Quiz  /  Valence Bond Class 10 MCQ Questions With Answers

  • 1. 
    A diatomic molecule like O2 is always_______ because electrons are shared ________.

  • nonpolar; equally
  • polar; equally
  • nonpolar; unequally
  • nonpolar; unequally

  • 2. 
    This is an example of a __________ bond.

  • non-polar covalent
  • polar covalent
  • ionic
  • metallic

  • 3. 
    Electronegativity is a measurement of the ability of a nucleus to...

  • attract bonding electrons
  • attract other nuclei
  • attract elenece in the non-valence energy levels
  • All of above

  • 4. 
    Carbon atom undergo

  • sp hybridization
  • sp2 hybridization
  • sp3 hybridization
  • dsp3 hybridization

  • 5. 
    In covalent bonds, electrons are ___________.

  • transferred
  • gained
  • lost
  • shared

  • 6. 
    If Boron bonds with Hydrogen, a ____________ bond forms.

  • polar covalent
  • nonpolar covalent
  • metallic
  • ionic

  • 7. 
    Which of the following is the correct Lewis structure for water?

  • A
  • B
  • C

  • 8. 
    What is the hybridization of a linear molecule?

  • sp
  • sp2
  • sp3
  • sp3d

  • 9. 
    What is the hybridization of the carbon (C) atoms in this molecule?

  • sp3
  • sp2
  • sp
  • unhybridized

  • 10. 
    Which molecule contains bonds with a GREATER polarity?

  • HCl
  • CCl4

  • 11. 
    What is the hybridization of the Carbon atom indicated by the arrow?

  • sp hybridization
  • sp2 hybridization
  • sp3 hybridization
  • dsp3 hybridization

  • 12. 
    Which molecule contains bonds of GREATER polarity?

  • H2O
  • OF2

  • 13. 
    What is the bond angle for the CH4 molecule?

  • 120°
  • 107°
  • 109.5°
  • 90°

  • 14. 
    The electronegativity difference in the bonds of CH4 (methane) is:

  • 0.4
  • 5.9
  • -0.4
  • 1.7

  • 15. 
    When you are asked to find bond polarity, compare EN values of each bonding atom to the central atom

  • true
  • false

  • 16. 
    Atoms that are sp2 hybridized form ____ pi bond(s).

  • 0
  • 1
  • 2
  • 3
  • 4

  • 17. 
    Partial charges like the ones shown here are called:

  • dipoles
  • deltas
  • ions
  • magnetic poles

  • 18. 
    A π (pi) bond is the result of the

  • overlap of two s orbitals
  • overlap of an s orbital and a p orbital
  • overlap of two p orbitals along their axes
  • sidewise overlap of two parallel p orbitals
  • sidewise overlap of two s orbitals

  • 19. 
    The electronegativity difference in the bonds of CCl4 (carbon tetrachloride) is:

  • 0.4
  • 0.5
  • 9.5
  • 5.5

  • 20. 
    How many electrons are represented by a single straight line in a Lewis structure?

  • 1
  • 2
  • 4
  • 6

  • 21. 
    In a polar covalent bond, electrons are shared ___________.

  • equally
  • unequally
  • between non-metals with similar electronegativities
  • between a metal and a non-metal

  • 22. 
    What is the hybridization of this molecule shown above

  • sp
  • sp2
  • sp3
  • sp4

  • 23. 
    Which molecule will undergo the following hybridization?

  • NH3
  • CH4
  • PCI3
  • SiH4

  • 24. 
    A bond with a partially negative end and a partially positive end is:

  • ionic
  • polar
  • non-polar
  • isometric
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