4.4: Lewis Structures and Polyatomic Molecules

Connectivity

Thinking about how atoms and electrons are arranged in a molecule gets harder when there are more than two atoms. Often you need to decide how the atoms are arranged before writing the Lewis structure.

Let's draw the structure for carbonic acid, H₂CO₃. First we need to know which atoms are connected together. That will tell us which atoms are sharing electrons.

We could put one atom in the middle of the structure and arrange all the others around it. That may work sometimes, but often it gives the central atom too many bonds. A second-row atom can't have more than eight electrons in its valence shell. As a result, a carbon can't have more than four bonds, because there is no room for more electrons.

Figure \(\PageIndex{1}\): A carbon atom with a problem: too many valence electrons.

We could try to attach all the atoms in a string. Long strings of atoms like this are not very common. There may be several reasons why this sort of arrangement isn't very stable. First, when we consider formal charge a little later, you will see that placing all the atoms in a row may cause unnecessary charge separation. Second, some atoms such as oxygen are not very stable when bonded to other atoms of the same kind. Repulsion between lone pairs may contribute to this instability. Because carbon often has no lone pairs, it is an exception and it can bond to itself.

Figure \(\PageIndex{2}\): A long string of atoms may still have problems when you start adding in the rest of the electrons.

A proposed structure for carbonic acid: a line of atoms in the order hydrogen-oxygen-carbon-oxygen-oxygen-hydrogen.

Note that when we try to arrange the atoms in either way, we would probably avoid putting a hydrogen in the middle. That's because hydrogen's octet is just two electrons, so it can usually only make one bond. Knowing the number of bonds that other atoms usually form can also be helpful.

Figure \(\PageIndex{3}\): Hydrogen atoms with problems: usually, atoms with lower numbers of valence electrons must be nearer the edge of the molecule.

Two structures for carbonic acid. Left; hydrogen at center, with five bonds to the other atoms. Right: two hydrogens in the interior positions of a chain of atoms.

Valence

Valence is the number of bonds an element usually forms - for example, the valence of carbon is four, nitrogen is three, oxygen is two, fluorine and hydrogen are one. Valence usually corresponds to the number of electrons needed to form an octet. However, there are exceptions: boron would need 5 electrons to form an octet, but since it only has three electrons to share, it can only form three covalent bonds.

Table \(\PageIndex{1}\) Typical valences (number of bonds formed) for several second-row atoms.

Table \(\PageIndex{1}\) Typical valences (number of bonds formed) for several second-row atoms.

atom	B	C	N	O	F
valence	3	4	3	2	1

Keeping valence in mind can help Lewis structures go more easily. In the case of carbonic acid, carbon might go in the middle, since it must form the most bonds to obtain an octet. Also, having two of the oxygens connected to hydrogens as well as to carbon helps them to attain their normal valence as well.

Figure \(\PageIndex{4}\): Knowledge of valence suggests the structure on the right is more likely.

Once the connectivity has been filled in, we have a skeletal structure of the compound. Now we just need to fill in the extra electrons. Six from each oxygen is 18; four from carbon makes 22; one from each hydrogen makes 24 total electrons.

Figure \(\PageIndex{5}\): Adding in the remaining 14 electrons leads to this structure.

The correct structure for carbonic acid. The central carbon has two bonds to an oxygen, and single bonds to two groups consisting of an oxygen and a hydrogen.

Coming up with a Lewis structure requires a number of steps, but it usually follows a familiar pattern.

Figure \(\PageIndex{6}\): A set of instructions for constructing a Lewis structure.

Steps for constructing lewis structures with formaldehyde as an example. Step 1: Connect the atoms. Since carbon has the highest valence of four, try putting it in the middle and attaching other atoms to it. Step 2: Is one connectivity more reasonable? One particular connectivity may be better because it more easily satisfies the valence of a given element. Step 3: Count how many electrons are used and how many are left over. Step 4: Fill in remaining electrons. Step 5: Rearrange electrons to fill octets on each atom.

Exercise \(\PageIndex{1}\)

Use the idea of valence to construct Lewis structures of the following compounds:

a) hydroxylamine, H₃NO b) ethene, C₂H₄ c) ethane, C₂H₆

Answer

Exercise \(\PageIndex{2}\)

Elements in the third row of the periodic table often behave similarly to elements in the second row. Use the idea of valence to construct Lewis structures of the following compounds:

a) PH₃ b) CS₂ c) SiH₄ d) PCl₃

Answer

Sometimes there will be more than one "correct" way to draw a Lewis structure for a given set of atoms. As an example, there are two different structures in nature with the formula C₂H₆O. These compounds, methyl ether and ethanol, are called isomers, meaning they are formed from the same (iso) things (mer).

Figure \(\PageIndex{1}\):

To help distinguish between isomers, formulae are sometimes written with structural abbreviations. Instead of writing C₂H₆O for both these compounds, we would write CH₃OCH₃ for methyl ether, suggesting the first carbon is connected to three hydrogens and an oxygen, the oxygen is connected to the second carbon, and the second carbon is connected to another three hydrogens.

In a similar way, ethanol would be abbreviated as CH₃CH₂OH.

Exercise \(\PageIndex{3}\)

Draw Lewis or Kekule structures for the following compounds:

a) propanol, CH₃CH₂CH₂OH b) acetic acid (or ethanoic acid), CH₃CO₂H

c) methylamine, CH₃NH₂ d) butanal, CH₃CH₂CH₂CHO

Answer

Exercise \(\PageIndex{4}\)

Draw at least two isomers for each of the following formulae:

a) C₃H₆ b) C₄H₁₀ c) C₄H₈ d) C₃H₆O

Answer

Sometimes, the decision about connectivity involves additional factors, other than valence. Here is a more detailed set of instructions:

Steps for Guessing Connectivity

IF the connectivity is not provided and you need to draw a Lewis Structure,

A. The first atom listed in the formula is often in the middle of the structure.

B. Most simple structures, especially for inorganic species, have an atom in the middle with several atoms connected to and branching out from this central one (as opposed to a linear chain of atoms). Thus, choose the middle atom to be

1. The atom in the lowest row of the periodic table (most likely to be able to use d orbitals to form more than 2 bonds as needed for “branching” structures)

2. The atom more in the center of the periodic table (group 4, then 3 or 5, etc) -has highest valence (valence=number of bonds formed)

3. The least EN atom is often in the middle.

C. Many simple structures are symmetric. This is not a law of nature but a simple observation!

X-M-X often favored over X-X-M

D. Oxyacids often have H’s on O’s; for example, HClO₄ has the connectivity H-O-ClO₃. The chlorine is attached to four different oxygen atoms, but one oxygen atom is also attached to a hydrogen.

E. Avoid three and four membered rings--they are not common, especially among inorganic species.

F. Avoid bonds between electronegative atoms (F-F, O-O, O-F, etc) . Such bonds are weak and tend to make molecules unstable, if not non-existent. Obviously the situation cannot be avoided in molecules like O₂, OF₂, F₂, etc.

Exercise \(\PageIndex{5}\)

Provide structures for the following compounds. Remember to think about common valences.

a) NF₃ b) N₂H₄ c) BF₃

d) SiF₄ e) Ge₂H₆ f) SnCl₄

g) ClNO h) AlBr₃ i) HCN

j) S₈ k) P₄ l) P₄O₆

Answer