Chemistry Word Scramble
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Term | Definition |
What property of all ionic compounds make them electrolytes? | they dissociate into ions |
What would you do to reduce the solubility of gas solute in a gas/liquid solution? | reduce the partial pressure of the gas above the solution |
Tyndall Effect | separation of light as it passes through colloid or suspension |
Solute | substance in lesser quantity that is dissolved |
Emulsion | a colloid of a liquid in a liquid |
Electrolyte | ionic compounds that dissolve into solution and conducts electricity |
Alloy | homogeneous mixtures of metals |
Immiscible | describes liquids that are insoluble in one another |
Saturated Solution | solution containing maximum amount of solute |
Supersaturated Solution | solution containing more solute than can theoretically dissolve at a given temperature |
Colloid | heterogeneous mixture in which particles cannot be separated by filtration |
Polar | molecules with uneven distribution of charge |
Solvent | dissolving medium, the substance in greater quantity |
Aqueous Solution | homogeneous mixture of water and dissolved substances |
Solvation | solute ions or molecules are surrounded by solvent molecules |
Tincture | homogeneous mixture of dissolved particles in alcohol |
Solution | homogeneous mixture of solute and solvent |
Solute + Solvent = | solution |
Solvent-Solvent | energy absorbed |
Solute-Solute | energy absorbed |
Solvent-Solute | energy released |
Dissociation | separation of an ionic solid into aqueous ions |
Ionization | breaking apart of some polar molecules into aqueous ions |
Dispersion | molecules stay intact |
Two substances with similar IMF | are likely to be soluble in one another |
Non-Polar molecules are soluble in | non-polar solvents |
Ionic compounds are more soluble | in polar solvents |
How do we know ions are present in aqueous solutions? | electrolytes |
Non-electrolytes | some compounds dissolve in water but do not conduct electricity |
Unsaturated Solution | when the solvent holds less solute than it normally can at a given temperature |
Solubility | the maximum amount of solute that will dissolve in a given quantity of solvent at a specific temperature |
Concentration | the amount of solute in a solution |
More solute, constant amount of solvent | more concentrated |
Less solute | less concentrated |
More solvent | less concentrated |
Less solvent | more concentrated |
Dilution | the procedure for preparing a less concentrated solution from a more concentrated solution |
3 Factors Affecting Solubility | the size of the solute/crystals the temperature of the solvent the vigor and duration of stirring |
Henry's Law States That | the solubility of a gas in a liquid is proportional to the pressure of the gas over the solution |
Henry's Law | c=kP |
c | concentration(M) of the dissolved gas |
k | a constant for each gas (mol/L x atm) that depends only on temperature |
P | pressure of the gas over the solution |
The solubility of gases | decreases at higher temperatures |
Colligative Properties | are properties of solutions that depend on the ratio of the number of solute particles to the number of solvent molecules in a solution, and not on the nature of the chemical species present |
Created by:
jordinlevy
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