ionic
London Dispersion Forces
Intermolecular forces are of the type(1) hydrogen bonds (2) dipole-dipole attractions (3) dispersion forces (van der Waals, etc.)
Dispersion forces (London dispersion forces) are generally the weakest type of intermolecular force. These forces are caused by temporary fluctuations in electron distribution around atoms or molecules, leading to weak attractions between them.
weak intermolecular forces because dry ice with sublime
van der Vaals forces of attraction and dipole-dipole interaction
The strength of intermolecular forces increases from CO2 (dispersion forces only) to CS2 (dispersion and dipole-dipole forces) to CSe2 (dispersion, dipole-dipole, and hydrogen bonding forces). This progression reflects the increasing polarity and molecular weight of the molecules, resulting in stronger intermolecular attractions.
Intramolecular forces are not intermolecular forces !
Hydrocarbons typically exhibit London dispersion forces as the predominant intermolecular force due to the presence of nonpolar carbon-carbon and carbon-hydrogen bonds. Additionally, larger hydrocarbons can also exhibit weak van der Waals forces. Overall, the intermolecular forces in hydrocarbons are relatively weak compared to compounds with polar covalent bonds.
HBr primarily exhibits dipole-dipole interactions due to the polarity of the H-Br bond. Additionally, HBr can also experience dispersion forces, caused by temporary dipoles that occur in all molecules.
Dipole forces and London forces are present between these molecules.
London Dispersion Forces
The type of intermolecular forces in Cl2Co (cobalt(II) chloride) would be predominantly ionic interactions between the cobalt cation and the chloride anions. These ionic bonds are formed through the electrostatic attraction between the positively charged cobalt ion and the negatively charged chloride ions.
These are intermolecular forces.
In Teflon, there are primarily London dispersion forces acting between the molecules. These forces result from temporary fluctuations in electron distribution that create temporary dipoles. There may also be some weak van der Waals forces present due to the nonpolar nature of the Teflon molecule.
Ionic and covalent bonds are examples of primary chemical bonds, which are forces that hold atoms together in a compound. Ionic bonds involve the attraction between positively and negatively charged ions, while covalent bonds involve the sharing of electron pairs between atoms.
In CaO, there would be ionic bonding between the calcium cations (Ca^2+) and oxide anions (O^2-), resulting in strong electrostatic forces of attraction. This ionic bonding is a type of non-covalent interaction between the positively and negatively charged ions.
The strongest intermolecular bond is the hydrogen bond, which forms between a hydrogen atom bonded to an electronegative atom (like oxygen or nitrogen) and another electronegative atom. Hydrogen bonds are stronger than dipole-dipole interactions and London dispersion forces.