9. Quantum Mechanics

Which quantum numbers are required to determine the energy of an electron in a many-electron atom?

Which of the following ranks the orbitals 1s, 2s, and 3s in order of increasing size?

Which one of the following sets of quantum numbers is not possible for an electron in an atom?

What is the smallest possible value of the principal quantum number (n) for an electron in an atom?

Which statement correctly describes the principal quantum number n for an electron in the state n=4, l=3, m=2, s=1/2?

Which of the following sets of quantum numbers is valid for an electron in an atom?

Which of the following sets of quantum numbers for an electron in a hydrogen atom is valid?

Which of the following combinations of quantum numbers is allowed for an electron in an atom?

Which type of orbital has the lowest energy for a given principal quantum number n?

Which atomic model treats electrons as waves?

Which characteristic of an electron in an atom is determined by the principal quantum number (n)?

In the quantum mechanical model of the atom, what does the principal quantum number n represent?

Which statement is true when the principal quantum number n equals 1 for an electron in an atom?

Two orbitals are described as 2s and 3s. Which quantum number(s) would be different for these two orbitals?

For a 3s^2 electron in phosphorus (atomic number 15, electron configuration: 1s^2 2s^2 2p^6 3s^2 3p^3), what is the value of the third quantum number (magnetic quantum number, m_l) for this electron?