Topic 2 Flashcards
Dative covalent
-Donation of lone pair
-as the other element is electron deficient/only 6 outer shell electrons
water and carbon dioxide
-oxygen more electronegative than carbon and hydrogen
-leaves a dipole
-carbon dioxide symmetrical so dipoles cancel out
-water has lone pairs and have a v shape
thermal decomposition
-ionic and covalent bond
-strong bonds within ion
-produce co2 and one other product
aluminium chloride and aluminium fluoride
aluminium chloride:
-small molecule
-weak London forces
Aluminium fluoride:
-fluorine more electronegative
-more polar bonds
-giant structure
-more E needed
water and hydrogen fluoride
-More hydrogen bonds in water
-require more E
Solubility of methanol in water
-OH group hydrogen bonds to water
-180 degrees
-strength of that hydrogen bond is greater than bonds between methanol molecules
Solubility of chloroethene with water
-insoluble
-forms London forces and permanent dipole interactions with water
Different solubilities
-insoluble in water as it doesn’t form hydrogen bonds
-soluble in hexane as London forces in both are similar in strength so resultant force is similar
Metallic bonding
-regular lattice of positive cations
-sea of delocalised electrons
-strong electrostatic forces of attraction
-lots of E needed
Factors affecting ionic bond strength
-as the charge of cation increase, stronger attraction-give example
-smaller the radius of cation, stronger attraction
Phosphorus and nitrogen
-phosphorus can expand outer shell to have more than 8 electrons
-nitrogen can only have 8 on outer shell
Bond angle
-lone pair-bond pair is greater than bond pair-bond pair
Phosphorus chloride
both molecule and bond are polar
Existence of ions in ionic bonding
In electron density maps nothing surrounds both cation and anion
water and ice
-lattice
-h bond longer than covalent bond
