Question

Q1: True or False: (2 points each) Write letter (T) for the correct and (F) for incorrect statement in each of the following: 1) ( ) The allowed values of $\ell$ when the principal quantum number is n = 5 are 5. 2) ( ) The principal quantum number is responsible for the orientation of the orbitals. 3) ( ) The degree to which particle momentum is fuzzy is given by the magnitude of uncertainty in momentum. 4) ( ) The size of the atomic orbital is determined by the orbital quantum number $\ell$. 5) ( ) Zeeman effect experiment provided a striking evidence for the quantization of the energy of atoms. 6) ( ) Electron spin quantum number ($s = \frac{1}{2}$) is a well-known quantity in classical physics. 7) ( ) High resolution spectrometer shows that hydrogen atom lines are having doublet nature. This is due to the interaction between the orbital angular momentum and the spin angular momentum. 8) ( ) The total quantum number $j$ is used to characterize the splitting of atomic energy levels, such as the spin-orbit splitting which leads to the sodium doublet. 9) ( ) If the space quantization were due to the magnetic quantum number $m_\ell$, $m_\ell$ states is always even and should have produced an even number of lines. 10) ( ) For a particle in a box, the quantum uncertainty in position can be calculated from expectation values as: $\Delta x = \sqrt{(x^2) - (x)^2}$

          Q1: True or False: (2 points each) Write letter (T) for the
correct and (F) for incorrect statement in each of the following:
1) ( ) The allowed values of $\ell$ when the principal quantum number is n = 5 are 5.
2) ( ) The principal quantum number is responsible for the orientation of the
orbitals.
3) ( ) The degree to which particle momentum is fuzzy is given by the magnitude
of uncertainty in momentum.
4) ( ) The size of the atomic orbital is determined by the orbital quantum number $\ell$.
5) ( ) Zeeman effect experiment provided a striking evidence for the quantization
of the energy of atoms.
6) ( ) Electron spin quantum number ($s = \frac{1}{2}$) is a well-known quantity in classical
physics.
7) ( ) High resolution spectrometer shows that hydrogen atom lines are having
doublet nature. This is due to the interaction between the orbital angular momentum
and the spin angular momentum.
8) ( ) The total quantum number $j$ is used to characterize the splitting of atomic
energy levels, such as the spin-orbit splitting which leads to the sodium doublet.
9) ( ) If the space quantization were due to the magnetic quantum number $m_\ell$, $m_\ell$
states is always even and should have produced an even number of lines.
10) ( ) For a particle in a box, the quantum uncertainty in position can be calculated
from expectation values as: $\Delta x = \sqrt{(x^2) - (x)^2}$

Q1: True or False: (2 points each) Write letter (T) for the
correct and (F) for incorrect statement in each of the following:
1) ( ) The allowed values of ℓ when the principal quantum number is n = 5 are 5.
2) ( ) The principal quantum number is responsible for the orientation of the
orbitals.
3) ( ) The degree to which particle momentum is fuzzy is given by the magnitude
of uncertainty in momentum.
4) ( ) The size of the atomic orbital is determined by the orbital quantum number ℓ.
5) ( ) Zeeman effect experiment provided a striking evidence for the quantization
of the energy of atoms.
6) ( ) Electron spin quantum number (s = (1)/(2)) is a well-known quantity in classical
physics.
7) ( ) High resolution spectrometer shows that hydrogen atom lines are having
doublet nature. This is due to the interaction between the orbital angular momentum
and the spin angular momentum.
8) ( ) The total quantum number j is used to characterize the splitting of atomic
energy levels, such as the spin-orbit splitting which leads to the sodium doublet.
9) ( ) If the space quantization were due to the magnetic quantum number mℓ, mℓ
states is always even and should have produced an even number of lines.
10) ( ) For a particle in a box, the quantum uncertainty in position can be calculated
from expectation values as: Δ x = √((x^2) - (x)^2)

Added by Timothy C.

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