1. 6.02 Chemical Bonds and Lewis Structure When atoms transfer or share electrons:
Dr. Fred Omega Garces
Chemistry 100
Miramar College
Gilbert N.Lewis ( )
An American chemist, many considered him one of the greatest of all chemists. He laid the foundations of our current understanding of bond formation.

2. Compound classification by electron interactions
The diagram below shows how electrons interact between atoms to form compounds. When electrons are transferred, the compounds are ionic. The class of compounds called salts are in this category. When electrons are shared, covalent bonds are formed and this class of compound are called molecular compounds. When electrons are not evenly shared, the compounds are called polar covalent molecules.
If the electrons from atoms making up the compound are mutually shared, these compounds are called Covalent Compounds.
If the electrons from the atoms making up the compound are transferred between atoms, these compounds are called ionic compounds.
If the electrons are
unequally shared, then these are called polar covalent compounds.

3. Octet Rule Exceptions:
Atoms and ions are most stable when they have complete outer shell filled with e-. (or when they have eight electrons in their valence shell).
Exceptions:
i. (Some compounds can accommodate more than 8 e- )
Elements in third period (especially transition metals)
ii. (Some compounds will not lose or accept e-)
Boron will not form B+3 because a small atom (B) can’t stabilize the concentrate charge, likewise C and Si hardly forms +4 ions.
Carbon, Silicon is not stable by donating or accept electrons. Instead, it is easier for these elements to share electrons.

4. Forming Compounds from Elements
Principle of electrical neutrality allows prediction of formulas of ionic compounds. Na Na +
Force of attraction between ions
lead to ionic bond formation.
[Ne] 3s 1
[Ne] e - Na + Cl -
NaCl Cl Cl -
[Ne] 3s 2 3p 5
[Ne]3s 2 3p 6
Ionic bond forms between Na+ and Cl- due to electrostatic attraction between cation and anion.
LATTICE ENERGY

5. Covalent Compounds Atoms mutually share their electrons
Consider 2 Fluorine combining through e- transfer
The F+ is very unstable and will not sacrifice its e- to satisfy the other F.
The preferred combination is through e- sharing
When electrons are shred by two nonmetals (fluorine), each atom is able to obtain an octet.

6. Covalent Molecules with multiple bonds
Consider two oxygen atoms. Eact oxygen atom has six valence electrons and requires two more valence electrons each to possess eight electrons in its outer most orbital (Octet Rule). By sharing two electrons a piece four electrons are shared between the two oxygen atom. This results in a double bond and each oxygen completing the octet.
Consider 2 oxygen atoms
O O
Consider 2 Nitrogen atoms
The same strategy can be applied to two nitrogen atoms. Three electrons from each nitrogen atom are shared between the two nitrogen atoms resulting in a total of six valence electrons being shared forming a triple bond between the nitrogen atoms.
N N

7. Lewis Dot Formulas of Molecules
All elements in the periodic table possesses valence electron which can be represented by dots. The representation is known as "Lewis Dot Symbol. The Lewis Dot symbol for the selected elements are shown below. The valence electrons for each of these elements correspond to the group number above each family.
VALENCE ELECTRONS

8. Valence electrons: Number of bonds
Non-metallic elements tend to form covalent bonds.
Covalent compounds are formed by nonmetallic elements. In general there is a pattern on how many bonds each element from of family will possess based on its valence electrons. The table below summarizes the number of covalent bonds from certain elements.
In general, these are the number of bonds formed by these atoms.

9. Lewis Structure (Mostly for Molecular Compounds)
Lewis Structure (Mostly for Molecular Compounds) ...according to the Octet Rule
Using the Octet Rule, Molecular Lewis structure can be written. Molecular Lewis Structures are chemical representation showing how valence electrons are arranged in a chemical substance.
When compounds are formed they tend to follow the Octet Rule (OR).
Octet Rule: Atoms will share e- until it is surrounded by eight valence electrons.
Rules of the game-
i) Octet Rule works mostly for second period elements.
Many exceptions especially with 3rd period elements (d-orbitals)
ii) H prefers 2 e-, duet Rule, Only for Hydrogen through Beryllium (At.# 1 – 4)
iii) :C: N: :O: :F:
4 u.p. 3u.p. 2u.p. 1u.p. up = unpaired e-
4 bonds 3 bonds 2 bonds 1 bond
O=C=O N N O = O F - F
iv) H & F are terminal in the structural formula (Never central) . . . . . . . . .

10. Lewis Structure by Periodic Group
Examples of Lewis Structures according to Periodic Group
Calculate Number of Electrons Remaining
Use Remaining Electrons to Achieve Noble Gas Configuration
Total Valence Electrons
Draw Single Bonds
Check Number of Electrons around element
Compound
a) HF = H-F
b) N = N-N
c) NH (1) =
d) CH (1) =
e) CF (7) =
f) NO = N-O
H, 2
F, 8
N,8
H, 2
N, 8
H, 2
C, 8
F, 8
C, 8
N, 8
O, 8

11. Covalent Compound: Lewis Structure
Consider the following chemicals- H C N F O
Formaldehyde
Difluoromoethyne
Nitroglycerine

12. Covalent Compound: Lewis Structure
Consider the following chemicals-
Formaldehyde
Difluoromoethyne
Nitroglycerine

13. Lewis Structure dot structure via inspection
Consider the following carbon dioxide:
O C O Elements/Atomic sequence
Lewis dot symbol
Applying Octet rule
Carbon dioxide Lewis Structure O .. C

14. Lewis Structure by Bond Determination
1. (Connectivity) From the Chemical Formula, determine the atom connectivity for the structure.
i. Given a chemical formula, ABn, A is the central atom and B flanks (surround) the A atom. i.e., NH3, NCl3, NO2. In these examples, N is central in the structure.
ii. H and F are never central atoms.
2. (# of Bond) Determine the number of bonds in the compound, by calculating the theoretical Octet electrons (Oe) minus the total valence electrons (TVe). Oe is the theoretical number of electrons necessary for each atom in the structure to obtain a Noble Gas electron configuration, while TVe is the actual number of total valence electron for each atom in the structure.
3. (Remaining e-) Calculate the number of remaining electrons in the compound by taking the total valence electron (TVe) minus the number of electrons that was used to form bonds. Remaining e- divide by 2 = lone pairs.
Complete Lewis structure by drawing atomic connectivity. Write bonds in the structure and place remaining electrons to selected atoms in the structure to give each atom an octet. Keep in mind that the H-atom is satisfied with 2 electrons (duet).

15. Lewis Dot Structure of CO2 by Bonds Table
A. Calculate Octet electrons (Oe-) and Total Valence electrons to determine number of bonds
B. Calculate the number of bonds in compound structure.
# bonds = (Oe - TVe) 2
bonds = (24- 16) = 8 =
C. Calculate the remaining electrons to add to structure to complete Lewis dot structure.
Remaining e- = TVe - e- used in bonding.
= = 8 e-Remaining
CO Oe TVe
1 C 1•(8)= •(4) = 4
2 O 2•(8)= 16 2•(6)= 12
Chg
Writing Lewis Structure: First determine atom connectivity keeping in mind that H and F can never be central atoms. Generally when given the formula, ABn, A is the central atom in the structure (but not always), and B atoms flank the central atom. Next use information from the above calculations. Total of 16e- in CO2, of which 8 electrons are used to form 4 bonds and 8 remaining electrons are used to complete Lewis structure. .. O C O C O C
1. Write atom connectivity for CO2.
2. Draw the four bonds in the structure.
3. Place the remaining 8 electrons in the structure to complete the Lewis Structure

16. Lewis Dot Structure of SO2 by Bonds Table
A. Calculate (Oe-) and (TVe)
SO2 Oe Tve
1 S 1•(8)= 8 1•(6) = 6
2 O 2•(8)= 16 2•(6)= 12
Writing Lewis Structure:
3. Place the remaining 12 electrons in the structure such that each atom has an octet to complete the Lewis Structure
1. Write atom connectivity for SOs.
2. Draw the four bonds in the structure.

17. Lewis Dot Structure of SO2 by Bonds Table
A. Calculate (Oe-) and (TVe)
B. Number of Bonds.
# bonds = (24- 18) = 6 = 3 bonds
C. Remaining electrons.
Remaining e- = = 12 e- Remaining
SO2 Oe TV e-
1 S 1•(8)= 8 1•(6) = 6
2 O 2•(8)= 16 2•(6)= 12
Bonding Electrons (24- 18) = 6
D. Lone Pairs.
Remaining e- / 2 = 12/2 = 6 LP
Writing Lewis Structure:
3. Place the remaining 12 electrons in the structure such that each atom has an octet to complete the Lewis Structure
1. Write atom connectivity for SOs.
2. Draw the three bonds in the structure. S O S O

18. Lewis Dot Structure of ClO4- by Bonds Table
A. Calculate (Oe-) and (TVe)
B. Number of Bonds.
# bonds = (Oe- TVe) = # bonds 2
# bonds = (40- 32) = 8 = 4 bonds
C. Remaining electrons.
Remaining e- = = 24 e-Remaining
ClO Oe TV e
1 Cl 1•(8)= 8 1•(7) = 7
4 O 4•(8)= 32 4•(6)= 24
Chg [ClO4-] 1
Writing Lewis Structure:
3. Place the remaining 24 electrons in the structure such that each atom has an octet to complete the Lewis Structure
1. Write atom connectivity for ClO4-.
2. Draw the four bonds in the structure. O Cl

19. Lewis Dot Structure of PO3-3 by Bonds Table
A. Calculate (Oe-) and (TVe)
B. Number of Bonds.
# bonds = (Oe- TVe) = # bonds 2
# bonds = (32- 26) = 6 = 3 bonds
C. Remaining electrons.
Remaining e- = = 20 e-Remaining
PO Oe T Ve
1 P 1•(8)= 8 1•(5) = 5
3 O 3•(8)= 24 3•(6)= 18
Chg
Writing Lewis Structure:
3. Place the remaining 20 electrons in the structure such that each atom has an octet to complete the Lewis Structure
1. Write atom connectivity for PO3-3.
2. Draw the three bonds in the structure. 3 O P O P P

20. Lewis Dot Structure of H2PO3- by Bonds Table
A. Calculate (Oe-) and (TVe)
B. Number of Bonds.
# bonds = (Oe- TVe) = # bonds 2
# bonds = (36- 26) = 10 = 5 bonds
C. Remaining electrons.
Remaining e- = = 16 e-Remaining
H2PO Oe Tve
1 P 1•(8)= 8 1•(5) = 5
3 O 3•(8)= 24 3•(6)= 18
2 H •(2)= 4 2•(1)= 2
Chg
Writing Lewis Structure:
3. Place the remaining 16 electrons in the structure such that each atom has an octet to complete the Lewis Structure
1. Write atom connectivity for H2PO3-.
2. Draw the five bonds in the structure. O P O P H H H H

21. Lewis Structures: Examples
i) CH2ClF ii) SiO2
iii) HNO3 iv) SO42- O Si 2-
a) Linear b) bent (trigonal) c) trigonal
d) tetrahedral e) pyramidal f) bent (tetrahedral)

22. Lewis Structures: Examples
i) CH2ClF ii) SiO2
iii) HNO3 iv) SO42- O Si 2-
a) Linear b) bent (trigonal) c) trigonal
d) tetrahedral e) pyramidal f) bent (tetrahedral)

23. Exception to Octet Rule
There are generally three type of exception to the Octet Rule
1. Odd e- : Compounds with odd number of electrons (generally considered radicals which tend to be very reactive)
2. e- deficient : Compounds with a central atom with less than eight electrons in its valence shell. (Usually the central atom is B or Be)
3. Valence shell expansion: Compounds with a central atom with more than eight electrons in its valence shell. (Usually the central atom is in the third, fourth, fifth etc… period)

24. Exception: Valence shell expansion
Some atoms can accommodate more than an octet especially if the central atom is from the 3rd, 4th, ... period. i.e., PCl6, SF4, AsF6-
Modification of Bond Table:
• Determine the total valence electron.
• Determine the minimum # of bonds.
• Determine remaining electrons
Re = (TVe-) - (# e- in bonding)
• Assign remaining electrons to outer most atoms to satisfy octet rule (Except H-atom).
• Assign all remaining electrons to central atom.

25. Summary Compounds, elements coming together:
i) electrons are shared between elements
•if there is mutually sharing, covalent compounds forms
•if there is unequal sharing, polar covalent compounds forms.
ii) electron transfer occurs, ionic compounds forms (next section).
Lewis Structure Determination:
i) Molecular Formula
ii) Atomic Sequence (H and F are terminal)
iii) Determine the # of bonds
Oe- and TVe-
# of Bonds = (Oe - TVe-) / 2
iv) Determine remaining electrons
Re = (TVe-) - (# e- in bonding)
v) Make sure all atoms satisfy octet rule
(Except H which is satisfied with 2 electrons)