Chapter 5 Chemistry Study Guide – Flashcards
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Electromagnetic Spectrum
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Visible light is form of energy that exhibits wavelike behavior as it travels through space.
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Wavelength (?)
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is the shortest distance between equivalent points on a continuous wave. measured from crest to crest or trough to trough
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Frequency (?)
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is the number of waves that pass a given point per second. measured in Hz. 1/v
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C = ??
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C = 3.00 x 10? m/s in a vacuum Electromagnetic Wave relationship
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As wavelength increases,
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frequency decreases
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Quantum
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is the minimum amount of energy that can be gain or lost by an atom.
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Equantum = h?
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h = Plank's constant = 6.626 x 10?³? J?s v = frequency Equantum = energy Equation shows energy of radiation increases as radiation frequency decreases
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photon
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massless particle that carries a quantum of energy
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Ground state
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the lowest allowable energy state of an atom
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n, quantum number,
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assigned to each orbit, energy level
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Excited state
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when an electron is not in it's ground state
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Heisenburg Uncertainty Principle
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states that it is fundamentally impossible to know precisely both the velocity and position of a particle at the same time
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Aufbau principle
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states that each electron occupies the lowest energy orbital available.
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Pauli exclusion principle
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states that a maximum of two electrons can occupy a single atomic orbital, but only if the electrons have opposite spins.
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Hund's rule
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states that single electrons with the same spin must occupy each equal energy orbital before additional electrons with opposite spins can occupy the same orbitals
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Valance Electrons
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defined as electrons in the atom's outermost orbitals - generally those orbitals associated with the atom's highest principal energy level.
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S Orbital
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- shaped like a circle
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P Orbital
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- shaped like dumbbells
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D Orbital
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- shaped like double dumbbells
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F Orbital
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- too complex to draw or describe
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Four quantum numbers per electron
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describe location and energy in the atom.
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"n"
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principle quantum number and represents the energy level of the electron. Maximum # of e? = 2n²
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"l"
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sub level of the electron, which depends on the type of orbital describes the orbital shape withing an energy level
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"m"
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describes orientation of orbital in space
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"s"
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describes spin of electron
