Notice the numbers on the diagram.

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Presentation transcript:

Notice the numbers on the diagram. How many bonds form between two O atoms in O2? What about N2?

Sigma-bonding and Pi-bonding Understanding single, double, and triple bonds

Sigma (σ) bonding Valence bond theory describes covalent bonds as the result of the overlap of half-filled orbitals. A sigma bond is any covalent bond between two atoms that involves a direct, head-on overlap of orbitals.

Sigma (σ) bonding All covalent bonds involving s orbitals (basically bonds involving H atoms!) are sigma bonds. All covalent bonds involving hybrid orbitals are sigma bonds. p-orbitals can form sigma bonds, but not all bonds involving p-orbitals are sigma. THE FIRST BOND BETWEEN TWO ATOMS IS ALWAYS A SIGMA BOND!

Pi (π) bonding A pi bond is any covalent bond between two atoms that involves the sideways overlap of parallel orbitals. Pi bonds may involve p-orbitals or d-orbitals, but for our course, we will focus on the p-orbitals.

Pi bonding Unhybridized p-orbitals will arrange themselves perpendicular to the plane where sigma bonds are occurring. Remember from math class – two lines perpendicular to the same plane are parallel!

Pi bonding THE SECOND AND THIRD BONDS BETWEEN TWO ATOMS ARE ALWAYS PI BONDS! A double covalent bond (two lines in a Lewis structure) consists of one sigma bond and one pi bond. A triple covalent bond consists of one sigma bond and two pi bonds.