Wave functions describe orbitals in a hydrogen atom. Each function is characterized by 3 quantum numbers: n, 1, and mj. If the value of n =1: The quantum number I can have values from| The total number of orbitals possible at the n =1 energy level is ( to If the value of 1= 3: The quantum number mị can have values from | The total number of orbitals possible at the l= 3 sublevel is to

Wave functions describe orbitals in a hydrogen atom. Each function is characterized by 3 quantum numbers: n, 1, and mj. If the value of n =1: The quantum number I can have values from| The total number of orbitals possible at the n =1 energy level is ( to If the value of 1= 3: The quantum number mị can have values from | The total number of orbitals possible at the l= 3 sublevel is to

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter7: The Structure Of Atoms And Periodic Trends

Section7.1: The Pauli Exclusion Principle

Problem 2RC

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Similar questions

(a) Use the radial wave function for the 3p orbital of a hydrogen atom (see Table 5.2) to calculate the value of r for which a node exists. (b) Find the values of r for which nodes exist for the 3s wave function of the hydrogen atom.
Which of the following is a valid set of quantum numbers for an electron in a hydrogen atom? (a) n = 1, = 0, m = 0, ms = 1 (b) n = 1, = 1, m = 0, ms = 1/2 (c) n = 1, = 0, m = 1, ms = + 1/2 (d) n = 1, = 0, m = 0, ms = 1/2
• identify an orbital (as 1s, 3p, etc.) from its quantum numbers, or vice versa.
What experimental evidence supports the quantum theory of light? Explain the wave-particle duality of all matter .. For what size particles must one consider both the wave and the particle properties?
Which of the following sets of quantum numbers correctly represents a 4p orbital? (a) n = 4, = 0, m = 1 (b) n = 4, = 1, m = 0 (c) n = 4, = 2, m = 1 (d) n = 4, = 1, m =2
Investigating 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.
Why is the electron in a Bohr hydrogen atom bound less tightly when it has a quantum number of 3 than when it has a quantum number of 1?
What are quantum numbers? What information do we get from the quantum numbers n, l, and ml? We define a spin quantum number (ms), but do we know that an electron literally spins?