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09 Molecular Geometry and Polarity Online Quiz Questions

Use this free practice quiz with 20 questions to review 09 Molecular Geometry and Polarity, test your knowledge, and prepare for your next test or exam.

20 questions
01
Choose one
1 point

A central atom has three bonded atoms and one lone pair, represented as AX₃E. What is the molecule’s molecular geometry?

  1. A

    Tetrahedral

  2. B

    Trigonal pyramidal

  3. C

    Trigonal planar

  4. D

    Bent

02
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1 point

A central atom has two bonded atoms and one lone pair (AX₂E). Which combination of molecular geometry and typical bond angle best fits this arrangement?

  1. A

    Linear, with an angle of 180°

  2. B

    Trigonal planar, with an angle of 120°

  3. C

    Bent, with an angle usually below 120°

  4. D

    Bent, with an angle usually above 120°

03
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1 point

A Lewis structure shows a central atom with one double bond, one single bond, and one lone pair. How many electron regions surround the central atom, and what is their electron-domain geometry?

  1. A

    Three regions; trigonal planar

  2. B

    Four regions; tetrahedral

  3. C

    Two regions; linear

  4. D

    Five regions; trigonal bipyramidal

04
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1 point

A central atom has four bonding regions and no lone pairs (AX₄). Which molecular geometry and typical bond angle should be predicted?

  1. A

    Trigonal planar; about 120°

  2. B

    Trigonal pyramidal; less than 109.5°

  3. C

    Seesaw; about 90° and 120°

  4. D

    Tetrahedral; about 109.5°

05
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1 point

Which sequence correctly orders electron-pair repulsions from strongest to weakest in VSEPR theory?

  1. A

    Bonding pair–bonding pair > lone pair–bonding pair > lone pair–lone pair

  2. B

    Lone pair–lone pair > lone pair–bonding pair > bonding pair–bonding pair

  3. C

    Lone pair–bonding pair > bonding pair–bonding pair > lone pair–lone pair

  4. D

    All three interactions have equal strength

06
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1 point

A central atom has four bonded atoms and one lone pair (AX₄E), for a total of five electron regions. Which molecular geometry and lone-pair placement are predicted?

  1. A

    T-shaped, with an axial lone pair

  2. B

    Square pyramidal, with a basal lone pair

  3. C

    Seesaw, with an equatorial lone pair

  4. D

    Trigonal pyramidal, with a central lone pair

07
Choose one
1 point

For a central atom with three bonded atoms and two lone pairs (AX₃E₂), which arrangement follows when the lone pairs take the preferred positions in a trigonal-bipyramidal electron arrangement?

  1. A

    T-shaped, with both lone pairs equatorial

  2. B

    Seesaw, with both lone pairs axial

  3. C

    Trigonal planar, with both lone pairs equatorial

  4. D

    Linear, with both lone pairs axial

08
Choose one
1 point

A central atom has five bonded atoms and one lone pair (AX₅E), giving six electron regions. What is its molecular geometry?

  1. A

    Seesaw

  2. B

    T-shaped

  3. C

    Square planar

  4. D

    Square pyramidal

09
Choose one
1 point

A central atom has four bonded atoms and two lone pairs (AX₄E₂). Which molecular geometry and relative placement of the lone pairs are predicted?

  1. A

    Square pyramidal, with adjacent lone pairs

  2. B

    Square planar, with opposite lone pairs

  3. C

    Tetrahedral, with adjacent lone pairs

  4. D

    Trigonal planar, with opposite lone pairs

10
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1 point

Each C=O bond in CO₂ is polar. Given that CO₂ is linear, what conclusion follows about the molecule’s overall polarity?

  1. A

    The molecule is nonpolar because the two C=O dipoles cancel

  2. B

    The molecule is polar because each C=O bond is polar

  3. C

    The molecule is polar because linear molecules cannot have canceling dipoles

  4. D

    The molecule is nonpolar because its C=O bonds are nonpolar

11
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1 point

H₂O has two polar O–H bonds, but its molecular geometry is bent. Which reasoning correctly explains its overall polarity?

  1. A

    The O–H dipoles cancel because the two bonds are identical

  2. B

    The molecule is nonpolar because it has only two bonds

  3. C

    The O–H dipoles do not cancel because the molecule is bent

  4. D

    The molecule is nonpolar because lone pairs are excluded from molecular geometry

12
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1 point

BCl₃ is trigonal planar, while CH₃Cl is tetrahedral. Which explanation correctly accounts for the different molecular polarities of these two molecules?

  1. A

    BCl₃ is polar because trigonal-planar molecules always have a net dipole; CH₃Cl is nonpolar because it is tetrahedral

  2. B

    Both molecules are nonpolar because each has a symmetric electron-domain geometry

  3. C

    Both molecules are polar because each contains polar bonds

  4. D

    BCl₃ is nonpolar because its identical bond dipoles cancel; CH₃Cl is polar because its bond dipoles do not cancel

13
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1 point

A central atom has bonds to two atoms and two lone pairs. Which pair of geometries correctly describes it?

  1. A

    Electron-domain geometry: bent; molecular geometry: tetrahedral

  2. B

    Electron-domain geometry: tetrahedral; molecular geometry: bent

  3. C

    Electron-domain geometry: tetrahedral; molecular geometry: tetrahedral

  4. D

    Electron-domain geometry: trigonal planar; molecular geometry: bent

14
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1 point

A Lewis structure has a central atom double-bonded to one atom, single-bonded to a second atom, and bearing one lone pair. Which choice correctly gives the number of electron regions and both geometries?

  1. A

    Three regions; trigonal planar electron-domain geometry and bent molecular geometry

  2. B

    Four regions; tetrahedral electron-domain geometry and bent molecular geometry

  3. C

    Three regions; trigonal planar electron-domain geometry and trigonal planar molecular geometry

  4. D

    Two regions; linear electron-domain geometry and linear molecular geometry

15
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1 point

Both NH₃ and H₂O have four electron regions around the central atom. Which explanation best accounts for the H–O–H bond angle being smaller than the H–N–H bond angle?

  1. A

    H₂O has fewer electron regions, so its bonds are forced closer together.

  2. B

    NH₃ has more lone pairs, so it experiences greater compression.

  3. C

    H₂O has more lone pairs, whose repulsions compress its bond angle more.

  4. D

    The number of lone pairs is the same, so VSEPR predicts equal bond angles.

16
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1 point

A central atom has four bonded atoms and one lone pair (AAX₄E). Which molecular geometry and lone-pair position are predicted by VSEPR?

  1. A

    Trigonal bipyramidal molecular geometry, with the lone pair axial

  2. B

    Seesaw molecular geometry, with the lone pair equatorial

  3. C

    T-shaped molecular geometry, with the lone pair equatorial

  4. D

    Square pyramidal molecular geometry, with the lone pair axial

17
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1 point

For a central atom with two bonded atoms and three lone pairs (AAX₂E₃), which pair of geometries is predicted?

  1. A

    Trigonal bipyramidal electron-domain geometry and linear molecular geometry

  2. B

    Trigonal bipyramidal electron-domain geometry and T-shaped molecular geometry

  3. C

    Linear electron-domain geometry and linear molecular geometry

  4. D

    Trigonal planar electron-domain geometry and bent molecular geometry

18
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1 point

A central atom has four bonded atoms and two lone pairs (AAX₄E₂). Which combination of electron-domain geometry and molecular geometry is predicted when the lone pairs adopt their preferred positions?

  1. A

    Octahedral electron-domain geometry and square pyramidal molecular geometry

  2. B

    Tetrahedral electron-domain geometry and square planar molecular geometry

  3. C

    Octahedral electron-domain geometry and square planar molecular geometry

  4. D

    Octahedral electron-domain geometry and seesaw molecular geometry

19
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1 point

CO₂ and H₂O both contain polar bonds. Which conclusion correctly accounts for their different molecular shapes and overall polarities?

  1. A

    Both are polar because each contains polar bonds.

  2. B

    Both are nonpolar because each has two bonds to the central atom.

  3. C

    CO₂ is polar and H₂O is nonpolar because only CO₂ has a linear shape.

  4. D

    CO₂ is nonpolar because its dipoles cancel; H₂O is polar because its dipoles do not cancel.

20
Choose one
1 point

BCl₃ is trigonal planar, while CH₃Cl is tetrahedral. Which comparison correctly uses both surrounding-atom identity and bond-dipole cancellation to determine their polarity?

  1. A

    Both molecules are nonpolar because both have symmetric shapes.

  2. B

    BCl₃ is nonpolar because its identical bond dipoles cancel; CH₃Cl is polar because its bond dipoles do not cancel.

  3. C

    BCl₃ is polar because it has polar bonds; CH₃Cl is nonpolar because it is tetrahedral.

  4. D

    Both molecules are polar because each has polar bonds.