are brought together
You find these in proteins (ion pairs) ionic bonds, their strength is governed by coulomb's law
Dipole Dipole forces, between two polar molecules, Polar molecules have permanent dipoles. Chlorine is more elctronegative then hydrogen
So the shared electrons in the H-Cl bond are more attracted to chlorine making this end of the molecule partially negative. Because electrons are pulled away from hydrogen, it becomes partially positive. This is fixed and permenant. As a result, HCl and other polar molecules experience an intermolecular attraction called the dipole dipole force
A dipolar molecule (HCl) near a polarisiable non-polar molecule (Diffuse electrons Large atomic radius ) can include electron distributions to form transient dipoles- these being induced dipoles
Dipole moment helps to predict the polarity of molecules
Dipole moment is equal to the magnitude of the charge times the distance between the charges (d)
Molecules can be more electronegative by having more electrons around them
Dipole dipole interaction
When two polar molecules meet electrostatic attraction between those two molecules so you would therefore need energy to pull them apart
Hydrogen bonding
Van der waal forces
Nobel gasses full outer shell, electrons are probabilistic hey are not in a fixed orbit around things,
It takes very little energy to put the nobel gasses in gas form because there is no van der waal forces between them
Chemical reactions