11106911
Description
Flashcards by Elisa Lorenz, updated more than 1 year ago
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Created by Elisa Lorenz
over 6 years ago
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| Question | Answer |
| Aqueous | A water solution, indicated by the notation "(aq)". For example, HCl (aq) indicates a water solution of hydrochloric acid. |
| Atom | The smallest particle of an element that represents its physical and chemical properties. |
| Average Kinetic Energy | Energy of motion; the temperature of a substance is a measure of its average kinetic energy. |
| Boiling Point | The temperature at which a phase change occurs from liquid to gas as energy is absorbed. A liquid will boil at the temperature at which its vapor pressure equals the pressure on the liquid (atmospheric pressure). |
| Celsius | A temperature scale with set points of 0° for the freezing point of water at 1 atm (the ice-water equilibrium), and 100° for the boiling point of water at 1 atm (the water-steam equilibrium); abbreviated as "°C". |
| Chemical Reaction (Change) | The formation of a new substance with its own physical and chemical properties. Examples of chemical reactions include: single replacement, double replacement (substitution), decomposition, and synthesis. |
| Compound | A substance composed of two or more different elements chemically combined in a definite ratio. A compound can be decomposed by a chemical change. |
| condensation | The change in state of matter from a gas (vapor) to a liquid. Heat is released in this phase change. |
| Crystal | A solid with a regular geometric pattern. All true solids have a crystalline structure. Crystals contain particles arranged in a regular geometric pattern. Particles of matter are constantly vibrating even in the solid phase. |
| Density | Mass per unit volume. |
| Deposition | A phase change in which a gas turns directly into a solid, skipping the liquid phase; the settling out of material from a solution. |
| Element | A substance that cannot be decomposed by chemical change. All known elements are listed in the Periodic Table. |
| Endothermic Reaction | A reaction in which the products contain more energy than the reactants. Energy is absorbed in an endothermic reaction. |
| Evaporation | A change in state from liquid to gas; energy is absorbed. |
| Exothermic Reaction | A reaction in which the products contain less energy than the reactants. Energy is released in an exothermic reaction. |
| freezing | The change in phase of a substance from a liquid to a solid. The substance releases energy. |
| Freezing Point | The temperature at which a substance changes from a liquid to the solid phase. Contrast with the melting point. At the freezing point, both the liquid and solid phases are in equilibrium at atmospheric pressure. |
| Gas | A phase of matter that takes the shape and volume of its container. The gaseous phase of matter is represented by the notation "(g)". |
| Gram | A unit of mass in the metric system; symbol is "g". |
| Heat | A flow of energy from an area of higher temperature to an area of lower temperature. |
| Heat of Vaporization | The energy required to vaporize a unit mass of a liquid at its normal boiling point. |
| Heating and Cooling Curve | A graph representing the changes in the phases of matter. |
| Kelvin | An absolute temperature scale; the temperature measured in Kelvins is equal to the temperature in degrees Celsius + 273. The span of 1 K is equal to the span of 1°C. 0 K = absolute zero = −273°C. |
| Joule | A unit of energy . |
| Kinetic Energy | The energy of motion, as opposed to potential energy (energy of position). Temperature measures average kinetic energy |
| Liquid | A phase of matter that has definite volume but takes the shape of its container. Matter in the liquid phase indicated by the notation "(l)". |
| Mass | A measure of the amount of matter; often measured in grams (g). |
| Matter | Anything that has mass and takes up space. |
| melting | A phase change from a solid to a liquid. |
| Mixture | A combination of two or more distinct substances differing in properties and composition. The composition of a mixture can vary. |
| Molecule | The smallest particle of an element or compound capable of independent existence and formed by covalently bonded atoms in a definite ratio. A molecular compound can be decomposed by a chemical change. |
| Phase change | Change in state of matter. The addition or removal of heat energy can cause the form of matter to change between solid, liquid, and vapor. |
| Physical Change | A change in the phase of matter or in its physical properties, such as shape, mass, volume, or density. |
| Potential Energy | Energy of position rather than of motion, such as the energy stored in a chemical bond; contrast with kinetic energy. |
| Specific heat capacity | The amount of energy (in joules) it takes to raise the temperature of one gram of a substance by 1 Kelvin. |
| Specific Heat of Water | The amount of heat needed to raise the temperature of 1 gram of water by 1 Kelvin; a heat value equal to 4.18 J/g·K. |
| Standard Temperature and Pressure (STP) | For any gas, STP is defined as 0°C (273 K) and 760 mm of mercury (760 torr), or 101.3 kPa (kilopascals) or 1 atmosphere, of pressure. |
| Sublimation | A change from a solid directly into a gas without passing through the liquid phase. |
| Substance | Matter in which all samples have identical properties and composition. |
| Temperature | A measure of the average kinetic energy of the molecules that make up a substance; how "hot" or "cold". Temperature is measured in degrees Celsius (°C) or Kelvin (K). |
| Vaporization | Evaporation. The change in phase or state from a liquid to a vapor (gas). Evaporation of water is a cooling process. |
| Volume | The amount of space occupied by matter. |
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