Chemical Bonding Mr Sonaji V Gayakwad Asst professor

Chemical Bonding Mr. Sonaji V. Gayakwad Asst. professor Dept of chemistry Mrs. K. S. K. College, Beed

Theories of Covalent Bonding Valence Bond (VB) Theory and Orbital Hybridization The Mode of Orbital Overlap and the Types of Covalent Bonds Molecular Orbital (MO)Theory and Electron Delocalization

Valence Bond Theory • Linus Pauling and others applied the principles of quantum mechanics to molecules • They reasoned that bonds between atoms would occur when the orbitals on those atoms interacted to make a bond • The kind of interaction depends on whether the orbitals align along the axis between the nuclei, or outside the axis

Orbital overlap and spin pairing in three diatomic molecules. Hydrogen, H 2 Hydrogen fluoride, HF Fluorine, F 2

Bond Angles in Carbon Compounds electron configuration = 1 s 22 p 2 2 p orbitals with one electron in each. Can p orbitals with one electron in each find the place where the 3 rd p orbital should be? If they can, the bond angles should be 90 o. Orbitals with one electron in each will overlap to form single bonds. But…the bond angles are 109. 5 o!

• To adjust for these inconsistencies, it was postulated that the valence atomic orbitals could hybridize before bonding took place – one hybridization of C is to mix all the 2 s and 2 p orbitals to get four orbitals that point at the corners of a tetrahedron

Hybrid Orbitals • The number of standard atomic orbitals combined = the number of hybrid orbitals formed – combining a 2 s with a 2 p gives two 2 sp hybrid orbitals – H cannot hybridize!! • its valence shell only has one orbital • The number and type of standard atomic orbitals combined determines the shape of the hybrid orbitals • The particular kind of hybridization that occurs is the one that yields the lowest overall energy for the molecule

Carbon Hybridizations Unhybridized 2 p 2 s sp hybridized 2 sp 2 p sp 2 hybridized 2 sp 2 sp 3 hybridized 2 sp 3 2 p

sp 3 Hybridization • Atom with four electron groups around it – tetrahedral geometry – 109. 5° angles between hybrid orbitals • Atom uses hybrid orbitals for all bonds and lone pairs

Bonding with Valence Bond Theory • According to valence bond theory, bonding takes place between atoms when their atomic or hybrid orbitals interact – “overlap” • To interact, the orbitals must either be aligned along the axis between the atoms, or • The orbitals must be parallel to each other and perpendicular to the interatomic axis

Methane Formation with sp 3 C

Ammonia Formation with 3 sp N

Orbital Diagrams of Bonding • “Overlap” between a hybrid orbital on one atom with a hybrid or nonhybridized orbital on another atom results in a s bond • “Overlap” between unhybridized p orbitals on bonded atoms results in a p bond

CH 3 NH 2 Orbital Diagram s s 1 s H s s s C s 1 s H s s sp 3 s s 1 s H sp 3 N

Formaldehyde, CH 2 O Orbital Diagram p p. C s s C sp 2 1 s H s p. O sp 2 O

The sp 2 hybrid orbitals in BF 3.

Hybrid orbitals overlap to form a s bond. Unhybridized p orbitals overlap to form a p bond.

HCN Orbital Diagram p. C s sp C 1 s H 2 p s p. N sp N

3 sp d • Atom with five electron groups around it – trigonal bipyramid electron geometry – Seesaw, T–Shape, Linear – 120° & 90° bond angles • Use empty d orbitals from valence shell • d orbitals can be used to make p bonds

The conceptual steps from molecular formula to the hybrid orbitals used in bonding. Step 1 Molecular formula Step 2 Lewis structure Molecular shape and e- group arrangement Step 3 Hybrid orbitals

Molecular Orbital Theory • In MO theory, we apply Schrödinger’s wave equation to the molecule to calculate a set of molecular orbitals – in practice, the equation solution is estimated – we start with good guesses from our experience as to what the orbital should look like – then test and tweak the estimate until the energy of the orbital is minimized • In this treatment, the electrons belong to the whole molecule – so the orbitals belong to the whole molecule – delocalization