Concept explainers
Interpretation: Using eq. 1.16, the energies of atomic orbitals of hydrogen with n=1, 2, 3, 4 and 5 are to be determined and relative spacings of the energy levels is to be explained.
Concept Introduction:
Atomic orbitals are regions of space around the nucleus of an atom where an electron is likely to be found and it describes the wave like behavior of one electron or pair of electron in an atom.
The most commonly filled orbitals are s, p, d, and f. Each such orbital can filled by a maximum of two electrons, each with opposite spin.
Each atomic orbital may be uniquely labelled by a set of four quantum numbers: n, l,
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Inorganic Chemistry
- Give the ground-state electron configurations of the fol- lowing elements: (a) P (b) Тс (c) Hoarrow_forward6. Gallium arsenide (GaAs) is used in the red lasers of bar-code readers. (a) Write the full, ground state electron configuration of both gallium and arsenic. (b) Identify how many valence electrons each atom has. (c) Using electron configurations, show what the most likely ions to form would be for both Ga and As. (d) Predict whether (i) the most likely ion for gallium be smaller or larger than its neutral atom and (ii) the arsenic ion be smaller or larger than its neutral atom. Explain your predictions.arrow_forwardWrite the complete ground-state electron configuration of Cu²⁺. For multi-digit superscripts or coefficients, use each number in succession.arrow_forward
- Consider an electron in the N shell. (a) What is the smallest orbital angular momentum it could have? (b) What is the largest orbital angular momentum it could have? Express your answers in terms of h and in SI units. (c) What is the largest orbital momentum this electron could have in any chosen direction? Express your answers in terms of h and in SI units. (d) What is the largest spin angular momentum this electron could have in any chosen direction? Express your answers in terms of h and in SI units. (e) For the electron in part (c), what is the ratio of its spin angular momentum in the z-direction to its orbital angular momentum in the z direction? E and d no answerarrow_forward5. (a) Use the hydrogen-like model z2 (in eV) En --13.6 to calculate the total energy of the three electrons of lithium (Li), which has the electron configuration: 1s? 2s'. The three ionization energies for Li(g) are: IE, = 5.392 ev; IE2 = 75.64 eV; IE = 122.5 ev. With the help of Koopman's theorem, what is the total energy of ropulsion between lithium's three electrons (in kJ mol')?arrow_forwardConsider an electron in the N shell. (a) What is the smallest orbital angular momentum it could have? (b) What is the largest orbital angular momentum it could have? Express your answers in terms of h and in SI units. (c) What is the largest orbital angular momentum this electron could have in any chosen direction? Express your answers in terms of h and in SI units. (d) What is the largest spin angular momentum this electron could have in any chosen direction? Express your answers in terms of h and in SI units. (e) For the electron in part (c), what is the ratio of its spin angular momentum in the z-direction to its orbital angular momentum in the z-direction?arrow_forward
- Use the noble-gas notation and write the ground-state electronic configurations of the following ions:(a) O2- (b) Tl3+ (c) V3+arrow_forwardQ2: a- Explain how such a model uses potentials such as a square well and a harmonic oscillator to try and predict the magic numbers. b- Describe what causes the existence of "magic numbers" for protons and neutrons in nuclei. Why are nuclei which have these magie numbers more stable than other nuclei? Draw any analogies with the energy levels of atomic electrons. c- Discuss briefly the failures of the shell model. ofarrow_forwardConsider these ground-state ionization energies of one-electron species:H=1.31X10³kJ/mol ,He⁺=5.24X10³kJ/mol Li²⁺=1.41X10⁴kJ/mol (a) Write a general expression for the ionization energy of anyone-electron species. (b) Use your expression to calculate theionization energy of B⁴⁺. (c) What is the minimum wavelengthrequired to remove the electron from the n=3 level of He⁺?(d) What is the minimum wavelength required to remove the electron from the n=2 level of Be³⁺?arrow_forward
- Write the noble gas orbital box electronic configuration of (i) S, and (ii) Ca*.arrow_forwardConsider an electron in the N shell. Express your answers in terms of h and in SI units. (a) What is the smallest orbital angular momentum it could have? (b) What is the largest orbital angular momentum it could have? (c) What is the largest orbital angular momentum this electron could have in any chosen direction? (d) What is the largest spin angular momentum this election could have in any chosen direction?arrow_forwardWould you expect Rb or Sr+ to have the higher ionization? [A] Justify your answer in terms of electron configuration, effective nuclear charge, and electron repulsions as appropriate. Be detailed and complete.arrow_forward
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