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04/14 Chemical Bonding and Molecular Structure Quiz Online Quiz Questions

Use this free practice quiz with 20 questions to review 04/14 Chemical Bonding and Molecular Structure, test your knowledge, and prepare for your next test or exam.

20 questions
01
Choose one
1 point

Which formula represents the simplest electrically neutral ratio of magnesium ions, Mg2+, to chloride ions, Cl−?

  1. A

    MgCl

  2. B

    MgCl2

  3. C

    Mg2Cl

  4. D

    Mg2Cl2

02
True or false
1 point

A Lewis structure by itself shows the actual three-dimensional shape of a molecule.

  1. A

    True

  2. B

    False

03
Choose one
1 point

What is the molecular geometry of NH3 according to VSEPR theory?

  1. A

    Linear

  2. B

    Trigonal planar

  3. C

    Trigonal pyramidal

  4. D

    Tetrahedral

04
Choose one
1 point

Which molecule is polar overall because its polar bond dipoles do not cancel as a result of its molecular geometry?

  1. A

    CO2

  2. B

    CCl4

  3. C

    H2O

  4. D

    BF3

05
Choose one
1 point

A species has 6 electrons in bonding molecular orbitals and 2 electrons in antibonding molecular orbitals. What bond order does molecular orbital theory predict?

  1. A

    0

  2. B

    1

  3. C

    2

  4. D

    4

06
Choose all
1 point

Select all statements that correctly compare ionic and molecular bonding.

  1. A

    Ionic compounds commonly form extended crystal lattices.

  2. B

    Molecular compounds are normally made of cations and anions in a crystal lattice.

  3. C

    Molten ionic compounds can conduct electricity because ions can move.

  4. D

    A covalent bond is formed by transferring an electron completely from one atom to another.

07
Fill in the blank
1 point

For nitrate resonance structures, the atoms retain the , while the π electrons and negative charge are over the oxygen atoms.

08
Choose all
1 point

Select all statements that correctly describe resonance structures and their resonance hybrid.

  1. A

    The atomic connectivity remains the same.

  2. B

    The atoms must be rearranged between structures.

  3. C

    Only electrons, such as lone pairs or π electrons, are repositioned.

  4. D

    The total number of electrons changes between structures.

  5. E

    The resonance hybrid is generally more stable than an individual contributing structure.

09
True or false
1 point

A solid ionic compound normally conducts electricity because its ions are free to move through the crystal lattice.

  1. A

    True

  2. B

    False

10
True or false
1 point

Molecular orbital theory explains the paramagnetism of O2 by predicting unpaired electrons in separate antibonding π* orbitals.

  1. A

    True

  2. B

    False

11
Written response
1 point

In the important Lewis structure of CO with a C≡O triple bond and one lone pair on each atom, what is the formal charge on carbon?

12
Written response
1 point

In the nitrate ion, three equivalent N–O bonds share one additional pi bond. What is the exact average N–O bond order?

13
Fill in the blank
1 point

In VSEPR theory, a double bond counts as electron region, and NH3 has a electron-domain geometry.

14
Open ended
1 point

For NH4+, determine the total number of valence electrons, describe its Lewis structure, identify its molecular geometry and approximate bond angle, and calculate the formal charge on nitrogen and the total formal charge.

15
Choose one
1 point

Why does molten sodium chloride conduct electricity whereas solid sodium chloride generally does not?

  1. A

    Solid sodium chloride conducts because its ions are fixed in a lattice.

  2. B

    Molten sodium chloride conducts because its ions can move; solid sodium chloride generally does not because its ions are fixed in the crystal lattice.

  3. C

    Molten sodium chloride cannot conduct because its ions have neutralized one another.

  4. D

    Solid sodium chloride conducts because its molecules rotate through the lattice.

16
Choose one
1 point

How many total valence electrons must be represented in a Lewis structure for the nitrate ion, NO3−?

  1. A

    18

  2. B

    23

  3. C

    24

  4. D

    26

17
Written response
1 point

What is the molecular geometry of NH3?

18
Choose one
1 point

In the Lewis structure of CO described in the material, what is the formal charge on the carbon atom?

  1. A

    +1

  2. B

    −1

  3. C

    0

  4. D

    +2

19
Written response
1 point

What term describes alternative Lewis representations that have the same atomic connectivity but different placements of electrons?

20
Choose one
1 point

Why is CO2 nonpolar even though each C=O bond is polar?

  1. A

    CO2 is polar because it contains two polar C=O bonds.

  2. B

    CO2 is polar because carbon is less electronegative than oxygen.

  3. C

    CO2 is nonpolar because its linear bond dipoles cancel.

  4. D

    CO2 is nonpolar because its C=O bonds are nonpolar.