Question

List the intermolecular forces that you would find in the following substance: C₄H₁₀.

A) London dispersion forces
B) Dipole-dipole forces
C) Hydrogen bonding
D) Ionic forces

Answer 1

In C4H10 (butane), the intermolecular forces present are London dispersion forces, due to its nonpolar nature and lack of significant electronegative atoms capable of forming dipole-dipole interactions or hydrogen bonds.

Step-by-step explanation:

The intermolecular forces found in C4H10 (butane) are primarily London dispersion forces. Butane is a nonpolar molecule; therefore, the primary intermolecular force acting between its molecules are London forces.

London forces are a type of van der Waals force caused by the temporary uneven distribution of electrons in an atom or molecule, which leads to a temporary dipole that induces a dipole in adjacent molecules. As butane lacks any notable electronegative atoms (such as F, O, or N) directly bonded to hydrogen, it does not form hydrogen bonds. Additionally, there are no permanent dipoles within the molecule, so dipole-dipole forces are also absent. Since butane is covalently bonded, it does not exhibit ionic forces, which are characteristic of ionic compounds.