Bonding And Molecular Structure

36 Questions | Total Attempts: 34

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Bonding And Molecular Structure

Questions and Answers
  • 1. 
    VSEPR predicts an , molecule will be which of the following shapes?
    • A. 

      Tetrahedral

    • B. 

      Trigonal Bipyramidal

    • C. 

      Square Pyramid

    • D. 

      Trigonal Planar

  • 2. 
    The shortest bond would be present in which of the following substance?
    • A. 

      I2

    • B. 

      CO

    • C. 

      CCl4

    • D. 

      O2 (2-)

  • 3. 
    Which of the following does not have one or more  bonds?
    • A. 

      H2O

    • B. 

      HNO3

    • C. 

      O2

    • D. 

      N2

  • 4. 
    Which of the following is polar?
    • A. 

      SF4

    • B. 

      XeF4

    • C. 

      CF4

    • D. 

      SbF5

  • 5. 
    Resonance structures are necessary to describe the bonding in which of the following?H2O
    • A. 

      H2O

    • B. 

      ClF3

    • C. 

      HNO3

    • D. 

      CH4

  • 6. 
    An explanation of the equivalent bond lengths of the nitrite ion is:
    • A. 

      Ionic bonds

    • B. 

      Hybrid orbitals

    • C. 

      Resonance structures

    • D. 

      Van der Waals attractions

  • 7. 
    Most organic substances have low melting points. This may be because, in most cases, the intermolecular forces are:
    • A. 

      Ionic bonds

    • B. 

      Hybrid orbitals

    • C. 

      Resonance structures

    • D. 

      Van der Waals attractions

  • 8. 
    Which of the following has more than one unshared pair of valence electrons on the central atom?
    • A. 

      BrF5

    • B. 

      NF3

    • C. 

      IF7

    • D. 

      ClF3

  • 9. 
    • A. 

      Sp3

    • B. 

      Sp3d

    • C. 

      Sp

    • D. 

      Sp2

  • 10. 
    The only substance listed below that contains ionc, sigma, and pi bonds is:
    • A. 

      Na2CO3

    • B. 

      HClO2

    • C. 

      H2O

    • D. 

      NaCl

  • 11. 
    The electron pairs point toard the corners of which geometrical shape for a molecule with spy hybrid orbitals?
    • A. 

      Trigonal planar

    • B. 

      Octahedron

    • C. 

      Trigonal bipyramid

    • D. 

      Trigonal pyramid

  • 12. 
    Regular tetrahedral molecules or ions include which of the following?
    • A. 

      SF4

    • B. 

      NH4+

    • C. 

      XeF4

    • D. 

      ICl4-

  • 13. 
    Which molecule or ion in the following list has the greatest number of unshared electrons around the central atom?
    • A. 

      CF4

    • B. 

      ClF3

    • C. 

      BF3

    • D. 

      NH4+

  • 14. 
    Which of the following molecules is the most polar?
    • A. 

      NH3

    • B. 

      N2

    • C. 

      CH3I

    • D. 

      BF3

  • 15. 
    • A. 

      PH3

    • B. 

      CH4

    • C. 

      H2)

    • D. 

      NO2

  • 16. 
    Which of the following processes involves breaking an ionic bond?
    • A. 

      H2(g) + Cl2(g) --> 2HCl

    • B. 

      2KBr(s) --> 2K(g) + Br2(g)

    • C. 

      Na(s) --> Na(g)

    • D. 

      2C2H6(g) + 7O2 --> 4CO2() + 6H2O(g)

  • 17. 
    Compounds are ___ substances that have a fixed proportion of elements. 
  • 18. 
    ____ react with ____ to form ionic bonds, and ____ react with other ____ to form covalent bonds.
  • 19. 
    Please fill answer below
  • 20. 
    The Lewis electron-dot structure is a way of representing an element and its valence electrons. 
    • A. 

      True

    • B. 

      False

  • 21. 
    Atoms tend to ____, ____, or ____ electrons to achieve the same electronic configuration as the nearest noble gas. 
  • 22. 
    Atoms are generally the least stable when they have a complete octet (eight electrons).
    • A. 

      True

    • B. 

      False

  • 23. 
    Ionic bonds result when a metal loses electrons to form ____ and a nonmetal gains those electrons to form an ____.
  • 24. 
    Ionic bonds can also result from the interaction of polyatomic ions.
    • A. 

      True

    • B. 

      False

  • 25. 
    The attraction of the opposite charges (anions and cations) forms the ____ bonds.
  • 26. 
    In covalent bonding, two atoms ____ one or more electron pairs
  • 27. 
    If the electrons are not shared equally, the bond is a non polar covalent bond, but unequal sharing to its electronegativity. 
    • A. 

      True

    • B. 

      False

  • 28. 
    The element that will have the greatest attraction for a bonding pair electrons is related to its ____. 
  • 29. 
    Electronegativity values increase from ____ to ____ on the periodic table and decrease from ____ to ____.
  • 30. 
    Molecular geometry, the arrangement of atoms in 3D space, cannot be predicted using the VSEPR theory. This theory says the electron pairs around a central atom will not try to get as far as possible from each other to minimize the repulsive forces. 
    • A. 

      True

    • B. 

      False

  • 31. 
    The valence bond theory describes ____ bonding as the overlap of atomic orbitals to form a new kind of orbital, a hybrid orbital.
  • 32. 
    The number of hybrid orbitals is the same as the number of atomic orbitals that were mixed together. 
    • A. 

      True

    • B. 

      False

  • 33. 
    In the valence bond theory, ____ bonds overlap n a line drawn between the two nuclei, while pi bonds result from the overlap of atomic orbitals above and below a line connecting the two atomic nuclei.
  • 34. 
    A double or triple bond is always composed of one sigma bond and the rest pi bonds. 
    • A. 

      True

    • B. 

      False

  • 35. 
    ____ occurs when more than one Lewis structures can be written for a molecule. The actual structure of the molecule is an average of the Lewis resonance structures. 
  • 36. 
    The lower the bond order, the shorter and stronger the bond. 
    • A. 

      True

    • B. 

      False