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Chapter #5 The Periodic Law

Chapter #5 The Periodic Law. 5-1 History of the Periodic Table. Cannizzaro (1826-1910) developed a method for measuring atomic masses and interpreting the results of the measurements. Stanislao Cannizzaro. Mendeleev (1834-1907) Created the 1 st periodic table by increasing atomic mass.

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Chapter #5 The Periodic Law

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  1. Chapter #5 The Periodic Law

  2. 5-1 History of the Periodic Table • Cannizzaro (1826-1910) developed a method for measuring atomic masses and interpreting the results of the measurements. Stanislao Cannizzaro

  3. Mendeleev (1834-1907) Created the 1st periodic table by increasing atomic mass. Dmitri Mendeleev

  4. Moseley (1887-1915) set up the periodic table according to increasing atomic number. Henry Moseley

  5. The word "periodic" means that there is a repeating pattern. • Examples of things that are periodic are, days of the week, the months of the year, the seasons, etc.. • In regards to the periodic table of elements, periodic refers to the properties of the elements that repeat with each row (period) of the table.

  6. The modern periodic law states: The chemical and physical properties of the elements are periodic functions of their atomic numbers. • Put in other words, when the elements are arranged in order of increasing atomic number, there is a periodic repetition of their properties.

  7. The periodic table is an arrangement of the elements in order of their atomic numbers so that elements with similar properties fall in the same family (group).

  8. 5-2 Electron Configuration and the Periodic Table • Families 1 & 2 = s-block • Families 3-12= d- block • Families 13-18= p-block • Lanthanide and Actinide series= f-block

  9. Group (Family) 1- Alkali Metals- combine vigorously with many nonmetals very reactive, not found in nature as free elements. (Video)

  10. Group 2-Alkaline-Earth Metals- they are harder, denser, stronger, and have higher melting points than group 1 • not found in nature as free elements.

  11. Copper Iron • Groups 3-12- Transition metals they have metallic properties. Cobalt Chromium

  12. Main-group elements are the p-block and s-block elements. • Group 13- Boron's Family • Group 14- Carbon’s Family • Group 15- Nitrogen's Family • Group 16- Oxygen’s Family • Group 17- Halogens the most reactive nonmetals they form “salts” • Group 18- Noble Gases- Least reactive family. WHY????

  13. F-Block • Lanthanides- “rare earths” all shiny reactive metals. • Actinides- all unstable and radioactive. 1st 4 found naturally all the rest are lab-made. Cerium

  14. 5-3 Electron configuration and Periodic Properties Small • Atomic Radius- is one-half the distance between the nuclei of identical atoms joined in a molecule. BIG

  15. Ionization Energy-the energy required to remove 1 e- from an atom of an element (lose electrons) • Ion- is an atom or group of atoms that have a charge (+ or -).

  16. Electron Affinity- is the energy change that occurs when a electron is acquired by a neutral atom (gain e-).

  17. One electron is removed Positive because e- Ions • Cation- positive ion • Anion- negative ion Ion of Sodium (Na+) 11 protons 10 electrons Atom of Na 11 protons 11 electrons One e- added Atom of Cl 17 protons 17 electrons Ion of Chlorine (Cl-) 17 protons 18 electrons

  18. Valence e- (outer most) the e- available to be lost, gained, or shared in the formation of chemical compounds. • Groups 13-18 • Val e- = group # - 10 ANIONS CATIONS

  19. Electronegativity:  relative tendency of an atom to attract electrons to itself when it is bonded to another atom. *It follows the same trend as electron affinity and ionization energy.  It increases across a period and up a group. *The most active metals (lower left) have lowest electronegativities.  Francium has the lowest electronegativity. *Non-metals (upper right) have the highest electronegativities.  *Flourine has the highest electronegativity of all                other elements.

  20. Work Cited • “Ion Cartoon”. Drawing. Aug. 8, 2006. http://ccmm.fc.ul.pt/vnunes/ensino/quimica2.htm • “Canizzaro”. Photo. Aug. 8, 2006. http://www.unipa.it/~cheminor/ • “Mendeleev”. Photo. Aug. 8, 2006. http://academic.brooklyn.cuny.edu/chem/howell/chem11/octetSet1.htm • “Moseley”. Photo. Aug. 8, 2006. http://home.iitk.ac.in/~sreerup/bso203/Moseley.jpg • “Mendeleev Table and history of the periodic table”. Photo. Aug. 8, 2006. http://www.batesville.k12.in.us/bms/Staff/smithhomepage/webquests/Mendeleevtable.gif • “Periodic Table”. Gif. Aug. 8, 2006. http://imagine.gsfc.nasa.gov/docs/features/topics/instrument_design/periodic.gif

  21. “Blocks of the Periodic table”. Diagram. Aug. 8, 2006. http://boomeria.org/chemlectures/menu.html • “Sodium Pictures”. Picture. Aug. 8, 2006. http://www.theodoregray.com/PeriodicTable/Stories/011.2/ • “Magnesium”. Picture. Aug. 8, 2006. http://www.theodoregray.com/PeriodicTable/Elements/012/index.s7.html • “Transition metal pictures”. Photo. Aug. 8, 2006. http://www.theodoregray.com/PeriodicTable/Elements/TransitionMetals/index.s7.html • “F-Block elements”. Photo. Aug. 8, 2006. http://www.theodoregray.com/PeriodicTable/Elements/095/index.s7.html • “Periodic Table of Elements”. Chart. Aug. 9, 2006. http://users.erols.com/kdennis/periodictable.jpg

  22. “Atomic Radii Chart”. Diagram. Aug. 8, 2006. http://www.colorado.edu/physics/2000/periodic_table/periodic_properties.html • “Electron Affinity Chart”. Diagram. Aug. 8, 2006. http://www.chemistry.ohio-state.edu/~grandinetti/teaching/Chem121/lectures/periodic%20trends/affinity.html • “Electronegativity chart and information”. Diagram. Aug. 9, 2006. http://www.homewood.k12.al.us/~kreaves/Chemicalbonding.htm • “Ionization energy chart”. Diagram. Aug. 9, 2006. http://neon.mems.cmu.edu/27201/ionization-enthalpy-1-c.gif • “Sodium and Chlorine ions”. Aug. 9, 2006. http://www.dgpc.ulaval.ca/bio90192/chap1/ions.htm • Holt, Rinehart and Winston. Modern Chemistry. Harcourt Brace & Company. 1999.

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