From Lewis To Shape And Polarity

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  • 1/11 Questions
      Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options - ProProfs

      Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options

    • The molecular shape is bent, with an angle of 105 between bonds
    • The molecular shape is linear with an angle of 180 between bonds
    • The molecular shape is trigonal planar with an angle of 120
    • The molecular shape is tetrahedral with an angle of 109.5
    • The bond between C and H is polar
    • The bonds between C and H is non-polar
    • The molecule is symetrical
    • The molecule is non-symetrical
    • The molecule is polar
    • The molecule is non-polar
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From Lewis To Shape And Polarity - Quiz
About This Quiz

Explore molecular geometry, bond angles, polarity, and symmetry in this quiz. Assess your understanding of how molecular shapes influence chemical properties and behaviors, enhancing your grasp of fundamental chemistry concepts.

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  • 2. 
    Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options - ProProfs

    Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options

    • The molecular shape is bent, with an angle of 105 between bonds

    • The molecular shape is linear with an angle of 180 between bonds

    • The molecular shape is trigonal planar with an angle of 120

    • The molecular shape is bent with an angle of 120

    • The bonds are polar

    • The bonds are non-polar

    • The molecule is symetrical

    • The molecule is non-symetrical

    • The molecule is polar

    • The molecule is non-polar

    Correct Answer(s)
    A. The molecular shape is linear with an angle of 180 between bonds
    A. The bonds are polar
    A. The molecule is symetrical
    A. The molecule is non-polar
    Explanation
    The given answer states that the molecular shape is linear with an angle of 180 between bonds. This means that the molecule is arranged in a straight line, and the bond angle between the atoms is 180 degrees. Additionally, the answer states that the bonds are polar, indicating that there is an uneven distribution of electron density in the bonds. However, it also states that the molecule is symmetrical, which means that the arrangement of atoms is balanced and there is no net dipole moment. Therefore, the molecule is non-polar.

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  • 3. 
      Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options - ProProfs

      Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options

    • The molecular shape is bent, with an angle of 105 between bonds

    • The molecular shape is linear with an angle of 180 between bonds

    • The molecular shape is trigonal planar with an angle of 120

    • The molecular shape is bent with an angle of 120

    • The bonds are polar

    • The bonds are non-polar

    • The molecule is symetrical

    • The molecule is non-symetrical

    • The molecule is polar

    • The molecule is non-polar

    Correct Answer(s)
    A. The molecular shape is trigonal planar with an angle of 120
    A. The bonds are polar
    A. The molecule is symetrical
    A. The molecule is non-polar
    Explanation
    The correct answer is that the molecular shape is trigonal planar with an angle of 120, the bonds are polar, the molecule is symmetrical, and the molecule is non-polar. This is because in a trigonal planar shape, the central atom is surrounded by three bonded atoms and there are no lone pairs of electrons. The bond angle in a trigonal planar shape is 120 degrees. The bonds are polar because there is a difference in electronegativity between the atoms involved in the bonds. However, the molecule is symmetrical, which means that the polar bonds cancel out each other's effects, resulting in a non-polar molecule.

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  • 4. 
      Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options - ProProfs

      Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options

    • The molecular shape is bent, with an angle of 105 between bonds

    • The molecular shape is trigonal pyramidal with an angle of 107 between bonds

    • The molecular shape is trigonal planar with an angle of 120

    • The molecular shape is tetrahedral with an angle of 109.5

    • The bonds are polar

    • The bonds are non-polar

    • The molecule is symetrical

    • The molecule is non-symetrical

    • The molecule is polar

    • The molecule is non-polar

    Correct Answer(s)
    A. The molecular shape is tetrahedral with an angle of 109.5
    A. The bonds are polar
    A. The molecule is symetrical
    A. The molecule is non-polar
    Explanation
    The correct answer is the molecular shape is tetrahedral with an angle of 109.5, the bonds are polar, the molecule is symmetrical, and the molecule is non-polar. The tetrahedral shape is determined by the presence of four bonded atoms around the central atom. The bond angle of 109.5 is characteristic of a tetrahedral shape. The bonds are polar because there is a difference in electronegativity between the atoms involved in the bond. However, the molecule is symmetrical, which cancels out the polarity and makes the molecule overall non-polar.

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  • 5. 
      Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options - ProProfs

      Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options

    • The molecular shape is bent, with an angle of 105 between bonds

    • The molecular shape is trigonal pyramidal with an angle of 107 between bonds

    • The molecular shape is trigonal planar with an angle of 120

    • The molecular shape is bent with an angle of 120

    • The bonds are polar

    • The bonds are non-polar

    • The molecule is symetrical

    • The molecule is non-symetrical

    • The molecule is polar

    • The molecule is non-polar

    Correct Answer(s)
    A. The molecular shape is trigonal pyramidal with an angle of 107 between bonds
    A. The bonds are polar
    A. The molecule is non-symetrical
    A. The molecule is polar
    Explanation
    The given answer states that the molecular shape is trigonal pyramidal with an angle of 107 between bonds. This means that the molecule has a central atom bonded to three other atoms and has one lone pair of electrons, resulting in a pyramid-like shape. The answer also states that the bonds are polar, indicating that there is an unequal distribution of electron density between the atoms involved in the bonding. Additionally, the answer states that the molecule is non-symmetrical, meaning that it does not possess a plane of symmetry. Finally, the answer states that the molecule is polar, indicating that it has a net dipole moment due to the presence of polar bonds and an uneven distribution of electron density.

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  • 6. 
      Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options - ProProfs

      Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options

    • The molecular shape is bent, with an angle of 105 between bonds

    • The molecular shape is trigonal pyramidal with an angle of 107 between bonds

    • The molecular shape is trigonal planar with an angle of 120

    • The molecular shape is tetrahedral with an angle of 109.5

    • The bond between C and H is polar

    • The bonds between C and cl is polar

    • The molecule is symetrical

    • The molecule is non-symetrical

    • The molecule is polar

    • The molecule is non-polar

    Correct Answer(s)
    A. The molecular shape is tetrahedral with an angle of 109.5
    A. The bonds between C and cl is polar
    A. The molecule is non-symetrical
    A. The molecule is polar
    Explanation
    The given answer states that the molecular shape is tetrahedral with an angle of 109.5 degrees, which means that the central atom is surrounded by four bonded atoms and has a bond angle of 109.5 degrees. It also states that the bond between C and Cl is polar, indicating that there is an unequal sharing of electrons between these atoms. The answer further states that the molecule is non-symmetrical, meaning that it does not possess symmetry in its structure. Lastly, it mentions that the molecule is polar, indicating that there is an overall dipole moment in the molecule due to the presence of polar bonds.

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  • 7. 
      Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options - ProProfs

      Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options

    • The molecular shape is bent, with an angle of 105 between bonds

    • The molecular shape is linear with an angle of 180 between bonds

    • The molecular shape is trigonal planar with an angle of 120

    • The molecular shape is tetrahedral with an angle of 109.5

    • The bond between Be and H is polar

    • The bonds between Be and H is non-polar

    • The molecule is symetrical

    • The molecule is non-symetrical

    • The molecule is polar

    • The molecule is non-polar

    Correct Answer(s)
    A. The molecular shape is linear with an angle of 180 between bonds
    A. The bond between Be and H is polar
    A. The molecule is symetrical
    A. The molecule is non-polar
    Explanation
    The given answer states that the molecular shape is linear with an angle of 180 degrees between bonds. This means that the molecule is arranged in a straight line, with the two atoms bonded to the central atom in opposite directions. The answer also states that the bond between Be and H is polar, indicating that there is an uneven distribution of electron density in the bond. Additionally, it states that the molecule is symmetrical, meaning that it can be divided into two equal halves that are mirror images of each other. Finally, it states that the molecule is non-polar, suggesting that the overall distribution of charge in the molecule is even.

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  • 8. 
    Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options: - ProProfs

    Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options:

    • The molecular shape is bent, with an angle of 105 between bonds

    • The molecular shape is linear with an angle of 180 between bonds

    • The molecular shape is trigonal planar with an angle of 120

    • The molecular shape is bent with an angle of 120

    • The bonds are polar

    • The bonds are non-polar

    • The molecule is symetrical

    • The molecule is non-symetrical

    • The molecule is polar

    • The molecule is non-polar

    Correct Answer(s)
    A. The molecular shape is bent, with an angle of 105 between bonds
    A. The bonds are polar
    A. The molecule is non-symetrical
    A. The molecule is polar
    Explanation
    The correct answer is that the molecular shape is bent, with an angle of 105 between bonds. This means that the molecule has a bent or V-shape structure. The bonds in the molecule are polar, meaning there is an unequal distribution of electron density between the atoms involved in the bond. The molecule is non-symmetrical, as it does not possess any planes of symmetry. Due to the polar bonds and non-symmetrical structure, the molecule is polar, meaning it has a positive and negative end.

    Rate this question:

  • 9. 
      Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options - ProProfs

      Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options

    • The molecular shape is bent, with an angle of 105 between bonds

    • The molecular shape is trigonal pyramidal with an angle of 107 between bonds

    • The molecular shape is trigonal planar with an angle of 120

    • The molecular shape is tetrahedral with an angle of 109.5

    • The bond between C and H is polar

    • The bonds between C and O is polar

    • The molecule is symetrical

    • The molecule is non-symetrical

    • The molecule is polar

    • The molecule is non-polar

    Correct Answer(s)
    A. The molecular shape is trigonal planar with an angle of 120
    A. The bonds between C and O is polar
    A. The molecule is non-symetrical
    A. The molecule is polar
    Explanation
    The given molecule is described as having a trigonal planar shape with a bond angle of 120 degrees. This means that the central atom is bonded to three other atoms in a flat, triangular arrangement. The bonds between carbon (C) and oxygen (O) are polar, indicating an unequal sharing of electrons between the atoms. The molecule is described as non-symmetrical, meaning that it does not have a plane of symmetry. Lastly, the molecule is described as polar, indicating that there is an overall uneven distribution of charge within the molecule.

    Rate this question:

  • 10. 
      Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options - ProProfs

      Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options

    • The molecular shape is bent, with an angle of 105 between bonds

    • The molecular shape is linear with an angle of 180 between bonds

    • The molecular shape is trigonal planar with an angle of 120

    • The molecular shape is bent with an angle of 120

    • The bonds are polar

    • The bonds are non-polar

    • The molecule is symetrical

    • The molecule is non-symetrical

    • The molecule is polar

    • The molecule is non-polar

    Correct Answer(s)
    A. The molecular shape is trigonal planar with an angle of 120
    A. The bonds are polar
    A. The molecule is symetrical
    A. The molecule is non-polar
    Explanation
    The correct answer is that the molecular shape is trigonal planar with an angle of 120 degrees. This means that the molecule has three atoms bonded to the central atom in a flat, triangular shape. The bonds are polar, indicating that there is an uneven distribution of electron density between the atoms involved in the bond. However, despite the polar bonds, the molecule is symmetrical, resulting in a cancellation of the polarities and making the overall molecule non-polar.

    Rate this question:

  • 11. 
      Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options - ProProfs

      Determine the molecular shape, bond angle, bond polarity, symetry and polarity of this molecule, check the correct options

    • The molecular shape is bent, with an angle of 105 between bonds

    • The molecular shape is trigonal pyramidal with an angle of 107 between bonds

    • The molecular shape is trigonal planar with an angle of 120

    • The molecular shape is tetrahedral with an angle of 109.5

    • The bond between C and O is polar

    • The bonds between C and O is polar

    • The molecule is symetrical

    • The molecule is non-symetrical

    • The molecule is polar

    • The molecule is non-polar

    Correct Answer(s)
    A. The molecular shape is trigonal pyramidal with an angle of 107 between bonds
    A. The bonds between C and O is polar
    A. The molecule is non-symetrical
    A. The molecule is polar
    Explanation
    The given answer states that the molecular shape is trigonal pyramidal with an angle of 107 between bonds. This means that the central atom is bonded to three other atoms and has one lone pair, resulting in a pyramidal shape. The answer also states that the bond between carbon (C) and oxygen (O) is polar, indicating that there is an unequal sharing of electrons between these atoms. Furthermore, it states that the molecule is non-symmetrical, meaning that it does not possess a plane of symmetry. Finally, it states that the molecule is polar, indicating that it has a net dipole moment due to the unequal distribution of charges.

    Rate this question:

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Our quizzes are rigorously reviewed, monitored and continuously updated by our expert board to maintain accuracy, relevance, and timeliness.

  • Current Version
  • Mar 21, 2023
    Quiz Edited by
    ProProfs Editorial Team
  • Nov 11, 2012
    Quiz Created by
    Ssamreth
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