1 Chapter 9 Orbitals and Covalent Bonds. 2 Two types of Bonds l Sigma (  ) bonds from overlap of orbitals l They are between the atoms Pi bond (  bond)

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Presentation transcript:

1 Chapter 9 Orbitals and Covalent Bonds

2 Two types of Bonds l Sigma (  ) bonds from overlap of orbitals l They are between the atoms Pi bond (  bond) above and below atoms and l Between adjacent p orbitals. A  bond makes the first and a  bond makes the second bond of a double bond

3 Localized e- model: Summary n Draw the Lewis structure(s) (resonance) n Determine arrangement of e - pairs using the VSEPR model. n Specify hybrid molecular orbitals need to accommodate the e - pairs. n Do the steps in this order! n on.html on.html on.html

4 Summary of sigma & pi bonds Single bond - composed of one  comprised of overlapping orbitals  Single bond - composed of one  comprised of overlapping orbitals  Double bond - composed of one  and one  is between p orbitals)  Double bond - composed of one  and one  is between p orbitals)  Triple bond - composed of one  and two  bonds. Triple bond - composed of one  and two  bonds. n Know this for the online homework!

5 Molecular Orbital Summary n 1. Molecular orbitals are either bonding or antibonding; n 2. Bonding orbitals are lower in energy than corresponding atomic orbitals while antibonding orbitals are higher; n 3. MO theory helps explain paramagnetism & diamagnetism; n 4. MO theory obviates "resonance", replacing it with delocalized pi bonding. s/ch6.htm s/ch6.htm

6 Magnetism n Magnetism has to do with electrons. n Paramagnetism attracted by a magnet. n Associated with unpaired electrons. n Diamagnetism repelled by a magnet. n Associated with paired electrons. n B 2 is diamagnetic.

7 Bond Order n The difference between the number of bonding electrons and the number of antibonding electrons divided by two.

8 Bond Order n The difference between the number of bonding electrons and the number of antibonding electrons divided by two. n E.g., H 2 has 2 bonding electrons (the covalent bond) and 0 antibonding (no other electrons). n B.O. = (2 - 0) ÷ 2 = 1 n H 2 1- ion has 2 bonding + 1 antibonding n B.O. = (2 - 1) ÷ 2 = 1/2 n The non-ion is more stable because it has the higher bond order.

9 Bond Order n Use bond order to explain why He is monoatamic vs. diatomic. n He bond order = (2 - 0) ÷ 2 = 1 n He 2 has 2 bonding and 2 anti-bonding n (2 - 2) ÷ 2 = 0 n So He is monoatomic is more stable because it has the higher bond order. n End of our part of 9.2

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