molecular forces

surface tension

tendency of a liquid’s surface molecules to stick together, creating a skin-like surface caused by cohesive forces

The viscosity

the resistance of liquids to flow due to the internal friction between its molecules

The Capillarity

result of surface forces that is often described as the rise or depression of a liquid in a small passage

The boiling point

the temperature at which a liquid gets hot enough that it starts to form bubbles continuously and turn into gas

The freezing point

the temperature at which a liquid gets cold enough that its molecules slow down and lock into a solid structure

conductivity

ability of solids to allow electric current or heat to pass through

pliability

most solids resist deformation. However, it depends on the type of solid and the forces between its particles. Rigid solids have stronger resistance because their particles are tightly bound. Metals, on the other hand, have more flexible atom arrangements which allows them to bend or stretch without breaking.

Melting point

the temperature at which a solid turns into a liquid as its particles gain enough energy 

Sublimation point

temperature at which a solid changes directly into a gas without becoming a liquid

solubility

ability of solids to dissolve in liquids, forming a homogeneous solution at a given temperature and pressure.

density

refers to how tightly the particles of solids are arranged within a given space. In most solids, the particles are closely packed in fixed positions, giving them a definite shape and making them feel heavy or substantial for their size.

Crystalline

regarded as the ‘true solids’, they are composed of atoms that are arranged in an ordered and symmetrical pattern that is repeated over the entire crystal

Ionic crystalline

crystalline composed of oppositely charged ions, a positive cation and a negative anion

Covalent Crystalline

Consist of atoms connected by a continuous network of covalent bonds

molecular cystallines

Formed by molecules held together by weak intermolecular forces

metallic crystallines

composed of metal atoms surrounded by a sea of mobile electrons, these solids are known for their opaque and lustrous characteristics

Amorphous

also called as pseudo solids, they are composed of a particles that do not have a repeating lattice pattern

Intermolecular forces

otherwise known as the attractive forces between the particels.

Dipole-Dipole

occurring between the oppositely charged poles of polar molecules, they typically result when two dipolar molecules interact with each other through space

Ion-Dipole

Occurring between an ion and a polar molecule, the ion of ion-dipole forces forms an attraction with an oppositely charged pole of a neighboring molecule.

London Dispersion

proposed by Fritz London, it is a weak intermolecular force that comes from the interactive forces of instantaneous dipoles.

Hydrogen Bonds

occurring to polar molecules that contain an oxygen, nitrogen, or fluorine that are covalently bonded to a hydrogen atom, the hydrogen bonds are relatively strong intermolecular forces.

Temperature

the heating and cooling of a substance can change the kinetic energy of their particles, allowing them to alter their phases significantly

pressure

The intermolecular forces between two molecules can also be called: