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TOPIC 3 PERIODICITY

TOPIC 3 PERIODICITY. 3.1 PERIODIC TABLE. The arrangement of elements in the periodic table helps to predict their electron configuration. NATURE OF SCIENCE (1.9)

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TOPIC 3 PERIODICITY

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  1. TOPIC 3PERIODICITY 3.1 PERIODIC TABLE

  2. The arrangement of elements in the periodic table helps to predict their electron configuration. NATURE OF SCIENCE (1.9) Obtain evidence for scientific theories by making and testing predictions based on them – scientists organize subjects based on structure and function; the periodic table is a key example of this. Early models of the periodic table from Mendeleev, and later Moseley, allowed for the prediction of properties of elements that had not yet been discovered. ESSENTIAL IDEA

  3. The development of the periodic table took many years and involved scientists from different countries building upon the foundations of each other’s work and ideas. INTERNATIONAL-MINDEDNESS

  4. What role did inductive and deductive reasoning play in the development of the periodic table? What role does inductive and deductive reasoning have in science in general? THEORY OF KNOWLEDGE

  5. The elements on the Periodic Table are arranged in order of increasing atomic number which is the number of protons in the nucleus. • There are over 110 elements recognized by the IUPAC and the search for elements that exist in nature is over. • The only way to extend the Periodic Table is to make elements artificially. THE PERIODIC TABLE

  6. The Periodic Table was first proposed in 1869 by the Russian chemist Dmitri Mendeleyev. He grouped the known elements into families, leaving gaps corresponding to elements that should exist but had not yet been discovered. Chemistry is not the study of a random collection of elements, but of the trends and patterns in their chemical and physical properties.

  7. The IB data booklet Periodic Table labels the groups 1 to 18. • The numbers 1A to 8A on the classroom periodic table are known as the representative or main group elements. • The gap between groups 2A and 3A (columns 3-12) is filled by the transition elements. • Be familiar with the location of the lanthanides and actinides at the bottom of the Periodic Table.

  8. The group numbering scheme from group 1 to group 18, as recommended by IUPAC, should be used. GUIDANCE

  9. The periodic table is arranged into four blocks associated with the four sub-levels – s, p, d, and f. UNDERSTANDING/KEY IDEA3.1.A

  10. http://www.wyzant.com/resources/lessons/science/chemistry/periodic-tablehttp://www.wyzant.com/resources/lessons/science/chemistry/periodic-table

  11. The periodic table consists of groups (vertical columns) and periods (horizontal rows). UNDERSTANDING/KEY IDEA3.1.B

  12. The periodic number (n) is the outer energy level that is occupied by electrons. UNDERSTANDING/KEY IDEA3.1.C

  13. The rows on the Periodic Table are called periods. • The period number (n) is the outermost energy level. • The columns are called groups. • The group number of the representative elements 1A – 8A give the number of valence electrons.

  14. The number of the principal energy level and the number of the valence electrons in an atom can be deduced from its position on the periodic table. UNDERSTANDING/KEY IDEA3.1.D

  15. The row tells you the energy level. • The number of electrons in the outer shell tells what Group or column to which the element belongs. • You may be given an element and asked how many outer shell electrons exist. • This is simply found by looking at the Group number (We have always referred to it as the “pink” number on our classroom Periodic Table.)

  16. The periodic table shows the positions of metals, non-metals and metalloids. UNDERSTANDING/KEY IDEA3.1.E

  17. http://2012books.lardbucket.org/books/introduction-to-chemistry-general-organic-and-biological/s05-07-the-periodic-table.htmlhttp://2012books.lardbucket.org/books/introduction-to-chemistry-general-organic-and-biological/s05-07-the-periodic-table.html

  18. Metals • Good conductors of heat and electricity • Malleable – can be beaten into thin sheets • Ductile – can be drawn into wires • Shiny or have luster • Tend to lose electrons in chemical reactions • Non-metals • Poor conductors of heat and electricity • Tend to gain electrons in chemical reactions • Can be solid, liquid or gas • Metalloids • Have both metallic and non-metallic properties

  19. The terms alkali metals, halogens, noble gases, transition metals, lanthanides and actinides should be known. GUIDANCE

  20. http://2012books.lardbucket.org/books/introduction-to-chemistry-general-organic-and-biological/s05-07-the-periodic-table.htmlhttp://2012books.lardbucket.org/books/introduction-to-chemistry-general-organic-and-biological/s05-07-the-periodic-table.html

  21. Be able to deduce the electron configuration of an atom from the element’s position on the periodic table and vice versa. APPLICATION/SKILLS

  22. Classroom practice.

  23. International Baccalaureate Organization. Chemistry Guide, First assessment 2016. Updated 2015. Brown, Catrin, and Mike Ford. Higher Level Chemistry. 2nd ed. N.p.: Pearson Baccalaureate, 2014. Print. Most of the information found in this power point comes directly from this textbook. The power point has been made to directly complement the Higher Level Chemistry textbook by Catrin and Brown and is used for direct instructional purposes only. Citations

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