Question

try: for each pair of compounds:
circle the compound of each pair that would have the higher melting and boiling point (ie. stronger imfs).

a. nacl and hcl
b. h₂o and n₂o
c. co and co₂

Explanation:

Step1: Analyze the intermolecular forces (IMFs) in NaCl and HCl

NaCl is an ionic compound. Ionic compounds have strong ionic bonds (a type of IMF). HCl is a polar covalent compound. It has dipole - dipole forces. Ionic bonds are stronger than dipole - dipole forces.

Step2: Analyze the intermolecular forces (IMFs) in \(H_2O\) and \(N_2O\)

\(H_2O\) can form hydrogen bonds. \(N_2O\) has dipole - dipole forces. Hydrogen bonds are stronger than dipole - dipole forces.

Step3: Analyze the intermolecular forces (IMFs) in \(CO\) and \(CO_2\)

\(CO\) is a polar molecule with dipole - dipole forces. \(CO_2\) is a non - polar molecule with London dispersion forces. Dipole - dipole forces are stronger than London dispersion forces.

Answer:

a. NaCl; b. \(H_2O\); c. \(CO\)