CH4, also known as methane, is not capable of forming hydrogen bonds because it lacks the necessary electronegative atoms and hydrogen atoms bonded to them. Hydrogen bonds are a type of intermolecular force that occurs when a hydrogen atom is covalently bonded to a highly electronegative atom like nitrogen (N), oxygen (O), or fluorine (F).
In the case of methane (CH4), the carbon atom is bonded to four hydrogen atoms. Carbon is not as electronegative as nitrogen, oxygen, or fluorine, and the hydrogen atoms in methane are not bonded to these highly electronegative atoms. Therefore, methane does not have the required conditions to form hydrogen bonds.
Instead, methane molecules are held together by weaker van der Waals forces, which are much weaker than hydrogen bonds. This is why methane is a gas at room temperature and has a relatively low boiling point compared to substances that can form hydrogen bonds.