Chemical Bonding And Molecular Structure CBSE Questions & Answers

Chemical Bonding And Molecular Structure

This is Chemistry Class 11 Chemical Bonding and Molecular Structure CBSE Questions & Answers. There are 15 questions in this test with each question having around four answer choices.

Questions & Answers

1
Structures of \({\text{CO}}_3^{2 - }\). ion given below explains the phenomenon of in terms of
Question 1 figure 1
  • A
    dipole moment
  • B
    isomerism
  • C
    resonance
    Correct
  • D
    isoelectronic ionic character
2
The product of the magnitude of the charge and the distance between the centres of positive and negative charge.
  • A
    ionic character
  • B
    Dipole moment
    Correct
  • C
    electronegativity
  • D
    covalent character
3
the valence shell electron pair repulsion (vsepr) theory helps in the
  • A
    prediction of geometrical shapes of molecules
    Correct
  • B
    electronic configurations of atoms
  • C
    ionic formation of molecules
  • D
    prediction of lewis structure of molecules
4
In the formation of hydrogen molecule, overlapping of atomic orbitals which results in the pairing of electrons. These are:
  • A
    valence shell electrons with opposite spins.
    Correct
  • B
    valence shell electrons with same spins
  • C
    lone pair of electons
  • D
    valence shell electrons irrespective of the spins
5
In ${\text{NO}}_3^ - $ ion, the number of bond pairs and lone pairs of electrons on nitrogen atom are
  • A
    3, 1
  • B
    1, 3
  • C
    2, 2
  • D
    3, 0
    Correct
6
in case of a heteronuclear molecule like HF, the shared electron pair between the two atoms gets displaced more towards fluorine since the electronegativity of fluorine is far greater than that of hydrogen. This results in the molecule a
  • A
    Lewis structure
  • B
    dipole moment
    Correct
  • C
    resonance hybrid
  • D
    resonance
7
Elements in which apart from 3s and 3p orbitals, 3d orbitals also available for bonding In a number of compounds of these elements there are more than eight valence electrons around the central atom. One such example is
  • A
    HCl
  • B
    \({{\text{H}}_{\text{2}}}{\text{O}}\)
  • C
    \({\text{HN}}{{\text{O}}_{\text{3}}}\)
  • D
    \({{\text{H}}_{\text{2}}}{\text{S}}{{\text{O}}_{\text{4}}}\)
    Correct
8
The shift in electron density is symbolised by crossed arrow in the below diagram. It depicts
Question 8 figure 1
  • A
    dipole moment
    Correct
  • B
    Lewis structure
  • C
    resonance hybrid
  • D
    resonance
9
In \({\text{B}}{{\text{F}}_{\text{3}}}\), molecule below the dipole moment is zero although the B- F bonds are oriented at an angle of \({\text{12}}{0^0}\) to one another. Net dipole moment in \({\text{B}}{{\text{F}}_{\text{3}}}\), molecule is
Question 9 figure 1
  • A
    one
  • B
    zero
    Correct
  • C
    two
  • D
    three
10
The shape of the below molecule is
Question 10 figure 1
  • A
    see saw
  • B
    trigonal
  • C
    bent
    Correct
  • D
    rigonal planar
11
Polarity in a molecule and hence the dipole moment depends primarily on electronegativity of the constituent atoms and shape of a molecule. Which of the following has the highest dipole moment?
  • A
    $SO_2$
  • B
    $CO_2$
  • C
    HI
  • D
    $H_2O$
    Correct
12
Ionic crystalline compounds formed by ion-formation by electron transfer proves
  • A
    Molecular Orbital (MO) Theory
  • B
    Valence Bond (VB) Theory
  • C
    Valence Shell Electron Pair Repulsion VSEPR Theory
  • D
    electronic theory of chemical bonding
    Correct
13
The tetrahedral molecule below where there are two lone pairs of electrons is
Question 13 figure 1
  • A
    \({\text{B}}{{\text{F}}_{\text{3}}}\)
  • B
    \({\text{S}}{{\text{O}}_{\text{2}}}\)
  • C
    \({{\text{O}}_{\text{3}}}\)
  • D
    \({{\text{H}}_{\text{2}}}{\text{O}}\)
    Correct
14
The criterion of overlap of atomic orbitals is the main factor for the formation of :
  • A
    coordinate bonds
  • B
    electrovalent bonds
  • C
    ionic bonds
  • D
    covalent bonds
    Correct
15
Octet of electrons, represents a particularly stable electronic arrangement. Atoms achieve the stable octet when they are linked by chemical bonds. This rule is associated with one of the following theories
  • A
    Valence Shell Electron Pair Repulsion VSEPR Theory
  • B
    Lewis approach
    Correct
  • C
    Valence Bond (VB) Theory
  • D
    Molecular Orbital (MO) Theory