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Chemical Bondin...

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  • Question 1
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    Match list I (Complex ions) with list II (number of unpaired electrons) and select the correct answers:

    List IList II
    A$$[CrF_6]^{4-}$$1One 
    B$$[MnF_6]^{4-}$$2two
    C$$[Fe(CN)_6]^{4-}$$3zero
    D$$[Mn(CN)_6]^{4-}$$4four
    5five

  • Question 2
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    Assertion: In dilute benzene solutions, equimolar addition of $$R_3N$$ and $$HCl$$ produce a substance with a dipole moment. In the same solvent, equimolar addition of $$R_3N$$ and $$SO_3$$ produce a substance having an almost identical dipole moment.
    Reason:($$ N-S$$) bond is a more polar bond.

  • Question 3
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    Consider the given lewis dot structure:
    The formal charges on $$B$$ and $$F$$ are respectively.

  • Question 4
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    Directions For Questions

    In order to explain the shape and geometry of molecules, the valence bond theory was supplemented by the concept of hybridization. This is a hypothetical concept and has been introduced by Pauling and Slater. According to this concept, any number of atomic orbitals of an atom which differ in energy slightly may mix with each other to form new orbitals called hybrid orbitals. The process of mixing or amalgamation of atomic orbitals of nearly same energy to produce a set of entirely new orbitals of equivalent energy is known as hybridization.

    ...view full instructions

    In $$XeF_2$$, $$XeF_4$$ and $$XeF_6$$ the number of lone pairs on Xe is respectively__________.

  • Question 5
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    For the type of interactions:$$(I)$$ Covalent bond, $$(II)$$ van der waal's forces, $$(III)$$ Hydrogen bonding, $$(IV)$$ Dipole-dipole interaction, which represents the correct order of increasing stability?

  • Question 6
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    In which of the following molecules/species, all following characteristics are found?
    (a) Tetrahedral hybridisation.
    (b) Hybridisation can be considered to have taken place with the help of empty orbital(s).
    (c) All bond lengths are identical, i.e., all $$A - B$$ bond lengths are identical.

  • Question 7
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    The formal charges of $$N_{(1)}, N_{(2)}$$ and $$O$$ atoms in $$: \overset {. .}{N_{(1)}} = N_{(2)} = \overset {. .}{O}:$$ are respectively

  • Question 8
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    Which of the following best describes the term dipole moment?

  • Question 9
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    What is a non-bonding electron domain?

  • Question 10
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    Calculate the formal charges on oxygen atoms 1, 2, 3 respectively.

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