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• 2nd shell of an atom


  Maximum number of electrons: 8
• 2p orbital


  Maximum number of electrons: 6
• 3d subshell

  Maximum number of electrons: 10
• The number of electrons present in the 3d subshell is 10
• The number of electrons present in the 4th energy level (shell) of an atom is 18
• The number of orbitals in the d subshell is 5
• The number of orbitals in the p subshell is 3
• The number of quantum numbers needed to describe the state of an electron in an atom is 4
• 2s orbital


  Can hold a maximum of 6 electrons
• The Pauli Exclusion Principle states that electrons in the same orbital must have opposite spins
• Principal quantum number (n)

  Describes the size of the orbital
• Angular quantum number (l)

  Describes the shape of an orbital
• Spin quantum number (s)

  Describes the spin of an electron
• Magnetic quantum number (m)

  Distinguishes between orbitals of the same energy but different orientations
• d orbital

  • Dumbbell-shaped
• p orbital

  • Dumbbell-shaped
• s orbital

  • Spherical
• Spin Quantum number

  Either -1/2 or +1/2
• The statement that is NOT true regarding orbital diagrams is that electrons fill orbitals starting from the highest energy level
• 4d subshell

  Can hold a maximum of 10 electrons