Why do you think lone pairs of electrons create greater repulsion when located near other

lone pairs or bonding pairs? Orbitals containing lone pairs of electrons require more space

than orbitals containing bonding pairs. Why do you think this is the case? What does the

presence of one or more lone pairs of electrons do to the bond angles in a molecule (in other

words, do bond angles get larger, smaller, or remain unchanged?)

The shape of molecules depend on the number of electron pairs on the valence shell of the molecules. These electron pairs could be lone pairs or bond pairs. Lone pairs occupy more space around the central atom since it is attracted to only one nucleus compared to bond pairs which are attracted to two nuclei.

When lone pairs are present on the central atom in a molecule, they tend to "squeeze" the molecule thereby decreasing the bond angle in the molecule. Hence, presence of one or more lone pairs of electrons make the bond angles get smaller.

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