Hello, I wouldn't necessarily regard this as homework. While these are errors I believe I have found within an online course in which I am currently enrolled, my asking is simply carried out with interest in acquiring an accurate knowledge of entry-level chemistry. While studying polar molecules and various intermolecular forces, such as the London force, dipole-dipole interactions and hydrogen bonds, I came across a sample problem that appeared to contain some inaccuracies. In one section of the sample, my resource claims that Arsine (AsH3) is a polar molecule. This doesn't make sense to me. While the structure of Arsine isn't symmetrical, both hydrogen and arsenic have an electronegativity of 2.2. Would this not imply that the molecule is nonpolar, as no polarity due to a difference in the electronegativity of the bonded atoms is established? Also, within the same sample problem, my resource claims that hydrogen fluoride (HF) only contains hydrogen bonds and that hydrogen iodide (HI) only contains dipole-dipole interactions. While the aforementioned intermolecular interactions do occur within these two molecules respectively, can HF not also contain dipole-dipole interactions and the London force? Can HI not contain the London force in addition to its dipole-dipole interactions? Recognizing that only one type of intermolecular interaction is listed for each, I ask: is it common practice to only list the interaction that affects a molecule the most? I thank anyone who has taken the time to read and consider my concerns, your contributions are greatly appreciated. Thank you, Eric.