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Periodic Table

Learn how the periodic table is arranged and how to key it for different types of matter. Understand the properties and characteristics of elements in each group.

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Periodic Table

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  1. Periodic Table

  2. Aim 1 • To understand how the periodic table got its shape.

  3. Mendeleev • Arranged the Periodic Table according to atomic mass • This resulted in gaps and the table being out of order!

  4. Moseley • Arranged table by atomic number (or # of protons) • How the modern day periodic table is arranged • No more gaps! (we call this an observed regularity)

  5. THE PERIODIC TABLE… • Is made up of Periods and Groups. • PERIODS = HORIZONTAL ROWS (run left to right) • Elements in the same period have the same number of energy levels/shells

  6. practice

  7. Eight is great • OCTET = full VALENCE SHELL (8 e-) • ****except for Hydrogen (1) • Helium (2) • They only need 2 electrons to fill their valence shell

  8. groups • GROUPS = VERTICAL COLUMNS (run up & down) • Elements in the same group have very similar chemical reactivity! This is based on valence electrons

  9. Practice

  10. Crash Course Mendeleev

  11. Aim 2 • To “key” the periodic table in order to get as much information out of it as possible.

  12. The Periodic table can be “KEYED” for many things STP=

  13. solids • Solids (s) – most elements are solids at STP • a. Definite VOLUME • b. Definite SHAPE

  14. liquids • Liquids (l) – only TWO elements at STP (Br & Hg); • a. Definite VOLUME • b. Takes the SHAPE of the container

  15. aqueous • Aqueous (aq) – a STATE of matter in which one substance (a solute) is dissolved in another (a solvent); a solution • ex: NaCl(aq) • Salt (NaCl) is the solute, Water is the solvent

  16. gases • Gases (g) – H, N, O, F, Cl, & all of group 18 (noble gases) • a. No definite VOLUME • b. FILL their container uniformly

  17. Diatomic elements • Elements that are UNSTABLE ALONE in nature • PAIR UP in order to fill their VALENCE SHELLS • Perfect sharing • Contains 2 identical atoms

  18. Draw a lewis structure for 2 fluorine atoms • Put them together: • Use the 7- Up trick or:

  19. Types of Matter: Solid and Liquid • 1. Metals: • make up MOST of table • LEFT of or BELOW “staircase”—except HYDROGEN • all SOLIDS (except Hg(l) • Must have ALL FOUR properties of a metal

  20. Must have ALL FOUR properties of a metal: • 1. MALLEABLE : can be hammered/molded into sheets • 2. DUCTILE: can be drawn/pulled into wire • 3. have LUSTER: are shiny • 4. good CONDUCTORS: allow heat & electricity to flow through them

  21. conductors • Metals are good conductors due to their “sea of mobile valence electrons” • Metals like to lose electrons to become positive ions

  22. nonmetals • RIGHT of or ABOVE staircase • mostly GASES and SOLIDS @ STP—except Br(l) • NOT malleable/ductile; BRITTLE (shatter easily) • LACK luster (DULL) • NON or POOR conductors

  23. Nonmetals • Nonmetals like to gain electrons to become negative ions

  24. 3. Metalloids (semi-metals) • Have TWO properties of a metal • ALONG staircase (between METALS & NONMETALS on • table)—except Al • There are 6 metalloids you have to know!

  25. https://www.youtube.com/watch?v=hszrbXQKR-8 http://www.harcourtschool.com/activity/states_of_matter/

  26. Group 1- ALKALI METALS (FAMILY) •  Easily LOSE their one electron to become +1 ions • EXTREMELY reactive! Never found alone in nature •  Contains the MOST reactive metal: FRANCIUM (Fr) • https://www.youtube.com/watch?v=uixxJtJPVXk • https://www.youtube.com/watch?v=m55kgyApYrY

  27. What about hydrogen? • Not officially part of a group!! • Both a NONMETAL and a GAS • https://www.youtube.com/watch?v=v1TfPDlA1xE

  28. Group 2: ALKALINE EARTH METALS (FAMILY) • LOSE their two electrons to become +2 ions • FAIRLY reactive! Never found alone in nature https://www.youtube.com/watch?v=DFQPnHkQlZM

  29. Groups 3-12: TRANSITION METALS •  Form COLORED IONS in solution. Group 12 is the HEAVY METALS and they don’t form colors.  Tend to be UNPREDICTABLE!They can FORM DIFFERENT #’S OF BONDS

  30.  LEAST reactive group of metals • Nickel and Copper • https://www.youtube.com/watch?v=vwd4qsmUxwM

  31. The Lanthanide/Actinide Series – two rows on bottom of table (detached) • – Elements 58 – 71 & 90 - 103 • Actually belong to the TRANSITION METALS

  32. Groups 13-16: BCNO groups • MISCELLANEOUS groups • Metals, nonmetals, & metalloids found along the staircase (many different properties)

  33. Group 17: HALOGENS (FAMILIY) • https://www.youtube.com/watch?v=J7b2aBKa6-U •  Like to gain 1 electron to become ions with -1 charge •  Form SALTS/ /COMPOUNDS • (a metal and a nonmetal) called HALIDES

  34. Contains the most REACTIVE nonmetal: FLUORINE  All NONMETALS making up the group  Three states of matter found in group

  35. Group 18: NOBLE GASES (FAMILY) • UNREACTIVE or INERT •  Have OCTET .The most STABLE group; exist ALONE in nature •  Exception to the OCTET is He (only has 2 valence e-) • https://www.youtube.com/watch?v=1PSzSTilu_s • ASAP SCIENCE

  36. Practice • Name the two properties of nonmetals that make them unsuitable for use in electrical wiring. • Use the list of elements belwo to answer the questions

  37. Aim 3 • To identify the trends within the shape of the periodic table.

  38. electronegativity • This is the desire for an atom to GAIN ELECTRONS to gain a full octet • Going ACROSS A PERIOD, electronegativity INCREASES

  39. Going DOWN A GROUP, electronegativity DECREASES

  40. NONMETALSGAIN e- to achieve full OCTET!HIGH electronegativity values (seen on table S) Bullies • METALS LOSE e- to achieve full OCTET!LOW electronegativity values (seen on table S) Losers

  41. Values range from 0.0 to 4.0 on Table S in your CRT • Most electronegative element: with a value of • Least electronegative elements: with values of

  42. reactivity • ABILITY or TENDENCY of an element to go through a CHEMICAL change (or REACT with another element) • METALS: (recall: the most reactive metal is FRANCIUM) • Going across a period, reactivity DECREASES • Reason: Metals get more stable, moving further from Francium • Going down a group, reactivity INCREASES • Reason: • Radius is bigger, easier to remove an electron. Moving closer to Francium

  43. NONMETALS: (recall: the most reactive nonmetal is FLUORINE) • Going across a period, reactivity INCREASES (until you get to the NOBLE GASES → unreactive) • Reason: Moving closer to Fluorine, closer to the full octet • Going down a group, reactivity DECREASES • Reason: • Moving farther from Fluorine, increased shielding.

  44. Practice

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