Type of intermolecular forces

• The strength of the London dispersion force depends on the size, shape, and polarity of the molecule.
• Polar covalent bonds occur when there is an unequal sharing of electrons between two atoms with different electronegativities.
• Dipolar-dipole interactions occur between polar molecules with permanent dipoles.
• Dipole-dipole interactions are weaker than chemical bonds but stronger than van der Waals forces.
• Ionic compounds have strong electrostatic attractions between oppositely charged ions.
• Molecules with large dipole moments, such as polar molecules like HCl and NH3, have stronger dipole-dipole interactions.
• Dipole-dipole interactions occur between polar molecules with permanent dipoles.
• Hydrogen bonding is an attractive interaction that occurs when hydrogen atoms covalently bonded to highly electronegative elements such as fluorine, oxygen, or nitrogen interact with other highly electronegative elements.
• Dipoles are formed due to the difference in electronegativity between atoms.
• Hydrogen bonding occurs when hydrogen is attached to highly electronegative elements such as fluorine, oxygen, or nitrogen.
• Ionic compounds consist of positively charged metal ions (cations) and negatively charged nonmetal ions (anions).
• Hydrogen bonding involves the attraction between a partially positive hydrogen atom and a nearby negative charge.
• Intermolecular forces can be classified into three categories based on their strengths: weak (van der Waals), moderate (hydrogen bonding), and strong (ionic).
• Interactions between nonpolar molecules involve only London dispersion forces.
• Hydrogen bonding can be broken by increasing temperature or pressure.
• Water has high boiling point due to its ability to form extensive hydrogen bonds.
• The strength of dipole-dipole interactions depends on factors such as distance, orientation, and size of the dipoles involved.
• London dispersion forces are temporary dipoles caused by random fluctuations in electron distribution within atoms/molecules.
• London dispersion forces are temporary dipoles that form due to fluctuations in electron density within atoms and molecules.
• Stronger electrostatic attractions occur when there are more charges present.
• Dipole-dipole interactions occur when two polar molecules approach each other with opposite partial charges facing each other.
• Electric field (E) is represented by the equation E = F/q
• E is expressed in N/C (newton per coulomb)
• F is the electrostatic force expressed in N (newton)
• q is the charge expressed in coulombs (C)
• If q is positive, the direction of E is the direction of F
• The force on a negative charge is opposite to the direction of the electric field E
• Constant k = 8.99 x 10^9 N.m^2/C