Quantum Theory Flashcards
All forms of electromagnetic radiation travel at * in waves. The properties of a wave are its * (, distance between corresponding points on adjacent waves), * (, number of cycles the wave undergoes
per second), and * (the height of the wave), which is related to the * (brightness) of the light.
the speed of light (c) wavelength frequency amplitude intensity
All forms of * travel at the speed of light (c) in * .
The properties of a wave are its wavelength (,* ), frequency (, * ), and amplitude (* ), which is related to the
intensity (*) of the light.
electromagnetic radiation, waves,
distance between corresponding points on adjacent waves
number of cycles the wave undergoes per second
the height of the wave brightness
In everyday experience, light is diffuse and matter is chunky, but certain phenomena—* (the light emitted by hot objects), the * (the flow of current when light strikes a metal), and * (the specific colors seen when a substance is excited)—can only be explained if * consists of “*” (quanta) that occur in, and thus change by, * amounts. The energy of a quantum is related to its *
blackbody radiation photoelectric effect atomic spectra energy packets fixed frequency
In everyday experience, light is diffuse and matter is chunky, but certain phenomena— blackbody radiation (), the photoelectric effect (), and atomic spectra ()—can only be explained if energy consists of “packets” () that occur in, and thus change by, fixed amounts.
The energy of a quantum is related to its *
the light emitted by hot objects
the flow of current when light strikes a metal
the specific colors seen when a substance is excited
quanta
frequency
According to the Bohr model, an * consists of separate lines because an atom has certain allowable * (states). The energy of the atom changes when the electron * as the atom absorbs (or emits) light of a *
atomic spectrum
energy levels
moves from one orbit to another
specific frequency
According to the Bohr model, an atomic spectrum consists of * because an atom has * energy levels (states). The * of the
atom changes when the electron moves from one orbit to another as the atom
* of a specific frequency
separate lines,
certain allowable
energy
absorbs (or emits) light
Wave-particle duality means that * has * properties (as shown by the de Broglie wavelength and electron diffraction) and * has * properties (as shown by photons of light behaving like particles with momentum).
These properties are observable only on the *, and because of them, we can never know the * and * of an electron in an atom (uncertainty
principle)
matter - wavelike
energy - particle-like
atomic scale
position, speed
Wave-particle duality means that matter has wavelike properties (as shown by the * ) and energy has particle-like properties (as shown by ). These properties are observable only on the atomic scale, and because of them, we can never know the position and speed of an * in an atom ()
de Broglie wavelength and electron diffraction
photons of light behaving like particles with momentum
electron
uncertainty principle
According to the *, each energy level of the atom is associated with an * (wave function), a mathematical function describing the electron’s * in three dimensions. We can know the * of the electron being found within a particular tiny volume of space, but not its *. This probability decreases with * from the nucleus
quantum-mechanical model of the H atom atomic orbital position probability exact location distance
According to the quantum-mechanical model of the H atom, each * of
the atom is associated with an atomic orbital (*), a mathematical * describing the electron’s position in *. We can know the probability of the electron being found within a particular tiny volume of space, but not its exact location. This probability * with distance from the
nucleus
energy level,
wave function
function, three dimensions
decreases
Quantum numbers denote the * (n, principal), * (l, angular momentum), and * (ml, magnetic) of each atomic orbital. An * consists of *, which consist of *. There is a hierarchy of quantum
numbers, such that n limits *, which limits *
energy shape spatial orientation energy level, sublevels, orbitals l, ml
- denote the energy (), shape (),
and spatial orientation () of each atomic orbital. An energy level () consists of sublevels (*), which consist of orbitals. There is a hierarchy of quantum
numbers, such that n limits l, which limits ml
Quantum numbers n, principal l, angular momentum ml, magnetic n (principal), l (angular momentum)
In the H atom, there is only one type of electrostatic interaction: *. For the H atom only, the energy levels depend exclusively
on the
attraction between
nucleus and electron
principal quantum number (n)
In the * atom, there is only one type of *: attraction between nucleus and electron. For the H atom only, the * depend exclusively
on the principal quantum number (n)
H, electrostatic interaction
energy levels
