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Questions and Answers
The azimuthal quantum number (l) can only take values from 0 up to 1.
The azimuthal quantum number (l) can only take values from 0 up to 1.
False
The principal quantum number (n) must always be a positive integer excluding zero.
The principal quantum number (n) must always be a positive integer excluding zero.
True
Electrons can exist in discrete locations around the nucleus.
Electrons can exist in discrete locations around the nucleus.
False
The spin states of electrons are represented as +½ and -½.
The spin states of electrons are represented as +½ and -½.
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Each atomic orbital can accommodate a maximum of four electrons.
Each atomic orbital can accommodate a maximum of four electrons.
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Electrons possess both particle-like and wave-like properties.
Electrons possess both particle-like and wave-like properties.
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The magnetic quantum number (ml) can take on a value of 3 for p orbitals.
The magnetic quantum number (ml) can take on a value of 3 for p orbitals.
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The wavefunction describes a precise location of an electron within an atom.
The wavefunction describes a precise location of an electron within an atom.
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All orbitals sharing the same principal quantum number (n) belong to different shells.
All orbitals sharing the same principal quantum number (n) belong to different shells.
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The values of the spin-magnetic quantum number (ms) are represented by ↑ and ↓.
The values of the spin-magnetic quantum number (ms) are represented by ↑ and ↓.
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The maximum number of electrons that can occupy a d-orbital is 10.
The maximum number of electrons that can occupy a d-orbital is 10.
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An s-orbital can have multiple orientations in space.
An s-orbital can have multiple orientations in space.
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The spin quantum number for an electron can be either +⅔ or -⅓.
The spin quantum number for an electron can be either +⅔ or -⅓.
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In a p-sublevel, there are a total of six orbitals.
In a p-sublevel, there are a total of six orbitals.
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The effective nuclear charge felt by an electron is always equal to the actual nuclear charge.
The effective nuclear charge felt by an electron is always equal to the actual nuclear charge.
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The principal quantum number determines the shape of the orbital.
The principal quantum number determines the shape of the orbital.
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Two electrons in the same orbital must have opposite spins.
Two electrons in the same orbital must have opposite spins.
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The energy of a d subshell is lower than that of an s subshell in the same shell.
The energy of a d subshell is lower than that of an s subshell in the same shell.
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The boundary surface of an s-orbital represents about a 90% probability of finding the electron.
The boundary surface of an s-orbital represents about a 90% probability of finding the electron.
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The allowable values for the magnetic quantum number (ml) for a p sublevel are -1, 0, and +1.
The allowable values for the magnetic quantum number (ml) for a p sublevel are -1, 0, and +1.
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Study Notes
Orbitals and Bonding
- Electrons are not particles but have wave-like properties
- The Heisenberg Uncertainty Principle: due to the wave nature of an electron, we cannot accurately pinpoint its location
- The wave function is a mathematical expression summing up the probability of finding an electron
- An atomic orbital is the wave function of an electron in an atom; it is the region in space where there is likely to be an electron
- Each atomic orbital is defined by three quantum numbers:
- Principal (n): Labels the electron shell. The average distance of an electron from the nucleus increases with increasing n
- Azimuthal (l): Labels the subshells: s, p, d, f
- Magnetic (ml): Labels specific orbitals within a subshell
- Spin-magnetic (ms): Represents the spin state of electrons within orbitals, with two values: +½ and –½
Electron Spin
- Electrons have two spin states: ↑ (up) and ↓ (down), represented by the spin magnetic number (ms)
- +½ for an ↑ electron
- –½ for a ↓ electron
Electronic Configurations and Quantum Numbers
- Each electron orbiting the nucleus of an element possesses a unique set of four quantum numbers: n, l, ml, ms
-
Principal (n):
- Natural numbers excluding 0 (1, 2, 3...)
- Except for d-orbitals, the shell number matches the row on the periodic table
-
Azimuthal (l):
- Natural numbers including 0 up to (n – 1)
- 0 = s-orbital in the s-sublevel
- 1 = p-orbitals in the p-sublevel
- 2 = d-orbitals in the d-sublevel
- 3 = f-orbitals in the f-sublevel
-
Magnetic (ml):
- Integers between and including –l and +l
- l = 0 (s): 2 electrons in one s-orbital (ml = 0)
- l = 1 (p): 2 electrons in each of three p-orbitals (px (ml = –1), py (ml = 0), pz (ml = +1)
- l = 2 (d): 2 electrons in each of five d-orbitals (dxy (ml = –2), dxz (ml = –1), dyz (ml = 0), dx2 – y2 (ml = +1), dz2 (ml = +2))
-
Spin-magnetic (ms):
- Two rational numbers: +½, –½
- Electron spins in any one orbital are opposite (paired spins) denoted ↑↓
Orbital Energies
- In atoms with many electrons, electron-electron repulsion causes the energy of a d-subshell to be higher than an s-subshell in the next higher shell
- S-electrons are found close to the nucleus and penetrate more effectively than p-electrons
- The effective nuclear charge is less than the actual charge due to electron shielding from the nucleus
s-Orbitals
- S-orbitals are spherical
- An electron with a probability distribution given by a 1s orbital is a 1s electron
- Only one s-orbital exists per shell
- The surface of the orbital is a boundary surface: a sphere that encloses about a 90% probability of finding the electron
- All s-orbitals are spherical but differ in size: 1s > 2s > 3s
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Description
Test your understanding of atomic orbitals and the principles governing electron behavior, including wave functions and quantum numbers. This quiz covers key concepts such as the Heisenberg Uncertainty Principle and electron spin states. Perfect for students studying chemistry at the high school or introductory college level.
