Draw the structure of chlorine pentafluoride (ClF5) according to the VSEPR theory
The molecule is uncharged, so we can find that chlorine is in its +5 oxidation state. Since there are 5 Cl-F bonds, there are 5 bonding electron pairs around the central Cl atom. We also know that chlorine is in group 7, so it has 7 valence electrons. 5 out of those seven are "tied up" in the Cl-F bonds, thus the remaining two must form a non-bonding electron pair. We have 6 electron pairs (5 bonding and 1 non-bonding) to arrange around the chlorine center - which suggests an octahedral shape. However, since we have one electron pair, the shape of the molecule will be pyramidal.
PS
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