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Chemistry H
chemistry definitions
| Question | Answer |
|---|---|
| The capacity for doing work; it exsists in several forms including chemical, nuclear, electrical, radiant, mechanical, and thermal energies. | Energy |
| The quantity of heat that raises the temperature of 1 gram of pure water 1 degree celcius. | Calorie |
| The quantity of heat required to change an objects temperature by exactly 1 degree celcius. | Heat Capacity |
| A heat-absorbing process. | Endothermic Process |
| The measurement of heat changes for physical and chemical processes. | Calorimetry |
| The pressure exerted by each gas in a gaseous mixture. | Partial pressure |
| The energy that is transferred from on body to another because of a temperature difference. | Heat(q) |
| The SI unit of energy; 4.184 j = 1 calorie | joule |
| The quantity of heat, in joules or calories, required to raise the temperature of 1 gram of a substance 1 degree celcius | Specific Heat capacity |
| A heat-dissipating process | exothermic process |
| The tendancy of molecules and ions to move torward areas of lower concentration until the concentration is uniform throughout the system. | diffusion |
| The capacity for doing work; it exsists in several forms including chemical, nuclear, electrical, radiant, mechanical, and thermal energies. | Energy |
| The quantity of heat that raises the temperature of 1 gram of pure water 1 degree celcius. | Calorie |
| The quantity of heat required to change an objects temperature by exactly 1 degree celcius. | Heat Capacity |
| A heat-absorbing process. | Endothermic Process |
| The measurement of heat changes for physical and chemical processes. | Calorimetry |
| The pressure exerted by each gas in a gaseous mixture. | Partial pressure |
| The energy that is transferred from on body to another because of a temperature difference. | Heat(q) |
| The SI unit of energy; 4.184 j = 1 calorie | joule |
| The quantity of heat, in joules or calories, required to raise the temperature of 1 gram of a substance 1 degree celcius | Specific Heat capacity |
| A heat-dissipating process | exothermic process |
| The tendancy of molecules and ions to move torward areas of lower concentration until the concentration is uniform throughout the system. | diffusion |
| Equal volumes of gasses at the same temperature and pressure contain equal number of particles. | Avogadro's hypothesis |
| At constant volume and tempertaure, the total pressure of a mixture of gasses is the sum of the partial pressures of all the gasses present. | Dalton's Law of Partial Pressure |
| The heighth of a wave from the origin to the crest | amplitude |
| The arrangement of electrons around the nucleus of an atom in its ground state | Electron configuration |
| A series of energy waves that travel in a vacuum at three times ten to the tenth cm/s; includes radio waves, microwaves, visible light, infrared and ultraviolet light, xrays, and gamma rays. | Electromagnetic radiation |
| The number of wave cycles that pass a given point per unit of time; There is a inverse relationship between the frequency and wavelength of a wave. | Frequency |
| The pattern of frequencies obtained by passing light emitted by atoms of an element in the gaseous state through a prism; the emission sprectrum of each element is unique to that element. | Atomic emission spectrum |
| A region around the nucleous of an atom where an electron is likely to be moving. | energy level |
| The lowest energy level occupied by an electron when an atom is in its most stable energy state. | Ground state |
| The distance between to adjacent crests of a wave. | Wave length |
| The SI unit of frequency, equal to 1 cycle per second. | Hertz |
| A quantum of light; a discrete bundle of electromagnetic energy that behaves as a particle. | Photon |
| one-half the distance between the nuclei in a molecule consisting of identical atoms | Atomic radius |
| The tendancy for an atom to attract electrons to itself when it is chemically combined with another element. | Electronegativity |
| A vertical column of elements in the periodic table; the constituent elements of a group having similar chemical and physical properties | Group |
| Electrons are ejected by certain metals when they absorb light with a frequency above a threshhold frequency | Photoelectric effect |
| The amount of energy needed to move an electron from its present energy level to the next higher one | Quantum |
| The energy required to remove an electron from a gaseous atom. | Ionization energy |
| A horizontal row of elements in the periodic table. | Period |
| Electrons enter orbitals of lowest energy first | Aufbau Principle |
| An equation that describes the wavelength of a moving particle; it predicts that all matter exibits wave like motions. | de Broglie's Equations |
| It is impossible to know both the velocity and the postion of a particle at the same time. | Heisenberg uncertainty principle |
| When electrons occupy orbitals of equal energy, 1 electron enters each orbital until all orbitals contain 1 electron with their spins parallel. | Hund's Rule |
| No more than 2 electrons can occupy an atomic orbital; these electrons must have opposite spins. | Pauli exclusion principle |
| When the elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties. | Periodic Law |
| A process in which several atomic oribitals (such as s and p orbitals) mix to form the same number of equivalent hybrid orbitals. | Hybridization |
| Any atom or group of atoms with a negative charge. | Anion |
| A molecule, like water, in which one or more atoms is slightly negative and one or more is slightly positive, unless molecular geometry causes the polarities to cancel each other out. | Polar molecule |
| A pair of valence electrons that is not involved in bonding. | Unshared pair |
| Valence-shell electron-pair repulsion theory; because electron pairs repel, molecules adjust there shapes so that valence electron pairs are as far apart as possible. | VSEPR theory |
| The weakest kind of intermolecular attraction; this attraction is thought to be caused by the motion of electrons. | Dispersion force |
| 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 structures. | Electron dot structure |
| Atoms react by gaining or losing electrons so as to require the stable electron structure of a noble gas, usually 8 valence electrons. | Octet rule |
| Any atom or group of atoms with a positive charge. | Cation |
| A chemical formula that shows the arrangment of atoms in a molecule or a polyatomic ion; each dash between 2 atoms indicates a pair of shared electrons. | Structural formula |
| an electron in the highest occupied energy level of an atom. | Valence electron |
| A term used to describe the weakest intermolecular attractions; These include dispersion forces and dipole interactions. | van der Walls force |
| A relatively strong intermolecular force in which a hydrogen atom that is covalently bonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom in the same molecule or one nearby. | Hydrogen bond |
| 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. | Surface tension |
| A solution in which the solvent is water. | Aqueous Solutions |
| Dissolved particles in a solution. | Solute |
| A surface active agent; any substance with molecules that interfere with the hydrogen bonding between water molecules, reducing surface tension; soaps and detergents are surfactants. | Surfactant |
| The dissolving medium in a solution. | Solvent |
| A compound that conducts an electric current in aqueous solution or in the molten state; all ionic compounds are electrolytes, but most covalent compounds are not. | Electrolyte |
| A compound that does not conduct electric current in aqueous solution or in the molten state. | Nonelectrolyte |
| A mixture whose particles are intermediate in size between those of a suspension and a solute solution. | Colloids |
| The chaotic movement of colloidal particles, caused by collision with particles of the solvent in which they are dispersed. | Brownian motion |
| To lose water of hydration; the process occurs when the hydrate has a vapor pressure higher than that of water vapor in the air. | Effloresce |
| A solution containing the maximum amount of solute for a given amount of solvent at a constant temperature and pressure; an equilibrium exsists between undissolved solute and ions in solution. | Saturated solution |
| Describes liquids that dissolve in each other. | Miscible |
| At a given temperature the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid. | Henry's Law |
| The concentration of solute in a solution expressed as the number of moles of solute dissolved in 1 liter of solution. | Molarity |
| A mixture from which some of the particles settle out slowly upon standing. | Suspensions |
| Scattering of light by particles in a colloid or suspension, which causes a beam of light to become visible. | Tyndal effect |
| The colloidal dispersion of one liquid in another. | Emulsion |
| A term describing salts and other compounds that remove moisture from the air. | Hygroscopic |
| A term describing a substance that removes sufficient water from the air to form a solution; The solution formed has a lower vapor pressure than that of the water in the air. | Deliquescents |
| Describes liquids that are in soluble in one another; oil and water are immiscible. | Immiscible |
| A solution that contains more solute than it can theoretically hold at a given temperature; excess solute precipitates if a seed crystal is added. | Supersaturated solution |
| A compound that produces hydrogen ions in a solution, is a hydrogen-ion donor, or an electron-pair acceptor. | Acid |
| 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. | Buffer |
| The positive ion formed when a water molecule gains a hydrogen ion; all hydrogen ions in aqueous solution are present as hydronium ions. | Hydronium ion |
| Method used to determine the concentration of a solution (often an acid or base); A solution of known concentration (the standard) is added to a measured amount of the solution of unknown concentration until an indicator signals the endpoint. | Titration |
| A compound that produces hydroxide ions in soultion, is a hydrogen-ion acceptor, or an electron-pair donor. | Base |
| a number used to denote the hydrogen-ion concentration, or acidity, of a solution; it is the negative logarithm of the hydrogen-ion concentration of a solution. | pH |
| The negative ion formed when a water molecule loses a hydrogen ion. | Hydroxide ion |
| An organic compound that contains only carbon and hydrogen. | Hydrocarbon |
| A very large molecule formed by the covalent bonding of repeating small molecules, known as monomers. | Polymer |
| An organic compound having an -OH(hydroxl) group; The general structure is R-OH. | Alcohol |
| A name originally given to the arenes because many of them have pleasant odors; any compound with bonding like that of benzene. | Aromatic compound |
| Proteins that act as biological catalysts; most of the reactions that occur in cells require catalysts. | Enzyme |
| A polymer of the ribonucleotides (RNA) or deoxyribonucleotides (DNA) found primarily in cell nuclei; Nucleic acids play an important role in the transmission of hereditary characteristics, protein synthesis, and the control of cell activities. | Nucleic acid |
| Any peptide with more than 100 amino acids. | Protein |
| an organic compound in which all carbon atoms are joined by single covalent bonds; It contains the maximum number of hydrogen atoms. | Saturated compounds |
| The control process by which hydrocarbons are broken down or rearranged into smaller, more useful molecules. | Cracking |
| A simple molecule that repeatedly | Monomers |
| An organic compound having amino (-NH2) in the carboxylic acid (-COOH) groups in the same molecule; proteins are made from the 20 naturally occured amino acids. | Amino acid |
| The name given to monomers and polymers of aldehydes and ketones that have numerous hydroxyl groups; Sugars and starches are carbohydrates. | Carbohydrate |
| A member of a large class of relatively water-insoluable inorganic compounds; Fats, oils, and waxes are lipids. | Lipid |
| One of the monomers that make up DNA and RNA; It consists of nitrogen-containing base ( a purine or pyrimidine), a sugar ( ribose or deoxyribose), and a phosphate group. | Nucleotides |
| The process used to make soap; it involves the hydrolysis of fats or oils by a hot aqueous alkali-metal hydroxide. | Saponification |
| An organic compound with one or more double or triple carbon-carbon bonds. | Unsaturated Compounds |
Created by:
HJ
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