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Lecture 5

Lecture 5. shells. 1s. K. 1s. 2. s. 2. p. L. 3. s. 3. p. M. 4. s. 3d. 3. d. 4. p. N. s. 4d. O. 5. 4. d. 5. p. 6. s. 5d. 5. d. 6. p. P. 7. s. 6d. 6. d. p block. d block. s block. 4. f. 5. f. f block. Electronic Configuration of Periodic Table.

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Lecture 5

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  1. Lecture 5

  2. shells 1s K 1s 2 s 2 p L 3 s 3 p M 4 s 3d 3 d 4 p N s 4d O 5 4 d 5 p 6 s 5d 5 d 6 p P 7 s 6d 6 d p block d block s block 4 f 5 f f block Electronic Configuration of Periodic Table

  3. Electronic Configuration of Periodic Table • Aufbau Principle: Add one proton to nucleus and one electron to the lowest-energy orbital available in the electron shell. • s block: 2 boxes  1 orbital  2 electrons. For s: l= 0; m= 0 i.e. 1 orbital on s subshell. • p block: 6 boxes  3 orbitals  with 2 electrons each. For p: l=1; m= -1, m= 0, m= 1 i.e. 3 orbitals on p subshell • d block: 10 boxes  5 orbitals  with 2 electrons each. For d: l= 2; m = -2, m = -1, m= 0, m =1, m =2 i.e. 5 orbitals on d subshell • f block: 14 boxes  7 orbitals  with 2 electrons each. For f: l =3; m =-3, m =-2, m =-1, m =0, m =1, m =2, m =3 i.e. 7 orbitals on f subshell

  4. Electron Energy Diagrams • A visual method of showing the energy of electrons within an element: 3 steps to build an energy diagram: • e.g. Iron [Fe] Z=26  26 protons  26 electrons • Step 1: Write down shorthand electronic configuration. • Step 2: Build energy diagram with subshells • Step 3: Fill in electrons with arrows counting up to Z. Step 1 1s2 2s2 2p6 3s2 3p6 4s2 3d6 (short hand)

  5. Electron Energy Diagrams • A visual method of showing the energy of electrons within an element: 3 steps to build an energy diagram: • e.g. Iron [Fe] Z=26  26 protons  26 electrons • Step 1: Write down shorthand electronic configuration. • Step 2: Build energy diagram with subshells • Step 3: Fill in electrons with arrows counting up to Z. Step 1 1s2 2s2 2p6 3s2 3p6 4s2 3d6 (short hand)

  6. Energy 3d 4s 3p 3s Step 2 2p 2s 1s Step 3 Electron Energy Diagrams

  7. Valence Electrons • Every element has both core electrons and valence electrons, e.g. Magnesium: Mg Z=12  12 electrons: 1s2 2s2 2p63s2 core electrons valence electrons • Core electrons are electrons in fully filled shells • Valence electrons are electrons in the outermost shell that is not fully filled with the exception of the noble gases that all have fully filled shells He: 1s2, Ne: {He} 2s2 2p6, Ar: {Ne} 3s2 3p6, Kr: {Ar} 4s2 3d10 4p6, Xe: {Kr} 5s2 4d10 5p6. Rn: {Xe} 6s2 4f14 5d10 6p6 .

  8. Construction of the Periodic Table • Electron shells fill in a systematic fashion so that patterns can be recognised in the electronic configuration. • Elements listed in horizontal Rows are called Periods. A new period is started each time the value of the principle quantum number, n, increases, i.e. each time the valence electrons enter a new shell. • Arrange rows so that elements with similar electronic configuration lie above one another to form vertical columns called Groups, similar electronic configuration meaning similar chemistry.

  9. Group Properties • Group 1 - elements with only one valence electron: These are called the Alkali-Metal Group Electronic configuration 3Lithium Li {He}2s1 11Sodium Na {Ne}3s1 19Potassium K {Ar}4s1 37Rubidium Rb {Kr}5s1 55Cesium Cs {Xe}6s1 87Francium Fr {Rn}7s1 Physical Properties metals i.e good conductors, soft, low melting point and boiling point

  10. ; ; ; ; Group I Chemical Properties Na. + :Cl . →NaCl (Na+ and :Cl :- ) Alkali + Halogen →Ionic Compound Na. + H2O → NaOH + H+ Alkali + Water →Ionic Compound NaOH → Na+ + OH- • cations: positive ions (e.g. Na+, K+, H+) • anions: negative ions (Cl, OH) • Me → Me+ + e (Me = Alkali metal)

  11. Group 17 (or 7A) Halogens • Elements with one electron less than their nearest nobel gas: The Halogens: (Greek: halogen=salt former) Electronic Configuration: 9Fluorine F {He}2s22p5 17Chlorine Cl {Ne}3s23p5 35Bromine Br {Ar}4s23d104p5 53Iodine I {Kr}5s24d105p5 • Physical Properties: Highly coloured - volatile - non-metals - bad conductors - occur in nature as diatomic molecules X2 (X=Halogen), e.g. Cl2. F2 and Cl2 are gases, Br2 is a liquid and I2 is a solid.

  12. Chemical Properties of the Halogens X + H  HX or better: X2 + H2 2 HX X + Me  MeX (Me+ + X) (see group 1) • Aqueous solutions of HX contain high concentrations of H+, i.e. are acids: HX + H2O  H+ + X- + H2O

  13. Group 18 (or 8A) - The Noble Gases • Special group of elements within the periodic table. They all have full electron shells and are highly non-reactive. • Physical properties: Colourless gases (at normal temperature and pressure) – lowest boiling and melting points of all elements. • Chemical properties: The most chemically unreactive of all elements, up to recently thought to be totally unreactive and were called Inert Gas Elements. Summary • Groups (columns) have similar electronic configuration and similar chemistry, e.g., Noble gases have full shells, Alkali metals have one electron more than Noble gases. Halogens have one electron less than Noble gas configuration.

  14. Summary Continued. • Properties of Periods (Rows): Periods are characterised by the gradual filling of valence shells – all atoms in a period have different electronic configuration. • Similar chemical behaviour is not expected, however a gradual change of the metallic properties of Group 1 to the non-metallic properties of Group 17 is expected.

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