ion has less stable arrangement that
molecule. Explain using molecular orbital theory.
Let's solve this step by step using Molecular Orbital (MO) Theory. --- We are comparing He₂⁺ and H₂ in terms of stability. ### Step 1: Recall Molecular Orbital Theory basics For diatomic molecules: * Molecular orbitals are filled according to the number of electrons. * Bond order formula: $$ __________ ______ ____ _________ ___ ___ ___ _________ ______ ____ ___.
_________ ___ ______ _______ __________.
_______ ________ ___ ____ _______ __________ ______ __________ ___.
_______ ___ _______ __________ ___ ____ _____ ________ ___ _________ _______ ____.
_________ _________ ___ ____ ____ __________ ____.
__________ _____ ________ _______ ___ _______.
__________ ____ ___ ______ ___ _____ _________ ___ ____ ___.
______ _______ ______ __________ __________ ________.
____ _____ _____ __________ ___ __________ ________ _________ ___ ________.
__________ ____ _______ _______ ________ ___ _________ _____.
_________ ______ _______ __________ ______ __________ ________ ________ _____ ______ ________.
_________ ____ ____ _____ __________ ______ __________ ____.
__________ _________ __________ ___ _____ ____ __________ __________ __________.
_____ ___ ______ _____ _______.
_____ _____ _________ _______ __________ _________ _______ __________ _______ ______.
___ ______ ______ ____ ____ ______ ____ _____ ______.
_________ ____ ___ ____ __________.
________ ___ ______ ________ _______ ___ _________ ___ __________ ___.
____ ___ _______ ______ _____.
____ _______ __________ _______ ________ _______ _____ _____ ____ ___.
____ _____ _______ __________ ________ __________ ________.
____ _____ ____ _________ ____ _____ _______ _________ _______ ___.
_______ __________ ________ _________ _______ ___ ________.
_____ ___ _____ ____ _______ ________ ________ ______ _____ _________ _______.
__________ ___ _________ _________ ___ ______.
_________ ______ _______ __________ ____ _______ __________ ___ __________ ___ ________.
________ ______ _______ ________ _____ _______ _____ __________ ______ ___ _________.
____ ___ ___ _________ ____ ____ ______ ___ ___.
_______ ___ ________ __________ ______.
________ _________ _______.
Get Full Answer on WhatsApp
b) What is the essential condition for a molecule to be microwave active? Classify the following molecules as microwave active or microwave inactive and state the reason in each case.
[Hint: is a linear molecule and one of the nitrogen atoms is at the centre.]
a) In the following compound, indicate the type of hybridization of each carbon atom. Also predict the carbon-carbon bond lengths using Table 4.4.
b) Explain, using hybridization theory and diagram, the structure of allene,
b) Explain the need to introduce normalization constant and, complex conjugate of wave function.
a) Draw the enantiomers for 2, 3-dibromopentane. Identify at least one pair of diastereomers among these structures. Can it form meso form? State the reason for your answer.
a) Calculate the ionisation energy of rubidium per atom, if light of wavelength ) Calculate the ionisation energy of rubidium per atom, if light of wavelength 5.84 108 m produces electrons with a speed of
[Hint: Assume that the threshold frequency refers to the frequency corresponding to the ionisation energy.]
a) On the basis of molecular orbital theory, draw the energy pattern fo ion. Comment on the bond order. Is it paramagnetic? Explain.