Chemistry Intermolecular Forces

The force of attraction or repulsion between charged particles.

A force that attracts oppositely charged particles and repels similarly charged particles.

A molecule with a positive and negative pole due to an uneven distribution of electrons.

The interaction between two dipole molecules, where the positive end of one dipole is attracted to the negative end of the other.

The strength of electrostatic force is directly proportional to the product of charges and inversely proportional to the square of the distance between them.

A special type of dipole-dipole interaction occurring between a hydrogen atom bonded to a highly electronegative atom like oxygen, nitrogen, or fluorine.

The strength of hydrogen bonding depends on the number and arrangement of bonds, as well as the polarity of the molecules involved.

The temperature at which a liquid changes to a gas. Liquids with stronger intermolecular forces have higher boiling points because more energy is needed to break the attractions between molecules.

The temperature at which a solid changes to a liquid. Substances with stronger intermolecular forces have higher melting points.

A model used to explain the behavior of matter in different phases (solid, liquid, gas) based on the movement and interactions of particles.

The force of attraction between molecules in a liquid. Stronger intermolecular forces lead to higher viscosity, making the liquid flow slower.

The tendency of a liquid to resist an increase in its surface area. Stronger intermolecular forces lead to higher surface tension, making the liquid surface more resistant to disruption.

A repeating unit of a crystalline solid, creating a structured arrangement of particles.

A solid that lacks a well-defined arrangement of molecules, allowing it to flow like a liquid, but retains a fixed volume.

The attraction between molecules of the same type, like water attracting other water molecules.

The attraction between different types of molecules, like water clinging to a glass surface.

The upward movement of a liquid in a narrow tube or space due to the balance of cohesive and adhesive forces.

A solid with a regularly repeating arrangement of atoms or molecules, forming crystals.

Solids are rigid and resistant to changes in shape because their particles are tightly packed and organized.

Solids have a definite shape and volume because their particles are tightly packed and resist compression.

The resistance of a liquid to flow. Higher viscosity means the liquid flows slower.

The energy required to vaporize one mole of a liquid at its boiling point. It's a measure of the strength of intermolecular forces.

The higher the IMF, the more viscous the liquid. This is because the molecules are more strongly attracted to each other and resist flowing.

The stronger the intermolecular forces, the higher the boiling point. This is because more energy is needed to overcome the attractive forces and cause the molecules to vaporize.

Water is an excellent solvent due to its polarity and ability to form hydrogen bonds. It's a great dissolving agent for many substances.

Liquids with longer hydrocarbon chains generally have stronger intermolecular forces, leading to higher viscosity. Think of oil versus gasoline.

Glycerol is a molecule with many hydroxyl groups that can form hydrogen bonds. This gives it a high IMF and, as a result, high viscosity.

Acetone, ethanol, and water all exhibit dipole-dipole interactions, but the stronger hydrogen bonds in water contribute to its higher boiling point.

The ability of a substance to resist changes in temperature. Water has a high specific heat, meaning it takes a lot of energy to raise its temperature.

The amount of energy required to raise the temperature of 1 gram of a substance by 1 degree Celsius. This is a measure of how much heat energy is needed to change the temperature of a substance.

Water molecules have strong attractive forces called hydrogen bonds. These bonds require a lot of energy to break, leading to water's high specific heat.

The process of a substance changing from a liquid to a gas. Water has a high heat of vaporization, meaning it takes a lot of energy to turn liquid water into vapor.

A measure of the force that holds the surface of a liquid together. Water has a high surface tension due to strong hydrogen bonds between its molecules. This allows insects to walk on water and causes water droplets to form.

Ionic crystals are solid structures composed of positively and negatively charged ions held together by electrostatic forces. These forces are strong, resulting in hard solids with high melting points. Because the ions are tightly bound, they are poor electrical conductors in both solid and molten states. Examples include salts like NaCl.

The specific arrangement of ions within the crystal lattice is influenced by the size of the ions. Larger ions will occupy more space than smaller ions, affecting the overall structure.

Covalent crystals are characterized by strong covalent bonds between atoms, creating a rigid, three-dimensional network. This network structure leads to high melting points and poor electrical conductivity. Examples include diamond, graphite, and silicon carbide.

Ionic crystals are brittle because their rigid structure breaks easily when deformed. The strong electrostatic forces holding the crystal together are disrupted, causing the crystal to fracture.

Ionic crystals are poor electrical conductors because their ions are fixed in specific locations within the lattice. However, when melted or dissolved, the ions become mobile and can conduct electricity.