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Chapter 6

Chapter 6. Atomic Structure Hingham High School Mr. Clune. Development of the Periodic Table. mid-1800s, about 70 elements Dmitri Mendeleev – Russian chemist Arranged elements in order of increasing atomic mass Thus, the first “Periodic Table”. Dimitri Mendeleev.

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Chapter 6

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  1. Chapter 6 Atomic Structure Hingham High School Mr. Clune

  2. Development of the Periodic Table • mid-1800s, about 70 elements • Dmitri Mendeleev – Russian chemist • Arranged elements in order of increasing atomic mass • Thus, the first “Periodic Table”

  3. Dimitri Mendeleev

  4. Mendeleev Periodic Table

  5. Mendeleev • Left blanks for undiscovered elements • When discovered, good prediction • Problems or inconsistencies? • Co and Ni; Ar and K; Te and I

  6. New way • Henry Moseley – British physicist • Arranged elements according to increasing atomic number • The arrangement today • Symbol, atomic number & mass

  7. Henry Moseley

  8. Periodic table • Horizontal rows = Period • There are 7 periods • Periodic law: • Vertical column = Group (or family) Similar physical & chemical prop. Identified by number & letter

  9. Horizontal rows are called periods • There are 7 periods

  10. Vertical columns called groups Elements are placed in columns by similar properties Also called families

  11. Periodic Law When elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties.

  12. Groups of Elements The vertical columns in the Periodic Table. Elements in each group have similar properties.

  13. Groups of Elements Example: Group 11 Copper Silver Gold

  14. Metals - Metalloids – NonMetals

  15. Metals • 80% of the elements • Good Conductor • Heat • Electricity • High luster or sheen • Reflect light

  16. Metals • Ductile • (Pulled into wire) • Malleable • (Hammered into sheets)

  17. Non-Metals • Non-Metals are not Metals • (Properties unlike Metals) • Bad Conductors • (Except Carbon) • Brittle • (Shatter)

  18. Non-Metals • Most are Gases • Oxygen, Nitrogen, Hydrogen!! • Some are Solid • (Sulfur and Phosphorus) • Some are liquid • Bromine is a dark brown liquid.

  19. Areas of the periodic table • Group A elements = representative elements • Wide range of phys & chem prop. • Metals: electrical conductors, have luster, ductile, malleable

  20. Metalloids • Staircase separating Metals and Nonmetals • Properties similar to • Metals and Nonmetals • Sometimes acts like a metal. • Sometimes acts like a nonmetal.

  21. Silicon • Pure Silicon - Nonmetal. • Bad Conductor !!! • Add Boron • Conducts • electricity • SemiConductor

  22. Atomic Number • Electron • Configuration • Chemical Symbol • Name • Mass Number Squares in a Periodic Table Si 2 8 6 14 Silicon 28.086

  23. Noble Gases Non- Metals Metalloids Alkali Metals Alkaline Earth Metals Metals Halogens Transition Elements

  24. Electron ConfigurationinGroups

  25. H 1 Li 3 Na 11 K 19 Rb 37 Cs 55 Fr 87 Group 1 – _s1 1s1 1s22s1 1s22s22p63s1 1s22s22p63s23p64s1 1s22s22p63s23p64s23d104p65s1 1s22s22p63s23p64s23d104p65s24d10 5p66s1 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s1

  26. Group 18 – _p16 He 2 Ne 1s2 1s22s22p6 1s22s22p63s23p6 1s22s22p63s23p64s23d104p6 1s22s22p63s23p64s23d104p65s24d105p6 1s22s22p63s23p64s23d104p65s24d10 5p66s24f145d106p6 10 Ar 18 Kr 36 Xe 54 Rn 86

  27. S- block s1 s2 • Alkali metals all end in s1 • Alkaline earth metals all end in s2 • really should include He, but it fits better later. • He has the properties of the noble gases.

  28. d 10 Transition Metals -d block s1d5 s1d9 d1 d2 d3 d5 d6 d7 d8

  29. The P-block p1 p2 p6 p3 p4 p5 B C N O F Ne

  30. f6 f13 f1 f2 f3 f4 f5 f7 f8 f10 f12 f14 f11 f9 F - block • inner transition elements

  31. 1 2 3 4 5 6 7 • Each row (or period) is the energy level for s and p orbitals.

  32. 1 2 3 4 5 6 7 Transition Elements Inner Transition Elements

  33. Atomic Size } • Atomic Radius = half the distance between two nuclei of a diatomic molecule. Radius

  34. Trends in Atomic Size • Influenced by three factors: 1. Energy Level • Higher energy level is further away. 2. Charge on nucleus • More charge pulls electrons in closer. • 3. Shielding effect (blocking effect?)

  35. Group Trends H • As we go down a group... • each atom has another energy level, • so the atoms get bigger. Li Na K Rb

  36. Periodic Trends • As you go across a period, the radius gets smaller. • Electrons are in same energy level. • More nuclear charge. • Outermost electrons are closer. Na Mg Al Si P S Cl Ar

  37. Size generally increases Trends in Atomic Size

  38. Trends in Ionization Energy • The amount of energy required to completely remove an electron from a gaseous atom. • Removing one electron makes a 1+ ion. • The energy required to remove the first electron is called the first ionization energy.

  39. Ionization • Ion – A charged atom. Gains or loses electrons • Cation – Ion with a positive charge Loses electron(s) • Anion – Ion with a negative charge Gains electrons - + Na e- Cl

  40. Ionization Energy • The second ionization energy is the energy required to remove the second electron. • Always greater than first IE. • The third IE is the energy required to remove a third electron. • Greater than 1st or 2nd IE.

  41. Symbol First Second Third 1312 2731 520 900 800 1086 1402 1314 1681 2080 H HeLi BeB C N O F Ne 5247 7297 1757 2430 2352 2857 3391 3375 3963 11810 14840 3569 4619 4577 5301 6045 6276

  42. What determines IE • The greater the nuclear charge, the greater IE. • Greater distance from nucleus decreases IE • Filled and half-filled orbitals have lower energy, so achieving them is easier, lower IE.

  43. Group trends • As you go down a group, first IE decreases because... • The electron is further away.

  44. Periodic trends • All the atoms in the same period have the same energy level. • But, increasing nuclear charge • So IE generally increases from left to right.

  45. Energy generally increases Trends in Ionization Energy

  46. Trends in Ionic Size • Cations form by losing electrons. • Cations are smaller that the atom they come from. • Metals form cations. • Cations of representative elements have noble gas configuration.

  47. Ionic size • Anions form by gaining electrons. • Anions are bigger that the atom they come from. • Nonmetals form anions. • Anions of representative elements have noble gas configuration.

  48. Group trends • Adding energy level • Ions get bigger as you go down. Li1+ Na1+ K1+ Rb1+ Cs1+

  49. Periodic Trends • Across the period, nuclear charge increases so they get smaller. • Energy level changes between anions and cations. N3- O2- F1- B3+ Li1+ C4+ Be2+

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