1001 Chemical Bonds and Lewis Structurefaculty.sdmiramar.edu/fgarces/zCourse/All_Year/Ch...1 1001...

05.2015 1 1001 Covalent Bonds and Lewis Structure

Dr. Fred Omega Garces Chemistry 152

Miramar College

1001 Chemical Bonds and Lewis Structure When atoms transfer or share electrons:

Gilbert N.Lewis (1875 - 1946)

An American chemist, many considered him one of the greatest of all chemists. He laid the foundations of our current understanding of bond formation.


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.

MoleculesCovalent

IonicCompounds

Polar-Covalent

PurePureSubstancesSubstances

Compounds

•Sharing electrons•non-metals

•transfer electrons•metal + nonmetal

•unequal sharing electrons•metals or non-metals

If the electrons are unequally shared, then these are called polar covalent compounds.


Octet Rule 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).

Many exceptions: i. (Some compounds can accommodate more than 8 e- )

transition metals & 3rd - lower row elements

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.


Forming Compounds from Elements Principle of electrical neutrality allows prediction of formulas of ionic compounds.

Ionic bond forms between Na+ and Cl- due to electrostatic

attraction between cation and anion.

LATTICE ENERGY

Na Na +

[Ne] 3s 1 [Ne] e -

Cl Cl -

[Ne] 3s 2 3p 5 [Ne]3s 2 3p 6

Na + Cl - + NaCl

Force of attraction between ions lead to ionic bond formation.


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.

F

9 p10 n 9 p

10 n

F

9 p10 n

9 p10 n

F + F-

The preferred combination is through e- sharing

F

9 p10 n 9 p

10 n

F

9 p10 n

9 p10 n

F2When electrons are shred by two nonmetals (fluorine), each atom is able to obtain an octet.


Covalent Molecules with multiple bonds

Consider 2 Nitrogen atoms N

7 p7n

7p7 n

N N2

7 p7 n

7p7 n N N

Consider 2 oxygen atoms O

8 p8 n 8 p

8 n

O

8 p8 n

8p8n

O2

O O

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.

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.


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


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.


Using the Octet Rule, molecular Lewis structure can be derived. 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- (electron deficient)

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)

Lewis Structure ...according to the Octet Rule

. . . .

.

. . . .


Lewis Structure by Periodic Group Examples of Lewis Structures according to Periodic Group

Draw Single

Bonds Total

Valence

Electrons

Calculate Number of Electrons

Remaining

Use Remaining Electrons to Achieve

Noble Gas

Configuration Check Number of

Electrons H, 2 F, 8 N,8

N, 8 O, 8

H, 2 N, 8

H, 2 C, 8

F, 8 C, 8

a) HF 1 + 7 = 8 H-F 6

b) N2 5 + 5 = 10 N-N 8 c) NH3 5 + 3(1) = 8 2

d) CH4 4 + 4(1) = 8 0

e) CF4 4 + 4(7) = 32 24

f) NO+ 5 + 6 - 1 = 10 N-O 8

NH H

H

NH H

H

N N

FH

CH H

H

H

CH H

H

H

CF F

F

F

CF F

F

F

N O+

Compound


Consider the following chemicals- H C N F O Formaldehyde

Difluoromoethyne

Nitroglycerine

Covalent Compound: Lewis Structure


Consider the following chemicals- Formaldehyde

Difluoromoethyne

Nitroglycerine

Covalent Compound: Lewis Structure


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

Lewis Structure dot structure via inspection

..

..O C ..

..O

..O C O

......O ..

C

..O .. ..


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 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 the 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).


Lewis Dot Structure of CO2 by Bonds Table

B. Calculate the number of bonds in compound structure.

# bonds = (Oe - TVe) 2

= (24- 16) = 8 = 4 bonds 2 2

C. Calculate the remaining electrons to add to structure to

complete Lewis dot structure.

Remaining e- = TVe - e- used in bonding. = 16 - 8 = 8 e-Remaining

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 .. O C O ..

.. ..

3. Place the remaining 8 electrons in the structure to complete the Lewis Structure

A. Calculate Octet electrons (Oe-) and Total Valence electrons to determine number of bonds

CO2 Oe TVe 1 C 1•(8)= 8 1•(4) = 4 2 O 2•(8)= 16 2•(6)= 12 Chg 24 16

1. Write atom connectivity for CO2.

O C O

2. Draw the four bonds in the structure.


Lewis Dot Structure of SO2 by Bonds Table

Writing Lewis Structure: 3. Place the remaining 12 electrons in the structure such that each atom has an octet to complete the Lewis Structure

A. Calculate (Oe-) and (TVe)

SO2 Oe Tve 1 S 1•(8)= 8 1•(6) = 6 2 O 2•(8)= 16 2•(6)= 12

24 18

1. Write atom connectivity for SOs

.



Lewis Dot Structure of SO2 by Bonds Table

B. Number of Bonds.

# bonds = (24- 18) = 6 = 3 bonds 2 2

C. Remaining electrons.

Remaining e- = 18 - 6 = 12 e-Remaining



SO2 Oe TV e- 1 S 1•(8)= 8 1•(6) = 6 2 O 2•(8)= 16 2•(6)= 12

24 18

1. Write atom connectivity for SOs

.

2. Draw the three bonds in the structure.

S O O S O O S OO

D. Lone Pairs.

Remaining e- / 2 = 12/2 = 6 LP

Bonding Electrons (24- 18) = 6


Lewis Dot Structure of ClO4- by Bonds Table

B. Number of Bonds.

# bonds = (Oe- TVe) = # bonds 2

# bonds = (40- 32) = 8 = 4 bonds 2 2





ClO4- Oe TV e

1 Cl 1•(8)= 8 1•(7) = 7 4 O 4•(8)= 32 4•(6)= 24 Chg 1 40 32

1. Write atom connectivity for ClO4

-.


O

Cl OO

O

O

Cl O O

O

O

Cl OO

O


Lewis Dot Structure of PO3-3 by Bonds Table

B. Number of Bonds.


# bonds = (32- 26) = 6 = 3 bonds 2 2





PO3-3 Oe T Ve

1 P 1•(8)= 8 1•(5) = 5 3 O 3•(8)= 24 3•(6)= 18 Chg 3 32 26

1. Write atom connectivity for PO3

-3. 2. Draw the three bonds in the structure.

O

P O

O

O

Cl OO

O

O

P O

O

P

3


Lewis Dot Structure of H2PO3- by Bonds Table

B. Number of Bonds.


# bonds = (36- 26) = 10 = 5 bonds 2 2





H2PO3- Oe Tve

1 P 1•(8)= 8 1•(5) = 5 3 O 3•(8)= 24 3•(6)= 18 2 H 2•(2)= 4 2•(1)= 2 Chg 1 36 26

1. Write atom connectivity for H2PO3

-. 2. Draw the five bonds in the structure.

O

P O

O

O

P O

O H

H H

H :

:O P

O

O

H

H


Lewis Structures: Examples Example

i) CH2ClF ii) SiO2 iii) HNO3 iv) SO4

2-

H C F

Cl

H

O Si O

H

N OOO O S O

O

O 2-

a) Linear b) bent (trigonal) c) trigonal

d) tetrahedral e) pyramidal f) bent (tetrahedral)


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)

N O N O

B

F

F F

PF

F

FFF


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.


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)

1001 Chemical Bonds and Lewis Structurefaculty.sdmiramar.edu/fgarces/zCourse/All_Year/Ch...1 1001...

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