(a)
Interpretation:
From the given quantum numbers
Concept Introduction:
A subshell is one or more atomic orbitals with same n and l quantum numbers. The value of l is an integer that ranges from zero up to
(b)
Interpretation:
From the given quantum numbers
Concept Introduction:
Refer to part (a)
(c)
Interpretation:
From the given quantum numbers
Concept Introduction:
Refer to part (a)
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Chapter 5 Solutions
OWLv2 for Moore/Stanitski's Chemistry: The Molecular Science, 5th Edition, [Instant Access], 1 term (6 months)
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- How many electrons in an atom can have each of the following quantum number or sublevel designations?(a) n = 2, l = 1 (b) 3d (c) 4sarrow_forward(A) What is the wave length (in nanometers) of light having a frequency of 3.6 x 1013 Hz? (B) what is the frequency (in hertz) of light having a wavelength of 456 nm? (c) what is the frequency of light having a wave length of 147 nm? (d) what is the wave length (in meters) of radiation having a frequency of 9.64 x 107 Hz? (this is the type of radiation used by FM radio stations)arrow_forwardHow many electrons in an atom can have each of the follow-ing quantum number or sublevel designations?(a)n=2, l=1(b) 3d(c) 4sarrow_forward
- (a) Write out the full electron configuration of Calcium (Ca). (b) How many electrons are in the n=3 shell of Calcium?arrow_forwardA stellar object is emitting radiation at 1720 nm. A detector is capturing 9 x 107 photons per second at this wavelength. h 6.63 x 1034 3-s. c-2.998 x 10 m/s. (a) What is the total energy of the photons detected in one second? 9.96-12 x 1/s (b) What is the total energy of the photons detected in one hour? x 3/hr 3.50-8arrow_forward2. Hydrogen atoms absorb energy so that electrons can be excited to the n = 6 energy level. Electrons then undergo these transitions, among others: (a) n = 6 → n= 5 (b) n= 6 → n=4 (c)n=5→ n=3 (i) Which transition produces a photon with the least energy? (ii) Which transition produces a photon with the highest frequency? (iii) Which transition produces a photon with the shortest wavelength?arrow_forward
- (a) How does the Bohr model differ from the quantum mechanical model of the atom? Describe at least 2 differences.(b) Define each of the 4 quantum numbers (n, l, ml, ms) and what they physically represent about the orbital and/or electron.(d) How many quantum numbers are needed to completely define a specific orbital? Provide the quantum numbers for the 2s orbital.(d) How many quantum numbers are needed to completely define a specific electron? Provide the quantum numbers for the second electron to fill into a 2s orbital.arrow_forwardHow many electrons in an atom can have each of the following quantum number or sublevel designations? (a) n = 2, 1 = 1, m = 0 (b) 5s (c) n = 4,1 = 0arrow_forwardA green laser beam with a wavelength l = 532 nm has an energy of 3.85 x 10–3 J per pulse. What is the energy density of the laser expressed in term number of photon per pulse? (Planck constant, h = 6.63 x 10–34J.s; speed of light, c = 3.00 x 108 m/s; 1 nm = 10–9 m) (A) 5.81 x 1024 (B) 1.03 x 1025 (C) 1.03 x 1016 (D) 2.67 x 1015arrow_forward
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