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134 Cards in this Set
- Front
- Back
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Chemical |
A substance that has the same composition and properties wherever it is found. (Pg.21) |
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Chemistry |
The study of the composition, structure, properties, and reactions of matter. (Pg. 21) |
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Conclusion |
An explanation of an observation that has been validated by repeated experiments that support a hypothesis. (Pg.21) |
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Experiment |
A procedure that tests the validity of a hypothesis. (Pg.21) |
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Hypothesis |
An unverified explanation of a natural phenomenon. (Pg.21) |
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Observation |
Information determined by noting and recording a natural phenomenon. (Pg.21) |
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Scientific notation |
A form of writing large and small numbers using a coefficient that is at least 1 but less than 10, followed by a power of 10. (Pg.21) |
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Scientific method |
The process of making observations, proposing a hypothesis, and testing the hypothesis; after repeated experiments validate the hypothesis, it may become a theory. (Pg.21) |
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Theory |
An explanation for an observation supported by additional experiments that confirm the hypothesis. (Pg.21) |
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Celsius (°C) temperature scale |
A temperature scale on which water has a freezing point of 0°C and a boiling point of 100°C. (Pg.56) |
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Centimeter (cm) |
A unit of length in the metric system; there are 2.54cm in 1inch (in). (Pg.56) |
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Conversion factor |
A ratio in which the numerator and denominator are quantities from an equality or given relationship. For example, the two conversion factors for the equality 1kg = 2.2lb are written as: 2.20lb/1kg and 1kg/2.20lb (pg.56) |
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Cubic centimeter (cm^3, cc) |
The volume of a cube that has 1-cm sides; 1cm^3 is equal to 1mL. (Pg.56) |
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Density |
The relationship of the mass of an object to it's volume expressed as grams per cubic centimeter (g/cm^3), grams per milliliter (g/mL), or grams per liter (g/L). (Pg.56) |
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Equality |
A relationship between two units that measure the same quantity. (Pg. 56) |
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Exact number |
A number obtained by counting or by definition. (Pg.56) |
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Gram (g) |
The metric unit used in measurements of mass. (Pg.56) |
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International system of units (SI) |
The official system of measurement throughout the world, except for the United States, that modified the metric system. (Pg.56) |
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Kelvin (K) temperature scale |
A temperature scale on which the lowest possible temperature is 0 K. (Pg.56) |
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Kilogram (kg) |
A metric mass of 1000g, equal to 2.20lb. the kilogram is the SI standard unit of mass. (Pg.56) |
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Liter (L) |
The metric unit for volume that is slightly larger than a quart. (Pg.56) |
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Mass |
A measure of the quantity of material in an object. (Pg.56) |
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Measured number |
A number obtained when a quantity is determined by using a measuring device. (Pg.56) |
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Meter (m) |
The metric unit of length that is slightly longer than a yard. The meter is the SI standard unit of length. (Pg.56) |
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Metric system |
A system of measurement used by scientists and in most countries of the world. (Pg.56) |
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Milliliter (mL) |
A metric unit of volume equal to one-thousandth of a liter (0.001 L). (Pg.56) |
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Prefix |
The part of the name of a metric unit that procedes the base unit and specifies the size of the measurement. All prefixes are related on a decimal scale. (Pg.56) |
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Second (s) |
A unit of time used in both the SI and metric systems. (Pg. 56) |
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SI |
See International System of Units (SI). (Pg.56) |
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Significant figures (SFs) |
The numbers recorded in a measurement. (Pg.56) |
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Specific gravity (sp gr) |
A relationship between the density of a substance and the density of water: Sp gr = density of sample/density of water (Pg.56) |
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Temperature |
An indicator of the shortness or coldness of an object. (Pg.56) |
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Volume (V) |
The amount of space occupied by a substance. (Pg.56) |
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Boiling |
The formation of bubbles of gas throughout a liquid. (Pg. 90) |
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Boiling point (bp) |
The temperature at which a liquid changes to gas (boils) and gas changes to liquid (condenses). (Pg.90) |
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Calorie (cal) |
The amount of heat energy that raises the temperature of exactly 1 g of water by exactly 1°C. (Pg.90) |
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Change of state |
The transformation of one state of matter to another; for example, solid to liquid, liquid to solid, liquid to gas. (Pg.90) |
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Chemical change |
A change during which the original substance is converted into a new substance that has a different composition and new physical and chemical properties. (Pg.90) |
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Chemical properties |
The properties that indicate the ability of a substance to change into a new substance. (Pg. 90) |
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Compound |
A pure substance consisting of two or more elements, with a definite composition, that can be broken down into simpler substances only by chemical methods. (Pg. 90) |
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Condensation |
The change of state from a gas to a liquid. (Pg.90) |
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Cooling curve |
A diagram that illustrates temperature changes and changes of state for substance as heat is removed. (Pg. 90) |
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Deposition |
The change of a gas directly into a solid; the reverse of sublimation. (Pg. 90) |
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Element |
A pure substance containing only one type of matter, which cannot be broken down by chemical methods. (Pg.90) |
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Energy |
The ability to do work. (Pg. 90) |
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Energy value |
The kilocalories (or kilojoules) obtained per gram of the food types: carbohydrate, fat, and protein. (Pg.90) |
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Evaporation |
The formation of a gas (vapor) by the escape of high-energy particles from the surface of a liquid. (Pg.90) |
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Freezing |
The change of state from liquid to solid. (Pg. 90) |
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Freezing point (fp) |
The temperature at which a liquid changes to a solid (freezes) and a solid changes to a liquid (melts). (Pg. 90) |
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Gas |
A state of matter that does not have a definite shape or volume. (Pg. 90) |
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Heat |
The energy associated with the motion of particles in a substance. (Pg.90) |
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Heat of fusion |
The energy required to melt exactly 1 g of a substance as it's melting point. For water, 80. Cal (334 J) is needed to melt 1 g of ice; 80. Cal (334 J) is released when 1 g of water freezes at 0°C. (Pg.90) |
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Heat of vaporization |
The energy required to vaporize exactly 1 g of a substance at its boiling point. For water, 540 cal (2260 J) is needed to vaporize 1 g of liquid; 1 g of steam gives off 540 cal (2260 J) when it condenses at 100°C. (Pg. 90) |
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Heating curve |
A diagram that illustrates the temperature changes and changes of state of a substance as it is heated. (Pg. 90) |
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Joule (J) |
The SI unit of heat energy; 4.184 J = 1 cal. (Pg.90) |
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Kinetic energy |
The energy of moving particles. (Pg. 90) |
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Liquid |
A state of matter that takes the shape of its container but has a definite volume. (Pg. 90) |
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Matter |
The material that makes up a substance and has mass and occupies space. (Pg.90) |
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Melting |
The change of state from a solid to a liquid. (Pg. 90) |
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Melting point (mp) |
The temperature at which a solid becomes a liquid (melts). It is the same temperature as the freezing point. (Pg.90) |
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Mixture |
The physical combination of two or more substances that are not chemically combined. (Pg. 90) |
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Physical change |
A change in which the physical properties of a substance change but it's identity stays the same. (Pg.90) |
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Physical properties |
The properties that can be observed or measured without affecting the identity of a substance. (Pg. 90) |
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Potential energy |
A type of energy related to position or composition of a substance. (Pg. 90) |
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Pure substance |
A type of matter that has a definite composition. (Pg. 91) |
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Solid |
A state of matter that has its own shape and volume. (Pg. 91) |
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Specific heat (SH) |
A quantity of heat that changes the temperature of exactly 1g of a substance by exactly 1°C. (Pg. 91) |
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States of matter |
Three forms of matter: solid, liquid, and gas. (Pg. 91) |
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Sublimation |
The change of state in which a solid is transformed directly to a gas without forming a liquid first. (Pg. 91) |
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Alkali metal |
An element in group 1A (1), except hydrogen, that is a soft, shiny metal with one electron in its outermost energy level. (Pg. 137) |
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Alkaline earth metal |
An element in group 2A (2) that has two electrons in its outermost energy level. (Pg. 137) |
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Atom |
The smallest particle of an element that retains the characteristics of the element. (Pg. 137) |
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Atomic mass |
The weighted average mass of all the naturally occurring isotopes of an element. (Pg. 137) |
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Atomic mass unit (amu) |
A small mass unit used to describe the mass of extremely small particles such as atoms and sub-atomic particles; 1 amu is equal to one-twelfth the mass of 12/6C atom. (Pg. 137) |
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Atomic number |
A number that is equal to the number of protons in an atom. (Pg. 138) |
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Atomic size |
The distance between the outermost electrons and the nucleus. (Pg. 138) |
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Atomic symbol |
An abbreviation used to indicate the mass number and atomic number of an isotope. (Pg. 138) |
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Chemical symbol |
An abbreviation that represents the name of an element. (Pg. 138) |
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d block |
The block of ten elements from groups 3B (3) to 2B (12) in which electrons fill the five d orbitals in the d sublevels. (Pg. 138) |
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Electron |
A negatively charged subatomic particle having a minute mass that is usually ignored in mass calculations; it's symbol is e^-. (Pg. 138) |
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Electron configuration |
A list of the number of electrons in each sublevel within an atom, arranged by increasing energy. (Pg. 138) |
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f block |
The block of 14 elements in the rows at the bottom of the periodic table in which electrons fill the seven f orbitals in the f sublevels. (Pg. 138) |
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Group |
A vertical column in the periodic table that contains elements having similar physical and chemical properties. (Pg.138) |
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Group number |
A number that appears at the top of each vertical column (group) in the periodic table and indicates the number of electrons in the outermost energy level. (Pg. 138) |
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Halogen |
An element in group 7A (17)- fluorine, chlorine, bromine, iodine, astatine, and tennessine- that has seven electrons in its outermost energy level. (Pg. 138) |
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Ionization energy |
The energy needed to remove the least tightly bound electron from the outermost energy level of an atom. (Pg. 138) |
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Isotope |
An atom that differs only in mass number from another atom of the same element. Isotopes have the same atomic number (number of protons), but different numbers of neutrons. (Pg. 138) |
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Lewis symbol |
The representation of an atom that shows valence electrons as dots around the symbol of the element. (Pg. 138) |
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Mass number |
The total number of protons and neutrons in the nucleus of an atom. (Pg. 138) |
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Metal |
An element that is shiny, malleable, ductile, and a good conductor of heat and electricity. The metals are located to the left of the heavy zigzag line on the periodic table. (Pg. 138) |
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Metallic character |
A measure of how easily an element loses a valence electron. (Pg. 138) |
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Metalloid |
An element with properties of both metals and nonmetals located along the heavy zigzag line on the periodic table. (Pg. 138) |
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Neutron |
A neutral subatomic particle having a mass of about 1 amu and found in the nucleus of an atom; it's symbol is n or n^0. (Pg. 138) |
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Noble gas |
An element in group 8A (18) of the periodic table, generally unreactive and seldom found in combination with other elements, that has eight electrons (helium has two electrons) in its outermost energy level. (Pg. 138) |
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Nonmetal |
An element with little or no luster that is a poor conductor of heat and electricity. The nonmetals are located to the right of the heavy zigzag line on the periodic table. (Pg. 138) |
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Nucleus |
The compact, extremely dense center of an atom, containing the protons and neutrons of the atom. (Pg. 138) |
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Orbital |
The region around the nucleus where electrons of a certain energy are most likely to be found. The s orbitals are spherical; the p orbitals have two lobes. (Pg. 138) |
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Orbital diagram |
A diagram that shows the distribution of electrons in the orbitals of the energy levels. (Pg. 138) |
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p block |
The elements in group 3A (13) to 8A (18) in which electrons fill the p orbitals in the p sublevels. (Pg. 138) |
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Period |
A horizontal row of elements in the periodic table. (Pg. 138) |
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Periodic table |
An arrangement of elements by increasing atomic number such that elements having similar chemical behavior are grouped in vertical columns. (Pg. 138) |
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Proton |
A positively charged subatomic particle having a mass of about 1 amu and found in the nucleus of an atom; it's symbol is p or p^+. (Pg. 138) |
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Representative element |
An element in the first two columns on the left of the periodic table and the last six columns on the right that has a group number 1A through 8A or 1, 2, and 13 through 18. (Pg. 138) |
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s block |
The elements in groups 1A (1) and 2A (2) in which electrons fill the s orbitals. (Pg.138) |
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Subatomic particle |
A particle within an atom; protons, neutrons, and electrons are subatomic particles. (Pg. 138) |
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Sublevel |
A group of orbitals of equal energy within an energy level. The number of sublevels in each energy level is the same as the principal quantum number (n). (Pg.138) |
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Transition element |
An element in the center of the periodic table that is designated with the letter "B" or the group number of 3 through 12. (Pg.138) |
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Valence electrons |
Electrons in the outermost energy level of an atom. (Pg. 138) |
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Alpha particle |
A nuclear particle identical to a helium nucleus, symbol a or 4/2He. (Pg.169) |
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Becquerel (Bq) |
A unit of activity of a radioactive sample equal to one disintegration per second. (Pg. 169) |
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Beta particle |
A particle identical to an electron, symbol 0/-1e or B, that forms in the nucleus when a neutron changes to a proton and an electron. (Pg. 169) |
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Chain reaction |
A fission reaction that will continue once it has been initiated by a high-energy neutron bombarding a heavy nucleus such as uranium-235. (Pg. 169) |
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Curie (Ci) |
A unit of activity of a radioactive sample equal to 3.7x10^10 disintegrations/s. (Pg.169) |
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Decay curve |
A diagram of the decay of a radioactive element. (Pg. 169) |
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Equivalent dose |
The measure of biological damage from an absorbed dose that has been adjusted for the type of radiation. (Pg.169) |
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Fission |
A process in which large nuclei are split into smaller nuclei, releasing large amounts of energy. (Pg. 169) |
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Fusion |
A reaction in which large amounts of energy are released when small nuclei combine to form larger nuclei. (Pg.169) |
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Gamma ray |
High-energy radiation, symbol 0/0y, emitted by an unstable nucleus. (Pg.169) |
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Gray (Gy) |
A unit if absorbed dose equal to 100 rad. (Pg. 169) |
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Half-life |
The length of time it takes for one-half of a radioactive sample to decay. (Pg.169) |
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Positron |
A particle of radiation with no mass and a positive charge, symbol B^+ or 0/+1e, produced when a proton is transformed into a neutron and a positron. (Pg.169) |
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Rad (radiation absorbed dose) |
A measure of an amount of radiation absorbed by the body. (Pg.169) |
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Radiation |
Energy or particles released by radioactive atoms. (Pg.169) |
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Radioactive decay |
The process by which an unstable nucleus breaks down with the release of high-energy radiation. (Pg.169) |
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Radiosotope |
A radioactive atom of an element. (Pg.169) |
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Rem (radiation equivalent in humans) |
A measure of the biological damage caused by the various kind of radiation (rad X radiation X biological factor). (Pg. 169) |
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Sievert (Sv) |
A unit of biological damage (equivalent dose) equal to 100 rem. (Pg.169) |
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How many sig figs are in: 45 |
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How many sig figs are in: 0.046 |
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How many sig figs are in: 7.4220 |
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How many sig figs are in: 5002 |
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How many sig figs are in: 3800 |
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Road map |
If the problem is asking us to convert units of measurement we need to show how we're going to be taking these steps: G/cm^3 ->->-> lb/ft^3 (1.00g/1cm^3) (1lb/454g) (2.54cm/1in)^3 (12in/ft)3 = ~62.37lb/ft^3 |
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Heating curve (picture) |
Pg. 85 |
