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Pearson Chemistry Chapter 5 Vocabulary

Terms in this set (21)

Energy level
the fixed energies an electron can have.
Quantum
the amount of energy needed to move an electron from one energy level to another energy level.
Quantum mechanical model
the modern description of the electrons in atoms.
Atomic orbital
the model describing the probability of finding an electron at various locations around the nucleus.
Electron configuration
the ways in which electrons are arranged in various orbitals around the nuclei of atoms.
aufbau principle
the rule that electrons occupy the orbitals of lowest energy first.
Pauli exclusion principle
an atomic orbital may describe at most two electrons, each with opposite spin direction.
Spin
a quantum mechanical property of electrons that may be thought of as clockwise or counterclockwise.
Hund's rule
electrons occupy orbitals of the same energy in a way that makes the number of electrons with the same spin direction as large as possible.
Amplitude
the wave's height from zero to the crest.
Wavelength
The distance between two corresponding parts of a wave, e.g. between two crests.
Frequency
the number of cycles to pass a given point per unit of time.
Hertz (Hz)
the basic SI unit of frequency (cycles per second)
Electromagnetic radiation
includes radio waves, microwaves, infrared waves, visible light, ultraviolet waves, X-rays, and gamma rays.
Spectrum
a continuous range of wavelengths and frequencies.
Atomic emission spectrum
the wavelengths of spectral lines that are characteristic of an element.
Planck's constant
A fundamental constant, h, that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule·second.
Photoelectric effect
refers to the emission of electrons from a metal when certain frequencies of light shine on the metal.
Photons
light quanta (pieces).
Ground state
when an electron has its lowest possible energy.
Heisenberg uncertainty principle
states that it is not possible to know both the velocity and the position of a particle at the same time.
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