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similar to molarity but depends on the mass of solvent

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useful for relating the volume of a solution to the quantity of solute contained in that volume

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useful when dealing with gases, have no units, sum
of the mole fractions of all components of a solution must equal 1

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Parts per Million (ppm) or Parts per Billion (ppb)

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Parts per Million (ppm) or Parts per Billion (ppb)

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express the concentration of very dilute solutions, similar to mass percentage but use 10⁶ (a million) or 10⁹ (a billion), respectively, in place of 100 as a multiplier for the ratio of the mass of solute to the mass of solution

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simplest quantitative expressions of concentration

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copper

gold

zinc

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Sucrose or table sugar

Hydrocarbons

Sulfur

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Sodium chloride (NaCl)

Magnesium oxide (MgO)

Calcium carbonate (CaCO₃)

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diamond

graphite

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interaction between a Na+ ion and water (H₂O): where the sodium ion and oxygen atom are attracted to each other, while the sodium and hydrogen are repelled by each other

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two chlorine molecules: both chlorine atoms are bonded through a covalent bond which forms by equal sharing of valence electrons between two chlorine atoms

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water (H₂O)

chloroform (CHCl₃)

ammonia (NH₃)

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hydrogen chloride (HCl)

carboxylic acids (i.e., acetic acid)

amino acids

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simplest because every lattice point in a crystal is occupied
by an atom of the same metal

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lattice points are occupied by molecules

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atoms are held together in an extensive three dimensional network entirely by covalent bonds

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composed of charged species (anions and cations)

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The intermolecular forces within the solids define
their physical and chemical properties.

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Electrostatic interaction between a charged ion and a molecule that has a dipole.

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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.

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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

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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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London Dispersion Forces or Van der Waal Forces

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London Dispersion Forces or Van der Waal Forces

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Liquids, Solids and Phase Diagrams: Intermolecular Forces of Attraction (IMFA)

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Liquids, Solids and Phase Diagrams: Intermolecular Forces of Attraction (IMFA)

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states that the volume of a gas equals a constant value multiplied by its temperature as measured on the Kelvin scale.

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a statement that under the same conditions of temperature and pressure, equal volumes of different gases contain an equal number of molecules.

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states that the pressure of a given amount of gas held at constant volume is directly proportional to the Kelvin temperature

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states that the pressure (p) of a given quantity of gas varies inversely with its volume (v) at a constant temperature.

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