Valence Bond Theory:
•
A discussion of valence bond theory is based on the knowledge of atomic
orbitals, electronic configuration of elements, overlap criteria of atomic
orbitals and principles of variation and superposition.
•
Orbital Overlap Concept of Covalent Bond: When two atoms approach
each other, partial merger of two bonding orbitals, known as overlapping
of the orbitals occurs.
•
Depending upon the type of overlapping, the covalent bonds may be
divided as sigma (H) bond and Pi (
p ) bond.
•
Sigma (H) bond: This type of covalent bond is formed by the end to end
(hand on) overlapping of bonding orbitals along the inter-nuclear axis.
The overlap is known as head on overlap or axial overlap. The sigma bond
is formed by any one of the following types of combinations of atomic
orbitals. Sigma (H) bond can be formed by
- s overlapping, s - p
overlapping,
p - p Overlapping etc.
•
Pi ( p ) Bond: This type of covalent bond is formed by the sidewise overlap
of the half- filled atomic orbitals of bonding atoms. Such an overlap is
known as sidewise or lateral overlap.
42. Hybridization:
•
In order to explain characteristic geometrical shapes of polyatomic
molecules concept of hybridization is used.
•
The process of intermixing of the orbitals of slightly different energies so
as to redistribute their energies resulting in the formation of new set of
orbitals of equivalent energies and shape.
43. Atomic orbitals used in different types of hybridization.
Shapes of
molecules/ions
It was proposed by PAULING for complexes. To explain metalligand bonding Pauling put forward new assumptions which is known as V B T . According to this theory :- Nature of Metal-ligand bond are purely covalent in nature. Central metal ion contains vaccant (n-1)d,ns,np and nd orbitals. LIgand contains lone pair which is full filled orbital. Central metal ion and ligand over lap to each other and produce metal-ligand bond. Covalent bond inwhich donar and acceptor species are found generally known as co-ordination bond here ligands are known as donar species and centrl metal is acceptor species. in other words metal-ligand bonding are special type of covalant bonding which is known as co-ordinate bond [Mn+ ..L]. Geometry of the complex ion depends upon the types nof overlaping or nature of overlaping. After overlaping of metal ligand- A. if an unpaired e- remains inthis complex then such type of complexea are called paramagnetic in nature. b. if all e- are paired then such complexs are dimagnetic and coloured.
The valence cell theory assumes that each atom in a molecule will achieve a geometry. It minimizes the repulsion between electrons in the valence shell of that atom.
ovalent bonds form by the overlap of the atomic nucleus
what is 1st postulate
limitations of valence bond theory
Pure metals form a metallic bond, in which each atom contributes its valance electron or electrons as the case may be, to the common electron cloud shared by all the atoms of that particular piece of metal.
attachment theory is the bond you make with your mother as a infant. no bond then you find youself unhinged in society. Read "our need for others and its roots in infancy"
In valence bond theory this is how bonds are assumed to form. In MO theory thsi si not the case!.
Molecular orbital theory is more recent than Valence bond theory. Both theories have their adherents and recently VB theory has had a renaissance. They both have their strengths. Chemists use both and mix/match. Some very familiar concepts used every day by chemists spring originally from VB theory, electronegativity, hybridisation of atomic orbitals. MO theory has its advocates, an early triumph was the prediction of the paramagnetism of O2 whereas valence bond theory predicted O2 to be diamagnetic. One criticism of VB theory is that it starts from a description of bonds as localised pairs of electrons, whereas in MO all bonds are potentially delocalised.
covalent bond formed by equal sharing of valance electron while ionic bond forms between donation and accept-ion of valance electron.
metallic bond
A covalent bond in which electrons are shared unequally is polar.The valance electons are shared equally and the bond is nonpolar.
Generally a covalent bond is formed by the sharing of the electrons.
limitations of valence bond theory
An atom is a nucleolus and an associated electron cloud. They bond by swapping OR sharing (valance or outer) electrons.
With a covalent bond, atomic nuclei are sharing some of their valance electrons, which means that the electrons are in orbit around both (or all of) the nuclei in question. With an ionic bond, valance electrons are transferred from one atom to another. Once transferred, the electrons orbit only around the atomic nucleus that has received them.
Pure metals form a metallic bond, in which each atom contributes its valance electron or electrons as the case may be, to the common electron cloud shared by all the atoms of that particular piece of metal.
A. The geometry it will have
octet
A covalent bond forms when the orbitals of two atoms overlap and a pair of electrons occupy the overlap region is called covalent bond theory
Carbon = 4 valance electronsNitrogen = 5 valance electrons4 + 5 = 9 and 2 valance electrons used for the single bond, 9 - 2 = 73 hydrogens can attach to the carbon and 4 hydrogens can attach to the nitrogen, so.......7 hydrogen atoms would complete this molecule===================================