Chemistry Chapter 5

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52 Terms

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Electromagnetic radiation
a form of energy that exhibits wavelike behavior as it travels through space
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Wavelength
the shortest distance between 2 equivalent points on a continuous wave
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Units for wavelength
meter or nanometer
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Symbol for wavelength
lambda, λ
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Frequency
the number of waves that pass a given point per second
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Unit for frequency
hertz, 1/s
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Symbol for frequency
nu, ν
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Amplitude
the wave's height from the origin to a crest or trough
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Speed of light equation
c (speed of light, m/s) = λ (wavelength, m or nm) * ν (frequency, hertz)
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inversely
Wavelength and frequency vary ________.
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Electromagnetic spectrum
a spectrum that includes all forms of electromagnetic radiation
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Quantum theory
a theory created by Max Planck to explain how matter lost and gained only small, specific amounts of energy
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Quantum
the minimum amount of energy that can be lost or gained or gained by an atom
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Photon
a particle-like bundle of energy without mass that carries a quantum of electromagnetic energy
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Energy of a photon equation
E (energy, joules) = h (Planck's constant, joules * seconds) * ν (frequency, hertz)
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Spectroscopy
the method of studying substances exposed to energy
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Spectrum
the pattern of energy studied in spectroscopy
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Atomic emission spectrum
the set of frequencies or wavelengths of the electromagnetic waves emitted by atoms of the element
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unique
Each element produces a ________ line spectrum.
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Bohr's (planetary) model
an early atomic model of the hydrogen atom that was developed by studying the emission spectrum of hydrogen
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Accurate part of Bohr's model
the electron can only posses certain quantities of energy/ have certain allowed energy states
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Ground state
the lowest and most stable energy state
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Excited state
any state of energy that is more than the lowest amount
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Inaccurate part of Bohr's model
the electron moves around the nucleus in certain allowed circular orbits
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waves
Electrons should be thought of as ________ spread out in space. (Louis de Broglie)
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measurement
The act of ________ disturbs the object being measured.
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Heisenberg uncertainty principle
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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Quantum mechanical model
modern atomic model, a mathematical equation that treated an electron as a wave and solved the equation for the hydrogen atom
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Lowest energy level
1
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farther
The ________ the electron, the higher the energy level
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Energy sublevel
a subdivision of an energy level, assigned a letter: s, p, d, or f
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Atomic orbital
the volume around the nucleus in which the electron is likely to be found
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Sublevel "s"
spherical, 1 orientation
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Sublevel "p"
dumbbell, 3 orientations
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Sublevel "d"
cloverleaf, 4 orientations, dumbbell with donut, 1 orientation (5 orientations in total)
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Sublevel "f"
7 different orientations
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larger
The orbitals in the higher energy levels are ________ than the orbitals in the lower energy levels
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Max electrons in "s"
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Max electrons in "p"
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Max electrons in "d"
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Max electrons in "f"
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Electron configuration
a notation for showing how electrons are arranged in energy sublevels
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2
How many electrons can be in a sublevel
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Aufbau principle
sublevels are "filled" with electrons starting with the lowest energy sublevel
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Quantum numbers
a set of four numbers used to describe the properties in electrons in an atom
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Pauli exclusion principle
states that each electron in an atom has a unique set of 4 quantum numbers and that 2 electrons can be in an orbital only if they have opposite spins
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Abbreviated electron configuration
noble gas in brackets and portion of configuration that remains
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Orbital diagram
notation used to depict electrons in orbitals
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Hund's rule
the most stable arrangement of electrons within a sublevel is one with greatest number of parallel spins
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Degenerate
electrons with the same amount of energy
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Electron dot diagram/ Lewis dot structure
notation used tp symbolize atom's valence electrons
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Valence electron
the electrons in the outermost (largest) orbitals, determine element's properties