(a)
Interpretation:
All four possible sets of quantum numbers for an electron in
Concept Introduction:
Principal Quantum Number (n): In an atom, theelectron energy mainly depends on principal quantum number. The energy of an electron becomes lower when the value of n is smaller. The orbital size also depends on n. The size of orbital increases with increase in value of principal quantum number (n)
Magnetic Quantum Number(
Spin Quantum Number (
(b)
Interpretation:
All four possible sets of quantum numbers for an electron in
Concept Introduction:
Refer to part (a)
(c)
Interpretation:
All four possible sets of quantum numbers for an electron in
Concept Introduction:
Refer to part (a)
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Chemistry: The Molecular Science
- 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?arrow_forwardWhat is the maximum number of electrons that can occupy a f subshell (l = 3)?arrow_forward10. (a) Use the radial wave function for the 3p orbital of a hydrogen atom 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.arrow_forward
- Classify the following statementsas either true or false: (a) In a contourrepresentation of an orbital,such as the one shown here fora 2p orbital, the electron is confinedto move about the nucleuson the outer surface of the shape.(b) The probability density [ψ(r)]2gives the probability of findingthe electron at a specific distancefrom the nucleus.arrow_forward2. (a) What is the smallest atom in group 13?(b) What is the smallest atom of the atoms Te, In, Sr, Po, Sb? Why is that?arrow_forward(a) Assign a proper spectroscopic symbol (spdf...) to each subshell having the following set of quantum numbers n and I. (b) Indicate the number of orbitals in each subshell. (c) What is the maximum number of electrons that can be assigned to each subshell? If the answer is "none", give your reasoning. (a) n= 6,1 = 0; (b) n= 3, 1= 2; (c) n= 2,1 = 2; (d) n= 5, 1= 1; (e) n= 4,1= 3;arrow_forward
- What is the orbital angular momentum (as multiples of h) of an electron in the orbitals (a) 1s. (b) 3s. (c) 3d. (d) 2p. (e) 3p? Give the numbers of angular and radial nodes in each case.arrow_forwardDetermine the number of valence electrons and give the electronic confi guration of the valence electrons of each element: (a) nitrogen; (b) potassium.arrow_forwardWhat is meant by the ground state of an atom? (a) All of the quantum numbers have their lowest values (n = 1, l = m = 0). (b) The principal quantum number of the electrons in the outer shell is 1. (c) All of the electrons are in the lowest energy state, consistent with the exclusion principle. (d) The electrons are in the lowest state allowed by the uncertainty principle.arrow_forward
- Each electron in an atom may be characterized by a set of four quantum numbers. For each of the following parts, tell how many different sets of quantum numbers are possible, such that each set contains all the values listed: (a) n=4; (b) n=2, l=2; (c) n=2, l=0; (d) n=4, l=2, ml=+3; (e) n=4, l=3, ml=-2; (f) n=3, l=1, ml=0; (g) n=2, l=1arrow_forwardDetermine the number of valence electrons and give the electronic confi guration of the valence electrons of each element: (a) fl uorine; (b) krypton; (c) magnesium; (d) germanium.arrow_forward5. Draw orbital diagrams for the ground states of: (a) Terbium, Tb, a lanthanide element. (b) The manganese(II) ion, Mn2+. (c) The sulphide ion, S2–. (d) Silver, Ag.arrow_forward
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