Chemistry Energy Levels Essay

The nil of the subshell increases as follows4s& adeninelt4p&lt4d&lt4f * 4s has the greatest probability of being close to the heart * Subshells are limited to of electrons they corporation hold ( 2 electrons per orbital) s=21s orbital d=105d orbital p=63p orbitals f=147f orbitals Assessment * How many p subshells are in the 4th energy aim (n=4)? 34px 4py 4pz * What is the maximum material body of electrons that can occupy the 4p subshell? from each one p subshell can hold 2 electrons and therefore there are 3p orbitals with 2 electrons *What is the maximum number of electrons that can occupy the 4th energy 322n2=2(4)2 =2(16) =32 Creating Energy Level Diagrams * apply to show the relative energies of electrons in various orbitals under normal conditions * for each one orbital is indicated by a separate circle/square * in all orbitals of a accustomed subshell have the selfsame(prenominal) energy. Ie. The 3p orbitals in the 3p sublevels have the same energy * The spac ing between successive subshells decreases as the number of subshells increases co-occur of shells having different values of n.Assessment 1. How many d orbitals exist? 5 2. How many electrons can exist in the 3d orbitals? 10-2 in each of the 5d orbitals 3. How many electrons can exist in the n=2 level? 8-remember 2n2=2(2)2=8 4. How many electrons can one 4f orbital hold? 14-2 in each of the 7f orbitals 5. Which has a higher energy a px, py, or pz orbital? They all have the same energy. 6. Which electron can be effectuate farthest from the cell nucleus2s or 3s? 3s electrons 7. Which electrons can be found furthest from the nucleus2s or 2p. 2p is further. Fig. 3. 19Arrow orbital notation Aka Orbital Diagrams * Use circles or squares for the orbitals and arrows for the electrons * RULES * The Aufbau Principal- electrons will occupy lowest available energy level * Pauli Exclusion Principal- no two electrons have the same quantum numbers racket * Hunds Rule electrons remain un b racinged for as long as possible. Ex One electrons goes in each Px, Py, Pz, before they start to pair up Fig 3. 21 Electron Configuration Provides the same data as an energy level diagram but in a more concise format. * Li 1s2 2s1 C1s2 2s2 2p2 * Ne 1s2 2s2 2p? Use the pursuance concept map to help to determine the filling order of the orbitals * The likeness among elements within groups and the structure of the periodic table can be explained by electron compliance * Li 1s2 2s1 * Na 1s2 2s2 2p? 3s1 Short Hand Notation -Use symbol of noble gas with the same core electron configuration Ex. Na 1s2 2s2 2p? 3s1 Or Ne 3s1 Some unexpected Electron Configuration * typesetters case Cru and Cu Expected Actual Cr Ar 4s2 3d? Ar 4s1 3d? Cu Ar 4s2 3d? Ar 4s1 3d10 In each case, an electron is borrowed from the 4s subshell and placed in the 3d subshell. * Cr-3d subshell becomes half-filled * Cu-3d subshell becomes full * Half-filled and fully filled subshells tend to be more perpetual * Other expectations Ag Kr 4s2 3d10 Au Xe 4f14 5d10 6s1 Explaining Ion Charges * Remember s electrons are doomed before d electrons when dealing with transition metals. Ex1. Zn Zn Ar 4s2 3d10 Zn2+ Ar 3d10 (4s electrons are lost so that the 3d orbital remains full) Ex2. Pb Pb Xe 6s2 4f14 5d10 6p2 Pb2+ Xe 4f14 5d10 6p2 (The 6s electrons are lost)Pb4+ Xe 4f14 5d10 (The 6p electrons are lost as well as the 6s electrons) Quantum amount * Electron waves (orbitals) can be characterized by a set quantum numbers, n, l, ml, ms Principle quantum number (n) * Identifies the energy of an electron in an orbital * each orbitals that have the same value of n are said to be in the same shell * Range from n=1 to n=infinity * Determines the size of the electron wave how far the wave extends from the nucleus * As n increases the energies of the orbitals also increase Secondary quantum number (l)Divides the shells into littler groups called subshells * n determines the values of l * for any given n, l may ra nge from l=0 to l=n-1 * identifies the shape of the orbital survey of l 0 1 2 3 Letter appellative s(shape) p(principle) d(diffuse) f(fundamental) Magnetic quantum number (ml) * splits the subshells into individual orbits * identifies the orientation of the orbital * for any given value of l, ml has a value ranging from +l to l * e. g. If l=0, ml=0 for l=1, ml=+1, 0, -1 which correspond to the x, y and z orientations of the p orbitals.