Molecular orbital theory:
During the bond formation the atomic orbitals of individual atom will combine together to form equal number of molecular orbital. These orbitals are arranged in the order of increasing energy level, while in case of valence bond theory, the individual atomic orbital will directly involve in bond formation.
Bond order:
Bond order of the molecule indicates the number of bonds present between the pair of atoms.
Bond order is the measurement of the bond strength of a molecule.
An increase in the bond order shows the increase in the bond strength and therefore, a stable compound is formed.
Bond order can be calculated by using molecular orbital theory and molecular energy diagram.
Bond energy is defined as the amount of energy required to break all the bonds in one mole of a substance.
Bond length: The average distance between the two bonded atoms, Bond length is inversely proportional to the bond order.
Molecular orbitals:
Linear combinations of atomic orbitals are called molecular orbitals. These molecular orbitals are generally divided into two types:
(i)Bonding orbitals
(ii)Antibonding orbitals
Bond order in terms of molecular orbitals:
If the bond order is high, then the atoms are close to each order, then distance between the atom will be short and bond energy will be high.
General molecular orbital diagram: Valence shell electrons only
(a)
Molecular orbital diagram of molecule was given below, total of electrons in
Molecular orbital diagram of molecule was given below, There total of electrons in
Molecular orbital diagram of molecule was given below,
Total number of electrons in is
Bond order of the given molecules , ,
Since molecule have highest bond order it will have the highest bond energy and shortest bond distance.
(b)
The given molecule here is , the total number of electrons in is 14, molecular orbital diagram for this molecule was given below
The given molecule here is , the total number of electrons in is , molecular orbital diagram for this molecule was given below
Bond order of the given molecules and
The bond order of and was calculated as and , Therefore it was identified that is the molecule with highest bond order and hence it posses the shortest bond distance and highest bond energy.
Ans:Among the given set of molecules , and , the molecule with highest bond order is , so it posses the shortest bond distance and highest bond energy.
Among and , the molecule with highest bond order, shortest bond distance and highest bond energy is .
According to MO theory, which molecule or ion has the highest bond order? Highest bond energy?...
2. Use the MO theory to complete the following table and answer the questions that follow. (6 Pts.) Molecule/ion Bond order Paramagnetic/Diamagnetic N2 N2. N2 A) Which molecule/ion has the longest bond length? B) Which moleculefion has the strongest bond?
Which charge(s) on an O2 ion would give a bond order of 2.5? (consider MO theory) O-1 O +1 O two of these 0 -2 Which of the following species has a trigonal bipyramid structure? O NH3 O IFs O none of these OPCI O 13
Use the drawing of MO energy diagram for CO to predict the bond order. (Use the energy ordering of O2. ) Express your answer using two significant figures.
Use MO theory to determine the bond order and number of unpaired electrons in (a) O2-, (b) O2+, (c) gas phase BN, and (d) NO-. Estimate the bond lengths in O2- and O2+ using the Pauling formula, and the bond length in the O2 molecule (1.21 Å).
Draw the MO energy level diagrams for N2, N2+, and N2- Calculate the bond order for each. Which has the shortest bond? Which is/are paramagnetic? Draw the MO energy level diagram for O2- and calculate its bond order.
Using LCAO-MO theory, what is bond order of C2- (the one minus ion)?
Consider the carbon molecule and the C2+ molecular ion: (a) Give the bond order of each species. If a fraction is needed, use a decimal number. Bond order C2 = Bond order C2+ = (b) Predict which species should be paramagnetic. Is C2 paramagnetic? Is C2+ paramagnetic? (c) Predict which species has the greater bond dissociation energy. The species with the largest bond dissociation energy is: a. C2 b. C2+
Consider the fluorine molecule and the Fa molecular ion: (a) Give the bond order of each species. If a fraction is needed, use a decimal number. Bond order F2 = Bond order F2 = (6) Predict which species should be paramagnetic. Is F2 paramagnetic? Yes Is F2 paramagnetic? No (c) Predict which species has the greater bond dissociation energy. The species with the largest bond dissociation energy is: a a. F2 b. F2
Using the molecular orbital energy ordering for second-row homonuclear diatomic molecules in which the π2p orbitals lie at lower energy than the σ2p, predict the bond order in a molecule or ion with each of the following numbers of total valence electrons.(Use the drawing MO energy diagrams) Will the molecule or ion be diamagnetic or paramagnetic? Part A Determine the bond order in a molecule or ion with 4 valence electrons. Part B Will this molecule or ion be diamagnetic...
44) According to molecular orbital theory, the bond order of He-He in the He2 molecule is 2. 3 4