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Chemical Bonding and Molecular Structure Test - 5

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Chemical Bonding and Molecular Structure Test - 5
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Weekly Quiz Competition
  • Question 1
    1 / -0

    The product of the magnitude of the charge and the distance between the centres of positive and negative charge is called

    Solution

    A dipole moment is a measurement of the separation of two opposite electrical charges. Dipole moments are a vector quantity. The magnitude is equal to the charge multiplied by the distance between the charges and the direction is from negative charge to positive charge:

    µ=q x r

  • Question 2
    1 / -0

    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?

    Solution

    CO2 is linear, so even though the C−O bonds have individual dipole moments, the overall dipole moment is zero as these cancel out (they point in opposite directions, as shown in the diagram below).
    On the other hand, H2O is "bent", which means that the individual dipole moments of the bond are at an angle to each other and because of Presence of lp on head of O atom in H2O therefore it has max dipole moment.

  • Question 3
    1 / -0
    The octet rule is not valid for which of the following molecules?
  • Question 4
    1 / -0

    In the formation of hydrogen molecule, overlapping of atomic orbitals occur  which results in the pairing of electrons. These are:

    Solution

    overlapping of atomic orbitals having electrons of opposite spin take place in the formation of molecule to cancel the dipole moment.

  • Question 5
    1 / -0
    Which of the following is a correct set of molecule, hybridisation and shape?
  • Question 6
    1 / -0

    the valence shell electron pair repulsion (vsepr) theory helps in the

    Solution

    Valence shell electron pair repulsion (VSEPR) theory is a model used in chemistry to predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms. It is also named the Gillespie-Nyholm theory after its two main developers.

  • Question 7
    1 / -0
    Which of the following elements will combine to form an ionic compound?
  • Question 8
    1 / -0
    Directions: The following question has four choices out of which ONLY ONE is correct.

    Identify the least stable ion.
  • Question 9
    1 / -0
    Directions: The following question has four choices out of which ONLY ONE is correct.

    Which of the following compounds has/have all the atoms with a stable 8-electron inert gas configuration in their outermost shells?
  • Question 10
    1 / -0

    H.O.H bond angle in water is

    Solution

    Due to presence of two lone pairs on O in H2O bond angle reduce to 104.50  from 1090.

  • Question 11
    1 / -0
    Which of the following have similar geometry?
  • Question 12
    1 / -0

    The amount of energy required to break one mole of bonds of a particular type between two atoms in a gaseous state is called

    Solution

    Bond enthalpy, also known as bond energy, is the energy that is needed to break a particular bond in a gaseous compound. The unit that expresses bond enthalpy is kilojoules per mole, or kJ/mol.

  • Question 13
    1 / -0
    If the molecules of HCl were totally polar, the expected value of dipole moment would be 6.12 D (debye), but the experimental value of dipole moment would be 1.03 D. Calculate the percentage ionic character.
  • Question 14
    1 / -0
    Among LiCl, BeCl2, BCl3 and CCl4, the covalent bond character follows the order
  • Question 15
    1 / -0
    Identify the isostructural pair.
  • Question 16
    1 / -0
    The electronegativity difference between N and F is greater than that between N and H; yet the dipole moment of NH3 (1.5 D) is larger than that of NF3 (0.2 D). This is because
  • Question 17
    1 / -0
    Which one of the following has a regular tetrahedral structure?
  • Question 18
    1 / -0

    Bond angle helps us in

    Solution

    Bond angles also contribute to the shape of a molecule. Bond angles are the angles between adjacent lines representing bonds. The bond angle can help differentiate between linear, trigonal planar, tetraheral, trigonal-bipyramidal, and octahedral. The ideal bond angles are the angles that demonstrate the maximum angle where it would minimize repulsion, thus verifying the VSEPR theory.

  • Question 19
    1 / -0

    N2, CO and NO+ are isoelectronic molecules. Their respective bond order is :

    Solution

  • Question 20
    1 / -0

    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

    Solution

    because of slight shifting of electron towards more electronegative element like F in HF brings a small amount of negative charge on F and positive charge on H which results in dipole moment.

  • Question 21
    1 / -0
    Which of the following compounds contains both covalent and ionic bonds?
  • Question 22
    1 / -0
    Which one of the following pairs of molecules will have permanent dipole moment for both members?
  • Question 23
    1 / -0
    Which of the following pairs does CO2 resemble?
  • Question 24
    1 / -0
    Why does BeF2 have zero dipole moment whereas H2O has a positive dipole moment?
  • Question 25
    1 / -0

    For N2, bond order is

    Solution

    Bond order is the number of chemical bonds between a pair of atoms. in diatomic nitrogen N≡N, Triple covalent bond is present in nitrogen so the bond order is 3;

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