HL Bonding Hybridisation

Hybridization is a model which is used to explain the behavior of atomic orbitals during the formation of covalent bonds. When an atom forms a covalent bond with another atom, the orbitals of the atom become rearranged. This rearrangement results in the "mixing" of orbitals. From:

Hybridisation When atoms join together to form molecules, their atomic orbitals interact with each other to form hybrid orbitals

Hybridisation When atoms join together to form molecules, their atomic orbitals interact with each other to form hybrid orbitals This process is called hybridisation

Hybridisation When atoms join together to form molecules, their atomic orbitals interact with each other to form hybrid orbitals This process is called hybridisation The orbitals formed in this process are of the same energy

Hybridisation When atoms join together to form molecules, their atomic orbitals interact with each other to form hybrid orbitals This process is called hybridisation The orbitals formed in this process are of the same energy The orbitals are symmetrically arranged

Hybridisation When atoms join together to form molecules, their atomic orbitals interact with each other to form hybrid orbitals This process is called hybridisation The orbitals formed in this process are of the same energy The orbitals are symmetrically arranged 3 types - sp 3, sp 2 and sp

Hybridisation When atoms join together to form molecules, their atomic orbitals interact with each other to form hybrid orbitals This process is called hybridisation The orbitals formed in this process are of the same energy The orbitals are symmetrically arranged 3 types - sp 3, sp 2 and sp Hybridisation doesn’t just occur in carbon

sp 3 hybridisation E.g. methane, ammonia, water

sp 3 hybridisation E.g. methane, ammonia, water Methane contains 4 equal C - H bonds, therefore the outer shell electrons (2s 2 2p 2 ) have merged to form 4 hybrid sp 3 orbitals of equal energy

sp 3 hybridisation E.g. methane, ammonia, water Methane contains 4 equal C - H bonds, therefore the outer shell electrons (2s 2 2p 2 ) have merged to form 4 hybrid sp 3 orbitals of equal energy One electron is in each of the hybrid orbitals and can form a sigma bond with a hydrogen atom

sp 3 hybridisation in methane From

sp 3 hybridisation The four hybrid orbitals arrange themselves to be as far apart as possible because of the repulsion between the electrons This produces the tetrahedral shape of methane and a bond angle of 109.5º

sp 3 hybridisation in methane From

sp 3 hybridisation in water A similar thing occurs in water - 4 sp 3 hybridised orbitals are formed around the oxygen and spread out in a tetrahedral shape

sp 3 hybridisation in water A similar thing occurs in water - 4 sp 3 hybridised orbitals are formed around the oxygen and spread out in a tetrahedral shape Two of these orbitals contain lone/non- bonded pairs of electrons, and the other two form sigma bonds with the hydrogen atoms

sp 3 hybridisation in water A similar thing occurs in water - 4 sp 3 hybridised orbitals are formed around the oxygen and spread out in a tetrahedral shape Two of these orbitals contain lone/non- bonded pairs of electrons, and the other two form sigma bonds with the hydrogen atoms As the non-bonded pairs are closer to the centre of the molecule, they force the two O- H bonds slightly closer together forming a bond angle of 105 º

From: sp 3 hybridisation in water

From: sp 3 hybridisation in water

sp 2 hybridisation E.g. ethene - C 2 H 4, BF 3

sp 2 hybridisation E.g. ethene - C 2 H 4, BF 3 In ethene, one 2p orbital from each carbon atom forms a pi bond - this is not involved in hybridisation

sp 2 hybridisation E.g. ethene - C 2 H 4, BF 3 In ethene, one 2p orbital from each carbon atom forms a pi bond - this is not involved in hybridisation The remaining 2s orbital and two 2p orbitals hybridise to form three sp 2 orbitals, which form sigma bonds - two with hydrogen atoms and one between the C atoms

sp 2 hybridisation in ethene From:

Hybridisation in BF 3 From:

sp hybridisation E.g. ethyne (C 2 H 2 ), BeF 2

sp hybridisation E.g. ethyne (C 2 H 2 ), BeF 2 The 2s orbital hybridises with just one of the 2 p orbitals

sp hybridisation E.g. ethyne (C 2 H 2 ), BeF 2 The 2s orbital hybridises with just one of the 2 p orbitals In BeF 2 this is because there are only 2 electrons in the 2nd shell (1s 2 2s 2 )

sp hybridisation E.g. ethyne (C 2 H 2 ), BeF 2 The 2s orbital hybridises with just one of the 2 p orbitals In BeF 2 this is because there are only 2 electrons in the 2nd shell (1s 2 2s 2 ) In ethyne this is because two pi bonds are formed between the carbons leaving only 2 electrons on each carbon to form sigma bonds - one with a H atom and one with the other C atom

sp hybridisation in ethyne From:

sp hybridisation in BeF 2 From:

Question Identify the type of hybridisation in each of the carbon atoms in propene From:

Answer Identify the type of hybridisation in each of the carbon atoms in propene From: sp 3 sp 2