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4116122
Shapes Of Molecules
Descripción
Mind Map of the shapes of molecules
Sin etiquetas
chemistry
a-level
Mapa Mental por
Alexander Boon
, actualizado hace más de 1 año
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Creado por
Alexander Boon
hace más de 8 años
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Resumen del Recurso
Shapes Of Molecules
Molecules with lone pairs
Pyramidal
These molecules have 1 lone pair and 3 bonding pairs of electrons
Examples are: Ammonia(NH3) - Bond angle of 107 degrees
Non-Linear/Bent
These molecules have 2 lone pairs and 2 bonding pairs of electrons
Examples are: Water(H2O) - Bond angle of 104.5 degrees
If a molecule is tetrahedral, 1 lone pair will make it pyramidal
Adding another lone pair to this will result in a non-linear/bent shape
A lone pair of electrons is more electron dense than a bonded pair
As such, each lone pair reduces the bond angle by about 2.5 degrees
Molecules without lone pairs
Linear
These molecules have 2 bonding pairs of electrons
Examples are: H2 or CO2 - Bond angle of 180 degrees
Trigonal Planar
These molecules have 3 bonding pairs of electrons
Examples are: BF3 - Bond angle of 120 degrees
Trigonal Bipyramid
These molecules have 5 bonding pairs of electrons
Examples are: PCl5 - Bond angles of 90 and 120 degrees
The angle between the vertical bond and horizontal bond is 90 degrees. However, the angle between each horizontal bond is 120 degrees
Octahedral
These molecules have 6 bonding pairs of electrons
Examples are: SF6 - Bond angle of 90 degrees
Tetrahedral
These molecule have 4 bonding pairs of electrons
Examples are: Methane - CH4 - Bond angle of 109.5 degrees
Shapes of ions
The principles about molecular shapes can be applied to ionic shapes
As such in the example of an ammonium ion - NH4, the shape is tetrahedral
Thus meaning that it has 4 bonding pairs of electrons
However, it will also need to be surrounded by square brackets and have the displayed charge as it is an ionic molecule
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