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Unit 7 Reactions
Vocabulary terms
| Term | Definition |
|---|---|
| Accuracy | A measure of how close the average of all trials of for a measured value are to the true value of the measurement. |
| Activity Series | A list of elements in decreasing order of their reactivity. |
| Analytical Balance | Extremely accurate laboratory balance created to precisely measure the mass of an object. |
| Anchoring Event | Specific instances of a phenomenon that require scholars to pull together a number of science ideas in order to explain. |
| Anion | Negatively charged ion. |
| Aqueous (aq) | Water based solution that contains one or more dissolved substances; in equations this means that the substance denoted by the chemical formula is dissolved in a water solvent. |
| Atom | The smallest particle of an element. |
| Attraction | The non-contact force or interaction that pulls two or more substances or particles toward each other. |
| Avogadro’s Number | The number of particles found in one mole of a substance with an experimentally determined value of approximately 6.02 x 1023 particles per mole. |
| Balanced Equation | A chemical equation in which the same number of each type of atom is present on both the reactant and product sides. |
| Bond | General term used to describe the forces that hold atoms together in compounds. |
| Cation | Positively charged ion. |
| Charge | The net charge of an atom found by comparing the number of electrons to the number of protons. |
| Chemical Equation | A formula that uses symbols and numbers to communicate how chemical reactions occur. |
| Chemical Reaction | The processes of chemical change by which chemicals interact to form new chemicals with different compositions. |
| Chemical Species | The atoms, ions, or molecules involved in a chemical reaction. |
| Claim | A statement made as an explanation of data collected and analyzed or as an answer to a question. |
| Coefficient | The number in front of a chemical formula in a chemical reaction. |
| Complete Ionic Equation | A chemical equation that separates the compounds involved in a reaction into their ionic forms for aqueous substances and solid forms for insoluble substances. |
| Compound | A pure substance composed of identical particles containing atoms from more than one elemens held together by bonds that can only be separated or changed by chemical reactions. |
| Control Variable (aka Constant) | Anything that is held constant or limited in an investigation to minimize risk of error in the results. |
| Conversion Factor | A ratio of equivalent measurements. |
| Covalent Bond | A bond that involves two highly electronegativity atoms, usually nonmetals, sharing electrons in a distinctive location in such a way that all atoms in the particle achieve a stable octet. |
| Dependent Variable | The variable being tested and measured in an experiment, and is 'dependent' on the independent variable. |
| Dimensional Analysis (aka Factor-Label Method) | the mathematical conversion between an amount in one unit to the corresponding amount in a desired unit through multiplying by one or more conversion factors. |
| Double Replacement | Occurs when two ionic compounds exchange ions and produce two new ionic compounds. |
| Electron | Subatomic particle found outside the nucleus of the atom that has negligible mass and a negative charge equal and opposite to the proton. |
| Element | Substance that is composed of a single type of atom; a substance that cannot be decomposed by a chemical change; determined by the number of protons in the atom. |
| Energy (E) | The capacity to do work, usually measured in Joules (J). |
| Energy Level (aka Energy Shell) | A fixed distance from the nucleus of an atom where electrons may be found. |
| Essential Question | A question developed from an anchoring event that is investigated in order to develop an underlying explanatory model for the phenomenon. |
| Evidence | Knowledge, facts, or data (qualitative or quantitative) that supports the claim. |
| Explanatory Model | A proposed explanation made based on limited evidence as a starting point for further investigation. |
| Formula Equation | A symbolic representation of a chemical reaction where the reactants and products are expressed using their chemical formulas, chemical symbols and formulas instead of words. |
| Gas (g) | Matter that has an indefinite shape and indefinite volume. |
| Graduated Cylinder | A narrow, cylindrical container marked with horizontal lines to represent units of measurement and used to precisely measure the volume of liquids. |
| Half Reaction | The part of an overall reaction that represents, separately, either an oxidation or a reduction. |
| Independent Variable | The variable the experimenter manipulates or changes, and in many cases is assumed to have a direct effect on the dependent variable. |
| Inference | A conclusion reached on the basis of evidence and reasoning. |
| Insoluble | A way to describe a solute that will not dissolve into a solvent. |
| Ion | An atom of a single element that has gained or lost electrons, |
| Kelvin (K) | A scale of temperature that is the SI base unit of thermodynamic temperature (equivalent in size to the degree Celsius), first introduced as the unit used in the Kelvin scale. |
| Kinetic Energy | Form of energy that an object or a particle has by reason of its motion. |
| Law of Conservation of Mass | Matter can neither be created nor destroyed - only converted from one form of matter to another. |
| Liquid (l) | Matter that has an indefinite shape and definite volume. |
| Mass | The amount of matter present; measured in the base SI unit of grams (g). |
| Metal | Element found on the left side of the zig zag demarcation of the periodic table and made of multiple metal families with low electronegativities. |
| Miscibility | The property of two substances to thoroughly mix in all proportions to form a homogeneous mixture (solution). |
| Miscible | Two substances that mix completely in all proportions or concentrations to form a homogenized, equally distributed solution at the particulate level. |
| Mixture | Contains two or more substances that are not chemically combined. |
| Molar Mass | The mass, in grams, of one mole of a substance expressed in units of grams per mole (g/mol). The average atomic mass determined using the natural abundance of all isotopes of an element is the same as the molar mass of an element. |
| Mole | A way to count the number of particles of a substance by group, similar to a “pair” or a “dozen”; the amount of substance containing the same number of atoms, molecules, ions, or other entities as the number of atoms in exactly 12 grams of 12C. |
| Molecule | A group of atoms covalently bonded together, representing the smallest fundamental unit of a chemical compound that can take part in a chemical reaction. |
| Net Ionic Equation | Equation that only shows the particles directly involved in chemical change in a chemical reaction. |
| Neutron | Subatomic particle found in the nucleus of the atom that as an approximate mass of 1 amu that is neutral (no charge). |
| Nonmetal | Element found on the upper right of the zig zag demarcation on the periodic table made of multiple nonmetal families with nearly full or full octets. |
| Observation | Any data collected using any of the five senses, can be quantitative or qualitative. |
| Origin | The original position of the sample on the chromatography paper. |
| Oxidation Half Reaction | An equation that represents, separately, only the oxidation half of a redox reaction with lost electrons as a product. |
| Oxidation Number | A positive or negative number that is assigned to an atom to indicate its degree of oxidation (electron loss) or reduction (electron gain). This is not an ionic charge and the + or – sign is placed in front of the number (i.e. +1 not 1+). |
| Oxidized Species | A substance that has lost electrons during a chemical reaction, resulting in an increase in its oxidation state. |
| Paper Chromatography | A technique which is used to separate dissolved solutes in a homogenous solution based on their distribution between stationary and mobile phases. |
| Partial Charge | A charge value that is less than the elementary charge value of one on an atom within a molecule, written as partial positive (δ+) or partial negative (δ-). |
| Particle | Any basic unit of matter such as atoms, ions, molecules, formula units, etc. |
| Particulate Diagram | A visual representation in chemistry that depicts the microscopic structure of matter, |
| Phenomenon | Events or processes (“things that happen”) that are observable by the senses, or detectable by instruments. |
| Physical Property | A property of a substance that can be observed and measured without changing the chemical identity of the substance. |
| Polar | A physical property of compounds that describes a separation of charges, or unequal distribution of charge, resulting in partial positive and partial negative regions. |
| Polarity | A separation of electric charge leading to a bond or an entire molecule having a dipole moment. |
| Polyatomic Ion | An ion composed of two or more atoms covalently bonded together in such a way that it results in a charged particle that behaves as a single ion. |
| Precipitate | An insoluble product of a chemical reaction. |
| Precipitation Reaction | A reaction between aqueous solutions that results in the formation of an insoluble product. |
| Precision | A measure of how close all trials for a measured value are to one another. |
| Prefix | A word, letter, or number placed before another. |
| Product | A new substance formed as a result of a chemical reaction. |
| Pure Substance | A single tyoe of matter that cannot be separated into other kinds of matter by any physical means. |
| Qualitative | The determination of non-numerical information about a chemical species, a reaction, a system, etc. |
| Quantitative | The determination of numerical information about a chemical species, a reaction, a system, etc. |
| Random Error | An unpredictable, chance variation in a measurement that can occur due to inconsistent application of the procedure or other variables. |
| Rate | The speed at which a chemical or physical process occurs. |
| Ratio | Numerical comparison or relationship between two or more values. |
| Reactant | A substance that is present at the start of, and participates in, a chemical reaction. |
| Reasoning | The explanation of the “how” or “why” the evidence you have chosen supports your claim. |
| Redox Reaction | A reaction that involves the full or partial transfer of electrons from one reactant to another; also known as an oxidation-reduction reaction. |
| Reduced Species | A substance that has gained electrons during a chemical reaction, resulting in a decrease in its oxidation state. |
| Reduction Half Reaction | An equation that represents, separately, only the reduction half of a redox reaction with gained electrons as a reactant. |
| Repulsion | The non-contact force or interaction that pushes two or more substances or particles away from each other. |
| Roman Numeral | Symbols used in a system of numerical notation based on the ancient Roman system. The symbols needed are capital letters I (1) and V (5). |
| Saturated Solution | Solutions that contain the maximum amount of dissolved solutes in a given amount of solvent at a specific temperature. |
| Serial Dilution | A step-wise, repeated dilution of a known concentration sample to reduce a highly concentrated solution to a more usable concentration in a fixed and predictable ratio. |
| Single Replacement | Occurs when a single element replaces another element in a compound over the course of the reaction. |
| Solid (s) | Matter that has a definite shape and a definite volume. |
| Solubility | The maximum amount of solute that can dissolve in a specific amount of solute at a given temperature. |
| Solubility Curve | A graphical representation that shows how the solubility of a substance changes with temperature, typically plotted with temperature on the x-axis and the amount of solute dissolved (solubility) on the y-axis. |
| Soluble | A way to describe a solute that will dissolve into a solvent. |
| Solute | The substance being dissolved. |
| Solution | Mixture of solute and solvent. |
| Solvent | The substance doing the dissolving. |
| Spectator Ions | Ions present in solution during a chemical reaction between two or more aqueous solutions but do not directly take part in the chemical reaction and is found in solution both before and after the reaction unchanged. |
| State Symbol | A symbol used in equations to show if a substance is a solid, a liquid, a gas, or an aqueous solution. |
| Subscript | Number to the right of and slightly below the element symbol that communicates how many atoms of that element are within the substance. |
| Systematic Error | Errors that result from predictable changes in an experiment; errors that causes all measured quantities to be off by the same amount or the same proportion usually resulting in decreased investigative accuracy. |
| Temperature | Average kinetic energy of a substance, usually measured in Celsius or Kelvin in the context of chemical analysis. |
| Unbalanced Equation | A chemical equation in which the number of each type of atom on the reactant and product sides are not the same. |
| Valence Electron | An electron located in the outermost shell (or valence shell) of an atom. |
| Volume | The amount of space occupied by a substance, typically expressed in liters (L). |
| Weigh Boat | Open containers that is used to mass granulated, liquid, or solid samples. |
| Word Equation | The reactants and products are represented by their names, meaning they are written in word form instead of chemical formulas and quantities. |
| Yield Arrow (→) | Symbol that separates the beginning from the end of a process in an equation. |
| Yield | Refers to the end state of, or what is obtained from, a physical or chemical process; can be qualitative or quantitative. |
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