14.2: Hybridization Flashcards
What is required for the formation of a covalent bond?
Two orbitals with one electron from different atoms are required
What happens with the electron configuration of carbon and bonding?
Carbon forms four covalent bonds, but its e- configuration wouldn’t predict this
How is the ground state electron configuration modified during bonding?
a) An e- is promoted within the atom from the 2s orbital to the vacant 2p orbital
b) The amount of energy put in is compensated by the extra energy released on forming four bonds
c) Unequal atomic orbitals within an atom mix to form new hybrid atomic orbitals, which are degenerate
Definition of hybridization
Mixing of atomic orbitals in a particular atom to produce a new set of orbitals that have characteristics of the original orbitals and are better arranged in space for covalent bonding
How do hybrid orbitals differ from the parent orbitals?
They have different energies, shapes and orientation in space
How to find the hybridization of an atom?
By looking at the Lewis structure
sp3 hybridization (109.5°)
a) Methane contains four equal C-H bonds arranged tetahedrally with bond angles of 109.5.
b) One of the 2s electrons on the C atom is promoted to a 2p orbital and the three 2p orbitals and the one 2s orbital hybridize to form four sp3 hybrid orbitals
sp2 hybridization (120°)
a) In ethene, one of the 2s electrons is promoted to become a 2p e-.
b) Hybridization occurs leaving one unpaired electron in a p orbital.
c) A sigma bond with one carbon and with two hydrogens. A pi bond is formed between p orbitals of carbons
sp1 hybridization (180°)
a) In ethyne, one of the 2s e- is promoted to become a 2p e-
b) Hybridization occurs leaving two unpaired e- in the 2p orbitals on each carbon atom
c) sp hybrid orbital forms one sigma bond between the carbon atoms and one with the hydrogen atoms
d) Two pi bonds between two carbon atoms are formed when the p orbitals combine.
Special consideration
Lone pairs of electrons can also take part in hybridization
