Final answer:
True statements regarding the molecules involve the presence of polar bonds and potentially ionic bond formation, while the 'No Electronegativity Differences' and 'Nonpolar Molecule' would not be universally true without additional context about the molecules in question.
Step-by-step explanation:
When evaluating the statements about the molecules shown, one needs to consider the types of chemical bonds present, namely: polar bonds, nonpolar covalent bonds, ionic bonds, and hydrogen bonds. The presence of polar bonds is indicated by a difference in electronegativity between the bonded atoms, leading to an uneven distribution of electrons.
A nonpolar molecule is one where the electrons are shared equally between the atoms, or the polarities cancel each other out due to a symmetrical structure, such as in boron trifluoride (BF3). The statement 'No Electronegativity Differences' would be false in the context of polar bonds since a polar bond implies a difference in electronegativity.
An ionic bond forms when an electron is transferred from one atom to another, leading to the formation of ions which attract each other due to opposite charges. Ionic bonds typically occur between metals and nonmetals. The statement 'Ionic Bond Formation' refers to this kind of chemical interaction.
Lastly, hydrogen bonds are weak bonds that can occur between a hydrogen atom in one molecule and an electronegative atom in another molecule. It is important to note that a hydrogen bond is not a true bond but a strong form of a dipole-dipole interaction.