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1. Draw the Lewis structure of water showing all valence electrons with lines for covalent bonds and dots for unshared electrons. Add a box around each hydrogen- bonding donor site and add a circle around any hydrogen- bonding acceptor sites in your structure. (Hint: there are two of each. The equal number of donors and acceptors is why water hydrogen-bonds so well with other waters.) Draw the Lewis structure of hydrofluoric acid, HF, showing all valence electrons with lines for covalent bonds and dots for unshared electrons. Draw a second HF Lewis structure nearby. Show a dashed line connecting a hydrogen-bond acceptor in one molecule with the hydrogen-bond donor in the other molecule. 3. Draw the Lewis structure of formaldehyde, H2CO, showing all valence electrons with lines for covalent bonds and dots for unshared electrons. Add a box around each hydrogen-bonding donor site and add a circle around any hydrogen-bonding acceptor sites in your structure. Explain why pure formaldehyde does not exhibit hydrogen-bonding forces - why one molecule cannot hydrogen bond with another molecule. 4. Draw the Lewis structures of one H CO molecule and one HF molecule. These two can hydrogen bond with each other. Draw a dashed line between your two structures to show a hydrogen-bonding force between the two (acceptor in one and donor in the other).
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