Interpretation:
The four quantum numbers for the highest energy electron in ground state of lithium atom have to be determined.
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.
1. These quantum numbers are represented by
2. 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
3. The quantum number
4. The quantum number
The electronic configuration is defined as the distribution of electrons in various atomic orbitals of the atom. The electrons that are present in an outermost orbital are known as valence electrons whereas those present in the orbitals with lower quantum numbers are called core electrons. The general outer electronic configuration of
Electrons are filled in orbitals in accordance with three rules: Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. Aufbau principle states that electrons are filled in the orbitals from lower to higher energy level as follows:
Hund’s rule states that initially each orbital is singly occupied and then pairing occurs and Pauli’s exclusion principle states that the spin of two electrons in one orbital is always different.
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Chapter 7 Solutions
Chemistry: Principles and Practice
- • identify an orbital (as 1s, 3p, etc.) from its quantum numbers, or vice versa.arrow_forwardAssign a correct set of four quantum numbers for (a) Each electron in a nitrogen atom. (b) The valence electron in a sodium atom. (c) A 3d electron in a nickel atom.arrow_forwardWhat is the maximum number of electrons that can occupy a f subshell (l = 3)?arrow_forward
- According to a relationship developed by Niels Bohr, for an atom or ion that has a single electron, the total energy, En, of an electron in a stable orbit of quantum number n is En = [Z2/n2] (2.179 1018 J) where Z is the atomic number. Calculate the ionization energy for the electron in a ground-state He+ ion.arrow_forward6.96 When a helium atom absorbs light at 58.44 nm, an electron is promoted from the 1s orbital to a 2p orbital. Given that the ionization energy of (ground state) helium is 2372 kJ/ mol, find the longest wavelength of light that could eject an electron from the excited state helium atom.arrow_forwardInvestigating 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.arrow_forward
- 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_forwardWrite a complete set of quantum numbers (n, , m) that quantum theory allows for each of the following orbitals: (a) 2p, (b) 3d, and (c) 4f.arrow_forwardConsider the eight most abundant elements in the human body, as outlined in Exercise 156. Excluding hydrogen, which of these elements would have the smallest size? largest size? smallest first ionization energy? largest first ionization energy?arrow_forward
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