Chapter 7 – Electrons in Atom and the Periodic Table – Flashcards
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| Electromagnetic Spectrum |
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| a continuous rane of radiant energy that includes radio waves, infrared radiation, visible light, ultraviolet radiation, X-rays, and gamma rays |
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| Electromagnetic Radiation |
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| any form of radiant energy in the electromagnetic spectrum |
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| Wavelength |
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| the distance from crest to crest or trough to trough on a wave |
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| Frequency |
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| expresses the number of times a wave passes a given point in some unit of time (typically one second) |
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| Hertz |
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| the SI unit of frequency expresses in the units s-1 |
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| Frequency |
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| expresses the number of times a wave passes a given point in some unit of time (typically one second) |
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| Amplitude |
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| the height of the crest or the depth of the trough with respect to the center line of the wave; the intensity of a wave is related to this |
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| Refraction |
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| the bending of light as it passes from one medium to another with different densities |
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| Diffraction |
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| the bending of electromagnetic radiation as it passes around the edge of an object or through narrow openings |
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| Interference |
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| the interaction of waves that results in either reinforcing or canceling the amplitudes |
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| Frannofer Lines |
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| set of dark lines in the otherwise continuous solar spectrum |
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| Atomic Emission Spectra |
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| consist of bright lines on a dark background; appear at specific wavelengths; also called bright-line spectra |
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| Atomic Absorption Spectra |
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| consist of dark lines produced when free, gaseous atoms are illuminated by external sources of radiation; also called dark-line spectra |
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| Quantum |
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| the smallest discrete quantity of a particular form of energy |
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| Quantum Theory |
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| based on the idea that energy is absorbed and emitted in discrete quanta |
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| Quantized |
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| has values that are restricted to whole-number multiples of a specific base value; the base unit of energy is the quantum |
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| Planck's Constant |
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| the proportionality constant between the energy and frequency of electromagnetic radiation |
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| Photoelectric Effect |
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| occurs when light strikes a metal surface and an electric current (a flow of electrons) is produced |
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| Threshold Frequency |
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| the minimum frequency of light that is required to produce the photoelectric effect |
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| Photon |
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| quantum of electromagnetic radiation |
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| Work Function |
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| the amount of energy needed to dislodge an electron from the surface of a metal |
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| Energy Level |
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| an allowed state that an electron can occupy in an atom |
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| Electron Transitions |
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| movement of electrons between energy levels |
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| Ground State |
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| the lowest energy level available to an electron in an atom |
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| Excited State |
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| any energy state above the ground state |
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| Matter Wave |
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| the wave associated with any particle |
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| Standing Wave |
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| confined to a given space and has a wavelength that is related to L of the space |
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| Node |
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| a location in a standing wave that experiences no displacement |
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| Wave Mechanics |
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| the description of the wavelike behavior of particles on the atomic level |
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| Schrodinger Wave Equation |
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| describes the electron in hydrogen as a matter wave and indicates how it varies with location and time around the nucleus solutions to the wave equation are the energy levels of the hydrogen atom |
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| Wave Function |
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| a solution to the Schrodinger equation |
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| Orbitals |
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| defined by the square of the wave function; are regions around the nucleus where the probability of finding an electron is high |
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| Quantum Numbers |
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| unique combination of three integers that define each orbital |
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| Principal Quantum Numbers |
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| a positive integer that describes the relative size and energy of an atomic orbital or group of orbitals in an atom |
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| Angular Momentum Quantum Number |
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| an integer that may have any value from 0 to n-1; defines the shape of an orbital |
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| Magnetic Quantum Number |
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| an integers that may have any value from -l to +l; defines the orientation of an orbital in space |
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| Spin Magnetic Quantum Number |
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| either +1/2 or -1/2, indicating that the electron spin orientation is either up or down |
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| Pauli Exclusion Principle |
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| states that no two electrons in an atom each have the same set of quantum numbers |
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| Valence Electrons |
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| the electrons in the outermost shell of an atom and have the most influence on the atoms chemical behavior |
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| Core Electrons |
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| electrons in the files, inner-shell in an atom and are not involves in chemical reactions |
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| Degenerate |
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| orbitals that have the exact same energy level |
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| Hund's Rule |
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| states that lowest energy electron configuration of an atom is the configuration with the maximum of unpaired electrons in degenerate orbitals, all having the same spin |
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| Electron Configuration |
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| describes the distribution of electrons among the orbitals of an atom or ion |
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| Aufbau Principle |
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| the method of building electron configurations one electron at a time; one elctron is added to the lowest-energy orbitals of a ground-state atom; the electron configurations of atoms are built in sequence as atomic number increases in order across the rows of the periodic table |
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| Orbital Diagrams |
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| one way of showing the arrangement of electrons in an atom or ion using boxes to represent orbitals |
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| Isoelectronic |
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| atoms and ions that have identical numbers and configurations of electrons as each other |
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| Orbital Penetration |
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| occur when an electron in an outer orbital has some probability of being as close to the nucleus as an electron in an inner shell |
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| Screening |
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| the effect when inner-shell electrons protect outer-shell electrons from experiencing the total nuclear charge; also called shielding |
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| Effective Nuclear Charge |
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| the attractive force toward the nucleus experienced by an electron in an atom; its value is the positive charge on the nucleus reduced by the extent to which other electrons in the atom shield it from the nucleus |
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| Ionization Energy |
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| the amount of energy needs to remove one mole of electrons from a mole of ground-state atoms or ions in the gas phase |
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| Effective Nuclear Charge |
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| the attractive force toward the nucleus experienced by an electron in an atom; its value is the positive charge on the nucleus reduced by the extent to which other electrons in the atom shield it from the nucleus |
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| Ionization Energy |
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| the amount of energy needs to remove one mole of electrons from a mole of ground-state atoms or ions in the gas phase |
