Question

Need help understanding intermolecular attractive forces. I’m in chapter liquids and solids and mainly that was intermolecular is about. I need help understand the concept.

understanding density , pv=nrt, m1v1=m2v2,p1,v1=p2v2,

Answer 1

*****************ANS-Understanding Intermolecular forces************************

Intermolecular forces (IMF) are the forces which mediate interaction between molecules, including forces of attraction or repulsion which act between molecules and other types of neighboring particles, example, atoms or ions. Intermolecular forces are weak relative to intramolecular forces – the forces which hold a molecule together. For example, the covalent bond, involving sharing electron pairs between atoms, is much stronger than the forces present between neighboring molecules. Both sets of forces are essential parts of force fields frequently used in molecular mechanics.

******Attractive intermolecular forces are categorized into the following types:*********

********1.Hydrogen bonding.A hydrogen bond is the attraction between the lone pair of an electronegative atom and a hydrogen atom that is bonded to an electronegative atom, usually nitrogen, oxygen, or fluorine.The hydrogen bond is often described as a strong electrostatic dipole–dipole interaction. example H₂O

***********2.Ionic bonding-The attraction between cationic and anionic sites is a noncovalent, or intermolecular interaction which is usually referred to as ion pairing or salt bridge.It is essentially due to electrostatic forces, although in aqueous medium the association is driven by entropy and often even endothermic.EXAMPLE-NaCl

***********3.Ion–induced dipole forces-Dipole–dipole interactions are electrostatic interactions between molecules which have permanent dipoles. These interactions tend to align the molecules to increase attraction (reducing potential energy). An example of a dipole–dipole interaction can be seen in hydrogen chloride (HCl)

*************4.Ion–dipole forces-Ion–dipole and ion–induced dipole forces are similar to dipole–dipole and dipole–induced dipole interactions but involve ions, instead of only polar and non-polar molecules. Ion–dipole and ion–induced dipole forces are stronger than dipole–dipole interactions because the charge of any ion is much greater than the charge of a dipole moment. Ion–dipole bonding is stronger than hydrogen bonding

************5.van der Waals forces – Keesom force, Debye force, and London dispersion force-The first contribution to van der Waals forces is due to electrostatic interactions between charges (in molecular ions), dipoles (for polar molecules), quadrupoles (all molecules with symmetry lower than cubic), and permanent multip

****************understanding density**********************

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thank you very much ,good luck