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What value of wavelength is associated with the Lyman series for {image} {image}

1. 2. 3. 4. 5. What value of wavelength is associated with the Lyman series for {image} {image}. {image} {image} {image} {image} {image}. What wavelength (in {image} is associated with the Paschen series for {image} {image}. 330 2.1 1.9 0.4 590.

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What value of wavelength is associated with the Lyman series for {image} {image}

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  1. 1. 2. 3. 4. 5. What value of wavelength is associated with the Lyman series for {image} {image} • {image} • {image} • {image} • {image} • {image}

  2. What wavelength (in {image} is associated with the Paschen series for {image} {image} • 330 • 2.1 • 1.9 • 0.4 • 590

  3. Light is emitted by hydrogen atoms in the visible range for a hydrogen atom. Its wavelength is 434 nm. What value of {image} is associated with the light? {image} • 3 • 8 • 4 • 5 • 6

  4. An electron in a hydrogen atom makes a transition from the {image} to the {image} energy state. Determine the energy (in eV) of the emitted photon. • 0.28 • 2.49 • 1.13 • 10.2 • 0.20

  5. An electron in a hydrogen atom makes a transition from the {image} to the {image} energy state. Determine the wavelength of the emitted photon (in nm). • 246 • 614 • 389 • 182 • 1,451

  6. 1. 2. 3. 4. 5. A hydrogen atom is in its fourth excited state {image} . The linear momentum of the electron is _____ (in {image} . • {image} • {image} • {image} • {image} • {image}

  7. 1. 2. 3. 4. 5. How fast is the electron moving in the fourth Bohr orbit? • {image} • {image} • {image} • {image} • {image}

  8. 1. 2. 3. 4. 5. An electron is moving at a speed of {image} in the sixth Bohr orbit. Determine its de Broglie wavelength. • {image} • {image} • {image} • {image} • {image}

  9. 1. 2. 3. 4. 5. Suppose Bohr had chosen the potential energy of the electron in the hydrogen atom to be {image} when the electron is in the orbit with {image} He could do this by _____. • subtracting a constant 13.6 eV from the potential energy for all values of {image} • adding a constant 27.2 eV to the potential energy for all values of {image} • adding a constant 13.6 eV to the potential energy for all values of {image} • subtracting a constant 27.2 eV from the potential energy for all values of {image} • choosing {image} for the orbit where the kinetic energy of the electron is equal to the potential energy

  10. 1. 2. 3. 4. 5. The allowed values of {image} for the {image} ion are _____. • any real number • 3 to {image} • 1 to {image} • 1 to 9 • 2 to {image}

  11. 1. 2. 3. 4. One of the main problems with the Bohr model of the hydrogen atom when compared with the results of the methods of quantum mechanics used to describe atoms, was that the Bohr model predicted that _____. • the wavelength of the radiation emitted when an electron "jumps" from one allowed orbit to another is {image} • the energy of the ground state of the hydrogen atom is {image} • the potential energy function for the hydrogen atom is given by {image} • the ground state angular momentum is {image}

  12. The allowed values of {image} for the {image} shell in a {image} ion are _____. • 1, 2, 3 • 0, 1, 2, 3, 4 • 0, 1, 2 • 0, 1, 2, 3 • 1, 2, 3, 4

  13. 1. 2. 3. 4. 5. In the subshell of the {image} ion with orbital quantum number {image} the allowed values of the magnetic quantum number {image} are _____. • 0 to {image} • {image} to {image} • {image} to {image} • {image} to {image} • {image} to {image}

  14. 1. 2. 3. 4. 5. In a shell of the hydrogen atom with {image} the permitted values of the orbital magnetic quantum number {image} are _____. • 1, 0 • 0 • 2, 1, 0, -1, -2 • 2, 1, 0 • 1, 0, -1

  15. The number of states in the {image} ion corresponding to the principle quantum number {image} are _____. • 50 • 79 • 52 • 25 • 8

  16. 1. 2. 3. 4. 5. The {image} symbols represent values of the quantum number _____. • {image} • {image} • {image} • {image} • {image}

  17. 1. 2. 3. 4. 5. The {image} symbols represent values of the quantum number _____. • {image} • {image} • {image} • {image} • {image}

  18. 1. 2. 3. 4. 5. The energy needed to remove an electron from the first excited state of a {image} ion is _____. • 287 eV • 31 eV • 28 eV • 26 eV • 116 eV

  19. 1. 2. 3. 4. 5. Of the following states, {image} {image} {image} {image} {image} {image} and {image} the one which is NOT allowed is _____. • {image} • {image} • {image} • {image} • {image}

  20. 1. 2. 3. 4. 5. For the following allowed transitions, which photon would have the least wavelength when an electron "jumps" from one energy level, characterized by the quantum number {image} , to another? • {image} to {image} • {image} to {image} • {image} to {image} • {image} to {image} • {image} to {image}

  21. 1. 2. 3. 4. 5. The energy needed to change a {image} ion in the second excited state into a {image} ion is _____. • 305.1 eV • 50.3 eV • 8.7 eV • 10.5 eV • 6.0 eV

  22. 1. 2. 3. 4. 5. If {image} is the radial probability density function for an electron in the ground state of a hydrogen atom, the most probable value for {image} can be found from _____ . • {image} • {image} • {image} • {image} • {image}

  23. 1. 2. 3. 4. 5. The probability density for the {image} state is given by {image} . The probability of finding the particle somewhere in space is _____. • {image} • {image} • {image} • {image} • {image}

  24. 1. 2. 3. 4. 5. A {image} ion undergoes a transition from the {image} to the {image} state. The energy of the emitted photon is _____. • 0.60 eV • 3.11 eV • 1.89 eV • 78.0 eV • 487 eV

  25. 1. 2. 3. 4. 5. The radial portion of the de Broglie wave function for an electron in the ground state of the hydrogen atom is {image} where {image} is the Bohr radius. The probability of finding the electron is _____ . • {image} • {image} • {image} • {image} • {image}

  26. 2. 1. 3. 4. 5. The probability density of a particle at a distance {image} from the nucleus is essentially the _____ . • probability per unit area of finding the particle within a unit area centered on {image} • probability per unit volume of finding the particle within a small volume about {image} • probability of finding the particle within a small volume about {image} • probability per unit length of finding the particle within a unit length of {image} • {image}

  27. 2. 1. 3. 4. 5. Of the following states of the hydrogen atom, {image} {image} {image} {image} {image} which answer lists all the states that are not spherically symmetrical? • {image} • {image} • {image} • {image} • {image}

  28. 1. 2. 3. 4. Which of the following statements is true? • {image} can never be perpendicular to {image} • {image} can never be aligned parallel to {image} • {image} can be aligned parallel to {image} • {image} must be perpendicular to {image}

  29. 1. 2. 3. 4. 5. A hydrogen atom in the {image} state has a total angular momentum (in terms of {image} ) of magnitude _____ . • {image} • {image} • {image} • {image} • {image}

  30. In 1921, Stern and Gerlach performed an experiment that first demonstrated _____ . • energy quantization • magnetic orbital quantization • space quantization • orbital angular momentum quantization • that particles behave like waves

  31. 2. 1. 3. 4. 5. The total angular momentum for a {image} electron is _____ . • {image} • {image} • {image} • {image} • {image}

  32. 1. 2. 3. 4. 5. What angle does the orbital angular momentum make with the {image} axis of a hydrogen atom in the state {image} {image} {image} • {image} • {image} • {image} • {image} • {image}

  33. 1. 2. 3. 4. 5. When using the Pauli Exclusion Principle, we assume the particle's spin angular momentum is of magnitude _____ . • {image} • {image} • {image} • {image} • {image}

  34. 1. 2. 3. 4. 5. The {image} component of spin angular momentum is equal to _____ . • {image} • {image} • {image} • {image} • {image}

  35. The Hund's rule states _____ . • no two atoms can have the same set of quantum numbers • when an atom has orbitals of equal energy, the order in which they are filled by electrons is such that a maximum number of electrons have unpaired spins • when an atom has orbitals of equal energy, the maximum number of electrons will be paired spins • no two electrons in the same atom can have the same set of quantum numbers • there is an inherent uncertainty in the position and momentum of a particle

  36. Forbidden transitions and selection rules suggest that _____ . • a photon has linear momentum • a photon has energy • a photon has angular momentum • a photon has mass • a photon has parity

  37. 1. 2. 3. 4. Characteristic x-rays can be produced by bombarding targets with electrons. These x-rays occur when _____ . • electrons from higher shells fill the vacant lower shell • photons are emitted with wavelengths on the order of {image} • electrons from lower shells fill the higher shell • photons are emitted with energies on the order of {image}

  38. 1. 2. 3. 5. 4. The ground state configuration of scandium {image} is _____ . • {image} • {image} • {image} • {image} • {image}

  39. 1. 2. 3. 4. 5. Iodine {image} and bromine {image} are similar to chlorine in that they have _____ electron(s) in the outermost shell. • five {image} • four {image} • five {image} • two {image} • one {image}

  40. When electrons fill a subshell in which the orbitals have equal energy, the order in which the orbitals are filled is such that _____ . • a maximum number of electrons has unpaired spins • a minimum number of electrons first fills the next energy level • a maximum number of electrons has intrinsic angular momentum • the minimum number of electrons has the same set of quantum numbers • a minimum number of electrons has unpaired spins

  41. In a completely filled atomic shell, _____ . • the intrinsic spin of the electrons does not produce a resultant magnetic moment • the orbital motion of the electrons produces a resultant magnetic moment • the electrons do not contribute to paramagnetic or ferromagnetic effects • the first and third above answers are correct • all of the above are correct

  42. 1. 2. 3. 4. 5. Which of the following, in which {image} and {image} have integer values, is a correct formula for a wavelength emitted by a hydrogen atom? • {image} • {image} • {image} • {image} • {image}

  43. 1. 2. 3. 4. 5. In the Bohr model of the hydrogen atom, the total energy of the electron-proton system is _____ . • {image} • {image} • {image} • {image} • {image}

  44. 1. 2. 3. 4. 5. In terms of {image} , where {image} the radii of the allowed orbits in the Bohr model of the hydrogen atom are given by {image} _____ . • {image} • {image} • {image} • {image} • {image}

  45. 1. 2. 3. 4. 5. Quantum physics agrees with the classical physics limit when _____ . • the difference in energy between adjacent quantized levels becomes vanishingly small • all electron spins are paired so that {image} • the total energy is a small multiple of the energy in the lowest quantized state • there is a vacancy in an inner level in the atom • the total angular momentum is a small multiple of {image}

  46. 1. 2. 3. 4. 5. In an atom that has an electron in a sub-shell for which {image} with respect to the magnetic field vector {image} the magnetic moment vector {image} of the electron is allowed to be oriented in _____ . • {image} discrete directions • {image} discrete directions • any direction • {image} discrete directions • {image} discrete directions

  47. 1. 2. 3. 4. 5. The number of electrons in the {image} {image} subshell in gallium {image} is _____ the number of electrons in the {image} {image} subshell in indium {image} • {image} times • {image} times • {image} times • equal to • {image} times

  48. 1. 2. 3. 4. 5. In an allowed electron transition in a hydrogen atom, _____ . • {image} • {image} • {image} • {image} • {image}

  49. 1. 2. 3. 4. 5. An energy of 3.4 eV is needed to ionize an electron from the first excited state of a hydrogen atom. What wavelength is needed if a photon accomplishes this task? • 360 nm • 780 nm • 140 nm • 370 nm • 510 nm

  50. A hydrogen atom is in its ground state. Incident on the atom are many photons each having an energy of {image} The result is that _____. • the atom is excited to a higher allowed state • the atom is ionized • the photons pass by the atom without interaction

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