Question

During hydrate formation from aqueous solution water can be associated in different forms. Indicate the wrong combination.

(i) Coordinated water-${\left[ {Cr{{\left( {{H_2}O} \right)}_6}} \right]^{3 + }}3C{l^ - }$

(ii) Interstitial water $BaC{l_2}.2{H_2}O$

(iii) Hydrogen bonded water-${\left[ {Cu{{\left( {{H_2}O} \right)}_4}} \right]^{2 + }} + S{O_4}^{2 - }.{H_2}O$

(A) (i)

(B) (ii)

(C) (iii)

(D) None of these.

Answer 1

We know that the intermolecular interactions found in the liquid molecules are weaker than the intramolecular interactions that clutch the atoms jointly within molecules and polyatomic ions. Greater the intermolecular forces are greater and are going to be the melting and boiling point.

The three major sorts of intermolecular interactions are,

1. Dipole-dipole interactions

2. London dispersion forces

3. Hydrogen bonds

Complete step by step answer:

As we know that the coordinated water is water that's a ligand during a metal complex. The metal atom and therefore the water molecules are held together by coordinate bonds.

Therefore, option A is incorrect.

We must remember that the interstitial water is water that's present within the interstitial sites of a space lattice.

Therefore, option B is incorrect.

We must remember that the hydrogen-bonded water is the water that's linked to some other ion by hydrogen bonding.

Therefore, option C is also incorrect.

So, the correct answer is Option D.

Note:

Now we can discuss about the details of intermolecular interactions as,

London Dispersion forces:

As we know, the London dispersion forces are weak interactions because they are the temporary changes in electron density during a molecule. All covalent compounds show London dispersion forces. This force is the only intermolecular force found in nonpolar compounds.

Now we see the details about dipole-dipole interaction as,

Dipole-dipole interactions:

We must remember that dipole–dipole interactions are electrostatic interactions between molecules which have stable dipoles. This interaction is greater than the London forces however it is weaker than ion-ion interaction because only fractional charges are involved. The positive end of a polar molecule will magnetize the negative end of the opposite molecule and influence its position.

Hydrogen bond:

In a molecule, when an atom is connected to a highly electronegative atom, it attracts the shared pair of electrons further so it becomes a somewhat negative end while the reverse end becomes slightly positive. The negative end of the molecule pulls the positive end and as a result, a weak bond is made between them. This bond is named a hydrogen bond.

There are two types of the hydrogen bond. They are,

- Intermolecular hydrogen bond.

- Intramolecular Hydrogen bond.