Lewis Structure Practice Problems

Write the appropriate Lewis structures for these free radicals ･CH₃ and ･CH(CH₃)₂.

These two molecules CH₃S(=O)H and CH₃C(=O)H seem to have similar structures. However, the S atom of S=O bond in CH₃S(=O)H adopts a pyramidal geometry, while the C atom of C=O bond in CH₃C(=O)H adopts a planar geometry. Draw the Lewis structures for CH₃S(=O)H and CH₃C(=O)H with the appropriate hybridizations, and explain these observations.

Draw Lewis structures with the appropriate formal charges for these compounds and ions (CH₃)₂O—BCl₃, H₃CNH₃⁺, NaOC(CH₃)₃, and (CH₃)₂C=OH⁺.

Write Lewis structures with the appropriate formal charges for these compounds and ions C₂H₅⁺, C₂H₅⁻, LiBH₄, and KBH₃CN.

Draw Lewis structures for the following molecular formulas: C₂H₄ (one double bond), C₄H₆ (two double bonds), and C₄H₆ (one triple bond). Mark all non-bonding electrons in each structure.

What is the number of valence electrons that Si contributes to Lewis structures?

We are given an incomplete structure and the remaining valence electrons. Complete the Lewis dot structure by connecting atoms with bonds and, if necessary, by adding lone pairs while keeping in mind that each atom must have a full octet.

From the given incomplete structure, illustrate the completed Lewis dot structure by placing bonds between atoms and placing the necessary lone pairs. Keep in mind that each atom must have a full octet.

We are given a framework of the arrangement of atoms in a structure and some of the valence electrons below. Complete the Lewis dot structure by placing bonds between atoms and lone pairs on atoms, if necessary. Keep in mind that each atom must have a full octet.

Draw the Lewis structure of NCl ₄⁺.

Carbenes, one class of reactive intermediates, are neutral species where a carbon bears a lone pair of electrons. Draw the Lewis structure of dimethyl carbene.

For the following compound:
(i) Draw the appropriate Lewis structure.
(ii) Identify the type of orbital used by every carbon to make chemical bonds and estimate the bond angles.

CH₃CN

For the following compound:
(i) Draw the appropriate Lewis structure.
(ii) Identify the type of orbital used by every carbon to make chemical bonds and estimate the bond angles.

HCOOCH₃

Draw three appropriate Lewis structures for the species given below.
C₄H₈O

Draw two appropriate Lewis structures for the species given below.

C₂H₄O

Write the appropriate Lewis structure for the species CsOH.

Draw the Lewis structure of H₃PO₄.

Provide the Lewis structure of the compound CH₄O.

Provide the Lewis structure of the given: NH₄O⁺

Give the Lewis structures and molecular formulas for the following line-angle structures:

(i)

(ii)

Both SF₄ and SF₆ are stable molecules. What are their Lewis structures?

What are the complete Lewis structures for the compounds listed below? (Note: Include the lone pair electrons.)

(i)

(ii)

Provide the complete Lewis structures for the following compounds. (Note: Include the lone pair electrons.)

(i)

(ii)

Give the molecular formulas and draw the Lewis structures corresponding to the following line–angle structures.

Give the molecular formulas and draw the Lewis structures of the following line–angle structures:

Draw the Lewis structures.

(i) diethylamine, CH₃CH₂NHCH₂CH₃

(ii) dimethyl ether, CH₃OCH₃

(iii) 1-bromoethane, CH₃CH₂Br

Illustrate the Lewis structures for the following:

(i) Two compounds with the molecular formula C₅H₁₂

(ii) Two compounds with the molecular formula of C₃H₈O

Draw the plausible Lewis structure of oxirane, a relatively reactive ether, and compare the bond angles of oxirane's carbon (C) atoms to those of acyclic ethers.

Draw the Lewis structure of the given molecule and label the orbitals that overlap to form each bond, including carbon-to-hydrogen bonds and the bond angle around each nonhydrogen atom.

Draw the Lewis structure of the given molecule and label the orbitals that overlap to form each bond and the bond angle around each atom except hydrogen.