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Do All Substances Dissolve? - Coggle Diagram
Do All Substances Dissolve?
FACTORS IMPACTING SUBSTANCES DISSOLVING
Tempreture
Solids:
As temperature increases, energy is input into the solution, therefore increasing kinetic energy of intramolecular (ionic, metallic, covalent network latice) or intermolecular (covalent molecular) forces breaking to a higher degree. Thus, greater amounts of substance are able to dissolve
Gases:
As temperature increases the solubility of gases in liquids decreases. This inversely proportional relationship is due to increasing temperature increasing gas molecules' kinetic energy. Thus, they are easily released into the atmosphere instead of contained within the solution.
Polarity of substances (solute/solvent)
Non-polar
Non-Polar substances dissolve in other non-polar substance.
Polar
Polar substances consisting oppositely charged poles dissolve in other substances with oppositely charged poles.
Polar and Polar:
The oppositely charged poles of either polar substances are attracted to one other, breaking the original secondary bonds to form intermolecular bonds with the polar and polar substances: dissolving occurs.
Polar in Ionic
: Ionic substances have oppositely charged ends due to the positive and negative ions. Opposite polar and ionic ions form ion-dipole bonds. The ionic solids dissolve in polar substances. (Strongest form of intermolecular forces when dissolving)
Surface Area to Volume Ratio
Solid solute: Decreasing or increasing surface area determines the amount of solid exposed to the solvent, impacting the dissolving rate.
Time
Stirring/Agitation
Does not impact how much of the solute can be dissolved in a solvent. However, impacts the rate of dissolving. As stirring allows new solute particles to come in contact with water particles due to the constant movement. When solute particles sit at the bottom of the solution with no mixing, less water particles interact with the solute particles at a time.
Molar Mass
The molar mass and molecular size are inversely proportional. Therefore, the greater the molar mass of a solute molecule, the greater its size. Indicating the same impact on solubility as size. As it will be more difficult for the solvent molecule to wrap around a greater solvent molecule to properly form bonds with the solute molecules.
Molecular Size
As molecular size increases (solute), it becomes difficult for solvent molecules to wrap around the solute molecules in order to form bonds and dissolve.
Pressure
Gases dissolve in liquid solvent
: At low pressures, gases move freely throughout the atmosphere, with minimum dissolving in water. At higher pressures, gases experience higher collision frequencies with the liquid solvent, allowing gas molecules to dissolve.
Electronegativity
Viscocity
pH
SUBSTANCES
Ionic compounds
Ionic lattice
Primary bonds are broken with solubility
Covalent compounds
Bonding types
Dispersion forces
2 non-polar substances forming temporary dipoles when the electrons momentarily distort asymmetrically around the nucleus. Weakest forces requiring minimum energy to break.
Dipole-Dipole
Two polar substances bonding to form a compounds with partially charged poles.
Hydrogen Bonding
Strongest molecular bond. Forming between
Covalent network lattice
Ion-dipole
Metals
Metallic lattice
States of matter
Solid
Dissolve in liquids.
Liquid
Soluble in gases and solids
Gas
Dissolve in other gases easily
Require certain pressures and tempretures to dissolve in liquids.
Purity
Impure
Pure
MEASURING DISSOLVING
QUALATATIVE DATA:
Observations and appearance of solubility occuring. E.g solids particles remaining or dissolved and disappeared.
Clear liquids
Separation of the two layers are visible if substances do not dissolve in one another.
QUANTITATIVE DATA
Measuring through mass g/mL and comparing between various substances to conclude which substance are soluble and which are not soluble
TERMS