Classification of Matter
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| Pure substance | a uniform substance made up of one type of particle, which can be either an element or a compound.
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| Matter | anything that has mass and takes up space
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| Element | A pure substance that cannot be broken down by normal chemical or physical means.
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| Mixture | two or more substances that are combined physically but not chemically
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| Oxygen | Discovered by Swedish chemist Karl Scheele and English chemist Joseph Priestley. The most common element in Earth’s crust.
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| Allotropes | Different forms of the same element in the same physical state of matter. They contain only one type of atom but the way the atoms are arranged is different.
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| Compound | A pure substance made up of two or more elements joined in a defined ratio.
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| Tin | One of the first metals used by humans. It is a silvery white metal that is very malleable.
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| ternary compound | made up of three different elements
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| binary compound | made up of two different elements
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| Homogeneous mixture | A type of mixture that appears uniform throughout. The components are mixed evenly (like apple juice).
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| Dalton's Law | The total pressure of a mixture of gases equals the sum of the pressures of the gases in the mixture, with each gas acting independently.
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| Solute | The substance that is dissolved in the solution.
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| Solution | a homogeneous mixture in which one or more substances (solutes) are dissolved in another substance (solvent).
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| soluble | A substance that dissolves in another substance.
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| solvent | The substance that the solute is dissolved in.
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| Heterogeneous mixture | A type of mixture in which the components are not mixed evenly or uniformly distributed throughout.
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| nonpolar | A substance that does not dissolve
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| Physical property | a property of matter that can be observed without changing the substance into another substance
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| coalescence | The process in which small droplets recombine to form bigger ones.
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| solids | have a definite volume and a definite shape, the particles are locked into place
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| chemical property | determined by the ability of a substance to react with or change into another substance (such as toxicity, flammability or reactivity)
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| Amorphous solids | made up of atoms or molecules that are locked into place. The atoms or molecules do not organize into a specific form.
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| Crystalline solids | made up of atoms or molecules that are organized in specific repeating patterns. These regular, repeating patterns form crystals.
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| Viscosity | a property of liquids that describes the “thickness” of the material
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| Liquids | have a definite volume but no definite shape
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| Gases | Have no definite volume and no definite shape.
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| Surface tension | A property of liquids that describes the attraction of liquid molecules at the surface.
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| Molecular mass | the mass of one molecule of a substance
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| effusion | the movement of gas particles through a small hole in a container from an area of high pressure to an area of low pressure (a balloon deflating over time)
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| Plasma | ionized gas. Some electrons in plasma atoms are free. This means they are not bound to an atom or a molecule
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| diffusion | the movement of particles from an area of high concentration to an area of low concentration
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| Melting | a change in state from a solid to a liquid
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| Physical change | any change in a substance’s form that does not change its chemical makeup (tearing or cutting a piece of paper)
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| Freezing | a change in state from a liquid to a solid.
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| Melting point | the temperature at which a substance begins to change from a solid to a liquid
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| Vaporization | a change in state from a liquid to a gas. The two main types of vaporization are evaporation and boiling.
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| Freezing point | The temperature at which a liquid begins to form a solid. The substance will remain at that temperature until freezing is complete.
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| Boiling | A vaporization process in which a liquid changes to a gas both below the surface and at the surface of the liquid.
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| Evaporation | a vaporization process that occurs at the surface of a liquid
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| Condensation | a change of state from a gas to a liquid
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| Boiling point | the temperature at which a liquid begins to form a gas.
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| Sublimation | a change of state directly from a solid to a gas (does not pass through a liquid state)
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| Dew point | The temperature at which a gas begins to condense into a liquid.
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| Chemical change | a change that takes place when atoms of a substance are rearranged.
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| Deposition | a change of state directly from a gas to a solid
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| Law of conservation of energy | energy can change from one form to another, but it cannot be created or destroyed
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| Thermal energy | the total energy of the particles in an object that responds to changes in temperature
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| Kinetic energy | energy of motion, the faster an object is moving, the more kinetic energy it has
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| Mechanical energy | It is determined by the motion or position of an object. The sum of its kinetic and potential energy.
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| Exothermic change | a change that gives off energy, releasing energy to its surroundings (any burning reaction)
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| Potential energy | stored energy (a ball at the top of a hill)
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| Separation process | a process that divides a mixture into two or more different parts (using a magnet to separate iron or a screen to separate pebbles)
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| Endothermic change | a change that takes energy from its surroundings (the formation of nitrous oxide)
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| filtrate | The collected liquid
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| filtration | a way of separating a mixture based on differences in size between the particles that make up different parts of the mixture (filter paper)
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| Precipitate | the solid that forms from the solution
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| precipitation | a means of separating a component in a solution by reacting it with another substance to form a solid
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