Concept explainers
(a)
Interpretation:
The notation of subshell if
Concept Introduction:
The acceptable wave function is characterized by a set of four quantum numbers. These quantum numbers are related to the shape, size of the electron wave and the location of the electron in space.
These quantum numbers are represented by
The notation of subshell is used to determine by a combination of both principal quantum number and angular quantum number. In notation, numerical values of
(b)
Interpretation:
The notation of subshell if
Concept Introduction:
Refer to part (a).
(c)
Interpretation:
The notation of subshell if
Concept Introduction:
Refer to part (a).
(d)
Interpretation:
The notation of subshell if
Concept Introduction:
Refer to part (a).
(e)
Interpretation:
The notation of subshell if
Concept Introduction:
Refer to part (a).
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Chemistry: Principles and Practice
- Give the notation (using letter designations for l) for the subshells denoted by the following quantum number. (Enter your answer in the format of 5p for 5p.) (a) n = 4, l = 0(b) n = 1, l = 0(c) n = 5, l = 3(d) n = 5, l = 2arrow_forwardIdentify the subshell in which electrons with the following quantum numbers are found:(a) n = 2, l = 1(b) n = 4, l = 2(c) n = 6, l = 0arrow_forwarda Suppose hydrogen atoms absorb energy so that electrons are excited to the n = 7 energy level. Electrons then undergo these transitions, among others: (a) n = 7 to n=1 (b) n = 7 to n= 6 (c) n = 2 to n= 1 Enter the letter (a, b, or c) for each. the smallest energy? the highest frequency? the shortest wavelength? b What is the frequency of a photon resulting from the transition n=6 → n=1? h = 6.62 × 10-34 J.sarrow_forward
- Microwave ovens heat food by the energy given off by microwaves. These microwaves have a wavelength of 5.00 3 106 nm. (a) How much energy in kilojoules per mole is given off by a microwave oven? (b) Compare the energy obtained in (a) with that given off by the ultraviolet rays (l <100 nm) of the Sun that you absorb when you try to get a tan.arrow_forwardThe work function of metal is the minimum energy required to produce photoelectric effect on that metal, and the work function for potassium metal is 2.30 eV (where 1 eV = 1.60 x 10–19 J).(a) What is the minimum energy in Joules required to eject an electron from potassium metal?(b) What is the longest wavelength of light, in nanometers (nm), capable of producing photoelectric effect on potassium metal? (c) Determine whether a photon of green light with = 512 nm would have sufficient energy to eject an electron from a potassium metal. (d) If an electron is ejected, determine the kinetic energy and the speed of the ejected electron, which has a mass of 9.11 x 10–31 kg. .(Planck’s constant, h = 6.626 x 10–34 J∙s.; speed of light, c = 3.00 x 108 m/s; 1 J = 1 kg∙m2/s2)arrow_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
- Calculate the energy of electron in hydrogen at quantum levels: (i) n = 1; (ii) n = 2, and (iii) n = 5, according to the Bohr’s model.(b) What is the energy change (E, in Joule) when an electron jumps from quantum level n = 5 to n = 2? Is energy gained or lost by the electron. (c) If energy is gained or lost in the form of electromagnetic radiation, what are the wavelength (; in nm) and frequency (; in s–1) of this radiation?(d) What is the longest wavelength (, in nm) of light that would have sufficient energy to excite an electron from energy level E1 to E; where E∞ = 0.0 J is the edge of the atomarrow_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_forwardWhich of the following represent valid sets of quantum numbers? For a set is invalid, explain briefly why it is not correct.(a) n = 3, ℓ = 3, mℓ = 0(b) n = 2, ℓ = 1, mℓ = 0(c) n = 6, ℓ = 5, mℓ = ‒1(d) n = 4, ℓ = 3, mℓ = ‒4arrow_forward
- In each of the following cases, demonstrate that 2n² is the number of sets of quantum numbers (e, me, m) possible for a hydrogen atom in the n-th shell. In each case, accomplish this by specifying the number of states in each subshell. Submit the numbers for all subshells, separated by spaces, in the single answer box for each case. (a) n = 1 2 (b) n = 2 122 (c) n = 3 242 (d) n = 4 362 (e) n = 5 482 Need Help? X X X X Read Itarrow_forwardBe sure to answer all parts.Consider the following energy levels of a hypothetical atom:E4 −2.21 × 10−19 J E3 −8.31 × 10−19 J E2 −1.35 × 10−18 J E1 −1.65 ×10−18J(a) What is the wavelength of the photon needed to excite an electron from E1 to E4? (b) What is the energy (in joules) a photon must have in order to excite an electron from E2 to E3? (c) When an electron drops from the E3 level to the E1 level, the atom is said to undergo emission. Calculate the wavelength of the photon emitted in this process.arrow_forwardA certain light wave has a measured frequency of 4.15 x 1014 s-1. What is the wavelength of this light in meters? On your answer sheet answer the following additional questions (b) What is the energy in joules per photon? (c) What is the energy per mole of photons? (d) What range of the electromagnetic spectrum is this wavelength?arrow_forward
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning