Lewis structures are based on the concept that all atoms want filled orbitals. U

Question

Lewis structures are based on the concept that all atoms want filled orbitals. Usually atoms want to duplicate the 8 valence (or outer) electrons of the noble gases. This is commonly called the Octet Rule. This can be done in two ways. One is to exchange (or transfer) electrons, which is done in the formation of ionic bonds. Another is to share electrons in covalent bonds. In this experiment, we will look at shared electrons in covalent bonds.

For each covalent molecule listed on the data sheet, you will:

Step 1: Step 2: Step 3:

Step 4: Step 5:

Step 6: Step 7: Step 8: Step 9:

Step 10:

Count the number of valence (or outer) electrons available for bonding.
For every atom-to-atom connection, make a single bond (a shared electron pair).

Distribute the remaining electrons available first to nonbonded pair positions (a maximum of six nonbonded pair electrons per atom, except H, which cannot have nonbonded pairs).

Identify atoms that need to have an octet but do not yet have one.

Rearrange electrons from nonbonded pairs of adjacent atoms to multiple bonds to satisfy the octet rule on atoms identified in step 4. Count the electrons to make sure that you still have the same number as you started with!

Build the molecule using the molecular model set.

Determine the molecular geometry or shape of the molecule.

Calculate the formal charge of each atom. Adjust Lewis structure if it will help the formal charge.

Analysis. Are the bonds nonpolar or polar covalent? Does the molecule have an overall dipole moment? How many resonance structures can you draw?

Have your instructor check your results before proceeding to the next molecule.

Molecule

Valence .e-

Lewis Structure

Molecular Shape

Formal Charge

Polar. Molecule?

Resonance

CH4

CH2Cl2

CH4O

H2O

H3O+

HF

Molecule

Valence e-

Lewis Structure

Molecular Shape

Formal Charge

Polar Molecule?

Resonance

NH3

N2

C2H6

C2H4

C2H2

C2H2Br2

SO2

Molecule

Valence .e-

Lewis Structure

Molecular Shape

Formal Charge

Polar. Molecule?

Resonance

CH4

CH2Cl2

CH4O

H2O

H3O+

HF

Explanation / Answer

Molecule

Valence .e-

Lewis Structure

Molecular Shape

Formal Charge

Polar. Molecule?

Resonance

CH4

CH2Cl2

CH4O

H2O

H3O+

HF

Molecule

Valence .e-

Lewis Structure

Molecular Shape

Formal Charge

Polar. Molecule?

Resonance

CH4

CH2Cl2

CH4O

H2O

H3O+

HF

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