Electron Orbitals Heisenberg 1 The Uncertainty principle states
Electron Orbitals Heisenberg 1. The ______ Uncertainty _______ principle states that it is impossible to determine simultaneously both the position and the velocity of an electron or any other particle.
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 ______ momentum _______ quantum number (l) indicates the shape of the orbital.
Electron Orbitals (l) 0 1 2 3 Orbital Type s p d 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
Electron Orbitals aufbau 2. The ____ principle states that an electron will occupy the lowest-energy orbital that can receive it.
Electron Orbitals 3. Hund’s ____ 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.
Electron Orbitals 1. The arrangement of electrons in an atom is known as the atom’s Electron ______ configuration _________. One type of electron configuration is orbital notation ___________.
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