How do you calculate bond order? What are it's uses and how do you find the number of pairs in anti-bonding?
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Answers
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Introduction to Bond Order
The bond order is something that pairs two atoms with their atoms. Furthermore, finding the bond of an atom is not difficult if you know the electron and shell of electrons.
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Bond order is an atomic level phenomenon, in which the elements share their electrons to fill their valance shell. Also, it can bond two or more substance together in a compound.
Bond Order
Calculating Bond Order Method- 1 (to find bond order quickly, 1/2 bond order)
Antibonding Electrons- According to the molecular orbital theory, Bond order is half of the difference between bonding and anti-bonding electrons.
Bond order = Number of the electrons in bonding molecule – Number of the electrons in the anti-bonding molecule(antibonding electrons)/ 2
Furthermore, the higher the bond order the more stable the molecule will become. In addition, the more the electron that enters the orbital the more stable the molecule will become. Besides, each electron that enters the anti-bonding molecule will destabilize the new molecule.
Suppose in the shell of a hydrogen atom can hold 2 electrons but there is only 1 electron. Also, when 2 hydrogen atom come together they share their electrons to complete each other’s y shell.
In this way, two orbital forms and no orbital forced to move to higher orbital. Thus the binding order of the hydrogen atom is
Bond order = Number of the electrons in bonding molecule – Number of the electrons in anti-bonding molecule / 2
Bond Order = 2-0 / 2 = 1
This form the common molecule H2 or hydrogen gas.
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Answer:
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Explanation:
Calculating the bond:
If there are more than two atoms in the molecule, follow these steps to determine the bond order:
1.Draw the Lewis structure.
2.Count the total number of bonds.
3.Count the number of bond groups between individual atoms.
4.Divide the number of bonds between atoms by the total number of bond groups in the molecule.
Number of pairs in antibonding:
In chemical bonding theory, an antibonding orbital is a type of molecular orbital (MO) that weakens the chemical bond between two atoms and helps to raise the energy of the molecule relative to the separated atoms. Such an orbital has one or more nodes in the bonding region between the nuclei. The density of the electrons in the orbital is concentrated outside the bonding region and acts to pull one nucleus away from the other and tends to cause mutual repulsion between the two atoms. This is in contrast to a bonding molecular orbital, which has a lower energy than that of the separate atoms, and is responsible for chemical bonds.
The number of antibonding electron pairs in O2-2 molecular ion on the basic of molecular orbital theory is. Solution : O22 consists of four antibonding electron pair [1sand2s have two antibonding, electron pair and 2px,2py have two antibonding electron pair].
Uses of calculating the bond:
It involves calculating the present value of a bond's expected future coupon payments, or cash flow, and the bond's value upon maturity, or face value. As a bond's par value and interest payments are set, bond valuation helps investors figure out what rate of return would make a bond investment worth the cost.
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