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Chapter 4 Arrangement of Electrons in Atoms 4-1 The Development of the New Atomic Model • Rutherford’s atomic model – nucleus surrounded by fastmoving electrons- not complete model Wave Nature of Light • Electromagnetic Radiation- form of energy that exhibits wavelike behavior • Ex: visible light, microwaves, x-rays • Electromagnetic Spectrum- encompasses all forms of EM radiation Electromagnetic Spectrum • Wavelength (λ )- shortest distance between equivalent points on a continuous wave • Measured crest to crest or trough to trough • Frequency (ν )- number of waves that pass a given point per second • 1 Hertz (Hz) = 1 wave per second; SI unit of frequency • Amplitude- wave’s height from the origin to a crest or from origin to trough • Speed of light = wavelength x frequency • C = λν • Photoelectric Effectelectrons are emitted from a metal’s surface when light of a certain frequency shines on the surface • Ex: calculator with photoelectric cell Particle Nature of Light • Quantum conceptproduces glowing light of hot objects • Quantum- minimum amount of energy that can be gained or lost by an atom • Equantum = hv • E = energy • V = frequency • h = Planck’s constant; 6.626 x 10-34 J•s • J is joule; SI unit for energy • Photon- particle of EM radiation with no mass that carries a quantum of energy • Ephoton = hv • Ground State- lowest allowable energy state of an atom • Excited State- when an atom gains energy • Line Emission Spectrumset of frequencies of the EM waves emitted by atoms of the element • Unique to each element, used for identification • Continuous spectrum • Bohr Model of the Atomproposed that hydrogen atom has only certain allowable energy states Sect. 4-2: The Quantum Model of the Atom • Electrons as waves…De Broglie applies light’s wave-particle duality to electrons/Bohr’s model • Heisenberg Uncertainty Principle – impossible to know position and velocity at same time • Schrödinger wave equation • Quantum theory – describes mathematically the wave properties of electrons • Orbital – probable location of electron around nucleus Atomic Orbitals and Quantum numbers • Quantum numbers – specify properties of atomic orbitals and electrons in orbitals • solutions to Schrödinger wave equation • Principal quantum number (n) – represents main energy level (shell) & tells how many sublevels • Positive integers (1,2,3,etc.) • Total # orbitals per shell = n2 • Total # electrons per shell =2n2 • Angular momentum quantum number (l) – indicates shape of orbital (sublevel) • l = zero and all positive integers less than or equal to n-1 • l=0, s orbital (spherical) • l=1, p orbital (dumbbell) • l=2, d orbital • l=3, f orbital • Magnetic quantum number (m) – indicates the orientation of orbital around nucleus • range from -2 to +2, depending on sublevels • Spin Quantum number – indicates spin state of electron • can only equal ½ or -½ • orbital holds 2 max electrons & they must have opposite spins Sect. 4-3: Electron Configurations • Electron configuration – arrangement of electrons in an atom Rules for Electron Configurations • Aufbau principle – lowest energy level fills first • Pauli exclusion principle – electrons in same orbital, opposite spin • Hund’s rule – orbitals of equal energy must all have 1 electrons before a second can be added • Orbital Notation (Diagram) – lines, arrows, principal quantum #, and sublevel letter • Electron Configuration Notation – principal quantum #, sublevel letter, and superscript (# e-) • Noble Gas Notation – shortened version of electron configuration notation • Deviations from normal electron configurations (more stable with pulling one from s to halffill or fill d) • Chromium • Copper