Quiz  /  Hydrogen Bonding Class 9 MCQ Questions With Answers

  • 1. 
    Intermolecular force present in CHF3

  • H bond
  • dipole dipole
  • Wan Der Waals forces
  • ionic

  • 2. 
    The bond created by the electrostatic attraction between metal cations and non-metal anions

  • Hydrogen bonding
  • Covalent bonding
  • Ionic Bonding
  • Dipole-dipole forces
  • Metallic bonding

  • 3. 
    A molecule containing polar covalent bonds is always polar.

  • True
  • False

  • 4. 
    CHECK ALL THAT APPLY:Check all statements that are true of Van der Waals Interactions.

  • Very Weak
  • Brief Interactions
  • Occur when molecules are very close.
  • All of above

  • 5. 
    What is considered a Hydrogen Bond?

  • H-Pb
  • H-Fe
  • H-O
  • All of the above

  • 6. 
    The dominant type of intermolecular attractions between molecules with a hydrogen atom bonded directly to a nitrogen atom

  • Hydrogen bonding
  • Covalent bonding
  • Van Der Waals forces
  • Dipole-dipole forces
  • Ionic bonding

  • 7. 
    The Hydrogen atoms in the molecule shown have this charge:

  • Positive
  • Partial Positive
  • Negative
  • Partial Negative

  • 8. 
    Which of these is not an intermolecular force?

  • covalent bonding
  • hydrogen bonding
  • Van Der Waals forces
  • dipole-dipole forces

  • 9. 
    Which formula represents a nonpolar molecule?

  • HBr
  • H2S
  • CBr4
  • PCl3

  • 10. 
    Which noble gas has the highest boiling point?

  • Xe
  • Kr
  • Ar
  • He

  • 11. 
    Hydrogen Bonds typically occur between atoms of hydrogen involved in this type of bond:

  • Ionic
  • Nonpolar Covalent
  • Polar Covalent
  • Nonpolar AND Polar Covalent

  • 12. 
    Intermolecular forces are the forces

  • within molecules
  • between molecules

  • 13. 
    TRUE OR FALSE:Hydrogen bonds are very strong interactions between two atoms.

  • True
  • False

  • 14. 
    CHECK ALL THAT APPLY:Electronegative atoms that are often involved in Hydrogen Bonds.

  • Nitrogen
  • Fluorine
  • Oxygen
  • All of above

  • 15. 
    All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces. Which of these has ONLY London forces?

  • I2
  • NH3
  • OCl2
  • SH2

  • 16. 
    Intermolecular forces for: NH3

  • Dispersion Force
  • Dipole dipole
  • Hydrogen bonding

  • 17. 
    The bond created when the difference in electronegativity between two atoms is greater than 1.8

  • Hydrogen bond
  • Non-polar covalent bond
  • Ionic bond
  • Polar covalent bond
  • Metallic bond

  • 18. 
    Which of the following molecules, based on the elements present, would be most polar?

  • HF
  • H2
  • HCl
  • HBr

  • 19. 
    Which substance would have the weakest intermolecular forces of attraction?

  • CH4
  • NaCl
  • H2O
  • MgF2

  • 20. 
    What explains the very high melting and boiling point of water

  • Strong dipole-dipole bonds between water molecules
  • Strong hydrogen bonds between water molecules
  • Dispersion forces which are present in all molecules
  • Asymmetrical shape of the polar bonds.

  • 21. 
    Which of the following geometries could be nonpolar?

  • bent
  • tetrahedral
  • trigonal pyrimidal
  • none of the above

  • 22. 
    Intermolecular force present in HCl?

  • dipole dipole
  • Van Der Waals forces
  • H-bond
  • ionic

  • 23. 
    Intermolecular force present in Cl2?

  • dipole dipole
  • H-bond
  • Van Der Waals forces
  • metallic

  • 24. 
    In general, substances with stronger intermolecular forces have ________ boiling points than those with weaker forces

  • Higher
  • Lower
  • The same

  • 25. 
    Determine the type of intermolecular force present in SiO2.

  • dipole dipole
  • Van Der Waals forces
  • ionic
  • covalent network

  • 26. 
    Which is the second strongest intermolecular force, after hydrogen bonding?

  • dipole-dipole attraction
  • Wan Der Waals forces

  • 27. 
    The Oxygen atoms in the molecule shown have this charge:

  • Positive
  • Partial Positive
  • Negative
  • Partial Negative
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