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Introducing the Elements

Introducing the Elements. The Element Song. 1869: Dmitri Mendeleev. Russian chemist Arranged elements in tabular form so that elements with similar properties were in the same column When listed in order by mass, elements generally repeat properties in groups of 8 (Law of Octaves).

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Introducing the Elements

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  1. Introducing the Elements The Element Song

  2. 1869: Dmitri Mendeleev • Russian chemist • Arranged elements in tabular form so that elements with similar properties were in the same column • When listed in order by mass, elements generally repeat properties in groups of 8 (Law of Octaves)

  3. The First Periodic Table • Most tables at the time listed elements by mass • Mendeleev also arranged elements by mass, but left several “holes” in his table and occasionally reversed the order of elements to fit the properties of others in that column • The “holes” were later filled in with newly discovered elements that had the properties predicted by Mendeleev’s table. • The reason for the reversal of elements was explained later by Henry Moseley, who noted that the elements were in order by atomic number (number of protons) rather than by mass

  4. Know the following Elements • 1-20, 24-30, 33, 35-38, 47, 48, 50, 53-56, 78, 79, 80, 82, 86, 92 • Names and symbols

  5. Sodium • Mercury • Zinc • Bromine • Calcium • Fluorine • Helium • Manganese • Nickel • Uranium 11. C 12. O 13. Pb 14. Sn 15. Cr 16. Mg 17. Ba 18. K 19. Si 20. Ag

  6. boron • berylluim • iron • chlorine • lithium • magnesium • argon • cobalt • potassium • phosphorous 11. Al 12. Cd 13. As 14. Pt 15. Cu 16. Sr 17. Ba 18. Ne 19. Rn 20. Kr

  7. Hydrogen • Most abundant element in the universe Why? • Makes up most the mass of stars • Can be H+ (hydrogen ion) or H- (hydride ion) • Used in Fuel Cells: How Stuff Works • In Fusion, H is converted to He

  8. Alkali Metals: Li, Na, K, Rb, Cs, Fr • Most reactive of the metals, +1 ions • Stored under kerosene or mineral oil • Na and K most important • Na2CO3 and NaHCO3 two important compounds • K is an important plant nutrient (macronutrient) • Fertilizers: N-P-K (Not found in nature in elemental form)

  9. Alkaline Earth Metals: Be, Mg, Ca, Sr, Ba, Ra • Harder, more dense, and less reactive than alkali metals • Ca, Sr, and Ba most alike • Hard Water: Ca2+ and Mg2+ ions • Epsom salt: MgSO4 Boiler Scale

  10. …..more on the alkaline earths • CaCO3 is limestone becomes marble • Limestone is most abundant rock in the earth’s crust • CaO “Lime” or “quicklime” • CaSO4 “Plaster of Paris” (building material) Plaster of Paris footprints

  11. Do You Know? • Most abundant element in the universe? • Most abundant rock in the earth’s crust? • Formula for the “plaster of Paris”? • Ions found in “hard” water? • Three numbers of fertilizer? • How do alkaline earth metals compare to the alkali metals in (a) reactivity and (b) density?

  12. Aluminum Group: B, Al, Ga, In, Tl • Aluminum by far the most important • Third most abundant element in the earth’s crust • Important metal: abundant, light weight, strong • Al2O3 coating prevents corrosion

  13. Carbon Group: C, Si, Ge, Sn, Pb • Very diverse group of elements • C is the basis for organic compounds • CO2 and CO3-2 inorganic carbon • CO2 one of the earliest gases in the atmosphere • Carbon cycling one of the most important • Two basic parts: (1) photosynthesis (2) respiration

  14. Disrupting the carbon cycle • CO2 is a greenhouse gas (GWP=1) • Increasing concentration by: • Burning fossil fuels • Removing vegetation • Preindustrial 1800: 280 ppm • 1959: 316 ppm • 2010: 388 ppm • 2011: 391 ppm

  15. Silicon - Si • Second most abundant element in the Earth’s crust • Found in clay, sand, sandstone, silica rock, quartz, other minerals • Many different bonding combinations • Is a semiconductor (Silicon Valley)

  16. Tin (Sn) and Lead (Pb) • Many Industrial Uses • Pb is a “heavy metal” and is toxic to many organs in the human body • Impedes the development of the nervous system • Taken out of gasoline in the late 1970’s and removed from most paints

  17. The Halogens F, Cl, Br, I, At • Group 17 – halogen means (salt former) • The most reactive nonmetals • F and Cl are gasses • Br is a liquid • I is a solid

  18. Total Molar Composition of Seawater (Salinity = 35)[7]

  19. Bonding: Influences • Valence Electrons • Nuclear Charge • Atomic Size/Radius • Distance between attractions • Screening or Shielding Effect

  20. Valence Electrons

  21. Core Configurations • Why? – Shows/focuses on the valence electrons. • Write the configuration for arsenic. • 1s22s22p63s23p64s23d104p3 • or • [Ar] 4s23d104p3 • How many valence electrons?

  22. Write the electron configuration and orbital notation for chlorine. • 1s22s22p63s23p5 • Now write its core configuration. • [Ne] 3s23p5 • How many valence electrons?

  23. Atomic Radius: How is it measured? • Half the distance between nuclei of two covalently bonded atoms of the same element. • Why not just measure from the nucleus to the outer edge of the atom?

  24. Atomic Radius

  25. Radius trends • Group trend? Radius increases down a group • Why? Adding new energy levels • Period trend? Radius decreases across a period • Why? Increasing nuclear charge has the effect of pulling electron cloud closer.

  26. Ions and their formation • Cations • Formed by the loss of electrons • Positively charged • Usually formed from metals • Are always smaller than the atom they are formed from • Anions • Formed by the gain of electrons • Negatively charged • Usually formed from nonmetallic elements • Are always larger than the atom they are formed from

  27. Ionization Energy • The energy required to remove an electron from an isolated, neutral, gaseous atom. • First ionization energy – energy required to remove a first electron from an atom. • Second ionization energy – energy required to remove a second electron from an atom. • Third ionization energy - ???? • Etc . . . .

  28. First Ionization Energies

  29. First Ionization energies • Group trend – IE1 decreases down a group. Why? • Valence electrons are further from the nucleus and the shielding effect is greater down a group. • Shielding effect – occurs when core electrons “shield” or interfere with the attraction that the nucleus has for the valence electrons.

  30. . . . IE cont. . . . • Period trend – IE1 is larger as you move across a period, left to right. Why? • Atoms are smaller so valence electrons are closer to the nucleus and . . . . . • . . . the nuclear charge is greater with no change in shielding effect (electrons are going in the same energy level)

  31. Ionization Energy Increasing Trend Periodic Table

  32. Successive Ionization Energies Where do the largest jumps occur for each Element and why do you think this happens?

  33. Electronegativity • A measure of the ability of an atom to attract electrons to itself when bonded to other atoms.

  34. Electronegativity

  35. Electronegativities

  36. Place these elements in order of increasing: Ge, P, N, and Si (a) atomic radius (b) first ionization energy (c) electronegativity 2. Write the core configuration for the following elements: S, Ca, Sn • How many valence electrons does each element in #2 have?

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