Intermolecular forces occur between, rather than within, molecules. Ion – dipole interaction and dip — Physical Chemistry Chemistry Question

Part 1: Ion–Dipole Interactions
The bonding of an ion, such as Na⁺, with a polar molecule, such as water, is an example of an ion–dipole interaction. Shown below are a sodium ion, a water molecule, and a crown ether compound.

8.1 Draw the geometrical structure of the product resulting from the interaction between the sodium ion and water molecules.

8.2 Draw a diagram showing the interaction between the sodium ion and the crown ether molecule.

Part 2: Dipole–Dipole Interactions
A hydrogen bond may be regarded as a particular kind of dipole–dipole interaction. Strong hydrogen bonding forces are seen among molecules in which hydrogen is bound to a highly electronegative atom, such as nitrogen, oxygen, or fluorine.
–O–H+···N–
Compared to other intermolecular forces, hydrogen bonds are relatively strong; their energies are of the order of 15 to 40 kJ mol–1. Hydrogen bonding is so strong that, in some cases, it survives even in a vapor.
8.3 In gaseous hydrogen fluoride, many of the HF molecules are associated into (HF)₆. Draw the structure of this hexamer.

8.4 Draw a diagram showing the hydrogen–bonding interactions between two acetic acid (CH₃CO₂H) molecules.

Part 3: Hydrogen–bonding in Living Matter
Some chemical reactions in living matter involve complex structures such as proteins and DNA, and in these reactions certain bonds must be easily broken and reformed. Hydrogen bonding is the only type of bonding with energies of just the right magnitude to allow this.
The key to DNA’s functioning is its double–helical structure with complementary bases on the two strands. The bases form hydrogen bonds to each other.

The organic bases found in DNA
8.5 There are two kinds of hydrogen–bonded base pairs, T–A and G–C, in DNA. Draw these two base pairs, showing the hydrogen–bonding interactions.