Concept explainers
(a)
Interpretation:
The electron configuration for the given atom is to be labeled as a ground state or an excited state.
Concept introduction:
According to the Aufbau principle, the electrons are firstly filled into the orbitals having lower energy. The electrons are filled in the orbitals as,
(b)
Interpretation:
The electron configuration for the given atom is to be labeled as a ground state or an excited state.
Concept introduction:
According to the Aufbau principle, the electrons are firstly filled into the orbitals having lower energy. The electrons are filled in the orbitals as,
(c)
Interpretation:
The electron configuration for the given atom is to be labeled as a ground state or an excited state.
Concept introduction:
According to the Aufbau principle, the electrons are firstly filled into the orbitals having lower energy. The electrons are filled in the orbitals as,
(d)
Interpretation:
The electron configuration for the given atom is to be labeled as a ground state or an excited state.
Concept introduction:
According to the Aufbau principle, the electrons are firstly filled into the orbitals having lower energy. The electrons are filled in the orbitals as,
(e)
Interpretation:
The electron configuration for the given atom is to be labeled as a ground state or an excited state.
Concept introduction:
According to the Aufbau principle, the electrons are firstly filled into the orbitals having lower energy. The electrons are filled in the orbitals as,
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Chapter 12 Solutions
Student Solutions Manual for Ball's Physical Chemistry, 2nd
- An excited atom can release some or all of its excess energy by emitting a(n) and thus move to a lower energy state.arrow_forwardFor each of the following combinations of quantum numbers, make changes that produce an allowed combination. Count 3 for each change of n, 2 for each change of I, and 1 for each change of mi. What is the lowest possible count that you can obtain? a n = 3, I = 0, mi = 2 b n = 5, I = 5, mi = 4 c n = 3, I = 3, mi = 3 d n = 5, I = 6, mi = 3arrow_forwardIn X-ray fluorescence spectroscopy, a material can be analyzed for its constituent elements by radiating the material with short-wavelength X rays, which induce the atoms to emit longer-wavelength X rays characteristic of those atoms. Tungsten, for example, emits characteristic X rays of wavelength 0.1476 nm. If an electron has an equivalent wavelength, what is its kinetic energy?arrow_forward
- How does the wavelength of a fast-pitched baseball compare to the wavelength of an electron traveling at 110 the speed of light? What is the significance of this comparison? See Example 2-3.arrow_forward6.49 Which of these electron configurations are for atoms in the ground state? In excited states? Which are impossible? (a) 1s22s1, (b) 1s22s22p3, (c) [Ne] 3s23p34s1, (d) [Ne] 3s23p64s23d2, (e) [Ne] 3s23p64f 4, (f) 1s22s22p43s2arrow_forwardHow far from the nucleus in angstroms (1 angstrom =11010 m) is the electron in a hydrogen atom if it has an energy of 8.721020 J?arrow_forward
- State which of the following sets of quantum numbers would be possible and which impossible for an electron in an atom. a n = 2, I = 0, mi = 0, ms=+12 b n = 1, I = 1, mi = 0, ms=+12 c n = 0, I = 0, mi = 0, ms=12 d n = 2, I = 1, mi = 1, ms=+12 e n = 2, I = 1, mi = 2, ms=+13arrow_forward6.105 When we say that the existence of atomic spectra tells us that atoms have specific energy levels, are we using deductive or inductive reasoning?arrow_forwardGive the possible values of a. the principal quantum number, b. the angular momentum quantum number, c. the magnetic quantum number, and d. the spin quantum number.arrow_forward
- 6.85 The visible lines in the hydrogen atom emission spectrum arise from transitions with a final state with n = 2. In what spectral region should we expect to find transitions that have a final state of n = 1 ? Explain your reasoning using an energy level diagram similar to the one in Problem 6.26.arrow_forwardWhat is the difference between an atom’s ground state and an excited state?arrow_forwardInvestigating Energy Levels Consider the hypothetical atom X that has one electron like the H atom but has different energy levels. The energies of an electron in an X atom are described by the equation E=RHn3 where RH is the same as for hydrogen (2.179 1018 J). Answer the following questions, without calculating energy values. a How would the ground-state energy levels of X and H compare? b Would the energy of an electron in the n = 2 level of H be higher or lower than that of an electron in the n = 2 level of X? Explain your answer. c How do the spacings of the energy levels of X and H compare? d Which would involve the emission of a higher frequency of light, the transition of an electron in an H atom from the n = 5 to the n = 3 level or a similar transition in an X atom? e Which atom, X or H, would require more energy to completely remove its electron? f A photon corresponding to a particular frequency of blue light produces a transition from the n = 2 to the n = 5 level of a hydrogen atom. Could this photon produce the same transition (n = 12 to n = 5) in an atom of X? Explain.arrow_forward
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