What is the strongest intermolecular force that occurs between methane (CH4) and ammonia (NH3)?
A. Dipole-dipole forces
B. Hydrogen bond
C. London dispersion forces
D. Dipole-induced dipole attractions
D. Dipole-Induced Dipole Atrractions
Well, let me tell you, the intermolecular force between methane (CH4) and ammonia (NH3) is a real gas. No, I'm just kidding! It's actually dipole-dipole forces. You see, the polar molecule ammonia and the not-so-polar molecule methane can have attractions based on their slight positive and negative charges. So, the answer is A. Dipole-dipole forces. Keep reaching for the stars, intermolecular forces!
The strongest intermolecular force that occurs between methane (CH4) and ammonia (NH3) is hydrogen bonding.
To determine the strongest intermolecular force between methane (CH4) and ammonia (NH3), we need to analyze the molecular properties of each compound.
Methane (CH4) is a nonpolar molecule, where all carbon-hydrogen (C-H) bonds have similar electronegativity. As a result, methane does not possess a permanent dipole moment and does not form hydrogen bonds. The main intermolecular force acting on methane is London dispersion forces, which occur due to temporary fluctuations in electron density.
Ammonia (NH3), on the other hand, is a polar molecule, with the nitrogen atom being more electronegative than the hydrogen atoms. As a result, ammonia exhibits a dipole moment, with the nitrogen having a partial negative charge and the hydrogens having partial positive charges. This polarity allows ammonia to form hydrogen bonds with other ammonia molecules, as the hydrogen atom can bond with the lone pair of electrons on nitrogen. Hydrogen bonds are significantly stronger than London dispersion forces.
Comparing the two compounds, methane and ammonia, the strongest intermolecular force occurring between the two is hydrogen bonding. Therefore, the correct answer is B. Hydrogen bond.