General Chemistry 1 Quarter 2: Module 1-3 Quiz

Quantum Numbers

• The principal quantum number, n, indicates the main energy levels or shells in an atom.
• The range of possible values for the azimuthal quantum number, ℓ, is 0 to n-1.
• The azimuthal quantum number, ℓ, specifies the characteristic energy of orbitals and their electrons.
• The magnetic quantum number, mℓ, determines the orientation of orbitals in space.
• The spin quantum number, ms, determines the intrinsic spin of an electron, with possible values of +1/2 or -1/2.
• The maximum number of electrons that can be accommodated in a 4d subshell is 10.

Orbital Characteristics

• A shell with principal quantum number n has a total of n^2 orbitals.
• The maximum number of electrons that can occupy an f subshell is 14.
• The azimuthal quantum number, ℓ, indicates the shape of orbital sublevels.
• ℓ has a value of 1 for p orbitals and 3 for f orbitals.
• The magnetic quantum number, mℓ, splits the subshells into individual orbitals.
• Possible values for mℓ when ℓ=3 are -3, -2, -1, 0, 1, 2, and 3.

Electron Configuration

• The total number of orbitals for a shell with principal quantum number n=4 is 16.
• A shell with principal quantum number n can accommodate a maximum of 2n^2 electrons.

Magnetism

• The term that refers to the magnetic state of an atom with one or more unpaired electrons is paramagnetism.

Test your knowledge of the electronic structure of atoms with this quiz covering the essential learning competencies related to quantum numbers, magnetic properties, and orbital diagrams. Explore the theory of quantum mechanics and its application in describing electrons in atoms.