Which of the following is incorrect?

Options

A. Boiling points of ethers, such as diethyl ether and structure such as `n-`pentane are about the same.
B. Dimethyl ether `(Me_(2)O)`is highly soluble in water whicle diethyl ether `(Et_(2)O)` is only sparingly soluble.
C. Tetrahydrofuran

is highly soluble in water but diethyl ether `Et_(2)O)` is almost insoluble
D. Tetrahydrofruan and dilhydrofuran are equally soluble in water.

Answer

D

Explanation

The greater the electron density on the oxygen, the stronger is the `H` bond and the more soluble is the ether. In dihydrofuran, some electron density on the oxygen atom is drained away because of extended `pi` bonding with the double. Bond, as shown for the singnificant portion of the molecule:

Thus it is less soluble than tetrahydrofuran.
(3) Because methylene groups of `THF` are tied back by ring system and do not offer hindrance to hydrogen bonding of its oxygen steric hidrance to hydrogen bonding.
(2) Hydrogen bonding between `ET_(2)O` and `H_(2)O` is less efficient due to steric crowding around oxygen of `Et_(2)O` while the hydrogen bonding between `Me_(2)O` is much efficient due to small size of the methyl group.
(1) Because ethers are weakly polar, their intermolecular forces of attraction are about as weak as are those of hydrocarbons. Hence, the `bp's` are about the same: for ether `34.6^(@)C` and for `n-`pentane `36^(@)C`. However, ethers are much more souluble in `H_(2)O` becaruse of `H-`bonding between the oxygen of ethers and `H` of water. Hydrocarbons do not participate in `H-`bonding.