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Substance Element or compound that cannot be broken down into simpler components and maintain the properties of the original substance. Element Substance with atoms that are all alike. Compound Substance formed from two or more elements in which the exact combination and proportion of elements is always the same. Heterogeneous mixture Mixture, such as mixed nuts or a dry soup mix, in which different materials are unevenly distributed and are easily identified. Homogeneous mixture Solid, liquid or gas that contains two or more substances blended evenly throughout. Solution Homogeneous mixture that remains constantly and uniformly mixed and has particles that are so small they cannot be seen with a microscope. Colloid Heterogeneous mixture whose particles never settle. Suspension Heterogeneous mixture containing a liquid in which visible particles settle Physical property Any characteristic of a material, such as size or shape, that you can observe or attempt to observe without changing the identity of the material. Physical change Any change in size, shape or state or matter in which the identity of the substance remains the same. Chemical property Chemical change Any characteristic of a substance, such as flammability, that indicates whether it can undergo a certain chemical change. Change where the starting material is changed into a new substance giving or heat, light, forming a precipitate (solid), producing a gas, or changing color. Law of conservation of mass States that the mass of all substances present before a chemical change equals the mass of all the substances remaining after the change. Mass of the reactants equal the mass of the products. Kinetic theory Explanation of behavior of molecules in matter, states that all matter is made of constantly moving particles that collide without using energy. Melting point Temperature at which a solid begins to liquefy. Boiling point The temperature at which the pressure of the vapor in the liquid is equal to the external pressure acting on the surface. Plasma Matter consisting of positively and negatively charged particles. The type of matter that has the highest Kinetic energy. Atom The smallest particle of an element that still has the same properties of the element; the smallest unit of matter. Nucleus The center of an atom that contains 99.99% of an atoms mass. Proton A particle located in the nucleus of an atom that has a positive charge. Neutron A particle located in the nucleus of an atom that has no charge. You can find this particle by taking the mass number of an element minus the number of protons. Electron Particles outside of the nucleus that have a negative charge. Solid The state of matter that has a definite volume and a definitive shape. It also has the lowest kinetic energy out of all of the four states of matter. Liquid The state of matter that has a definite volume but no definite shape. Atomic number Number of protons in an atom’s nucleus. Mass number Sum of the number of protons and neutrons in an atoms nucleus. Isotope Atoms of the same element that have different number of neutrons. Average atomic mass Weighted average mass of the mixture of an element’s isotopes. Periodic table Organized list of all known elements that are arranged by increasing atomic numbers and by their physical and chemical properties. Group Vertical row on the periodic table Period Horizontal row on the periodic table. Gas The state of matter that has no definite volume or shape. Strong force Attractive force that acts between protons and neutrons to form the nucleus of an atom Radioactivity Process that occurs when a nucleus decays and emits alpha, beta or gamma radiation. Alpha particle Particle consisting of two protons and two neutrons that is emitted from a decaying atomic nucleus, whose energy can be stopped by a piece of paper. Transmutation The process of changing one element into another through radioactive decay. Beta particle Electron that is emitted from a decaying atomic nucleus that has an energy that can be stopped by lead that is 1 cm thick. Gamma ray Electromagnetic wave with no mass and no charge that travels the speed of light and has an energy that can be stopped by a concrete wall. Half-life Amount of times it takes for half the nuclei in a sample of a radioactive isotope to decay. Endothermic Reaction A reaction where the products absorb energy, such as a nail collecting rust. Exothermic Reaction A reaction where the products release energy into the atmosphere be means of heat, light or gas. Geiger counter Radiation detector that produces a click or flash of light when a charged particle is detected. Nuclear fission Process of splitting an atomic nucleus into two or more nuclei with smaller masses. Nuclear fusion Reaction in which two or more atomic nuclei form a nucleus with a larger mass. Chain reaction Ongoing series of fission reactions. Critical mass Amount of fissionable material required so that each fission reaction produces approximately one more fission reaction. Metal Element that typically is a hard, shiny solid, is malleable, and is a good conductor of heat and electricity. Malleable The ability of metals to be hammered or rolled into thin sheets. Ductile The ability of metals to be drawn into wires. Sublimation Going from a solid directly to a gas. Dry Ice is a well known example of this. Salt Compound formed when negative ions from an acid combine with positive ions from a base. Metalloid An element that shares some properties with metals and other properties with non-metals. Usually used when building computers. Chemical formula Chemical shorthand that uses symbols to tell what elements are in a compound and their ratios. Chemical bond The force that holds atoms together in a compound Ion A charged particle that has either fewer or more electrons than protons. Ionic bond A type of bond where the attraction formed between oppositely charged ions transfer electrons to form a stable bond. Covalent bond A type of bond where the attraction formed between atoms share electrons. Molecule A neutral particle that forms as a result of electron sharing. Oxidation number Positive or negative number that indicates how many electrons an atom has to gain, lose, or share in order to become stable. Chemical reaction The process in which one or more substances are changed into new substances. Reactant In a chemical equation, the substance that reacts. Solute The part of a solution that is dissolved by the solvent. Solvent A part of a solution that dissolves the solute. Solution Homogeneous mixture of two or more substances. An example would be salt water. Product In a chemical reaction, the new substance that is formed. Synthesis Reaction Chemical reaction in which two or more substances combine to form a different substance A + B AB Decomposition Reaction Chemical reaction in which one substance breaks down into two or more substances. AB A + B Single Replacement Reaction A chemical reaction in which one element replaces another element in a compound A + BC AC + B Double Replacement Reaction Chemical reaction that where both beginning elements replace each other to form new products. AC + BD AD + BC Base A compound that has a pH over 7 and tends to feel slippery, be corrosive and cause burns. Neutral Solution A solution that has a pH of 7. An example is pure water. Acid A compound that has a pH under 7 and tends to taste sour, and cause burns. Chemical equation Shorthand method to describe chemical reactions using chemical formulas and other symbols. Coefficient Number in a chemical equation that represents that number of units of each substance taking part in a chemical reaction.