Typicial CHemistry VOcab
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| Analytical Chemistry | The area of chemistry that focuses on the composition of matter
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| Applied Chemistry | research that is direct toward a practical goal or application
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| Biochemistry | the areas of chemistry that focuses on processes that take place in organisms
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| Biotechnology | the field that applies science to the production of biological products or processes
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| Chemistry | the study of the composition of matter and the changes that matter undergoes.
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| Experiment | -a repeatable procedure that is used to test a hypothesis
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| Hypothesis | a proposed explanation for an observation
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| Inorganic chemistry | the study of substances that in general do not contain carbon
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| Macroscopic | describes the world of objects that are large enough to see with the unaided eye
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| Matter | anything that has mass and occupies space
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| Microscope | describes the world of objects that can be seen only under magnification
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| Manipulated variable | the variable that is changed during an experiment; also called independent
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| Observation | information obtained through the senses; observation in science involving measurement
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| Organic chemistry | the study of compounds containing carbon
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| Physical Chemistry | the area of chemistry that deals with the mechanism, the rate and the energy transfer that occurs when matter undergoes change.
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| Pollutant | a material found in air, water, or soil that is harmful to humans and other organisms
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| Pure Chemistry | The pursuit of chemical knowledge for its own sake
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| Responding Variable | the variable that is observed during an experiment; dependent variable
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| Scientific Law | a concise statement that summarizes the results of many observations and experiments
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| Scientific Method | a logical, systematic approach to the solutions of a scientific problem; steps in the scientific method include making observations, testing hypotheses and developing theories
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| Technology | the means by which a society provides its members with those things needed and desired
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| Theory | a well tested explanation for a broad set of observations
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| Chemical Change | A change that produces matter with a different composition than the original.
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| Chemical property | The ability of a substance to undergo a specific chemical change.
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| Chemical reaction | A change in which one or more reactants change into one or more products; characterized by the breaking of bonds in reactants and the formation of bonds in products.
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| Chemical Symbol | A one
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| Compound | a substance that contains two or more elements chemically combined in a fixed proportion.
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| Distillation | A process used to separate dissolved solids from a liquid, which is boiled to produce a vapor that is then condensed into a liquid.
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| Element | the simplest form of matter that has a unique set of properties; an element cannot be broken down into simpler substances by chemical means.
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| Extensive property | A property that depends on the amount of matter in a sample.
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| Filtration | A process that separates a solid from the liquid in a heterogeneous mixture.
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| Gas | A form of matter that takes the shape and volume of its container; a gas has no definite shape or volume.
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| Heterogeneous Mixture | A mixture that is not uniform in composition; components are not evenly distributed throughout the mixture.
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| Homogeneous Mixture | A mixture that is uniform in composition; Components are evenly distributed and not easily distinguished.
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| Intensive Property | A property that depends on the type of matter in a sample, not the amount of matter.
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| Law of Conservation of Mass: In any physical change or chemical reaction mass is conserved; mass can be neither created or destroyed. |
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| Liquid | A form of matter that flows, has a fixed volume and a indefinite shape.
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| Mass | A measure of the amount of matter that an object contains; the SI base unit of mass is the Kilogram.
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| Mixture | A physical blend of two or more substances that are not chemically combined.
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| Phase | any part of a sample with uniform composition and properties.
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| Physical Change | A change during which some properties change but the composition of the material does not.
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| Physical Property | A quality or condition of a substance that can be observed of measured without changing the substances composition.
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| Precipitate | A solid that dorms and settles out of a liquid mixture.
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| Product | A substance produced in a chemical reaction.
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| Reactant | A substance present at the start of a reaction.
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| Solid | A form of matter that has definite shape and volume.
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| Solution | A homogeneous mixture; consists of solutes dissolved in a solvent.
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| Substance | Matter that has uniform and definite composition; either an element or a compound; also called a pure substance.
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| Vapor | Describes the gaseous state of a substance that is generally a liquid or a solid at room temperature.
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| Volume | A measure of the space occupied by a sample of matter.
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| Absolute Zero | The zero point on the Kelvin temperature scale, equivalent to -273.15°C.
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| Accepted Value | A quantity used by general agreement of the scientific community.
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| Accuracy | The closeness of a measurement to the true value of what is being measured.
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| Calorie(cal) | The quantity of heat needed to raise the temperature of 1 g of pure water 1°C.
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| Celsius Scale | The temperature scale on which freezing point of water is 0°C and the boiling point of water is 100°C.
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| Conversion Factor | a ratio of equivalent measurements used to convert a quantity from one unit to another.
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| Density | The ratio of mass of an object to its volume.
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| Dimensional Analysis | A technique of problem solving that uses the units that read part of measurements to help solve the problem.
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| Energy | The capacity for doing work or producing heat.
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| Error | the difference between the accepted value and the experimental value.
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| Experimental Value | a quantative value measured during an experiment.
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| Gram(g) | a metric mass unit equal to the mass of 1 cm3 of water at 4°C.
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| International System of Units(SI) | the revised version of the metric system adopted by international agreement in 1960
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| Joule(J) | the SI unit of energy; 4.184 J=Calorie
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| Kelvin Scale | the temperature scale in which freezing point is 273.15 K and the boiling point is 373.15K; 0K is absolute zero.
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| Kilogram(Kg) | the mass of 1 L of water at 4°C; it is the base unit of mass in SI.
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| Liter(L) | the volume of a cube measuring 10cm on each edge or 1000cm3; it is the common unprefixed unit of volume in the metric system.
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| Measurement | a quantivtive description that includes both a number and a unit.
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| Meter(m) | the base unit of length in SI
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| Percent error | the percent that a measured value differs from the accepted value.
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| Precision | describes the closeness or reproducibility of a set of measurements taken under the same conditions.
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| Scientific Notation | an expression numbers in the form m X 10n where m is equal to or greater than one and less than 10, and n is an integer.
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| Significant Figures | all the digits that can be known precisely in a measurements plus a last estimated digit.
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| Temperature | a measure of the average kinetic energy of particles in matter; temperature determines the direction of heat transfer.
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| Weight | a force that measure the pull of gravity one given mass.
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| Atom | the smallest particle of an element that retains its identity in a chemical reaction
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| Atomic Mass | the weighted average of the masses of the isotopes of an element
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| Atomic Mass Units(amu) | a unit of mass equal to one
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| Atomic Number | the number of protons in the nucleus of an atom of an element
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| Cathode Ray | the electrode at which reduction occurs
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| Dalton's Atomic Theory | the first theory to relate chemical changes to events at the atomic level
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| Electron | a negatively charged subatomic particle
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| Group | a vertical column of elements in the periodic table, the constituent elements of a group have similar chemical and physical properties
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| Isotopes | atoms of the same element that have the same atomic number but different atomic masses due to a difference in number neutrons
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| Mass Number | the total amount of protons and neutrons in the nuclear of an atom.
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| Neutron | subatomic particle that has no charge and a mass of 1 amu; found in the nucleus of an atom
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| Nucleus | the tiny dense central portion of an atom; composed of protons and neutrons
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| Period | horizontal row of elements in the periodic table
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| Periodic Table | an arrangement of elements in which the elements are separated into groups based on a set of repeating properties
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| Proton | a positively charged subatomic particle found in the nucleus of an atom
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| Amplitude | the height of a wave's crest
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| Atomic Emission Spectrum | the pattern formed when light passes through a prism or diffraction grating to separate it into different frequencies of light it contains.
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| Atomic Orbital | A mathematical expression describing the probability of finding an electron at various locations; usually represented by the region of space around the nucleus where there is a high probably of finding an electron
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| Aufbau Principle | the rule that electrons occupy the orbital's of lowest energy first
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| Electromagnetic Radiation | energy waves that travel in a vacuum at a speed of 2.998 X 108 m/s; includes radio, radar, micro, infrared, visible, ultraviolet, x
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| Electron Configurations | the arrangement of electrons of an atom in its ground state into various orbital's around the nuclei of atoms
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| Energy Levels | the specific energies an electron in an atom or other system can have
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| Frequency | the number of wave cycles that pass a given point per unit of time; frequency and wavelength are inversely proportional to each other.
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| Ground State | The lowest possible energy of an electron described by quantum mechanics.
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| Heisenberg Uncertainty Principle | it is impossible to know exactly both the velocity and the position of a particle at the same time
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| Hertz | the unit of frequency equal to one cycle per a second
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| Hund's Rule | electrons occupy orbital's of the same energy in a way that makes the number of electrons with the same spin direction as large as possible
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| Pauli Exclusion Principle | an atomic orbital may describe at most two electrons each with opposite spin directions
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| Photons | a quantum of light; a discrete bundle of electromagnetic energy that interacts with matter similarly to particles.
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| Quantum | the amount of energy needed to move an electron from one energy level to another
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| Quantum Mechanical Model | the modern description, primarily mathematical of the behavior of electrons in atoms.
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| Spectrum | wavelengths of visible light that are separated when a beam of light passes through a prism; range of wavelengths of EM radiation
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| Wavelength | the distance between adjacent crests in a wave
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| Alkali Metals | Any metal in group 1A of the periodic table
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| Alkaline Earth Metals | any metal in group 2A of the periodic table
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| Anion | Any atom or group of atoms with a negative charge
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| Atomic Radius | one
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| Cation | any atom or group of atoms with a positive charge
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| Electronegativity | the ability of an atom to attract electrons
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| Halogens | a nonmetal in group 7A of the periodic table
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| Inner Transition Metal | an element in the lanthanide or actinide series; the highest occupied s sublevel and nearby f sublevel of its atoms generally contain electrons; also called inner transition elements
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| Ion | an atom or group of atoms that has a positive or negative charge
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| Ionization Energy | the energy required to remove an electron from an atom in its gaseous state
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| Metalloids | an element that tends to have properties that are similar to those of metals and nonmetals
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| Metals | one of a class of elements that are good conductors of heat and electric current; metals tend to be ductile, malleable and shiny
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| Noble Gases | An element in group 8A of the periodic table; the s and p sublevels of the highest occupied energy level are filled
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| Nonmetals | an element that tends to be a poor conductor of heat and electric current; nonmetals generally have properties opposite to those of metals
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| Periodic Law | when the element are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties
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| Representative Elements | an element in an "A" group in the periodic table. As a group of these elements display a wide range of chemical properties and physical properties. In their atoms, the s and p sublevels in the highest occupied energy level are partially full
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| Transition Metal | one of the group B elements in which the highest occupied s sublevel and a nearby d sublevel generally contain electrons.
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| Alloys | a mixture composed of two or more elements, at least one of which is metal
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| Chemical Formula | An expression that indicates the number and type of atoms present in the smallest representative units of a substance
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| Coordination Number | the number of ions of opposite chare that surround each ion in a crystal
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| Electron Dot Structure | A notation that depicts valence electrons as dots around the atomic symbol of the element; the symbol represents the inner electrons and atomic nucleus; also called Lewis dot structure
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| Formula Unit | the lowest whole-number ratio of ions in the ionic compound; in magnesium chloride the ratio of magnesium ions to chloride ions is 1
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| Halide Ion | a negative ion formed when a halogen atom gains an electron
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| Ionic Bond | the electrostatic attraction that binds oppositely charged ions together
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| Ionic Compounds | a compound composed of positive and negative ions
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| Metallic Bonds | the force of attraction that holds metal together; it consists of the attraction of free-floating valence electrons for positively charged metal ions
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| Octet Rule | atoms react by gaining or losing electrons so as to acquire the stable electron structure of a Nobel gas, usually eight valence electrons
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| Valence Electron | an electron in the highest occupied energy level of an atom.
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| Bond Dissociation Energy | the energy required to break the bond between two covalently bonded atoms; this value is usually expressed in kJ per mol of a substance
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| Bonding Orbital | a molecular orbital that can be occupied by two electrons of a covalent bond
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| Covalent Bond | a bond formed by the sharing of electrons between atoms
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| Coordinate Covalent Bond | a covalent bond in which one atom contributes both bonding electrons
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| Diatomic Molecule | a molecule consisting of two atoms
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| Dipole | a molecule that has two poles or regions with opposite charges
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| Dipole Interactions | intermolecular forces resulting from the attraction of oppositely charged regions of polar molecules
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| Dispersion Forces | attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules
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| Double Covalent Bond | a bond in which two atoms share two pairs of electrons
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| Hybridization | the mixing of several atomic orbital's to form the same total number of equivalent hybrid orbital's
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| Hydrogen Bonds | attractive forces in which a hydrogen covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom
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| Molecular Compound | a compound that is composed of molecules
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| Molecular Formula | chemical formula of a molecular compound that shows the kinds and numbers of atoms present in a molecule of a compound
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| Molecular Orbital | an orbital that applies to the entire molecule
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| Molecule | a neutral group of atoms joined together by covalent bonds
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| Network Solids | a solid in which all of the atoms are covalently bonded to each other
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| Non | polar Covalent bond
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| Pi Bond | a covalent bond in which the bonding electrons are most likely to be found in sausage
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| Polar Bond | a covalent bond between atoms in which the electrons are shared unequally
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| Polar Covalent Bond | aka polar bond
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| Polar Molecule | a molecule in which one side of the molecule is slightly negative and the opposite side is slightly positive
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| Polyatomic Ion | a tightly bond group of atoms that behaves as a unit and has a positive or negative charge
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| Resonance Structure | one of the two or more equally valid electron dot structures of a molecule or polyatomic ion
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| Sigma Bond | a bond formed when two atomic orbital combine to form a molecular orbital that is symmetrical around the axis connection the two atomic nuclei
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| Single Covalent Bond | a bond formed when two atoms share a pair of electrons
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| Structural Formula | a chemical formula that shows the arrangement of atoms in a molecule or polyatomic ion; each dash between a pair of atoms indicates a pair of shared electrons
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| Tetrahedral Angle | a bond angle of 109.5 that results when a central atom forms four bonds directed toward the center of a regular tetrahedron
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| Triple Covalent Bond | a covalent bond in which three pairs of electrons are shared by two atoms
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| Unshared Pair | a pair of valence electrons that is no shared between atoms aka lone pair
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| Van der Waals Forces | the two weakest intermolecular attractions
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| VSEPR Theory | valence
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| Acid | a compound that produces hydrogen ions in solution
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| Base | a compound that produces hydroxide ions in solution
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| Binary Compound | a compound composed of two elements
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| Law of Definite Proportions | in samples of any chemical compound the masses of the elements are always in the same proportion
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| Law of Multiple Proportions | whenever two elements form more than one compound the different masses of one element combine with the same mass of the other elements to form simple whole umber ratios
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| Monatomic Ion | a single atom with a positive and negative charge resulting from the loss or gain of one or more valence electrons
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| Polyatomic Ion | a tightly bound group of atoms that behaves as a unit and has a positive or negative charge
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| Avogadro's hypothesis | equal volumes of gases at the same temperature and pressure contains equal numbers of particles
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| Avogadro's Number | the number of representatives particles contained in one mole of a substance; equal to 6.02 X 10 23particles
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| Empirical Formula | a formula with the lowest whole number ratio of elements in a compound
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| Molar Mass | a term used to refer to the mass of a mole of any substance
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| Molar Volume | the column occupied by one mole of gas at STP (22.4L)
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| Mole(mol) | the amount of substance that contains 6.02 X 10 23 representative particles of that substance.
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| Percent Composition | the percent by mass of each element in a compound
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| Representative Particle | the smallest unit into which a substance ca be broken down without a change in composition usually atoms molecules or ions.
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| Standard Temperature and Pressure(STP) | the conditions under which the volume of a gas is usually measured; 0 degrees Celsius and 101.3kPa or 1 atmosphere(atm)
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| Activity Series | a list of elements in order of decreasing activity; the activity series of halogens is Fl, Cl, Br, I
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| Balanced Equation | a chemical equation in which mass is conserved; each side of the equation has the same number of atoms of each element
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| Catalyst | A substance that speeds up the rate of reaction by lowering the activation energy barrier; the catalysts is not used up in the reaction.
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| Chemical Equation | an expression representing a chemical reaction; the formulas of the reactants (L) are connected by an arrow with the formulas for the products(r.)
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| Coefficients | a small whole number that appears in front of a formula to a balanced equation
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| Combination Reaction | or synthesis; is a chemical change in which two or more substances react to form a single new substance
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| Combustion Reaction | a chemical change in which an element or a compound reacts with oxygen, often producing energy in the form of heat and light.
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| Complete Ionic Equation | an equation that shows dissolved ionic compounds as dissociated free ions
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| Decomposition Reaction | a chemical change in which a single compound is broken down into two or more simpler products
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| Double Replacement Reaction | a chemical change that involves an exchange of positive ions between compounds
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| Net Ionic Equation | an equation for a reaction in solution showing only those particles that are directly involved in the chemical change
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| Single Replacement Reaction | a chemical change in which one element replaces a second element in a compound; also called displacement reaction
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| Skeleton Equation | a chemical equation that does not indicate the relative amounts of reactants and products
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| Spectator Ion | an ion that is not directly involved in a chemical reaction; an ion that does not change oxidation number or composition during reaction.
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| Actual Yield | the amount of product that forms when a reaction is carried out in the laboratory
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| Excess Reagent | a reagent present in a quantity that is more than sufficient to react with a limiting; any reactant that remains after the limiting reagent is used up in a chemical reaction
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| Limiting Reagent | any reagent that is used up first in a chemical reaction; it determines the amount of product that can be formed in the reaction
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| Mole Ratio | a conversion factor derived from the coefficients of a balanced chemical equation interpreted in terms of moles
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| Percent Yield | the ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction
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| Stoichiometry | the portion of chemistry dealing with numerical relationships in chemical reaction; the calculation of quantities of substances involved in chemical equations.
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| Allotrope | one of two or more different molecular forms of an element in the same physical state; graphite and diamond
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| Amorphous Solid | describes a solid that lacks an ordered internal structure; denotes a random arrangement of atoms
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| Atmospheric Pressure | the pressure exerted by atoms and molecules in the atmosphere surrounding earth, resulting from collisions of these particles with objects.
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| Barometer | an instrument used to measure atmospheric pressure
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| Boiling Point | the temperature at which vapor pressure of a liquid is just equal to the external pressure on the liquid (BP)
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| Crystal | a solid in which the atoms, ion or molecules are arranged in an orderly, repeating three dimensional pattern called a crystal lattice
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| Evaporation | vaporization that occurs at the surface of a liquid that is not boiling
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| Gas Pressure | results from the force exerted by a gas per unit surface area of an object; due to collisions of gas particles with the object
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| Glass | transparent fusion product of inorganic materials that have cooled to a rigid state without crystallizing
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| Kinetic Energy | the energy an object has because of its motion
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| Kinetic Theory | a theory explaining the states of matter, based on the concept that all matter consists of tiny particles that are in constant motion
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| Melting Point | the temperature at which a substance changes from a solid to a liquid; the melting point of water is 0 degrees Celsius (MP)
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| Normal Boiling Point | the boiling point of a liquid at a pressure of 101.3kPa or 1 atm
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| Pascal | the SI unit of pressure
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| Phase Diagram | a graph showing the conditions at which a substance exists as a solid, liquid or vapor
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| Standard Atmosphere(atm) | a unit of pressure; it is the pressure required to support 760 mm of mercury in a mercury barometer at 25 degrees Celsius
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| Sublimation | the process in which a solid changes to a gas or vapor without passing through the liquid state
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| Triple Point | the point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
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| Unit Cell | the smallest group of particles within a crystal that retains the geometric shape of the crystal
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| Vacuum | a space where no particles of matter exist
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| Vaporization | the conversion of liquid to a gas or vapor
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| Vapor Pressure | a measure of the force exerted by a gas above a liquid in a sealed container; a dynamic equilibrium exists between the vapor and the liquid
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| Boyle's Law | for a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure
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| Charles's Law | the volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant
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| Combined Gas Law | the law that describes the relationship among the pressure, temperature, and volume of an enclosed gas
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| Compressibility | a measure of how much the volume of matter decreases under pressure
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| Dalton's Law Of Partial Pressures | at constant volume and temperature the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases
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| Diffusion | the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout.
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| Effusion | the process that occurs when a gas escapes through a tiny hole in its container
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| Gay-Lussac's Law | the pressure of a gas is directly proportional to the Kelvin temperature if the volume is constant
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| Graham's Law of Effusion | the rate of effusion of a gas inversely proportional to the square root of its molar mass; this relationship is also true for diffusion of gases
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| Ideal Gas Constant | the constant in the ideal gas law with the symbol R that has the value 8.31 (L*kPa)/(K*mol)
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| Ideal Gas Law | the relationship PV =nRT which describes the behavior of an ideal gas
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| Partial Pressure | the contribution each gas in a mixture of gases makes to the total pressure
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| Aqueous Solution | water that contains dissolved substances
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| Browian Motion | the chaotic movement of colloidal particles, caused by collision with particles of the solvent in which they are dispersed
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| Colloid | a mixture whose particles are intermediate in size between those of a suspension and a solute solution
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| Electrolyte | a compound that conducts an electric current when it is in an aqueous solution or in the molten state; all ionic compound are electrolytes but most covalent compounds are not.
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| Emulsion | the colloidal dispersion of one liquid in another
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| Hydrate | a compound that has a specific number of water molecules bound to each formula unit
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| Nonelectrolyte | a compound that does not conduct an electric current in aqueous solution or in the molten state
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| Solute | dissolved particles in a solution
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| Solvation | a process that occurs when an ionic solute dissolves; in a solution, solvent molecules surround the positive and negative ions
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| Solvent | the dissolving medium in a solution
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| Strong Electrolyte | a solution in which a large portion of the solute exists as ions
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| Surfactant | any substance that that interferes with the hydrogen bonding between water molecules and thereby reduces surface tension; soap and detergents are surfactants
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| Suspension | a mixture from which some of the particles settle out slowly upon standing
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| Surface Tension | an inward force that tends to minimize the surface area of a liquid; it causes the surface to behave as if it were a thin skin
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| Tyndall Effect | scattering of light particles in a colloid or suspension, which causes a beam of light to become visible
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| Weak Electrolyte | a solution that conducts electricity poorly because only a fraction of the solute exists as ions
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| Boiling Point Elevation | the difference in temperature between the boiling point of a solution and the boiling point of a pure solvent
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| Concentrated Solution | a solution containing a large amount of solute
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| Concentration | a measurement of the amount of a solute that is dissolved in a given quantity of solvent; usually expressed in mol/L
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| Colligative Property | a property of a solution that depends solely upon the number of solute particles, and not upon their identities; boiling point elevation, freezing point depression and vapor pressure lowering are colligative
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| Dilute Solution | a solution that contains a small amount of solute
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| Freezing Point Depression | the difference I temperature between the freezing point of a solution and the freezing point of the pure solvent
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| Henry's Law | at a given temperature the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid
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| Immiscible | describes liquids that are insoluble in one another; oil and water
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| Miscible | describes liquids that dissolve one another in all proportions
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| Molal Freezing Point depression Constant | Kf, the change in freezing point for a 1 Molal solution of a nonvolatile molecular solute
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| Molal Boiling Point Elevation Constant | Kb, the change in boiling point for a 1 Molal solution of a nonvolatile molecular solute
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| Molality | (m) the concentration of solute in a solution expressed as the number of moles of solute dissolved in 1 kg or 1000 g of solvent
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| Molarity | (M) the concentration of a solute in a solution expressed as the number of moles of solute dissolved in 1L of solution
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| Mole Fraction | the ratio of the moles of solute in solution to the total number of moles of both solvent and solute
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| Saturated Solution | a solution containing the maximum amount of solute for a given amount of solvent at a constant temperature and pressure; an equilibrium exists between un-dissolved ions and dissolved ions in solution
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| Solubility | the amount of a substance that dissolves in a given quantity of solvent at specified conditions of temperature and pressure to produce a saturated solution
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| Supersaturated Solution | a solution that contains more solute than it can theoretically hold at a given temperature; excess solute precipitates if a seed crystal is added
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| Unsaturated Solution | a solution that contains less solute than a saturated solution at a given temperature and pressure
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||||
| Calorimeter | an insulated devise used to measure the absorption or release of heat in chemical or physical processes
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|
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| Calorimetry | the precise measurement of heat flow out of a system for chemical or physical processes
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| Chemical Potential Energy | energy stored in chemical bonds
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| Endothermic Process | a process that absorbs heat from the surrounding
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| Enthalpy | (H) the heat content of a system at constant pressure
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| Exothermic Process | a process that releases heat to its surroundings
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| Heat | (q) energy that transfers from one object to another because of a temperature difference between the objects
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| Heat Capacity | the amount of heat needed to increase the temperature of an object exactly 1°C
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|
||||
| Heat of Combustion | the heat of reaction for the complete burning of one mole of a substance
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| Heat of Reaction | the enthalpy change for a chemical equation exactly as it is written
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|
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| Hess's Law of Heat Summation | if you add two or more Thermochemical equations to give a final equation then you also add the heats of reaction to give the final heat of reaction
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|
||||
| Law of Conservation of Energy | in ay physical change or chemical reaction, mass is conserved; mass can be neither created or destroyed
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|
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| Molar Heat of Condensation | ( ∆Hcond) the amount of heat released by one mole of a vapor as it condenses to a liquid at a constant temperature
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| Molar Heat of Fusion | (∆Hfus) the amount of heat absorbed by one mole of a solid substance as it melts to a liquid at a constant temperature
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|
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| Molar Heat of Solidification | (∆Hsolid) the amount of heat lost by one mole of a liquid as it solidifies at a constant temperature
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|
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| Molar Heat of Solution | (∆Hsoln) the enthalpy change caused by the dissolution of one mole of a substance
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|
||||
| Molar Heat of Vaporization | (∆Hvap) the amount of heat absorbed by one mole of a liquid as it vaporizes at a constant temperature
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|
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| Specific Heat | the amount of heat needed to increases the temperature of 1 g of a substance 1°C; also called specific heat capacity
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|
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| Standard Heat of Formation | (∆Hf0) the change in enthalpy that accompanies the formation of one mole of a compound from its elements with all substances in their standard states at 25°C
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| Surroundings | everything in the universe outside of the system
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| System | a part of the universe on which you focus your attention
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|
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| Thermochemical Equation | a chemical equation that includes the enthalpy change
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|
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| Thermochemistry | the study of energy changes that occur during chemical reactions and changes in state
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|
||||
| Activated Complex | an unstable arrangement of atoms that exists momentarily at the peak of the activation-energy barrier; an intermediate or transitional structure formed during the course of a reaction
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|
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| Activation Energy | the minimum energy colliding particles must have in order to react
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|
||||
| Chemical Equilibrium | a state of balance in which the rates of the forward and reverse reactions are equal; no net charge in the amount of reactants and products occurs in the chemical system
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|
||||
| Collision Theory | atoms, ions, and molecules can react to form products when they collide, provided that the particles have enough kinetic energy
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|
||||
| Common Ion | an ion that is common to both salts in a solution; in a solution of silver nitrate and silver chloride Ag+ is the common ion
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|
||||
| Common Ion Effect | a decrease in the solubility of an ionic compound caused by the addition of a common ion
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|
||||
| Elementary Reaction | a reaction in which reactants are converted to products in a single step
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|
||||
| Entropy | (s) a measure of the disorder of a system; systems tend to go from a state of order(low) to a state of maximum disorder(high)
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|
||||
| Equilibrium Constant | (Keq) the ratio of product concentrations to react concentrations at equilibrium, with each concentration raised to a power equal to the umber of moles of that substance in the balanced chemical equation
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|
||||
| Equilibrium Position | the relative concentrations of reactants and products of a reaction that has reached equilibrium; indicates whether the reactants or products are favored in the reversible reaction
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|
||||
| First-Order Reaction | a reaction in which the reaction rate is proportional to the concentration of only one reactant
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|
||||
| Free Energy | the energy available to do work
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|
||||
| Gibbs Free Energy Change | ∆G the maximum amount of energy that can be coupled to another process to do useful work
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|
||||
| Inhibitor | a substance that interferes with the action of a catalysts
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|
||||
| Intermediate | a product of one of the steps in a reaction mechanism; it becomes a reactant in the next step
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|
||||
| Law of Disorder | it is natural tendency of systems to move in the direction of maximum chaos or disorder
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|
||||
| Le Chatliers Principle | when stress is applied to a system dynamic equilibrium, the system changes in a way that relieves the stress
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|
||||
| Nonspontaneous Reaction | a reaction that does not favor the formation of products at the specifies conditions
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|
||||
| Rate | describes the speed of change over an interval of time
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|
||||
| Rate Law | an expression relating the rate of reaction to the concentration of reactants
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|
||||
| Reaction Mechanism | a series of elementary reactions that take place during the course of a complex reaction
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|
||||
| Reversible Reaction | a reaction in which the conversion of reactants into products and the conversion of products into reactants occur simultaneously
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|
||||
| Solubility Product Constant | Ksp the equilibrium constant applied to the solubility of electrolytes; it is equal to the product of the concentration of the ions each raised to the power equal to the coefficient of the ion in the dissociation equation
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|
||||
| Specific Rate Constant | a proportionality constant relation the concentration of reactions to the rate of reaction
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|
||||
| Spontaneous Reaction | a reaction that favors the formation of products at the specified conditions; spontaneity depends on enthalpy and entropy changes
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|
||||
| Transition State | a term sometime used to refer to the activated complex
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|
||||
| Acid Dissociation Constant (Ka) | The ratio of the concentration of the dissociated form of an acid to the undissocitated form; stronger acids have larger Ka Values than weaker acids
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|
||||
| Acidic Solution | any solution in which the hydrogen-ion concentration is greater than the hydroxide-ion concentration
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|
||||
| Alkaline Solution | a basic solution
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|
||||
| Amphoteric | a substance that can act as both an acid and a base
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|
||||
| Base Dissociation Constant (Kb) | the ratio of the concentration of the conjugate acid times the concentration of the hydroxide ion to the concentration of conjugate base
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|
||||
| Basic Solution | any solution in which the hydroxide-ion concentration is greater than the hydrogen-ion concentration
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|
||||
| Buffers | a solution in which the pH remains relatively constant when small amounts of acid or base are added; a buffer can be either a solution of a weak acid and the salt of a weak acid or a solution of a weak base with the salt of a weak base
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|
||||
| Buffer Capacity | a measure of the amount of acid or base that may be added to a buffer solution before a significant change in pH occurs
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|
||||
| Conjugate Acid | the particle formed when a base gains a hydrogen-ion; NH4+ is the conjugate acid of the base NH3
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|
||||
| Conjugate Acid-Base Pair | two substances that are related by the loss or gain of a single hydrogen ion; ammonia (NH3) and the ammonia ion (NH4+) are a conjugate acid-base pair
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|
||||
| Conjugate Base | the particle that remains when an acid has donated a hydrogen ion; OH- is the conjugate base of the acid water
🗑
|
||||
| Diprotic Acid | any acid that contains two ionizable protons (hydrogen ions); sulfuric acid (H2SO4) is a Diprotic acid
🗑
|
||||
| End Point | the point in a titration at which the indicator changes color
🗑
|
||||
| Equivalent Point | the point of titration where the number of moles of hydrogen ions equals the number of moles of hydroxide ions
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|
||||
| Hydronium Ion(H3O+) | the positive ion formed when a water molecule gains a hydrogen ion
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|
||||
| Ion-Product Constant for Water(Kw) | the product of the concentration of hydrogen ions and hydroxide ions in water; it is 1*10-14 at 25 degrees Celsius
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|
||||
| Lewis Acid | any substance that can accept a pair of electrons to form a covalent bond
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|
||||
| Lewis Base | any substance that can donate a pair of electrons to form a covalent bond
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|
||||
| Monoprotic Acid | any acid that contains one ionizable proton (hydrogen ion); nitric acid is a Monoprotic acid
🗑
|
||||
| Neutral Solution | an aqueous solution in which the concentration of hydrogen and hydroxide ions are equal; it has a pH pf 7.0
🗑
|
||||
| Neutralization Reaction | a reaction in which an acid and a base react in a aqueous solution to produce a salt and water
🗑
|
||||
| pH | a number use to denote the hydrogen-ion concentration or acidity of a solution; it is the negative logarithm of the hydrogen-ion concentration of a solution
🗑
|
||||
| Salt Hydrolysis | a process in which the cations or anions of a dissociated salt accept hydrogen ions from water or donate hydrogen ions to water
🗑
|
||||
| Self-Ionization | a term describing the reaction in which two water molecules react to produce ions
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|
||||
| Standard Solution | a solution of known concentration used in carrying our a titration
🗑
|
||||
| Strong Acid | an acid that is completely (or almost completely) ionized in aqueous solution
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|
||||
| Strong Base | a base that completely dissociates into metal ions and hydroxide ions in aqueous solution
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|
||||
| Titration | process used to determine the concentration of a solution (often an acid or base) in which a solution of known concentration (the standard) is added to a measured amount of the solution of unknown concentration until an indicator signals the end point
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|
||||
| Tripotic Acid | any acid that contains three ionizable protons (hydrogen ions)
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|
||||
| Weak Acid | an acid that is only slightly ionized in aqueous solution
🗑
|
||||
| Weak Base | a base that reacts with water to form the hydroxide ion and the conjugate acid of the base
🗑
|
Review the information in the table. When you are ready to quiz yourself you can hide individual columns or the entire table. Then you can click on the empty cells to reveal the answer. Try to recall what will be displayed before clicking the empty cell.
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Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
To hide a column, click on the column name.
To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
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