Question

Which assumption about the space occupied by nonbonding (lone pair) electron pairs is mpst consistent with the experimental bond angles: do nonbonding pairs occupy more, less, or the same amount of space as bonding pairs?

Plese be thorough and ledgible in your answer

Answer 1

A covalent bond is formed between two atoms when a pair of electrons occupies the space between the atoms. This bonding pair of electrons thus defines a region in which it is most likely to find the electrons. We will refer to such a region as an electron domain. Likewise, a nonbonding pair (or lone pair) of electrons defines an electron domain that is located principally on one atom.

Molecular geometry, the bond lengths and angles, are determined experimentally.  Lewis structures can gives us an approximate measure of molecular bonding.  There is a simple procedure that allows us to predict overall geometry is the VSEPR, Valence Shell Electron Pair Repulsion.  The concept is that valence shell electron pairs are involved in bonding, and that these electron pairs will keep as far away from each other, due to electron-electron repulsion.

Hence, we can say that VSEPR theory is one perfect for the assumption about the space occupied by nonbonding (lone pair) electron pairs is most consistent with the experimental bond angles. The three assumptions done by it regarding the bond angles and distance are

• Lp- lp repulsion is the highest
• Bp - lp repulsion is in between and
• BP- bp repulsion is the lowest

Lp = lone pair of electrons

Bp= bonding pair of electrons

Hence depending on the repulsion the bond angel increases or decreases. If the repulsion is more the bond angel will increase and vice versa. Knowing all of the above we can say that nonbonding pairs occupy more amount of space as bonding pairs.