Module 6: Quantum Mechanics Flashcards
He extended the wave-particle duality of light that Einstein used to resolve the photoelectric-effect paradox to material particles
Louis de Broglie
he predicted that a particle should also exhibit the behavior of a wave
Louis de Broglie
Formula for de Broglie wavelength
λ = h / mV
Is de Broglie wavelength not a characteristic of particles?
No
two scientists that demonstrated experimentally that electrons can exhibit wavelike behavior
C.J. Davisson and L.H. Germer
Field of study that includes quantization of energy, wave-particle duality, and the Heisenberg uncertainty principle to describe matter
Quantum Mechanics
This principle states that it is fundamentally impossible to determine simultaneously and exactly both the momentum and the position of a particle
Heisenberg Uncertainty Principle
Unlike de Broglie who thought of the electron in terms of circular stationary waves, this person properly though in terms of three-dimensional stationary waves
Schrodinger
three-dimensional stationary waves that Schrodinger thought of
Wavefunction (ψ)
Who proposed the interpretation of wavefunction?
Max Born
he said that electrons are still particles and so the waves represented by ψ are not physical waves but are complex probability amplitudes
Max Born
the square of this describes the probability of the quantum particle being present near a certain location in space
Wavefunction (ψ)
It can be used to determine the distribution of the electron’s density
Wavefunction (ψ)
This describe the location or general description of an electron
Quantum numbers
A general region in an atom within which an electron is most probable to reside
Atomic orbital
The four quantum numbers
principal
angular momentum
magnetic
spin
this quantum number specify the shell an electron occupies in an atom
Principal quantum number (n)
this quantum number defines the location of the energy level and general size and energy of the orbital
Principal quantum number (n)
this quantum number determines the average distance form nucleus
Principal quantum number (n)
This quantum number’s values are 1, 2, 3, 4, ..
Principal quantum number (n)
As the principal quantum number (n), what happens to the distance from the nucleus and energy?
Increases
This quantum number defines the shape of the orbital which is dependent on where you can probably find electrons
Angular Momentum Quantum Number (l)
This quantum number is also known as the subshell
Angular Momentum Quantum Number (l)
This quantum number’s values are 0, 1, 2, (n-1)
Angular Momentum Quantum Number (l)
This quantum number describes the orientation of the orbital in space
Magnetic Quantum Number (ml)
This quantum indicates the region that an electron occupies within a subshell based on the shape of the subshell
Magnetic Quantum Number (ml)
This quantum number’s values are 0, +1, -1, +2, -2, (-l to +l)
Magnetic Quantum Number (ml)
This quantum number describes the orientation of electron spin
Spin Quantum Number (s)
A completely quantum phenomenon with no analogous in the classic al realm
Electron spin
Describes an intrinsic electron “rotating” or “spinning”
Electron Spin
This quantum number states that each electron acts as atiny magnet with an angular momentum, even though this rotation cannot be observed in terms of the spatial coordinates
Spin Quantum Number (s)
This quantum number’s values are either +1/2 or -1/2
Spin Quantum Number (s)
Value of spin quantum number (s) with a slightly higher energy in an external field than the other
s = -1/2
Principle that states no two electrons in the same atom can have exactly the same set of all the four quantum number
Pauli Exclusion Principle
Which orbital have the lowest energy
Orbitals closest to the nucleus of an atom
lowest to highest energy of subshells
s < p < d < f
This is the arrangement of electrons in the orbitals of an atom
Electron Configuration
Three information that an electron configuration have
Principal quantum number (n)
Orbital type (subshell ,l)
number of electrons in a particular subshell
unpaired electrons that behave like a magnet and attract others
Paramagnetic
Principle that states that the procedure in which the electron configuration of the elements is determined by “building” them in order of atomic number
Aufbau Principle
Principle that states that lowest energy level should be filled up first before the higher energy levels
Aufbau Principle
writing the electron configuration by abbreviation using the noble gas closest to the atom
Abbreviated Electron Configuration
the electron occupying the inner shell orbitals
Core Electrons
outer-shell electrons
Valence Electrons
type of electrons that correspond to noble gases electron configuration
Core Electrons
type of electrons that heavily contribute to an element’s properties and they are the electrons involved in chemical bonding
Valence Electrons
pictorial representations of the electron configuration, showing the individual orbitals and the pairing arrangement of electrons
Orbital diagrams
Electron configuration that is exceptions to the order of filling of orbitals that are indicated by Aufbau principle
Anomalous Electron Configuration
for this type of electron configuration, half-filled and completely-filled subshells apparently represent conditions of preferred stability
Anomalous Electron Configuration
electron configuration exceptions because the magnitude of the repulsion between electrons is greater than the differences in energy between subshells
Anomalous Electron Configuration
meaning of s, p, d and f?
sharp
principal
diffused
fundamental
formula for number of orbitals in a subshell
2l + 1
formula for total number of orbital
n e2 (n squared)
formula for maximum number of electrons
2n e2 ( 2 n squared)
