Bonding Shapes Flashcards
2 bonding pairs
Linear
180
3 bonding pairs
Trigonal planar
120
4 bonding pairs
Tetrahedral
109.5
5 bonding pairs
Trigonal bypyrimidal
90 and 120
6 bonding pairs
Octahedral
90
2 bonding pairs one lone pair
V - shape
117.5
3 bonding pairs 1 lone pair
Trigonal bypirimidal
107
4 bonding pairs 1 lone pair
See saw
89 and 119
5 bonding pairs and 1 lone pair
Square byprimid
89
2 bonding pairs 2 lone pairs
V - shape
104.5
3 bonding pairs 2 lone pairs
Trigonal planar
115
4 bonding pairs 2 lone pairs
Square planar
90
Difference in angle between bonding pairs and lone pair
2.5
What repel
Bonding pairs repel more than lone pairs as far apart as possible
3 things to look for in molecules
Type of bonding and type of intermolecular force
3 types of bonding
Ionic
Covelant ( simple molecular and macromolecular which is S c SiO2 )
Metallic
3 types of intermolecular forces
1 . Hydrogen between ONF with H
2. Permanent ( lone pairs )
3. induced ( increased in molecule size increase in elections so stronger induced dipole )
Electronegativity
The ability for an atom to attract a pair of electrons in a covelant bond
Fluorine has most electronegativity so look for molecules closest to F
Talk about polarity
Eg Cl more polar then C
How induced dipole forces arise
Random arrangent of electrons which leads to
Uneven distribution of electrons which leads to
Temporary dipole in one molecule but this
Induces a dipole in another molecule which is oppositely charged
Dipoles attract as opposite charges
How permanent dipole forces arise
Difference in Electronegativity which leads to bond polarity
Dipoles don’t cancel out so therefore an overall dipole occurs which an attraction between delta + and delta - of an molecule
Key points when drawing hydrogen bonding
- Make sure everything is in a straight line
- Make sure lone pairs are on O (2)
- Make sure partial charges are labelled
- Make sure hydrogen bonding dashed line is labelled
