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It is the number of moles of solute dissolved in one litre of a solution.

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It is made up of alternating positively-charged cations with negatively-charged anions. Ionic crystals are usually brittle, with high melting points. They can be made up of either atoms or molecules, as long as they are charged. A common example of an ionic solid would be sodium chloride (NaCl), known as table salt.

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They are made of metal atoms held together by metallic bonds. These metallic bonds are what give metals their malleability and ductility, as they allow the metal atoms to roll and slide past each other without breaking the material.

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They are made up of bonded molecules, unlike metallic and network crystals, which are made up of bonded atoms. Molecular bonds are relatively weak compared to atomic bonds and can be caused by a variety of intermolecular forces including dispersion forces and dipole-dipole forces.

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They are held together by covalent bonds between their constituent atoms. They are very hard solids, have high melting points and do not conduct electricity well. Common examples of covalent network solids are diamond and quartz.

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A crystalline solid is a type of solid whose fundamental three-dimensional structure consists of a highly regular pattern of atoms or molecules, forming a crystal lattice.

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An amorphous solid has no definite form, either geometric or crystalline. An amorphous solid is any non-crystalline solid that does not organize the atoms and molecules in a definite lattice pattern. There are glass, plastic, and gel solids.

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It is a state of matter characterized by particles arranged such that their shape and volume are relatively stable. The atoms and molecules in a solid can either be arranged in a regular pattern, making it a crystalline solid, or be arranged without a pattern, making it an amorphous solid.

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It is an electrostatic interaction between a charged ion and a molecule that has a dipole. It is an attractive force that is commonly found in solutions, especially ionic compounds dissolved in polar liquids.

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London Dispersion forces or  Van Der Waal forces 

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London Dispersion forces or  Van Der Waal forces 

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These are the weakest of the intermolecular forces and exist between all types of molecules, whether ionic or covalent—polar or nonpolar. Also, the breaking of London dispersion forces doesn’t require that much energy.

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This is a special kind of dipole-dipole interaction that occurs specifically between a hydrogen atom bonded to either an oxygen, nitrogen, or fluorine atom. Hydrogen bonding is a relatively strong force of attraction between molecules, and considerable energy is required to break hydrogen bonds.

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These forces occur when the partially positively charged part of a molecule interacts with the partially negatively charged part of the neighboring molecule.

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An ideal gas is a hypothetical gas whose pressure, volume, and temperature relationships are described completely by the ideal-gas equation.

PV = nRT

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The combined gas law expresses the relationship between the pressure, volume, and absolute temperature of a fixed amount of gas. For a combined gas law problem, only the amount of gas is held constant.

P₁V₁/T = P₂V₂/T

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Intermolecular forces are forces that exist between molecules.

Intermolecular forces are much weaker than the intramolecular forces of attraction but are important because they determine the physical properties of molecules like their boiling point, melting point, density, and enthalpies of fusion and vaporization.

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The gas laws discover the relationship of pressure, temperature, volume and amount of gas.

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(PRESSURE - VOLUME)

the volume of a gas at constant temperature varies inversely with the pressure exerted on it.

PV = constant P₁V1 = P₂V₂

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(VOLUME - TEMPERATURE)

the volume occupied by a fixed amount of gas is directly proportional to its absolute temperature, if the pressure remains constant.

V/T = constant V₁/T1 = V₂/T₂

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(VOLUME - AMOUNT)

For a constant temperature, volume increases with increasing amount of gas fed in the movable piston. Also note that fix amount of pressure is maintained.

V/n = constant V₁/n₁ = V₂/n₂

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(PRESSURE - TEMPERATURE)

the pressure of a given mass of gas varies directly with the absolute temperature of the gas, when the volume is kept constant

P/T = constant P₁/T1 = P₂/T₂