Question

which diatomic molecule has the smallest (lowest) dipole moment? a) f2 b) o2 c) n2 d) h2 e) all equal

Answer 1

Homonuclear diatomic molecules like F2, O2, N2, and H2 have no difference in electronegativity, resulting in a dipole moment of zero.

Step-by-step explanation:

For diatomic molecules, the dipole moment is determined by the bond dipole moment. Homonuclear diatomic molecules like F2, O2, N2, and H2 have no difference in electronegativity, resulting in a dipole moment of zero. Therefore, the correct answer is (e) all equal.

Answer 2

The diatomic molecules F₂, O₂, N₂, and H₂ are all homonuclear with zero dipole moment due to no difference in electronegativity, making their dipole moments equally the smallest value possible, which is zero. So the correct option is e.

Step-by-step explanation:

The question asks which diatomic molecule has the smallest (lowest) dipole moment among F₂, O₂, N₂, and H₂. Dipole moments depend on the difference in electronegativity between atoms. Homonuclear diatomic molecules, such as N₂, O₂, and F₂, have identical atoms with no difference in electronegativity, resulting in a dipole moment of zero. However, of the options provided, the diatomic molecule with the smallest dipole moment would be any one of these homonuclear diatomic molecules, since they all have a dipole moment of zero. It is important to note that H₂ is also a homonuclear diatomic molecule with no difference in electronegativity between the hydrogen atoms, thus it also has a dipole moment of zero. Consequently, the answer is that all options (F₂, O₂, N₂, and H₂) have equal dipole moments, which are the smallest possible values, zero.