🤓 Based on our data, we think this question is relevant for Professor Harwood & Towns' class at PURDUE.
Classify the species given below by the intermolecular forces present in a pure sample of each:
Ar H2 HCN HF BrCl5 NH3 CH3OH H2S PF5 CH2Cl2
Are they dispersion, dipole-dipole, or H-bond?
We’re being asked to identify the intermolecular forces present in each compound. Recall that there are several types of intermolecular forces:
1. Hydrogen bonding – occurs in compounds where hydrogen is directly connected to an electronegative element such as N, O, or F
2. Dipole-dipole interaction – occurs between two polar covalent compounds
3. Dispersion forces – occurs in all compounds. This is the primary intermolecular force exhibited by nonpolar compounds.
For this problem, we need to do the following steps:
Step 1: Determine the central atom in the molecule.
Step 2: Calculate the total number of valence electrons present.
Step 3: Draw the Lewis structure for the molecule.
Step 4: Determine the polarity and IMF of the molecule.
**we can skip these steps if the molecule is monoatomic/diatomic or has a simple structure