The molecule shown exhibits only London dispersion forces as the intermolecular forces. Dipole-dipole forces and hydrogen bonding are not present in the molecule. Therefore, the correct answer is a. 1 only
In the given molecule, we can identify the following intermolecular forces:
1. London dispersion forces:
London dispersion forces are present in all molecules. These forces result from temporary fluctuations in electron density, creating temporary dipoles. They are the weakest intermolecular forces and are caused by momentary imbalances in electron distribution. In the molecule shown, there are no permanent dipoles, but there can be temporary dipoles due to the random movement of electrons.
2. Dipole-dipole forces:
Dipole-dipole forces occur between polar molecules. A polar molecule has a permanent dipole moment due to an uneven distribution of electrons. In the given molecule, there are no polar bonds, so there are no dipole-dipole forces present.
3. Hydrogen bonding:
Hydrogen bonding occurs when hydrogen is directly bonded to a highly electronegative atom, such as nitrogen, oxygen, or fluorine. In the given molecule, there are no hydrogen atoms bonded to nitrogen, oxygen, or fluorine, so hydrogen bonding is not present.
Based on the analysis, the intermolecular forces present in the molecule shown are only London dispersion forces (1 only).