In the wonderful world of chemistry, the dissolved matter is everywhere. We all know that salt can easily dissolve in water, and oil is "unlike water." what's the secret behind that? Today, we're here to expose chemistry. MediumSimilar to the solubility principleThe mystery veil。
Similar to the theory of phase solubility, it is simply that substances with similar molecular structures can dissolve each other. This rationale is based on molecular interactions, including van der waals, hydrogen keys and solventization effects。
One, "mysterious power" between molecules
One, van der waald
Van der waals is a weaker attraction that exists among molecules and is much weaker than a chemical key. This power is not saturated and directed and is permanently present among all molecules. Van der waals can in turn be broken down into colour dissipation, induction and orientation。
Colour dissipation: it is the force of interaction between molecules instantaneously. The larger the general molecular mass, the greater the number of electrons in the molecule, the greater the molecule's deformation and the greater the dispersive power. For example, iodine molecules (i2) and carbon tetrachloride molecules (ccl4) are non-polar molecules, which are largely interaction through colour dispersion, allowing iodide to dissolve in carbon tetrachloride。
Inducing force: the interaction of the polar molecule's permanent meth with the other molecules that it induces. When the polar and non-polar elements are close to each other, the non-polar elements, acting under the inherently impervious function of the polar elements, become polarized, produce a temptation to the pup, and then induce the pup to attract each other to the inherently impervious level, creating a inducement. Of course, there are incentives between polar elements。
Orientation: when polar molecules are close to each other, they are inherently insinuated with extremes and alienated, or directed, thus generating direction. The larger the even-polar rectangular, the greater the orientation; the higher the temperature, the smaller the orientation。
Two, hydrogen
Hydrogen keys are specialMolecular forceIt's a little stronger than van der waals. When hydrogen atoms are combined with atoms with large negatives and small radiuss (e. G. Fluorine, oxygen, nitrogen, etc.) at co-prices, the strong attraction of these atoms to electrons makes hydrogen atoms almost “naked” protons, so that hydrogen atoms produce an electrostatic attraction between another atom with large negatives, small radiuss and isolated electrons, which is hydrogen. For example, large quantities of hydrogen keys exist among water molecules in water. The formation of hydrogen keys between hydrogen atoms in one water molecule and oxygen atoms in another water molecule gives the water many unique properties, such as higher boiling points, larger heat profiles, etc. At the same time, hydrogen keys play an important role in the dissolution of substances. Like ethanol (c2h5oh) is able to dissolve in any proportion with water, because hydrogen keys can be formed between hydroxyl (-oh) in ethanol molecules and hydroxyl radicals in water molecules。
3. Solventification effects
Solventization effects are the process by which a solvent molecule or ion interacts with a solvent molecule to form a solvent molecule or ion. In solution, the interaction of solute particles and solvent particles leads to dissolution. If solvents and solvents are non-polar molecules, such as iodine (i2) and carbon tetrachloride (ccl4), the interaction is dominated by chromosomal dispersion; if one is polar molecule, the other by non-polar molecules, such as iodine (i2) and ethanol (c2h5oh), the interaction is between molecules; and in the case of strong polar molecules, the orientation is predominant. If one solvent particle is an ion, it forms a hydrate ion in water, a ammonia ion in liquid ammonia and a solvent ion in other solvents. For example, when sodium chlorinated (nacl) dissolves in water, sodium ion (na+) is attracted by the oxygen atom at the end of the water molecule (with negative electricity), and chlorine ion (cl-) is attracted by the hydrogen atom at the end of the water molecule (with positive electricity) to form hydrate ion, thus allowing sodium chloride to dissolve in the water。
