Definition Flashcards
Response option
Specific operations performed in a specific order to accomplish the goals of the responses objective
Response objective
Statement based on realistic expectations of what can be accomplished when all allocated resources have been effectively deployed that provide guidance and direction for selecting appropriate strategies and the tactical direction of resources
Hazardous materials technician
Individual trained to used specialized protective clothing and control equipment to control the release of a hazardous material
Hazardous waste operations and emergency response (HAZWOPER)
U.S. regulations in Title 29 (labor) CFR 1910.120 for cleanup operations involving hazardous substances and emergency response operations for releases of hazardous substances
Overpack
- To enclose or secure a container by placing it in a larger container
- An outer container designed to enclose or secure an inner container
Solid
Substance that has a definite shape and size; the molecules of a solid generally have very little mobility
Liquid
Incompressible substance with a constant volume that assumes the shape of its container; molecules flow freely, but substantial cohesion prevents them from expanding as a gas would
Gas
Compressible substance, with no specific volume, that tends to assume the shape of a container. Molecules move about most rapidly in this state
Vapor
Gaseous state of a material that may normally be a solid or a liquid
Aerosol
Microscopic particles that may be a solid or a liquid
Dust
Airborne solid particles 0.1-50 microns in diameter. Particles less than 50 microns cannot be seen without a microscope
Mist
Aerosol of liquid particles suspended in air
Fog
Visible aerosol of a liquid formed by condensation
Expansion ratio
- Volume of a substance in liquid form compared to the volume of the same number of molecules of that substance in gaseous form
- Ratio of the finished foam volume to the volume of the original foam solution
International system of units (SI)
Modern form of the metric system of measurement that standardizes mathematical quantification
Pascals (Pa)
SI unit of measure used to indicate internal pressure and stress on a container
Millimeters of mercury (mmHg)
Unit of pressure measurement; not part of the SI currently defined as a rate rounded to 133 pascals. Rough equivalent to 1 torr
Bar
Unit of pressure measurement; not part of the SI. Equals 100,000 Pa
Torr
Unit of pressure measurement; not part of the SI. Measured as 1/760 of a standard atmosphere
Liquified gas
Confined gas that at normal temperatures exists in both liquid and gaseous states
Anhydrous
Materials containing no water
Hydrophobic
Material that is incapable of mixing with water
Hydrophilic
Material that is attracted to water. This material may also dissolve or mix in water
Density
Mass per unit of volume of a substance; obtained by dividing the mass by the volume
Specific gravity
Mass (weight) of a substance compared to the weight of an equal volume of water at a given temperature. A specific gravity less than one indicates a substance lighter than water; a specific gravity greater than one indicates a substance heavier than water
Vapor density
Weight of pure vapor or gas compared to the weight of an equal volume of dry air at the same temperature and pressure. A vapor density less than one indicates a vapor lighter than air; a vapor density greater than one indicates a vapor heavier than air
Molecular weight (MW)
Average mass of one molecule. This can be calculated as the sum of the atomic masses of the component atoms
Viscosity
Measure of a liquid’s internal friction at a given temperature. This concept is informally expensed as thickness, stickiness, and ability to flow
Safely data sheet (SDS)
Reference material that provides information on chemicals that are used, produced, or stored at facility. Form is provided by chemical manufacturers and blenders; contains information about chemical composition, physical and chemical properties, health and safety hazards, emergency response procedures, and waste disposal procedures
Celsius scale
International temperature scale on which the freezing point is 0C (32F) and the boiling point is 100C (212F) at normal atmospheric pressure at sea level
Fahrenheit scale
Temperature scale on such the freezing point is 32F (0C) and the boiling point at sea level is 212F (100C) at normal atmospheric pressure
Flash point
Minimum temperature at which a liquid gives off enough vapors to form an ignitable mixture with air near the surface of the liquid
Flammable liquid
Any liquid having a flash point below 100F (7.8C) and a vapor pressure not exceeding 40 psi absolute (276 kPa, 2.76 bar), per NFPA
Combustible liquid
Liquid having a flash point at or above 100F (37.8C) and below 200F (93.3C), per NFPA
Flammability
Fuel’s susceptibility to ignition
Flammable range
Range between the upper flammable limit and lower flammable limit in which a substance can be ignited
Lower flammable (explosive) limit (LFL)
Lower limit at which a flammable gas or vapor will ignite and support combustion; below this limit the gas or vapor is too lean or thin to burn (too much oxygen and not enough gas, so lacks the proper quantity of fuel)
Upper flammable (explosive) limit (UFL)
Upper limit at which a flammable gas or vapor will ignite; above this limit the gas or vapor is too rich to burn (lack the proper quantity of oxygen)
Oxidizer
Any material that readily yields oxygen or other oxidizing gas, or that readily reacts to promote or initiate combustion of combustible materials
Phase
Distinguishable part in a course, development, or cycle; aspect or part under consideration. In chemistry, a change off phase is marked by a shift in the physical state of a substance caused by a change in heat
Melting point
Temperature at which a solid substance changes to a liquid state at normal atmospheric pressure
Freezing point
Temperature at which a liquid becomes a solid at normal atmospheric pressure
Boiling point
Temperature of a substance when the vapor pressure equals atmospheric pressure. At this temperature, the rate of evaporation exceeds the rate of condensation. At this point, more liquid is turning into gas than gas is turning back into a liquid
Evaporation
Process of a solid or liquid turning into gas
Evaporation rate
Speed at which some material changes from a liquid to a vapor. Materials that change readily to gases are considered volatile
Volatility
Ability of a substance to vaporize easily at a relatively low temperature
Condensation
Process of a gas turning into a liquid state
Sublimation
Vaporization of a material from the solid to vapor state without passing through the liquid state
Critical point
The end point of an equilibrium curve. In liquid and vapor response, the conditions under which liquid and its vapor can coexist
Critical temperature
The minimum temperature above which a gas cannot Ben liquefied no matter how much pressure is applied
Critical pressure
The pressure necessary to liquefy a gas at its critical temperature
Auto ignition temperature
The lowest temperature at which a substance will ignite in air when there is no ignition source
Self-accelerating decomposition temperature (SADT)
The temperature above which the decomposition of an unstable substance continues unimpeded, regardless of the ambient or external temperature
Maximum safe storage temperature (MSST)
The maximum safe temperature at which a product can be stored. This temperature is well below the SADT
Polymerization
A special chemical reaction in which small-molecules compounds call monomers react with themselves to form larger molecules call polymers
Atom
The smallest complete building block of ordinary matter in any state
Nucleus
The positively charged central part of an atom, consisting of protons and neutrons
Proton
Subatomic particle with a physical mass and a positive electric charge
Neutron
Component of the nucleus of an atom that has a neutral electrical charge yet produces highly penetrating radiation; ultra high energy particle that has a physical mass but no electrical charge
Electron
Subatomic particle with a physical mass and a negative electric charge
Shell
Layer of electrons that orbit the nucleus of an atom. The innermost shell can hold up to two electrons, and each subsequent shell can hold eight
Atomic number
Number of protons in an atom
Atomic weight
Physical characteristic relating to the mass of molecules and atoms. A relative scale for atomic weights has been adopted, in which the atomic weight of carbon has been set at 12, although its true atomic weight is 12.01115
Compound
Substance consisting of two or more elements that have been united chemically
Reactive material
Substance capable of chemically reacting with other substances; for example, material that reacts violently when combined with air or water
Mixture
Substance containing two or more materials not chemically united
Solution
Uniform mixture composed of two or more substances
Slurry
Suspension formed by a quantity of granulated or powdered solid material that is not completely soluble mixed into a liquid
Alloy
Substance or mixture composed of 2 or more metals (or a metal & nonmetallic elements) fused together & dissolved into each other to enhance the properties or usefulness of the base metal
Periodic table of elements
Organizational chart showing chemical elements arranged in order by atomic number, electron configuration, and chemical properties
Atomic stability
Condition where an atom has a filled outer shell and is not seeking electrons. Stable atoms also have the same number of protons and electrons
Duet rule
Atoms with only one shell will attempt to maintain two electrons to fill the outer shell at all times, whether by gaining or losing electrons. A complete outer electron shell makes elements very stable
octet rule
Atoms with two or more shells will attempt to maintain eight electrons to fill the outermost shell at all times, whether by gaining or losing electrons. A complete outer electron shell makes elements very stable
Unstable material
Materials that are capable of undergoing chemical changes or that can violently decompose with little or no outside stimulus
Diatomic molecules
Molecules composed of only two atoms that may or may not be the same element
Covalent bond
Chemical bond formed between two or more non metals. This chemical bond results in a nonsalt
Ionic bond
Chemical bond formed by the transfer of electrons from a metal element to a nonmetal element. This chemical bond results in two oppositely charged ions
Ion
Atom that has lost or gained an electron, thus giving it a positive or negative charge
Cation
Atom or group of atoms carrying a positive charge
Anion
Atom or group of atoms carrying a negative charge
Resonant bond
Type of chemical bond in which electrons move freely between the compound atoms
Bond energy
The amount of energy needed to break covalent bonds
Exothermic reaction
Chemical reaction between two or more materials that changes that materials and produces heat
Endothermic reaction
Chemical reaction in which a substance absorbs heat energy
Hypergolic
Substance that ignites when exposed to another substance
Air-reactive material
Substance that reacts or ignites when exposed to air at normal temperatures.
Water-reactive material
Substance, generally a flammable solid, that reacts when mixed with water or exposed to humid air
Oxidation-reduction (redox) reaction
Chemical reaction that results in a molecule, ion, or atom gaining or losing an electron
Reducing agent
Due that his being oxidized or burned during combustion
Oxidizing agent
Substance that oxidizes another substance; can cause other materials to combust more readily or make fires burn more strongly
Oxidation
Chemical process that occurs when a substance combines with an oxidizer such as oxygen in the air; a common example is the formation of rust on metal
Polymerization
Chemical reactions in which two or more molecules chemically combine to form larger molecules; this reaction can often be violent
Monomer
A molecule that may bind chemically to other molecules to form a ploymer
Catalyst
Substance that modifies (usually increases) the rate of a chemical reaction without being consumed int he process
Inhibitor
Material that is added to products that easily polymerize in order to control or prevent an undersized reaction
Decomposition
Chemical change in which a substance breaks down into two or more simpler substances. Result of oxygen acting on a material that results in a change in the material’s composition; oxidation occurs slowly, sometimes resulting in the rusting of metals
Synergistic effect
Phenomenon in which the combined properties of substances have an effect greater than their simple arithmetic all sum of effects
Concentration
- Percentage (mass or volume) of a material dissolved in water (or other solvent)
- Quantity of a chemical material inhaled for purposes of measuring toxicity
Soluble
Capable of being dissolved in a liquid (usually water)
Solubility
Degree to which a solid, liquid, or gas dissolves in a solvent (usually water)
Polar solvents
- A material in which the positive and negative charges are permanently separated, resulting in their ability to ionize in solution and create electrical conductivity. Example include water, alcohol, esters, ketones, amines, and sulfuric acid
- Flammable liquids with an attraction for water
Miscible
Materials that are capable of being mixed in all proportions
Miscibility
Two or more liquids’ capability to mix together
Immiscible
Incapable of being mixed or blended with another substance
Polarity
Property of some molecules to have discrete areas with negative and positive charges
Water solubility
Ability of a liquid or solid to mix with or dissolve in water
Hydrocarbon
Organic compound containing only hydrogen and carbon and found primarily in petroleum products and coal
Alkane
A saturated hydrocarbon, with hydrogen in every possible location. All bonds are single bonds
Alkene
An unsaturated hydrocarbon with at least one double bond between carbon atoms
Alkyne
An unsaturated hydrocarbon with at least one triple bond
Aromatic hydrocarbon
A hydrocarbon with bonds that form rings
Maximum safe storage temperature (MSST)
Temperature below which the product can be stored safety. This is usually 20-30 degrees cooler than the SADT temperature, but may be more depending on the material
Self-accelerating decomposition temperature (SADT)
Lowest temperature at which product in a typical package will undergo a self-accelerating decomposition. The reaction can be violent, usually rupturing the package, dispersing original material, liquid and/or gaseous decomposition products considerable distances
Photonioization detector (PID)
Gas detector that measures volatile compounds in concentrations of parts per million and parts per billion
Acid
Compound containing hydrogen that reacts with water to produce bydronium ions; a proton donor; a liquid compound with a pH less than 7. Acidic chemicals are corrosive
Dissociation (chemical)
Process of splitting a molecule or ionic compounds into smaller particles, especially if the process is reversible
Base
Any alkaline or caustic substance; corrosive water-soluble compound or substance containing group-forming hydroxide ions in water solution that reacts with an acid to form a salt
Chemical burn
Injury caused by contact with acids, lye, and vesicants such as tear gas, mustard gas, and phosphorus
Thermal burn
- Injury caused by contact with flames, hot objects, and hot fluids; examples. Include scales and steam burns
- Any injury to living tissue from contact with extreme hot or cold materials
Radioactive material (RAM)
Material with an atomic nucleus that spontaneously decays or disintegrates, emitting radiation as particles or electromagnetic waves at a rate of greater than 0.002 microcuries per gram Ci/g)
Ionizing radiation
Radiation that causes a chemical change in atoms by removing their electrons
Nonionizing radiation
Series of energy waves composed of oscillating electric and magnetic fields traveling at the speed of light. Examples include ultraviolet radiation, visible light, infrared radiation, microwaves, radio waves, and extremely low frequency radiation
Ionize
Process in which an atom or molecule gains a negative or positive charge by gaining or losing electrons
Radioactive decay
Process in which an unstable radioactive atom loses energy by emitting ionizing radiation and conversion electrons
Radioisotope
Unstable atom that releases nuclear energy
Transmutation
Conversion of one element or isotope into another form or state
Half-life
The time required for a radioactive material to reduce to half of its initial value
Activity
Rate of decay of the isotope in terms of decaying atoms per second. Measured in becquerels (Bq) for small quantities of radiation, and curies (Ci) for large quantities of radiation
Bacquerel (Bq)
International system unit of measurement for radioactivity, indicating the number of nuclear decays/disintegration’s a radioactive material undergoes in a certain period of time