Quiz: Take The Ultimate Chemistry Exam Test!

23 Questions | Total Attempts: 214

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Quiz: Take The Ultimate Chemistry Exam Test!

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Questions and Answers
  • 1. 
    Which one of the following is most likely to be an ionic compound?
    • A. 

      CH4

    • B. 

      O2

    • C. 

      CaCl2

    • D. 

      NH3

  • 2. 
    Which of the following compounds has the greatest lattice energy?
    • A. 

      KBr

    • B. 

      KCl

    • C. 

      KI

    • D. 

      KF

  • 3. 
    Based on the tendency of atoms to gain or lose electrons to fulfill the octet rule, which of the following ions has an incorrect charge?
    • A. 

      Na+

    • B. 

      O2-

    • C. 

      Ca2-

    • D. 

      Cl-

  • 4. 
    Which of the following diatomic molecules has the longest bond length?
    • A. 

      N==N

    • B. 

      Br-Br

    • C. 

      F-F

    • D. 

      O==O

  • 5. 
    The measure of an atoms ability to attract electrons towards itself in a chemical bond is known as?
    • A. 

      Electronegativity

    • B. 

      Bond strength

    • C. 

      Electron affinity

    • D. 

      Bond order

  • 6. 
    Which of the following compounds has the greatest bond polarity?
    • A. 

      Cl-Br

    • B. 

      Cl-Cl

    • C. 

      NH3

    • D. 

      H-F

  • 7. 
    Calculate the oxidation number of the nitrogen atom in NH3.
    • A. 

      0

    • B. 

      +1

    • C. 

      -1

    • D. 

      -3

  • 8. 
    Which metal would most likely have the highest melting point?
    • A. 

      Li

    • B. 

      Na

    • C. 

      Ca

    • D. 

      K

  • 9. 
    Which bond type best describes the type of bond that will form between O and H?
    • A. 

      Nonpolar convalent

    • B. 

      Mostly ionic

    • C. 

      Mostly covalent

    • D. 

      Polar covalent

  • 10. 
    Based on your knowledge of bond energy, which of the following compounds would release the most energy during combustion?
    • A. 

      CH4

    • B. 

      C2H6

    • C. 

      C3H8

    • D. 

      C2OH6

  • 11. 
    Use VSEPR theory to predict the geometry of the SF6 molecule.
    • A. 

      T-shaped

    • B. 

      Trigonal bipyramidal

    • C. 

      Tetrahedral

    • D. 

      Octaheadral

  • 12. 
    The bond angles found in a molecule with AX5 geometry are?
    • A. 

      90 degrees

    • B. 

      120 degrees

    • C. 

      90 and 120 degrees

    • D. 

      109.5 degrees

  • 13. 
    Which of the following bonds has the most ionic character
    • A. 

      C-H

    • B. 

      H-F

    • C. 

      Na-I

    • D. 

      K-F

  • 14. 
    What is the CN bond order in H3CCN (assume all atoms obey the octet rule)?
    • A. 

      -1

    • B. 

      +1

    • C. 

      0

    • D. 

      +3

  • 15. 
    What is the formal charge on the nitrogen in hydroxylamine, H2NOH?
    • A. 

      -1

    • B. 

      0

    • C. 

      +1

    • D. 

      +5

  • 16. 
    Which of the following has the smallest bond angles?
    • A. 

      CO2

    • B. 

      NH3

    • C. 

      SO3

    • D. 

      XeF4

  • 17. 
    Which molecule has no dipole moment?
    • A. 

      BrF3

    • B. 

      SO2

    • C. 

      XeBr4

    • D. 

      H2O

  • 18. 
    Which of the following molecules is linear?
    • A. 

      NH3

    • B. 

      H2O

    • C. 

      H2S

    • D. 

      CO2

  • 19. 
    Which of the following statements is true of methane, CH4?
    • A. 

      It is a tetrahedral molecule

    • B. 

      It is a polar molecule

    • C. 

      It contains single and double bonds

    • D. 

      It contains 60% nitrogen by weight

  • 20. 
    Using the bond energies, calculate the enthalpy change for the following combustion reaction.
    • A. 

      -92 kJ/mol

    • B. 

      +921 kJ/mol

    • C. 

      -621 kJ/mol

    • D. 

      +621 kJ/mol

  • 21. 
    In the Lewis structure of nitrogen dioxide, NO2, how many pairs of electrons are bonding and how many are non-bonding?
    • A. 

      5 pairs bonding, 4 pairs non-bonding

    • B. 

      3 pairs bonding, 4 pairs non-bonding

    • C. 

      4 pairs bonding, 4 pairs non-bonding

    • D. 

      2 pairs bonding, 2 pairs non-bonding

  • 22. 
    Indicate the molecular geometry and the net dipole moment of H3CF
    • A. 

      Tetrahedral, AX4; net dipole moment arrow pointing to the right

    • B. 

      Pyramidal; net dipole moment arrow point to the left

    • C. 

      Bent; net dipole moment arrow pointing to the right

    • D. 

      Planar tetrahedral; net dipole moment arrow pointing to the right

  • 23. 
    Briefly explain why Co2 is non-polar and OCS is polar.
    • A. 

      CO2; O==C==O no dipole moment, cancels each out; OCS; O==C==S, contains a dipole moment,does not cancel each out

    • B. 

      CO2 O==C==O contains a dipole moment, does not cancel each other out; OCS O==C==) no dipole moment, cancel each out