3.8 Representations of Solutions

Solids and liquids exhibit what types of intermolecular forces?

All types

Interaction between substance with London Dispersion force and substance with London Dispersion force:

London Dispersion force

Example of interaction between substance with London Dispersion force and substance with London Dispersion force:

C7H16 + C5H12

Interaction between ion and polar molecule:

Ion-dipole

Example of interaction between ion and polar molecule:

Na+ + H2O

Interaction between substance with hydrogen bonding and substance with hydrogen bonding:

Hydrogen bonding

Example of interaction between substance with hydrogen bonding and substance with hydrogen bonding:

CH3OH + H2O

Interaction between polar molecule and polar molecule:

Dipole-dipole

Example of interaction between polar molecule and polar molecule:

HCl + CH3Cl

Interaction between ion and molecule with London-dispersion force:

Ion-induced dipole

Example of interaction between ion and molecule with London-dispersion force:

Na+ + C5H12

Interaction between polar molecule and molecule with London-dispersion force:

Dipole-Induced Dipole

Example of interaction between polar molecule and molecule with London-dispersion force:

H2O + Xe

For a positive ion, the negative end of the dipole for water is orientated towards:

The ion

For a negative ion, the positive end of the dipole for water is orientated towards:

The ion

The ability of two substances to mix without separating

Miscibility

What materials are miscible in each other?

Similar

Similar materials being miscible in each other means that:

Like dissolves like

Polar solvents dissolve:

Polar solutes

Nonpolar solvents dissolve:

Nonpolar solutes

Where do intermolecular forces exist in a solution?

Between solute particles, between solvent particles, and between solute and solvent particles

Do intermolecular forces in a solution promote or prevent the formation of a solution?

Either one or the other, depends

Intermolecular forces in a solution being able to either promote or prevent the formation of a solution depends on:

Solute/solvent combination

Is the tendency for solutes and solvents to mix strong or weak?

Strong

When will solutes and solvents not form a solution?

If the solvent-solvent and solute-solute attractions are strong compared to the solvent-solute interactions

When will solutes and solvents form a solution?

If the solvent-solute interactions (attraction) is greater than the solvent-solvent and solute-solute interactions, or if the solvent-solute interactions are relatively equal to the solvent-solvent and solute-solute interactions

Concentration can be represented in:

Particulate diagrams

How can concentration be represented in particulate diagrams?

By showing relative amounts of solute dissolved in solution

The more particles, the higher/lower the concentration

Higher

How to determine the difference in concentration between solutions when particulate drawings are compared to one another?

By calculating the ratio of individual particles