Chapter 1: Hybridization and Molecular Orbital Theory

What is the definition of hybridization?

It is two OR more atomic orbitals to form SAME number of hybrid orbitals, with SAME shape AND energy

What kind of atoms use hybrid orbitals? And what are these specific hybrid orbitals?

CARBON atoms; they use sp, sp², and sp³

When it comes to triple bonds, how are they formed?

-SIDE BY SIDE overlap of TWO 2p orbitals on ONE carbon

-On the SECOND carbon, TWO 2P orbitals overlap 2p orbitals of FIRST carbon

How many sigma/pi bonds are in a TRIPLE bond?

One sigma bond and two pi bonds

When it comes to ETHYLENE, rotation about the ALKANE bond is restricted. Why?

There is a PI bond; it must be broken first and then reformed

How is hybridization determined?

-count the number of ATOMS and N.B. electrons AROUND atom

-1 group= 1 lone pair/1 sigma bond/1 double bond/1triple bond

What is the hybridization, bond angle, and shape of an atom that does NOT have MULTIPLE bonds?

-sp³ hybridization

-109.5 degrees

-tetrahedral

What is the hybridization, bond angle, and shape of an atom that has ONE double bond?

-sp²

-120 degrees

-trigonal planar

What is the hybridization, bond angle, and shape of an atom with TWO double bonds OR one TRIPLE bond?

-sp hybridization

-180 degrees

-linear

For molecular orbital theory (including hydrogen gas), bonding/antibonding molecular orbitals (with ethylene), refer to the notebook