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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
What else can I help you with?
What is the theory of bonding in pure metals?
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.
Is chemical bond due to overlaping of atomic orbitals?
In valence bond theory this is how bonds are assumed to form. In MO theory thsi si not the case!.
What are the limitations of valence bond theory?
Valence bond theory has limitations as it provides a limited view of molecular bonding, especially when applied to complex molecules. It does not easily explain the molecular geometry and properties of molecules accurately as it assumes fixed bond angles and shapes. Additionally, it does not account for molecular orbitals and delocalized bonding in a comprehensive manner.
Why Molecular bond Theory is better than Valence bond theory?
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.
Can an electon be completely taken away from another atom in a convalent bond?
No, the atoms in a covalent bond are shared between atoms and even when the sharing is not equal, polar covalent bonds, it is still sharing and not electron is pulled into another elements valance shell.
What type of bond is it when one atom gains or loses a valance electron from a different atom?
metallic bond
What makes up an atom and how do they bond?
An atom is a nucleolus and an associated electron cloud. They bond by swapping OR sharing (valance or outer) electrons.
What is the theory of bonding in pure metals?
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.
How does a covalent bond compare to an ionic bond?
A covalent bond involves the sharing of electrons between atoms, creating a strong bond. In contrast, an ionic bond involves the transfer of electrons from one atom to another, creating a bond between positively and negatively charged ions. Ionic bonds are typically stronger than covalent bonds.
What is covalent bond theory?
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
What is ionic bonding structure?
Ionic bond is when a non-metal takes the metals valance electrons so both atoms can be balanced. Take NaCl for example. Na has one valance electron and Cl only needs one to get eight. So Cl takes Na's one valance electron...:Cl: Na. See the empty spot for Cl, that where Na's valance electron will go.'
When atoms share valence electrons to form a chemical bond what kind of bond is formed?
Chemical bonds don't form electrons; an element has valance electrons. Covalent bonds are formed when elements share their valance electrons. An element wants to have 8 valance electrons. That is when it is an "happy atom". For example, carbon has has four valance electons, so it typically bonds with hydrogen and oxygen to get those four valance electrons.
What is the electrons involve in chemical bond?
The answer is Valance Electrons. Electrons are negatively charged particles which exist in atoms. See link for more detail.
Chemical bonds have what kind of electrons?
well when chemical bond for them to be stable they have to form a octet where all the valance electrons add up to 8.
Is chemical bond due to overlaping of atomic orbitals?
In valence bond theory this is how bonds are assumed to form. In MO theory thsi si not the case!.
Why does carbon form the basis fo so many different kinds of compounds?
Because it can bond so well with itself. Note that its valance is 4, and that carbon can single, double, triple, or quadruple bond to carbon.
What bond is in carbon monoxide called?
AnswerCarbon have 4 valance electron and oxygen have 6 electronsso Actual electrons = 4+60=10Needed = 16so they share 6 electrons and 3 pairs, so tripple.triple bond
