(Polar molecules, Non-polar molecules, etc.)
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Bond angle determines if a molecule has lone pairs because lone pairs have strong repulsive factors that cause it to displace the other atoms, pushing other atoms closer together. This causes the bond angle between the other two atoms to decrease. Therefore, if there is a lone pair for part B, the shape will be bent or v-shaped and no longer linear.
Lone pairs are the reasons for the bond angles being closer together. We learned in class that the lone-lone pair repulsion strength is the greatest, followed by the lone-bonding pairs. We know that bonding pairs want to be as far apart as possible. Thus, the explanation for the bond angles being close together must be the existence of lone pairs.
the bond angle can determine whether an atom can, must, or cannot have lone pairs because the given bond angle in this exercise suggests the number of regions of e- density around the central atom. for part (a), the 120º bond angle means 3 regions of e- density around the central atom but since there are only 2 atoms bonded to the central atom, there must be a lone pair on the central atom as well.
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