Electron Orbitals Heisenberg 1. The ____________ ______________ principle states that it is impossible to determine simultaneously both the position and the velocity of an electron or any other particle. Uncertainty

Electron Orbitals pauli exclusion 1. The ______ ___________ principle states that no two electrons can have the same set of four quantum numbers.

Electron Orbitals principal a. The __________ quantum number (n), indicates the main energy level. Values of n are positive integers 1, 2, 3, and so on.

Electron Orbitals angular b. The ___________ _____________ quantum number (l) indicates the shape of the orbital. momentum

Electron Orbitals (l) Orbital Type s 1 p 2 d 3 f

Electron Orbitals magnetic c. The ____________ quantum number (ml) indicates the orientation of an orbital around the nucleus. Can have a value of –l through zero to +l.

Electron Orbitals spin d. The _____ quantum number (ms) has only two possible values, + ½ and – ½ , because only two electrons can exist in the same orbital and indicates one of the two fundamental spin states.

Electron Orbitals aufbau 2. The ________ principle states that an electron will occupy the lowest-energy orbital that can receive it.

Electron Orbitals 3. ________ rule states that orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singly occupied orbits have the same spin. Hund’s

Electron Orbitals 1. The arrangement of electrons in an atom is known as the atom’s ___________ _________________. One type of electron configuration is _________ ___________. Electron configuration orbital notation