Chapter 4 Question 17 Part D
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Chapter 4 Question 17 Part D
hy is a hydronium ion supposed to be linear even if it has two lone pairs on the central atom? Why is it also less than 109.5 degrees? Can someone please explain to me it is linear?
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Re: Chapter 4 Question 17 Part D
A hydronium ion, H3O+, is not linear. Because it has four atoms, it must be a more complex shape. There is a lone pair on the central atom, O, which means there are three bonds on the central atom, plus this lone pair. In total, that makes four electron densities for the entire molecule. Molecules with four electron densities adhere to the basic tetrahedral formation, which has bond angles set at 109.5 degrees. However, the lone pair on the Oxygen atom actually pushes the bonds to the H atoms further away from it. This decreases the angle at which the H atoms are bonded to the oxygen. (Keep in mind that lone pairs have highly repulsive forces against covalent bonds). The actual angle between the lone pair on the Oxygen and the H atoms bonded will be more than 109.5 degrees, and this angle is not what is being discussed to the problem or in the solution manual. But understand that the widening of these angles necessarily results in a shortening of the angles between each of the three H atoms.
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