6) Shapes of molecules and intermolecular forces Flashcards
Describe electron-pair repulsion theory (4)
- electron pairs surrounding a central atom determine the shape of the molecule or ion
- the electron pairs repel one another so that they are arranged as far apart as possible
- the arrangement of electron pairs minimises repulsion and thus holds the bonded atoms in a definite shape
- different numbers of electron pairs result in different shapes
What are wedges used for?
to help visualise 3D structures
A lone pair of electrons is _ and _ than a bonded pair. This results in a lone pair _ more strongly than a bonding pair.
slightly closer to the central atom
occupies more space
repelling
How much is the bond angle reduced per lone pair?
about 2.5 degrees
Define bond angle
the angle between two bonds at an atom
Give the name of the shape, its bond angle and an example for a molecule with 3 bonded pairs and 1 lone pair
pyramidal
107 degrees
NH3
Give the name of the shape, its bond angle and an example for a molecule with 2 bonded pairs and 2 lone pairs
non-linear
104.5 degrees
H2O
Give the shape, its bond angle and an example for a molecule with 2 electron pairs / regions
linear
180 degrees
CO2
Give the name of the shape, its bond angle and an example for a molecule with 3 electron pairs / regions
trigonal planar
120 degrees
BF3
Give the name of the shape, its bond angle and an example for a molecule with 4 electron pairs / regions
tetrahedral
109.5 degrees
CH4
Give the name of the shape, its bond angle and an example for a molecule with 6 electron pairs / regions
octahedral
90 degrees
SF6
Define electronegativity
a measure of the attraction of a bonded atom fro the pair of electrons in a covalent bond
Define Pauling electronegativity value
a value assigned as a measure of the relative attraction of a bonded atom for the pair of electrons in a covalent bond
What does Pauling electronegativity value depend upon?
an element’s position in the periodic table
as you go up and right electronegativity increases
What will happen if the electronegativity difference is large?
one bonded atom will have a much greater attraction for the shared pair of electrons than the other bonded atom
the more electronegative atom will have gained control of the e- and the bond will now be ionic rather than covalent
Give the electronegativity differences for the following types of bonding:
covalent
polar covalent
ionic
0
0 - 1.8
> 1.8
Describe a non-polar bond
the bonded pair of electrons is shared equally between bonded atoms that are the same / have the same or similar electronegativity values
Describe a pure covalent bond
when bonded atoms come from the same element and the electron pair is shared equally
Describe a polar bond
the bonded electron pair is shared unequally between the bonded atoms that are different and have different electronegativity values
Define dipole
a separation in electrical charge so that one atom of a polar covalent bond, or one end of a polar molecule, has a small positive charge and the other has a small negative charge
The atom with the larger electronegativity value has the _ charge. The atom with the smaller electronegativity value has the _ charge.
partially negative
partially positive
Define permanent dipole
a small charge difference that does not change across a bond, with positive and negative partial charges on the bonded atoms: the result of the bonded atoms have different electronegativities
Depending on the shape of a molecule dipoles may _ or _?
reinforce one another to produce a larger dipole over the whole molecule
cancel out if dipoles act in opposite directions
Define intermolecular force
an attractive force between molecules