Hydrogen Bonds

• Liquid water has a high melting and boiling point due to its strong hydrogen bonds between molecules.
• Intermolecular forces are responsible for the physical properties of liquids and solids.
• The stronger the intermolecular forces, the higher the boiling point.
• The strength of intermolecular forces depends on the type of bonding present, with covalent bonds being stronger than ionic or metallic bonds.
• Dipole-dipole interactions occur when two polar molecules interact with one another.
• The strength of the intermolecular forces determines whether a substance is solid, liquid or gas at room temperature
• Stronger intermolecular forces lead to higher melting/boiling points and lower vapor pressure
• Ionic compounds have very strong electrostatic attractions between oppositely charged ions, resulting in high melting points.
• London dispersion forces arise from temporary dipoles that form on nonpolar molecules.
• London dispersion forces arise from temporary dipoles that form within nonpolar molecules.
• Hydrogen bonding occurs when a hydrogen atom is attached to an electronegative element such as nitrogen, oxygen, or fluorine.
• Hydrogen bonding occurs when a hydrogen atom that is attached to an electronegative element (such as nitrogen, oxygen, or fluorine) forms a weak attraction to another nearby electronegative element.
• Weaker intermolecular forces lead to lower melting/boiling points and higher vapor pressures
• Hydrogen bonding is an especially strong type of dipole-dipole interaction that occurs only between certain types of molecules.
• Metallic solids are held together by delocalized electrons that move freely through the lattice structure, leading to high melting points due to the energy required to break these electron bonds.
• London dispersion forces arise from temporary dipoles that form around all atoms and molecules.
• Hydrogen bonding is a special case of dipole-dipole interaction where there is an especially strong attraction between a hydrogen atom attached to an electronegative element (such as nitrogen) and another nearby electronegative element.
• Hydrogen bonding occurs between hydrogen atoms attached to highly electronegative elements (F, O, N) and other highly electronegative elements.
• Ionic compounds have very strong electrostatic attractions between oppositely charged ions.
• Hydrogen bonding occurs when hydrogen atoms are covalently bonded to highly electronegative elements such as F, O, N, S, Se, Te.