What is the intermolecular force of HCN?
(d) HCN is a linear molecule; it does have a permanent dipole moment; it does contain N, however the nitrogen is not directly bonded to a hydrogen. Therefore dispersion forces and dipole-dipole forces act between pairs of HCN molecules.
In hydrogen bonds, the Hydrogen atom is the hydrogen bond donor, and the atom with the lone pair of electrons is the hydrogen bond acceptor. In the second example, the partially positive end of HF is shown hydrogen bonding to the partially negative portion of formaldehyde (H2CO).
- Plasma is when the electrons are "freed" from their host atoms for a short time, due to high temperatures. Fire is plasma, it responds to electric fields. Lightning is also plasma. When a column of electrons flows from sky to ground, the air that it passes through lights up with energy.
- Liquid is represented by the lava. Many gasses are emitted by the lava during an eruption. Plasma may even be present, in the form of electrical discharges in the sky above the erupting volcano. Tell the students that today they will make a play volcano and observe three states of matter: solid, liquid, and gas.
- Here are 10 examples of forms of plasma:
- the excited low-pressure gas inside neon signs and fluorescent lights.
- solar wind.
- welding arcs.
- the Earth's ionosphere.
- stars (including the Sun)
- the tail of a comet.
HF is a polar molecule: dipole-dipole forces. Hydrogen is bounded to F. Hydrogen bonds exist. There are also dispersion forces between HBr molecules. SO2 is a polar molecule: dipole-dipole forces.
- Only one of them, NO, has a permanent electric dipole moment and so it is the only molecule which can have dipole-dipole intermolecular interactions; NO will have a higher boiling point than either Ar or CH4. The only non-vanishing intermolecular interaction in the case of Ar and CH4 is a London dispersion interaction.
- Because the IMFs in HF are so much stronger than HBr (hydrogen bonds vs. dipole- dipole), I would expect HF to have a much higher boiling point than HBr. F2 and HBr are a pair of a polar and nonpolar molecule, so the IMFs they have are induced dipole because of the polar nature of HBr.
- Ion−Ion forces are much stronger than any intermolecular forces. I2 is a nonpolar molecular substance; only weak dispersion forces are possible. attractive forces that must be overcome are hydrogen bonding and dispersion forces. (b) Bromine (Br2) molecules are nonpolar.
Updated: 2nd October 2019