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By: 3rd Period Chemistry Actinide Angular Momentum Quantum Number Bohr De Broglie Degenerate Effective Nuclear Charge Electron Configuration Excited State Family Ground State Group Heisenberg Uncertainty Principle Hund’s Rule Ionization Energy Lanthanide Probability Density Quantum Number Line Spectrum Magnetic Quantum Number Noble Gas Node Nuclear Model of the Atom Orbital Pauli Exclusion Principle Period Photoelectric Effect Photon Quantum Theory Rare Earth Rutherford Schrödinger Spectrum Spin Quantum Number Transition Metal Wave-Particle Duality Work Function X-ray Photoelectron Spectroscopy Principal Quantum Number Actinide Highest level electron is in the 5f orbital Noble gas Atomic numbers 90-103 Angular Momentum Quantum Number 2nd quantum number Principal quantum number Symbol-l Bohr Developed the planetary model of the atom Aristotle planets De Broglie Wave-particle duality = h/mv Aristotle Degenerate There is no energy difference with orientations Multiple differences No difference N/a Effective Nuclear Charge Force felt by the outermost electron ineffective nuclear charge Outer force Electron Configuration List of electrons in each orbital Random group of electrons Electron list Excited State The orbitals that have more energy Ground state Further from the nucleus than the first Family Consists of elements with similar chemical properties columns period Ground State The orbital with the least amount of energy Excited state Group Consists of elements with similar chemical properties Period Heisenberg Uncertainty Principle Impossible to simultaneously determine the position/momentum of an electron Locked positions Hund’s Rule the lowest energy is for electrons to exist in separate orbitals with parallel spins Closest to the nucleus columns revolutions parallel Opposite spins Ionization Energy The energy required to remove an electron from an atom in the gaseous state Energy to add an electron to an element in the gaseous state Lanthanide Highest energy electron is in the 4f orbital Noble gas Line Spectrum Shows interactions between light and electrons occur at specific energies emission Magnetic Quantum Number 3rd quantum number Principal quantum number Noble Gas Especially stable, low-energy, don’t tend to combine with other elements, have s and p orbitals that are completely full remove electron Rare earth Interactions, light, electron Symbol- ml Far right of the periodic table actinides Node Region with zero probability of finding an electron orbital Nuclear Model of the Atom Rutherford’s model nucleus with electrons around it Aristotle’s model Orbital Region where finding an electron is high Node Pauli Exclusion Principle Every electron in an atom has a unique set of four quantum numbers Random set of numbers Period The highest value of n in the electron configuration of an element will be the same for all elements in a period. nucleus Basketball model/ gold foil Electron cloud Quantum numbers rows Family or group Photoelectric Effect process by which some metals emit electrons when exposed to light Keeping electrons Lose electrons in light Photon Light particle Dark particle Light Principal Quantum Number 1st quantum number Magnetic quantum number Symbol-n Probability Density Volume of space in which the electron is likely to be found nucleus Quantum Number Four values that completely describe an electron Atomic number Electron cloud N,l, ml, ms Quantum Theory there are specific choices rather than any value within a range Classical theories 1 or 2 but not 1.5 Rare Earth Highest energy electron is in the 4f orbital Noble gas lanthanide Rutherford Nuclear model of the atom Aristotle Gold foil Schrödinger Energy of a hydrogen electron has a wave Aristotle Hydrogen wave Spectrum A graph of the intensity of light versus its energy or wavelength black Spin Quantum Number Graph of intensity 4th quantum number Principal quantum number Symbol- ms Transition Metal the highest-energy electron is in a d orbital Noble gas Wave-Particle Duality The properties of light Properties of the dark side De Broglie Work Function the energy required for an electron to escape Energy required to hold an electron escape X-ray Photoelectron Spectroscopy X-rays are used to remove electrons from an atom Full shells x-rays Back to Top