Quiz  /  Chemical Bonding Molecular Structure Gate & PSU MCQ Questions With...

  • 1. 
    Which of the following molecules has Π bonds?

  • CO2
  • BF3
  • NH3
  • H2O

  • 2. 
    What is the formal charge for each of the Fluorine atoms

  • -1
  • +1
  • 0
  • +2

  • 3. 
    Water, H2O has molar mass 18 gmol-1 and boils at 373K while ethanol, C2H5OH has molar mass 46 gmol-1 and boils at 351K.Which is/are the correct explanation for the above statement?

  • H2O can form more H-bond compare to ethanol.
  • Both molecules are polar molecules with H-bond
  • Ethanol can only form dipole-dipole forces
  • Both A & B

  • 4. 
    Ammonium ion (NH4+) is an example for

  • Covalent compound
  • Ionic compound
  • Coordinate compound
  • Metallic compound

  • 5. 
    What is the formal charge on the bromine atom in this Lewis dot structure?

  • -1
  • +1
  • -2
  • +2

  • 6. 
    Which molecule exhibits resonance?

  • O3
  • BeCl2
  • CO2
  • NF3

  • 7. 
    Do ionic bonds share or transfer electrons?

  • Share
  • Transport

  • 8. 
    The most electronegative atom in the periodic table is:

  • Fluorine
  • Helium
  • Neon
  • Francium

  • 9. 
    If Bromine bonds with Hydrogen, a ____________ bond forms.

  • polar covalent
  • nonpolar covalent
  • metallic
  • ionic

  • 10. 
    What are the formal charges on the boron and nitrogen in the compounds BF3 and NH3?

  • -2 and +2
  • +2 and –2
  • 0 and 0
  • +1 and –1

  • 11. 
    The polarity of a bond between two elements can be best determined by

  • The difference in electronegativity between the elements
  • The difference in first ionization energy between the elements
  • The number of electrons shared in the bond
  • The difference in atomic radius between the elements

  • 12. 
    How many sigma and pi bonds does this have?

  • 1 sigma and 1 pi
  • 2 sigma and 1 pi
  • 1 sigma and 2 pi
  • 2 sigma and 2 pi

  • 13. 
    What is the hybridisation for central atom in IF4-?

  • sp2
  • sp3
  • sp3d
  • sp3d2

  • 14. 
    In chemical compounds, covalent bonds form when

  • the electronegativity difference between two atoms is very large.
  • electrons are completely transferred between two metals.
  • pairs of electrons are shared between two nonmetal atoms.
  • two nonmetal atoms are attracted to each other by opposite charges.

  • 15. 
    Is the following compound ionic or covalent:AlCl3

  • ionic
  • covalent

  • 16. 
    What is the measure of a tetrahedral bond angle?

  • 90 Degrees
  • 109.5 Degrees
  • 120 Degrees
  • 180 Degrees

  • 17. 
    What is the molecular shape of CH3Cl?

  • trigonal pyramidal
  • trigonal bipyramidal
  • tetrahedral
  • not enough information

  • 18. 
    Calculate the Formal Charge for the Oxygen Labeled 1

  • -1
  • +1
  • 0
  • -2

  • 19. 
    Determine the molecular geometry of the given structure.

  • Octahedral
  • Square Pyramidal
  • Trigonal Bipyramidal
  • See Saw

  • 20. 
    Ionic bonds are between...

  • Metal and Non-metal
  • Non-metal and Non-metal
  • Metal and Metal

  • 21. 
    What is the Molecular Geometry of the molecule?

  • Linear
  • Bent, 120o
  • Bent, 109.5o
  • Trigonal Planar

  • 22. 
    Calculate the Formal Charge for the Nitrogen

  • -1
  • +1
  • 0
  • -2

  • 23. 
    Which of these has dispersion forces?

  • I2
  • NH3
  • OCl2
  • SH2

  • 24. 
    The melting point of Aluminium is higher than Sodium because

  • The metallic bonding in aluminium is stronger than that in sodium
  • The atoms in aluminium are packed more closely that the atoms in sodium
  • The atomic size of aluminium is larger than sodium
  • The relative atomic mass of sodium is less than aluminium

  • 25. 
    Classify the following molecule.

  • polar
  • nonpolar

  • 26. 
    The molecule that uses sp3d hybrid orbital on the central atom is

  • BCl3
  • NCl3
  • ICl3
  • PCl3

  • 27. 
    London forces are stronger in heavier atoms or molecules, and weaker in lighter atoms or molecules. Which of these has the strongest London forces?

  • F2
  • Br2
  • I2
  • Cl2
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