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What is the value of the magnetic quantum number ml for the d orbital aligned with the z-axis?
Which type of orbitals has eight-lobed shapes?
What is the number of d orbitals in an electron energy level n ≥ 3?
What is the name of the d orbital with four lobes and a nodal plane?
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What is the value of the orbital angular momentum quantum number l for f orbitals?
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What is the purpose of the magnetic quantum number ml in describing atomic orbitals?
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What is the name of the value that describes the sign of the wave function in an orbital?
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What is the term for the region where the wave function equals zero?
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What is the term for the set of orbitals with the same value of n and l?
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In a hydrogen atom, what is the relationship between the energies of sublevels within the same level?
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What is the reason for the difference in energy between sublevels in atoms other than hydrogen?
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What is the correct sublevel name for a sublevel with n = 3?
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How many spherical nodes are there in a 2s orbital?
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Which magnetic quantum number corresponds to the p orbital that points along the y-axis?
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How many internal nodes are there in a 3s orbital according to the information provided?
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If an orbital has l = 2, what is the correct sublevel name for this orbital?
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How many lobes does a p orbital have?
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What is the main prediction of the classical theory of the photoelectric effect regarding the energy of a wave?
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What is the main difference between the classical theory and Einstein's explanation of the photoelectric effect?
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What is the term for the minimum frequency needed before electrons would be emitted, regardless of the intensity?
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According to Einstein's explanation, what is the effect of a shorter wavelength photon on the energy absorbed by the electron?
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What is the term for the energy required for an electron to escape the atom, according to Einstein's explanation?
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What is the main consequence of Einstein's proposal that light energy is delivered to the atoms in packets, called quanta?
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If a metal ejects electrons when struck by yellow light, what would happen when the same metal surface is struck with ultraviolet light?
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What happens to the excess energy when an electron is ejected from a metal surface?
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What is the relationship between the kinetic energy of ejected electrons and the frequency of the light that strikes the metal surface?
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What type of light will be emitted when gas atoms are excited via external energy?
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What is unique about the pattern observed when emitted light is passed through a prism or a diffraction grating?
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How does the energy of ultraviolet light compare to that of yellow light?
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What is the characteristic of electromagnetic waves that allows them to move through a vacuum at a constant speed?
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What is the reason why the speed of light is smaller in materials such as air?
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What is the term for the region where an electrically charged particle experiences a force?
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What is the term for the region where a magnetized particle experiences a force?
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What is the nature of electromagnetic radiation?
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What is the speed of light in a vacuum?
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Study Notes
Atomic Orbitals
- Electron energy levels (n ≥ 3) have five d orbitals with magnetic quantum numbers ml = -2, -1, 0, +1, +2.
- d orbitals have four lobes, except for dz2 which has two lobes and a toroid.
- Electron energy levels (n ≥ 4) have seven f orbitals with magnetic quantum numbers ml = -3, -2, -1, 0, +1, +2, +3.
- f orbitals are mainly eight-lobed, with some two-lobed with two toroids.
Orbital Shapes
- s orbitals have a spherical shape and symmetry.
- The number of spherical nodes in s orbitals is equal to n - 1.
- p orbitals have two lobes, with three p orbitals forming one p sublevel, each pointing along a different axis (px, py, pz).
Phase of an Orbital
- The sign of the wave function is called its phase.
- Orbitals can have positive or negative values, and nodes are where the wave function = 0.
- When orbitals interact, their wave functions may be in phase (same sign) or out of phase (opposite signs).
Describing an Orbital
- Each set of n, l, and ml describes one orbital.
- Orbitals with the same value of n are in the same principal energy level (principal shell).
- Orbitals with the same values of n and l are in the same sublevel (subshell).
Energy of Sublevels
- In a Hydrogen atom, all sublevels within the same level have the same energy.
- In all other atoms, sublevels have slightly different energies due to electron-electron repulsions.
Photoelectric Effect
- The energy of a wave is directly proportional to its amplitude and frequency.
- Experimental observations show that a minimum frequency (threshold frequency) is needed before electrons are emitted, regardless of intensity.
- Above-threshold frequency light from a dim source causes electron emission without lag time.
- Einstein proposed that light energy is delivered in packets (quanta or photons), and one photon at the threshold frequency gives the electron just enough energy to escape.
Atomic Spectra
- When individual atoms or molecules absorb energy, it is released quickly as light energy (photons).
- The emitted light is characteristic to that type of atom or molecule, forming an emission spectrum.
- Emission spectra are non-continuous, with only specific wavelengths present.
Light
- Light is a form of electromagnetic radiation, composed of perpendicular oscillating waves (electric field and magnetic field).
- Electromagnetic waves move through space (vacuum) at a constant speed (c ≈ 3.00 × 10^8 m/s).
- The speed of light in materials (e.g., air) is smaller.
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Description
Test your knowledge on electron orbitals and angular nodes, focusing on 2p orbitals, d orbitals, and their shapes according to quantum theory. Explore concepts such as ml values and orbital alignment in different planes.
