Filtration: A purification procedure in which solid particles are separated form a liquid by passing the mixture through a material that retains the solid particles and allows the liquid to pass through.
Filtrate: The liquid collected after it has been filtered.
Adsorbs: Attracts and holds on its surface, many substances that could give water a bad taste.
Percent Recovery: The percent of original foul water sample that is recovered as purified water.
Histogram: A graph or chart that shows the percent recovery obtained by all laboratory groups.
Range: The difference between the largest and smallest values in a data set.
Average or Mean: Value by adding all values together and dividing the sum by the total number of values.
Median: The middle value.
Electrical Conductivity: The focus on the presence of dissolved, electrically charged particles in the water.
Direct Water Use: The approximate volume represents that which can be directly measured.
Indirect Water Use: Hidden uses of water that may have never been considered.
Gaseous State: Water vapor in the air.
Liquid State: In lakes, rivers, oceans and rain.
Solid State: Ice is a common example.
Surface Water: If your home's water supply originated in a river or other body of water.
Groundwater: If your home's water supply originated in a well (it must be pumped to the surface).
Aquifer: A water-bearing layer of rock, sand, or gravel.
Matter: anything that occupies space and has mass. Examples are all solids, liquids and gases.
Physical Properties: Properties that can be observed and measured without changing the chemical makeup of the substance. Examples include, density, melting point, freezing point, and boiling point.
Density: The mass of material within a given volume.
Freezing Point: Another physical property.
Aqueous Solution: A water-based solution that is based on the Latin root for water.
Mixture: The result of when two or more substances combine and yet the substances retain their individual properties. Examples are homogeneous and heterogeneous mixtures.
Heterogeneous Mixture: Not the same or uniform composition. Examples are suspensions and colloids.
Suspension: A type of heterogeneous mixture that blocks light; often large, visible particles that tend to settle.
Tyndall Effect: The scattering of light.
Colloid: Often suspended microscopic particles; exhibit Tyndall effect.
Homogeneous Mixture: A mixture that is uniform throughout.
Solutions: Homogeneous mixtures that are often molecular sized particles that pass light.
Solute: The dissolved substance.
Solvent: The dissolving agent.
Particulate Level: The investigation of something at the level of its atoms and molecules.
Atoms: The building blocks of matter.
Element: Matter that is made up of only one kind of atom. Examples are oxygen and hydrogen.
Compound: Two or more atoms chemically bonded. Example is water. (More specific: a molecular compound)
Chemical Formulas: Compounds and elements
Substance: Homogeneous, definite composition and not physically separable. Examples are compounds and elements.
Molecule: The smallest unit of a molecular compound that retains the properties of that substance.
Macroscopic: A world filled with large-scale, readily observed things.
Models: Representations.
Chemical Symbols: The letters in this language's alphabet which are understood by scientists throughout the world.
Periodic Table of the Elements: All known elements are organized here. This is one of the most useful tools in a chemist's world.
Chemical Formula: Represents a different chemical substance.
Subscript: A number written below the normal line of letters, which indicates how many atoms of the element just to the left of the subscript are in one unit of the substance. Example: H2O
Chemical Equations: Chemical sentences that summarize the details of a particular reaction.
Chemical Reactions: Entail the breaking and forming of chemical bonds, causing atoms to become rearranged into new substances that have different properties from those of the original materials.
Reactants: The original (starting) substances in a chemical reaction.
Products: The new substance or substances formed from the rearrangement of the reactant atoms.
Diatomic Molecules: A handful of elements that exist as two bonded atoms of the same element.
Electrons: Negatively charged particles.
Protons: Positively charged particles.
Neutrons: Electrically neutral particles.
Ions: Electrically charged atoms or groups of atoms.
Ionic Compounds: Substances that are composed of positive and negative ions.
Anion: A negatively charged ion.
Cation: A positively charged ion.
Polyatomic Ion: An ion consisting of a group of bonded atoms.
Confirming Tests: A positive test that confirms that the ion in question is present.
Qualitative Tests: Tests that identify the presence or absence of a particular substance in a sample.
Quantitative Tests: Tests that determine the amount of a specific substance present in a sample.
Reference Solution: A solution of known composition used as a comparison.
Data: Objective pieces of information.
Saturated: Undissolved as a solid.
Solubility: The maximum quantity of a substance that will dissolve in a certain quantity of water at a specified temperature.
Solubility Curve: The graphical representation of this relationship is the solutes _______.
Unsaturated Solution: A solution that contains less dissolved solute than the amount that the solvent can normally hold at that temperature.
Supersaturated Solution: An unstable solution that contains more solute than could usually be dissolved at that temperature.
Polar Molecule: Uneven distribution of electrical charge, which means that each molecule has a partial positive region at one end and a partial negative region at the other end.
Concentration: How much solute is dissolved in a specific quantity of solvent or solution.
Percent: A way to express concentration; means parts solute per hundred total parts (solute plus solvent).
Parts Per Million (PPM): For solutions containing considerably smaller quantities of solute.
Parts Per Billion (PPB): For very low concentration.
Heavy-Metal Ions: Called "heavy metals" because their atoms have greater masses than those of essential metallic elements, are harmful to humans and other organisms.
Green Chemistry: Prevent pollution by eliminating the production and use of hazardous substances.
pH Scale: A convenient way to measure and report the acidic, basic, or chemically neutral character of a solution.
Alkaline: Basic pH solutions.
Acids: Made up of molecules including one or more hydrogen atoms including one or more hydrogen atoms that can be released rather easily in water solution.
Bases: Ionic substances
Molecular Substances: Substances that are composed of molecules.
Electronegativity: The ability of an element's atoms to attract shared electrons when bonding within a compound.
Unit 2 Vocab List:
Physical Properties: Color, density, and odor; properties that can be determined without altering the chemical makeup of the material.
Physical Change: The material remains the same, although its form appears to have changed.
Chemical Change: When a substance changes into one or more new substances.
Chemical Properties: Relate to any kind of chemical changes a substance undergoes, often determine the substances usefulness.
Combustion: Burning.
Luster: Shiny and reflect light.
Ductile: Can be drawn into wires
Metals: Include such elements as iron (Fe), tin (Sn), Zinc (Zn), and copper (Cu); have a luster, are malleable and conduct electricity; some react with acids as well as copper(II) and chloride solution.
Nonmetals: Carbon (C) and oxygen (O) are examples; usually are dull in appearance, are brittle, and do not conduct electricity.
Metalloids: Have properties that are intermediate to those of metals and nonmetallic properties. Examples are silicon (Si) and germanium (Ge).
Conductor: If the bulb lights, even dimly, electricity is flowing through the sample.
Nonconductor: If the bulb fails to light.
Malleable: Flatten without shattering.
Brittle: Shatters into pieces.
Atomic Number: The number of protons in an atom.
Nucleus: A concentrated region of positive charge (due to protons) in the center of an atom.
Mass Number: The total number of protons and neutrons in the nucleus of an atom.
Isotopes: Atoms with the same number of protons but different numbers of neutrons.
Periods: Horizontal rows.
Group or Family: Each vertical column in the periodic table.
Noble Gas Family: The right side of the table which consists of very unreactive (or even chemically inert) elements.
Halogen Family: The group containing fluorine, chlorine, and bromine-in the column just to the left of noble gases.
Atmosphere: Provides nitrogen, oxygen, neon, and argon.
Hydrosphere: Water and some dissolved minerals.
Lithosphere: The solid part of earth which provides the greatest variety of chemical resources. Examples are petroleum and metal-bearing ores.
Ore: A naturally occurring rock or mineral that can be mined and from which it is profitable to extract a metal or other material.
Minerals: Naturally occurring solid compounds containing the element or group of elements of interest.
Ductility: Ease of being drawn into thin wires.
Activity Series: Ranking elements in order of their chemical reactivities.
Reduction: Any chemical change in which a reactant can be considered to gain one or more electrons.
Reduced: Like reduction.
Oxidation: A reverse reaction in which an ion or other species can be considered to lose one or more electrons.
Oxidized: Any reactant that appears to lose one or more electrons is said to be _______.
Oxidation-Reduction Reactions/Redox Reactions: Oxidation and reduction occur together.
Reducing Agent: A reactant that provides electrons.
Electron-Dot Structure/Dot Structure: The resulting expression.
Oxidizing Agent: The species involved in removing electrons from the oxidized reactant.
Law of Conservation of Mater: Matter is neither created nor destroyed.
Balanced Chemical Equation: The number of atoms of each element is the same on the reactant side and product sides.
Coefficients: Indicate the relative number of units of each substance involved in the chemical reaction.
Formula Unit: This term is used when referring to the smallest unit of an ionic compound.
Mole: (symbolized mol) a counting unit; dozen; 6.02 X 10^23.
Molar Mass: The atomic weights of elements can be used to find the mass of one mole of any substance.
Percent Composition: The percent by mass of each material found in an item such as a coin.
Renewable Resources: Resources that can be replenished by natural processes; examples are animals, plants, fresh water and air, and fertile soil.
Nonrenewable Resources: Resources that cannot be readily replenished; examples are petroleum, natural gas, coal, metals, and oil.
Allotropes: Different forms of an element that each have distinctly different physical or chemical properties; examples are diamonds, graphite, and buckmisterfullerene.
Alloy: A solid combination of atoms of two or more metals.
Superconductivity: The ability to conduct an electric current without any electrical resistance.
Semi-Conductors: Somewhere in between metals and nonmetals; metalloids are semi-conductors.
Unit 3 Vocab List:
Crude Oil: Petroleum pumped from underground.
Hydrocarbons: Molecular compounds that only contain atoms of hydrogen and carbon.
Distillation: The separation of liquid substances according to their differing boiling points. Heating the components causes the one with the lower boiling point to vaporize and leave the distillation flask and then it will condense back to a liquid as it passes through a condenser.
Distillate: Each condensed liquid compound.
Fractions: Several distintive mixtures.
Fractional Distillation: The process of separating through large-scale oil refining.
Intermolecular Forces: Forces of attraction between molecules.
Carbon Chain: In hydrocarbon molecules, carbon atoms are joined to form this backbone where hydrocarbons are attached.
Valence Electrons: The electrons within an atom's unfilled outer shell.
Covalent Bond: The chemical bond formed between two atoms that share a pair of electrons.
Structural Formula: Another common representation of a covalently bonded molecule.
Alkanes: A series of hydrocarbons.
Molecular Formulas: Specify the number of each atom type within a molecule.
Condensed Formulas: More useful than molecular formulas.
Straight-Chain Alkanes: Each carbon atom is only linked to one or two other carbon atoms.
Branched-Chain Alkanes: One carbon atom can be linked to three or four other carbon atoms.
Structural Isomers: Molecules that have identical molecular formulas but different arrangements of atoms.
Matter: anything that occupies space and has mass. Examples are all solids, liquids and gases.
Physical Properties: Properties that can be observed and measured without changing the chemical makeup of the substance. Examples include, density, melting point, freezing point, and boiling point.
Density: The mass of material within a given volume.
Freezing Point: Another physical property.
Aqueous Solution: A water-based solution that is based on the Latin root for water.
Mixture: The result of when two or more substances combine and yet the substances retain their individual properties. Examples are homogeneous and heterogeneous mixtures.
Heterogeneous Mixture: Not the same or uniform composition. Examples are suspensions and colloids.
Suspension: A type of heterogeneous mixture that blocks light; often large, visible particles that tend to settle.
Tyndall Effect: The scattering of light.
Colloid: Often suspended microscopic particles; exhibit Tyndall effect.
Homogeneous Mixture: A mixture that is uniform throughout.
Solutions: Homogeneous mixtures that are often molecular sized particles that pass light.
Solute: The dissolved substance.
Solvent: The dissolving agent.
Particulate Level: The investigation of something at the level of its atoms and molecules.
Atoms: The building blocks of matter.
Element: Matter that is made up of only one kind of atom. Examples are oxygen and hydrogen.
Compound: Two or more atoms chemically bonded. Example is water. (More specific: a molecular compound)
Chemical Formulas: Compounds and elements
Substance: Homogeneous, definite composition and not physically separable. Examples are compounds and elements.
Molecule: The smallest unit of a molecular compound that retains the properties of that substance.
Macroscopic: A world filled with large-scale, readily observed things.
Models: Representations.
Chemical Symbols: The letters in this language's alphabet which are understood by scientists throughout the world.
Periodic Table of the Elements: All known elements are organized here. This is one of the most useful tools in a chemist's world.
Chemical Formula: Represents a different chemical substance.
Subscript: A number written below the normal line of letters, which indicates how many atoms of the element just to the left of the subscript are in one unit of the substance. Example: H2O
Chemical Equations: Chemical sentences that summarize the details of a particular reaction.
Chemical Reactions: Entail the breaking and forming of chemical bonds, causing atoms to become rearranged into new substances that have different properties from those of the original materials.
Reactants: The original (starting) substances in a chemical reaction.
Products: The new substance or substances formed from the rearrangement of the reactant atoms.
Diatomic Molecules: A handful of elements that exist as two bonded atoms of the same element.
Electrons: Negatively charged particles.
Protons: Positively charged particles.
Neutrons: Electrically neutral particles.
Ions: Electrically charged atoms or groups of atoms.
Ionic Compounds: Substances that are composed of positive and negative ions.
Anion: A negatively charged ion.
Cation: A positively charged ion.
Polyatomic Ion: An ion consisting of a group of bonded atoms.
Confirming Tests: A positive test that confirms that the ion in question is present.
Qualitative Tests: Tests that identify the presence or absence of a particular substance in a sample.
Quantitative Tests: Tests that determine the amount of a specific substance present in a sample.
Reference Solution: A solution of known composition used as a comparison.
Data: Objective pieces of information.
Saturated: Undissolved as a solid.
Solubility: The maximum quantity of a substance that will dissolve in a certain quantity of water at a specified temperature.
Solubility Curve: The graphical representation of this relationship is the solutes _______.
Unsaturated Solution: A solution that contains less dissolved solute than the amount that the solvent can normally hold at that temperature.
Supersaturated Solution: An unstable solution that contains more solute than could usually be dissolved at that temperature.
Polar Molecule: Uneven distribution of electrical charge, which means that each molecule has a partial positive region at one end and a partial negative region at the other end.
Concentration: How much solute is dissolved in a specific quantity of solvent or solution.
Percent: A way to express concentration; means parts solute per hundred total parts (solute plus solvent).
Parts Per Million (PPM): For solutions containing considerably smaller quantities of solute.
Parts Per Billion (PPB): For very low concentration.
Heavy-Metal Ions: Called "heavy metals" because their atoms have greater masses than those of essential metallic elements, are harmful to humans and other organisms.
Green Chemistry: Prevent pollution by eliminating the production and use of hazardous substances.
pH Scale: A convenient way to measure and report the acidic, basic, or chemically neutral character of a solution.
Alkaline: Basic pH solutions.
Acids: Made up of molecules including one or more hydrogen atoms including one or more hydrogen atoms that can be released rather easily in water solution.
Bases: Ionic substances
Molecular Substances: Substances that are composed of molecules.
Electronegativity: The ability of an element's atoms to attract shared electrons when bonding within a compound.
Unit 2 Vocab List:
Physical Properties: Color, density, and odor; properties that can be determined without altering the chemical makeup of the material.
Physical Change: The material remains the same, although its form appears to have changed.
Chemical Change: When a substance changes into one or more new substances.
Chemical Properties: Relate to any kind of chemical changes a substance undergoes, often determine the substances usefulness.
Combustion: Burning.
Luster: Shiny and reflect light.
Ductile: Can be drawn into wires
Metals: Include such elements as iron (Fe), tin (Sn), Zinc (Zn), and copper (Cu); have a luster, are malleable and conduct electricity; some react with acids as well as copper(II) and chloride solution.
Nonmetals: Carbon (C) and oxygen (O) are examples; usually are dull in appearance, are brittle, and do not conduct electricity.
Metalloids: Have properties that are intermediate to those of metals and nonmetallic properties. Examples are silicon (Si) and germanium (Ge).
Conductor: If the bulb lights, even dimly, electricity is flowing through the sample.
Nonconductor: If the bulb fails to light.
Malleable: Flatten without shattering.
Brittle: Shatters into pieces.
Atomic Number: The number of protons in an atom.
Nucleus: A concentrated region of positive charge (due to protons) in the center of an atom.
Mass Number: The total number of protons and neutrons in the nucleus of an atom.
Isotopes: Atoms with the same number of protons but different numbers of neutrons.
Periods: Horizontal rows.
Group or Family: Each vertical column in the periodic table.
Noble Gas Family: The right side of the table which consists of very unreactive (or even chemically inert) elements.
Halogen Family: The group containing fluorine, chlorine, and bromine-in the column just to the left of noble gases.
Atmosphere: Provides nitrogen, oxygen, neon, and argon.
Hydrosphere: Water and some dissolved minerals.
Lithosphere: The solid part of earth which provides the greatest variety of chemical resources. Examples are petroleum and metal-bearing ores.
Ore: A naturally occurring rock or mineral that can be mined and from which it is profitable to extract a metal or other material.
Minerals: Naturally occurring solid compounds containing the element or group of elements of interest.
Ductility: Ease of being drawn into thin wires.
Activity Series: Ranking elements in order of their chemical reactivities.
Reduction: Any chemical change in which a reactant can be considered to gain one or more electrons.
Reduced: Like reduction.
Oxidation: A reverse reaction in which an ion or other species can be considered to lose one or more electrons.
Oxidized: Any reactant that appears to lose one or more electrons is said to be _______.
Oxidation-Reduction Reactions/Redox Reactions: Oxidation and reduction occur together.
Reducing Agent: A reactant that provides electrons.
Electron-Dot Structure/Dot Structure: The resulting expression.
Oxidizing Agent: The species involved in removing electrons from the oxidized reactant.
Law of Conservation of Mater: Matter is neither created nor destroyed.
Balanced Chemical Equation: The number of atoms of each element is the same on the reactant side and product sides.
Coefficients: Indicate the relative number of units of each substance involved in the chemical reaction.
Formula Unit: This term is used when referring to the smallest unit of an ionic compound.
Mole: (symbolized mol) a counting unit; dozen; 6.02 X 10^23.
Molar Mass: The atomic weights of elements can be used to find the mass of one mole of any substance.
Percent Composition: The percent by mass of each material found in an item such as a coin.
Renewable Resources: Resources that can be replenished by natural processes; examples are animals, plants, fresh water and air, and fertile soil.
Nonrenewable Resources: Resources that cannot be readily replenished; examples are petroleum, natural gas, coal, metals, and oil.
Allotropes: Different forms of an element that each have distinctly different physical or chemical properties; examples are diamonds, graphite, and buckmisterfullerene.
Alloy: A solid combination of atoms of two or more metals.
Superconductivity: The ability to conduct an electric current without any electrical resistance.
Semi-Conductors: Somewhere in between metals and nonmetals; metalloids are semi-conductors.
Unit 3 Vocab List:
Crude Oil: Petroleum pumped from underground.
Hydrocarbons: Molecular compounds that only contain atoms of hydrogen and carbon.
Distillation: The separation of liquid substances according to their differing boiling points. Heating the components causes the one with the lower boiling point to vaporize and leave the distillation flask and then it will condense back to a liquid as it passes through a condenser.
Distillate: Each condensed liquid compound.
Fractions: Several distintive mixtures.
Fractional Distillation: The process of separating through large-scale oil refining.
Intermolecular Forces: Forces of attraction between molecules.
Carbon Chain: In hydrocarbon molecules, carbon atoms are joined to form this backbone where hydrocarbons are attached.
Valence Electrons: The electrons within an atom's unfilled outer shell.
Covalent Bond: The chemical bond formed between two atoms that share a pair of electrons.
Structural Formula: Another common representation of a covalently bonded molecule.
Alkanes: A series of hydrocarbons.
Molecular Formulas: Specify the number of each atom type within a molecule.
Condensed Formulas: More useful than molecular formulas.
Straight-Chain Alkanes: Each carbon atom is only linked to one or two other carbon atoms.
Branched-Chain Alkanes: One carbon atom can be linked to three or four other carbon atoms.
Structural Isomers: Molecules that have identical molecular formulas but different arrangements of atoms.
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