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8 terms

Chemistry Definitions 3

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Orbitals
regions where elecrons are found, located at various distances from the nucleus
Principal Quantum Number
(n)
Describes the energy level in which the electron can be found
Possible values=(1, 2, 3, 4, 5, 6, 7)
Azimuthal Quantum Number
(l)
Describes the shape of the orbital
0=s orbital 1=p orbital 2=d orbital 3=f orbital
Magnetic Quantum Number
(m_l)
The orientation of the orbital in space
Possible values=(-1, 0, 1)
Spin Quantum Number
(m_s)
Describes the apparent spin of the electron
Possible values=(+1/2 or -1/2)
Aufbau Principle
a principle that states electrons occupy the orbitals of lowest energy first
(one of the 3 Laws of Electron Configuration)
Pauli Exclusion Principle
a principle that states an atomic orbital may contain, at most, two electrons
(one of the 3 Laws of Electron Configuration)
Hund's Rule
a rule that states that only one electron must occupy all orbitals of equivalent energy in an energy level of an atom before "doubling up" may occur