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| 105788448 | polar molecule | molecule with unequal distribution of electrons | 0 | |
| 105788449 | cohesion | Equivalent to surface tension; the forces that cause the individual molecules to be attracted to each other and thus cohese; usually caused by polarity | 1 | |
| 105788450 | adhesion | the clinging of one substance to another; equivalent to capillary action | 2 | |
| 105845688 | surface tension | a measure of how difficult it is to stretch or break the surface of a liquid | 3 | |
| 105845689 | kinetic energy | the energy of motion | 4 | |
| 105845690 | heat | the total kinetic energy of a group of atomic particles | 5 | |
| 105845691 | temperature | the average kinetic energy of a group of atomic particles | 6 | |
| 105845692 | Celsius scale | the scale used to indicate temperature. Equals Kelvin -273.15 | 7 | |
| 105845693 | calorie | the amount of heat it takes to raise the temperature of 1 g of water by 1 degree Celsius. = 4.184 Joules | 8 | |
| 105845694 | Calorie | 1000 calories | 9 | |
| 105845695 | joule | unit of energy most commonly used | 10 | |
| 105845696 | specific heat | the amount of heat that must be absorbed or lost for 1 g of that substance to change its temperature by 1 degree C | 11 | |
| 105845697 | evaporative cooling | when a liquid evaporates, the remaining liquid remains cooler due to the loss of the particles with the most energy, the property of a liquid whereby the surface becomes cooler during evaporation, owing to a loss of highly kinetic molecules to the gaseous state. | 12 | |
| 105845698 | solution | a liquid that is a completely homogeneous mixture of two or more substances | 13 | |
| 105845699 | solvent | dissolving agent of a solution | 14 | |
| 105845700 | solute | substance that is dissolved in a solution | 15 | |
| 105845701 | hydration shell | the sphere of water molecules that encompass each dissolved ion in a solution | 16 | |
| 105845702 | hydrophilic | interacting readily with water; typical of polar compounds or those containing charged or electronegative atoms, type of molecule that interacts with water by dissolving in water and/or forming hydrogen bonds with water molecules | 17 | |
| 105845703 | aqueous solution | a solution in which water is the solvent | 18 | |
| 105845704 | colloid | a stable suspension of fine particles in a liquid | 19 | |
| 105845705 | hydrophobic | describes substances that are nonpolar and seem to repel water | 20 | |
| 105845706 | molecular mass | the sum of the masses of all the atoms in a molecule | 21 | |
| 105845707 | mole | abbreviated (mol). Equivalent to (6.02214179 × 10^23) particles. A count of the number of particles in a given specimen | 22 | |
| 105845708 | Avogrado's Number | (6.02214179 × 10^23) particles / mol | 23 | |
| 105845709 | Molarity | the number of moles of solute per liter of solution | 24 | |
| 105845710 | hydrogen ion | a single proton with a charge of 1+ (H+) | 25 | |
| 105845711 | hydroxide ion | water molecule that lost a proton H2O--> OH- | 26 | |
| 105845712 | hydronium ion | H3O+. May actually be 3 water molecules converged around one hydrogen ion. Often represented as H+ | 27 | |
| 105845713 | Acid | Usually increases the hydrogen ion concentration of a solution. Acts as a proton donater | 28 | |
| 105845714 | Base | Usually increases the hydroxide ion concentration in a solution and reduces Hydrogen ion concentration in a solution. Acts as a proton acceptor. | 29 | |
| 105845715 | pH | the negative logarithm(base 10) of the hydrogen ion concentration. pH = -log[H+] | 30 | |
| 105845716 | Buffer | substance that minimizes changes in the concentrations of H+ and OH- ions in a solution. Usually contains a weak acid and its corresponding base, such that they dissociate and recombine readily with other acids/bases that appear in solution | 31 | |
| 105845717 | Acid precipitation | rain, snow, or fog with a pH lower than pH 5.2 | 32 |
