Question

question 4 (1 point) what intermolecular bonds can occur between ammonia molecules

Explanation:

1. Identify the molecule's polarity and groups: Ammonia ($\ce{NH_3}$) has a trigonal pyramidal shape. Nitrogen is more electronegative than hydrogen, so the $\ce{N - H}$ bonds are polar, making the molecule polar overall. Also, nitrogen has a lone pair of electrons, and hydrogen is bonded to a highly electronegative atom (nitrogen, which is one of the atoms that can participate in hydrogen bonding, along with O and F).
2. Types of intermolecular forces:

• London Dispersion Forces (LDF): These are present in all molecules, including non - polar and polar ones. They arise from temporary fluctuations in electron distribution, creating temporary dipoles. Since $\ce{NH_3}$ is a molecule, it will have LDF.
• Dipole - Dipole Interactions: Because $\ce{NH_3}$ is a polar molecule (due to the polar $\ce{N - H}$ bonds and the molecular geometry), the permanent dipoles in different $\ce{NH_3}$ molecules will interact with each other. The positive end of one $\ce{NH_3}$ molecule (near the H atoms) will be attracted to the negative end (near the N atom with the lone pair) of another $\ce{NH_3}$ molecule.
• Hydrogen Bonding: Hydrogen bonding occurs when a hydrogen atom is bonded to a highly electronegative atom (N, O, or F) and is attracted to the lone pair of electrons on a highly electronegative atom in another molecule. In $\ce{NH_3}$, the H atoms are bonded to N (a highly electronegative atom), and the N atom has a lone pair. So, the H atom of one $\ce{NH_3}$ molecule can form a hydrogen bond with the lone pair of N in another $\ce{NH_3}$ molecule.

Answer:

The intermolecular bonds that can occur between ammonia ($\ce{NH_3}$) molecules are London Dispersion Forces, Dipole - Dipole Interactions, and Hydrogen Bonding.