Atomic Models and Quantum Numbers for handout shortened version new 4 slides per page

# 0 l2 l1 l angular momentum azimuthal

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Unformatted text preview: ic quantum number ml – Gives the direction or orientation of orbital as if influenced by a magnetic field ml = −l , (−l + 1), (−l +2), .....0, ......., (l−2), (l−1), l • Angular momentum (azimuthal) quantum number ‘l’ • l - shape of the orbital. l = 0, 1, 2, 3, 4, 5, .......(0 to n-1) l = s, p, d, f, g, h, ....... • These orbitals are the volume around the atom that the electrons occupy 90-95% of the time. • If l = 0 (or an s orbital), then ml = 0 – Notice that there is only 1 value of ml This implies that there is one s orbital per n value. n ≥ 1 • If l = 1 (or a p orbital), then ml = -1,0,+1 – There are 3 values of ml Thus there are three p orbitals per n value. n ≥ 2 This is one of the places where Heisenberg’s Uncertainty principle comes into play. Quantum Numbers ml • If l = 2 (or d orbital), then ml = -2,-1,0,+1,+2 – There are 5 values of ml Thus there are five d orbitals per n value. n ≥ 3 • If l = 3 (or f orbital), then ml = -3,-2,-1,0,+1,+2, +3 – There are 7 values of ml Thus there are seven f orbitals per n value, n ≥ 4 • Theoretically,...
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## This document was uploaded on 03/26/2014.

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