Chapter 1

Electronic Structure and Covalent Bonding

Dr. Sujatha KrishnaswamyChemistry Faculty

Chandler Gilbert Community College

What is organic chemistry?

“Organic” – until mid 1800’s referred to compounds from living sources (mineral sources were “inorganic”)

Wöhler in 1828 showed that urea, an organic compound, could be made from a minerals

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Today, organic compounds are those based on carbon structures.

Organic chemistry is a study of their structures and reactions

Includes biological molecules, drugs, solvents, dyes

Does not include metal salts and materials (inorganic)

Does not include materials of large repeating molecules without sequences (polymers)

Atomic Structure

Structure of an atom Positively charged nucleus (very dense, protons and neutrons) and smal

(10-15 m) Negatively charged electrons are in a cloud (10-10 m) around nucleus Neutral neutrons Electrons forms chemical bonds. Atomic number – number of protons in the nucleus Mass number – the sum of protons and neutrons in an atom Isotopes have the same atomic number but different mass number Atomic weight – average weighted mass of all atoms in an element Molecular weight – sum of atomic weights of all atoms in a molecule

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Distribution of Electrons in an Atom Quantum mechanics uses the mathematical equation

of wave motions to characterize the motion of an electron around a nucleus.

Wave functions or orbitals tell us the energy of the electron and the volume of space around the nucleus where an electron is most likely to be found.

The atomic orbital closer to the nucleus has the lowest energy.

Degenerate orbitals have the same energy. Give an example of degenerate orbitals.

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Distribution of Electrons in an Atom

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Electronic Configuration of Carbon

Atomic Number = 6

2p

2s

1s

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Electronic Configuration of Carbon

Atomic Number = 6

2p

2s

1s

Chemical Bonding Theory Van't Hoff and Le Bel proposed that the four

bonds of carbon have specific spatial directions

Atoms surround carbon as corners of a tetrahedron

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The Covalent Bond Some atoms form a chemical bond by sharing pairs of

electrons between them. A covalent bond consists of a pair of electrons shared

between two atoms.

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Polar Covalent Bonds

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Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons.

Bond Polarity

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Which bond is more polar?

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Problem 6

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Dipole Moments Dipole moment () - Net molecular polarity, due to difference in

summed charges

dipole moment (D) = = e x d

(e) : magnitude of the charge on the atom(d) : distance between the two charges

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Absence of Dipole Moments

In symmetrical molecules, the dipole moments of each bond has one in the opposite direction

The effects of the local dipoles cancel each other

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Useful information for writing Lewis structures

Page 13 Problem 13

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Write Lewis structures for -

Ethane, C2H6

Ethene, C2H4

Ethyne, C2H2

Acetic acid, CH3COOH

Ethyl amine, CH3CH2NH2

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Formal Charges

Problem 11

Formal charge observed with common bonding patterns

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sp3 Hybridization in Methane

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sp3 Hybridization in Ethane

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sp2 Hybridization in Ethylene

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sp2 Hybridization in Acetylene

Why cyclopentyne does not exist?

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Problem 28

Problem 29

Bond Lengths and Bond Strengths

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Drawing Organic Structures

Expanded structure Condensed structure Line angle structure

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Problem 14

Problem 18

Draw line angle structures for

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Problem 17