Problem 4. Consider these M iagrams for HE and HI. Note that the orbitals for the...

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Problem 4. Consider these MỌ điagrams for HE and HI. Note that the orbitals for the lone pairs on the the dtoms are omitted. Therefore, you see only ! valence electron shown for the fluorine atom and the iodine atom instead of 7 valence electrons for the F and the I atoms. Antibonding MO Anibonding MO 15p E H 1s H 1s F 2p Bonding MO Bonding MO H-F: Hi: a) Why does it make sense that the fluorine 2p atomic orbital is at a lower energy than the iodine Sp atomic orbital? Explain your answer. b) Draw a picture of the bonding MO of HF. How many nodes are there in this MO? C) The H-I bond is weaker (casier to break) than the H-F bond. Explain this observation, with refercnce to lhe MO diagans alaown al die top of this page. Problem 4. Consider these MỌ điagrams for HE and HI. Note that the orbitals for the lone pairs on the the dtoms are omitted. Therefore, you see only ! valence electron shown for the fluorine atom and the iodine atom instead of 7 valence electrons for the F and the I atoms. Antibonding MO Anibonding MO 15p E H 1s H 1s F 2p Bonding MO Bonding MO H-F: Hi: a) Why does it make sense that the fluorine 2p atomic orbital is at a lower energy than the iodine Sp atomic orbital? Explain your answer. b) Draw a picture of the bonding MO of HF. How many nodes are there in this MO? C) The H-I bond is weaker (casier to break) than the H-F bond. Explain this observation, with refercnce to lhe MO diagans alaown al die top of this page.

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4a The 2p orbital F is lower of that energy han F is more electronegative thus nucle... View the full answer