Chapter 6 Part 3; Many-electron atoms
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1 Chapter 6 Part 3; Many-electron atoms Read: BLB HW: BLB 6:59,63,64,67,71b-d,74,75,90,97; Packet 6:10 14 Know: s & atoms with many electrons Spin quantum number m s o Pauli exclusion principle o Hund's Rule Electron Configurations using periodic table Summary s Allowed for electrons in atom. Describes of electrons in these energy states. number shape? name of orbitals? s p d f QUANTUM NUMBERS n principal l azimuthal m l magnetic defines? Dr. Lori Stepan Van Der Sluys 1 Chapter 6 Part 3 Dr. Lori Stepan Van Der Sluys 2 Chapter 6 Part 3
2 Shells, Subshells and s Subshell Ex:3s defined by 2 Quantum Numbers (n, l) n=3, l=0 Subshell Ex: 3p defined by 2 Quantum Numbers (n, l) n=3, l=1 Shell Ex: 3rd shell defined by one Quantum Number (n) n=1 Subshell Ex: 3d defined by 2 Quantum Numbers (n, l) n=3, l=2 Ex:3s defined by 3 Quantum Numbers (n, l, ml) n=3, l=0, ml=0 Ex:3px defined by 3 Quantum # (n, m, ml) n=3, l=1, ml=? Ex:3pz n=3, l=1, ml=? Ex:3py defined by 3 Quantum # (n, m, ml) n=3, l=1, ml=? LRSVDS Chem 110 Chapter 6 Part 3 3 Ex:3dxy n=3, l=2, ml=? Ex:3dxz n=3, l=2, ml=? Ex:3dx2-y2 n=3, l=2, ml=? Ex:3dz2 n=3, l=2, ml=? Ex:3dyz n=3, l=2, ml=? Which quantum numbers are needed to define the subshell? 1 n only 2 n and l 3 l only 4 m l only 5 l and m l 6 n, l, and m l LRSVDS Chem 110 Chapter 6 Part 3 4
3 How are shells, subshells and orbitals related to energy? Energy Levels in the Hydrogen Atom Energy Levels in Many Electron Atoms Why? LRSVDS Chem 110 Chapter 6 Part 3 5 LRSVDS Chem 110 Chapter 6 Part 3 6
4 ORBITAL ENERGIES energy is: the energy needed to remove an electron from the orbital (positive) or the energy released when an electron goes into the empty orbital (negative). H atom: Energy does not depend on l or m l 2 1 E( n) = RH n 1 e atom with nuclear charge Z (He +, Li +2 ) Z E( n) = RH n Multi-electron atom: where : Z eff = effective nuclear charge Z eff = Z S S(n, l) S(n, l) = screening 2 Zeff ( n, l) = RH E n 2 Screening and Effective Charge See section 7.2 Electrons in inner orbitals act as screens for outer electrons. This is also called shielding. Outer electrons experience a lesser nuclear charge (less attraction), called effective charge (Z eff ) Approximate: Z eff Z m where m = (often use # of core electrons) General Trends in Screening For a given shell (fixed n) s orbital has electron density at nucleus (sees larger Z eff ) and has lower energy p orbital has no electron density at the nucleus and has higher energy screening increases: s < p < d E increases: E s < E p < E d LRSVDS Chem 110 Chapter 6 Part 3 7 LRSVDS Chem 110 Chapter 6 Part 3 8
5 Shielding Affects the Ordering of Energy Levels Electron spin Stern-Gerlach experiment neutral atoms (electrons) seem to possess magnetic moment that is quantized enter another quantum number spin magnetic quantum number: (m s ) How do the electrons fill the orbitals? In which order? How many electrons can go into an orbital? m s = + up m s = down LRSVDS Chem 110 Chapter 6 Part 3 9 LRSVDS Chem 110 Chapter 6 Part 3 10
6 More Complete Description of An Electron an electron in an atom is described by quantum numbers: Pauli exclusion principle: no two e in an atom can have the same four quantum numbers Consequences of the Pauli exclusion principle: each orbital can have a maximum of two e, each with opposite spin # of maximum # subshell orbitals of electrons s (l = ) p (l = ) d (l = ) f (l = ) Look at the periodic table! ELECTRON CONFIGURATIONS s are filled sequentially, lowest energy orbitals fill first: Aufbau principle (or building up principle) H Li Na He Be B C N O F Ne Now we have a problem: What is the electron configuration of carbon? Carbon 1s 2 2s 2 2p 2 1s 2 2s 2 2p x 2p y 2p z or 1s 2 2s 2 2p x 2p y 2p z LRSVDS Chem 110 Chapter 6 Part 3 11 LRSVDS Chem 110 Chapter 6 Part 3 12
7 Hund s rule fill set of degenerate orbitals (subshells) to keep maximum number of spins (parallel) minimizes electron-electron repulsions, thereby energy LRSVDS Chem 110 Chapter 6 Part 3 14 LRSVDS Chem 110 Chapter 6 Part 3 13
8 Electron Configurations past First Row Ne 1s 2 2s 2 2p 6 [Ne] Na 1s 2 2s 2 2p 6 3s [Ne]3s Mg [Ne] 3s 2 Al [Ne] 3s 2 3p Si [Ne] 3s 2 3p 2 P [Ne] 3s 2 3p 3 S [Ne] 3s 2 3p 4 Cl [Ne] 3s 2 3p 5 Ar [Ne] 3s 2 3p 6 filled subshell K [Ne] 3s 2 3p 6 4s new shell (row) Ca [Ne] 3s 2 3p 6 4s 2 Ca 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 Transition Metal Electron Configurations 4s fills 3d Exception: Cr and Cu (know these 2 exceptions!); Sc [Ar] 4s 2 3d 1 Ti [Ar] 4s 2 3d 2 V [Ar] 4s 2 3d 3 Cr [Ar] 4s 1 3d 5 half filled subshells Mn [Ar] 4s 2 3d 5 Fe [Ar] 4s 2 3d 6 Co [Ar] 4s 2 3d 7 Ni [Ar] 4s 2 3d 8 Cu [Ar] 4s 1 3d 10 filled d-subshell Zn [Ar] 4s 2 3d 10 [Ar] 4s 2 Core valence or or inner-shell outer-shell electrons electrons know the first row of transition metals as well as main group LRSVDS Chem 110 Chapter 6 Part 3 15 LRSVDS Chem 110 Chapter 6 Part 3 16
9 Order of filling 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 6s 6p 6d LRSVDS Chem 110 Chapter 6 Part 3 18 LRSVDS Chem 110 Chapter 6 Part 3 17
![(H) 1s 1 Li [He] 2s 1 Na [Ne] 3s 1 K [Ar] 4s 1 Rb [Kr] 5s 1 Cs [Xe] 6s 1 halogens (F, Cl, Br, I) have outer shell noble gases (inert) have](/docs-images/72/68044349/images/10-1.jpg "filled outer shell of Valence electrons determine the chemistry!")
10 Electron Configuration and the Periodic Table Location on Periodic Table is related to electron configuration Elements in the same row (family) have the same valence shell configuration. Example: alkali metals (row 1) have what valence electron configuration? (H) 1s 1 Li [He] 2s 1 Na [Ne] 3s 1 K [Ar] 4s 1 Rb [Kr] 5s 1 Cs [Xe] 6s 1 halogens (F, Cl, Br, I) have outer shell noble gases (inert) have filled outer shell of Valence electrons determine the chemistry! Electron Configurations of the Elements LRSVDS Chem 110 Chapter 6 Part 3 20 LRSVDS Chem 110 Chapter 6 Part 3 19
11 Before next class: Read: BLB 2.5; HW: BLB 2:35; 7:9,21,25,30,31,41a c,43a,e,f; 46, 49, 57, 91 Sup 7:1 12 Know: screening effects periodic properties atomic and ion sizes isoelectronic series electron configurations of ions ionization energies electron affinities LRSVDS Chem 110 Chapter 6 Part 3 21
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