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प्रश्न
Draw an orbital diagram of Hydrogen fluoride molecule
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उत्तर
s-p σ overlap
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संबंधित प्रश्न
BF3 molecule is planar but NH3 pyramidal. Explain.
Arrange the following compounds on the basis of lattice energies in decreasing (descending) order:
BeF2, AlCl3, LiCl, CaCl2, NaCl
What are the interacting forces present during the formation of a molecule of a compound?
Why is O2 molecule paramagnetic?
Assertion: Oxygen molecule is paramagnetic.
Reason: It has two unpaired electron in its bonding molecular orbital.
CaO and NaCl have the same crystal structure and approximately the same radii. If U is the lattice energy of NaCl, the approximate lattice energy of CaO is ______.
Draw the M.O diagram for oxygen molecule calculate its bond order and show that O2 is paramagnetic.
Discuss the formation of N2 molecule using MO Theory.
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Which one of the following sets CORRECTLY represents the increase in the paramagnetic property of the ions?
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Identify the CORRECT option according to MOT.
Of the ions Ti4+, Co2+ and Cr3+, ____________.
According to molecular orbital theory, antibonding molecular orbitals of O2 contain ____________.
According to molecular orbital theory, which of the following will NOT be viable?
Which element among the following does NOT form diatomic molecules?
Which of the following molecules has bond order zero?
The electronic configuration of Be2 molecule according MOT is ______.
Bonding in which of the following diatomic molecule(s) become(s) stronger, on the basis of MO Theory, by removal of an electron?
(A) NO
(B) N2
(C) O2
(D) C2
(E) B2
Choose the most appropriate answer from the options given below:
The correct statement with regard to \[\ce{H^+_2}\] and \[\ce{H^-_2}\] is:
Which element among the following does not form diatomic molecules?
Given below are two statements:
Statement I: A hypothetical diatomic molecule with bond order zero is quite stable.
Statement II: As bond order increases, the bond length increases. In the light of the above statements, chose the most appropriate answer from the options given below:
In \[\ce{O^-2}\], O2, and \[\ce{O^{2-}2}\] molecular species, the total number of antibonding electrons, respectively, are:
