Quiz  /  Chemical Bonding Molecular Structure Class 11 MCQ Questions With...

  • 1. 
    The geometry of a molecule with 3 bonded pairs of electrons and 0 lone pairs of electrons

  • Tetrahedral
  • Trigonal Planar
  • Bent
  • Trigonal Pyramidal
  • Linear

  • 2. 
    The geometry of a molecule with 2 bonded pairs of electrons and 0 lone pairs of electrons

  • Tetrahedral
  • Trigonal Planar
  • Bent
  • Trigonal Pyramidal
  • Linear

  • 3. 
    Based on the Lewis structure for H2O, the 3D molecular geometry predicted by VSEPR theory would be:

  • linear
  • bent
  • tetrahedral
  • planar

  • 4. 
    Provide the IUPAC name for NH4NO3.

  • ammonium nitrogen trioxide
  • nitrogen hydride nitrate
  • ammonium nitrate
  • ammonium (IV) nitrate

  • 5. 
    The geometry of a molecule with 2 bonded pairs of electrons and 2 lone pairs of electrons

  • Tetrahedral
  • Trigonal Planar
  • Bent
  • Trigonal Pyramidal
  • Linear

  • 6. 
    Which of the following pairs is unlikely to form a compound?

  • K and I
  • Ca and Cl
  • Fe and S
  • Ne and Ar

  • 7. 
    The geometry of a molecule with 4 bonded pairs of electrons and 0 lone pairs of electrons

  • Tetrahedral
  • Trigonal Planar
  • Bent
  • Trigonal Pyramidal
  • Linear

  • 8. 
    When an atom of sodium and an atom of fluorine combine, an ionic bond is formed. Which statement correctly describes the behavior of the valence electron in the ionic bond?

  • An electron from the fluorine atom moves to the sodium atom forming two ions
  • An electron from the sodium atom moves to the fluorine atom forming two ions
  • An electron from the fluorine atom is shared with the sodium atom forming one cation
  • An electron from the sodium atom is shared with the fluorine atom forming one anion

  • 9. 
    Based on the information provided, which of the following correctly identifies bond types?

  • X is ionic, Y is covalent
  • X is ionic, Y is hydrogen
  • X is covalent, Y is ionic
  • X is Hydrogen, Y is covalent

  • 10. 
    The reason that salt crystallines, such as KCl, are held together so well is because the cations are strongly attracted to:

  • neighboring cations
  • protons in the nucleus of the bonding atom
  • delocalized electrons
  • neighboring anions

  • 11. 
    Which of the following is the correct Lewis structure for ammonia?

  • A
  • B
  • C
  • D

  • 12. 
    Which statement best compares the properties of ionic and metallic substances?

  • The bonds of metallic substances are composed of delocalized electrons, the bonds of ionic compounds are composed of transferred electrons
  • The bonds of metallic substances are composed of isolated electrons, the bonds of ionic substances are composed of shared electrons
  • Metallic and ionic substances both have high melting points due to crystalline structure
  • Metallic substances insulate heat and electricity, ionic compounds conduct heat and electricity

  • 13. 
    Which of the following combinations could be described by the "sea of electrons" model?

  • gold-silver alloy
  • gold chloride
  • Cl2
  • NaCl

  • 14. 
    Compare thecarbon bonds in C2H6 and C2H2.

  • The doubles bonds in C2H2 are longer and stronger than the single bonds in C2H6
  • The double bonds in C2H2 are shorter and stronger than the single bonds in C2H6
  • The double bonds in C2H2 are shorter but weaker than the bonds in C2H6
  • Both molecules are nonpolar with identical bonds

  • 15. 
    When an element in group 2A combines with an element in group 5A, they produce a compound. What is the correct bonding ratio between these elements?

  • 2:3
  • 3:2
  • 2:5
  • 5:2

  • 16. 
    The geometry of a molecule with 3 bonded pairs of electrons and 1 lone pair of electrons

  • Tetrahedral
  • Trigonal Planar
  • Bent
  • Trigonal Pyramidal
  • Linear

  • 17. 
    Which of the following compounds is formed by a covalent bond?

  • CoCl2
  • C2H4
  • NaCl
  • NH4NO3

  • 18. 
    How many and what types of bonds form when hydrogen and oxygen combine?

  • 2 single bonds
  • 2 double bonds
  • 1 single bond
  • 1 double bond

  • 19. 
    Which compound will form when aluminum bonds with chlorine?

  • Al3Cl
  • AlCl
  • AlCl3
  • Al7Cl3

  • 20. 
    Two atoms in a molecule have exactly the same electronegativity values. Which of the following best describes the bond that they form and why?

  • an ionic bond forms because electrons will be transferred from one atom to another
  • a nonpolar covalent bond because electrons will be shared between the atoms equally
  • a polar covalent bond because electrons will be shared between the atoms unequally
  • a metallic bond because delocalized electrons will move between the nuclei

  • 21. 
    The geometry of a molecule with 1 bonded pair of electrons and 1 lone pair of electrons

  • Tetrahedral
  • Trigonal Planar
  • Bent
  • Trigonal Pyramidal
  • Linear

  • 22. 
    The geometry of a molecule with 2 bonded pairs of electrons and 1 lone pairs of electrons

  • Tetrahedral
  • Trigonal Planar
  • Bent
  • Trigonal Pyramidal
  • Linear

  • 23. 
    Limestone is a naturally occuring form of calcium carbonate. The correct formula for calcium carbonate is:

  • CaCO3
  • Ca2(CO3)2
  • Ca3CO
  • Ca2CO2

  • 24. 
    The geometry of a molecule with 1 bonded pair of electrons and 2 lone pairs of electrons

  • Tetrahedral
  • Trigonal Planar
  • Bent
  • Trigonal Pyramidal
  • Linear

  • 25. 
    Which of the following statements explains why the bond between hydrogen chloride is polar covalent?

  • Chlorine has a greater atomic mass than hydrogen
  • Chlorine has a greater electronegativity than hydrogen
  • Chlorine has a higher ionization energy than hydrogen
  • Chlorine has a greater number of valence electrons than hydrogen

  • 26. 
    Which of the following statements best explains why atoms bond?

  • atoms combine to make new substances
  • atoms combine to reduce chemical stability
  • atoms bond to change phase from a liquid to a solid
  • atoms bond to achieve chemical stability

  • 27. 
    Under standard conditions, water exists as a liquid, but H2S is a gas. This difference in phase can be explained by:

  • The hydrogen bonding between molecules in water
  • The hydrogen bonding between molecules in H2S
  • The greater molecular mass of H2S
  • The greater atomic radii of H2S

  • 28. 
    The lewis dot structure for a compound is shown. Which element could be represented by element X?

  • Bromine (Br)
  • Sulfur (S)
  • Nitrogen (N)
  • Silicon (Si)
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