Organic Chemistry Chapter 1 Summary

Pi bonds are...

"dumbbell" shape from sideways interaction of p orbitals

Carbon uses hybrid orbitals to form bonds in organic molecules:

1. In single bonds with tetrahedral geometry, carbon has four sp3 hybrid orbitals 2. In double bonds with planar geometry, carbon uses three equivalent sp2 hybrid orbitals and one unhybridized p orbital 3. Carbon uses two equivalent sp hybrid orbitals to form a triple bond with linear geometry, with two unhybridized p orbitals

Electronic structure of an atom described by wave equation:

Electrons occupy orbitals around the nucleus; Different orbitals have different energy levels and different shapes (s orbitals are spherical, p orbitals are dumbbell-shaped)Co

Atoms such as nitrogen and oxygen hybridize to form strong, oriented bonds:

The nitrogen atom in ammonia and the oxygen atom in water are sp3 -hybridized

Sigma bonds are...

Circular cross-section and are formed by head on interaction

Molecular orbital (MO) theory is...

bonds result from combination of atomic orbitals to give molecular orbitals, which belong to the entire molecule

What is an atom?

charged nucleus containing positively charged protons and netrually charged neutrons surrounded by negatively charged electrons

Covalent Bonds are...

electron pair is shared between atoms

Valence bond theory is...

electron sharing occurs by overlap of two atomic orbitals

What is organic chemistry?

the chemistry of carbon compounds

Draw an electron-dot structure for acetonitrile, C2H3N, which contains a carbon-nitrogen triple bond. How many electrons does the nitrogen atom have in its outer shell ? How many are bonding, and how many are non-bonding?

To address this question, we must realize that the nitrogen will contain 8 electrons in its outer shell. Six will be used in the C-N triple bond (shaded box), and two are non-bonding. H : H:C:C:::N: : H