Periodic Table  of Elements<br />Chapter 6 Notes<br />
Modern Periodic Table<br />Designed by Demitri Mendeleev based on atomic mass (1869)<br />Modified by Henry Moseley based ...
Classifying Elements<br />
Properties of Metals & <br />Nonmetals<br />Nonmetals<br /><ul><li>Poor conductors
Brittle
Most are gases at room temp
Solids (sulfur & phosphorus) are dull</li></ul>Metals<br /><ul><li>Conduct heat & electricity
Malleable
Solid at room temp (except Hg)
High luster/sheen</li></ul>Gold<br />Bromine Gas<br />
sToP & tHinK – metal or nonmetal<br />1.  A gaseous substance that partially conducts electricity.<br />2.  Solid that is ...
Elements in the same group have similar properties!  (Periodic Law)<br />Group 1 - Alkali Metals<br />Group 2 - Alkaline E...
State the name of the group / family for each:<br />Magnesium<br />Bromine<br />Argon<br />Has 8 valence electrons<br />Gr...
A groups - representative elements (s and p blocks, except noble gases)<br />Display varied properties by column<br />B gr...
Atomic Radius<br />
Let’s Look @ Atomic Radius<br />Decreases across the period (row/horizontal)<br />Increases down the group (column/vertica...
SToP & THinK<br />1.  Why does atomic radius decrease as you move from left to right on the PT?<br />2.  Why does atomic r...
 Anions (- charged) larger than <br />neutral atom of the same element<br />Anions Ionic Radius<br />
CationsIonic Radius<br />Cation(+ charged) smaller than <br />            neutral atom of the same element<br />
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Periodic table trends power point presentation

  1. 1. Periodic Table of Elements<br />Chapter 6 Notes<br />
  2. 2. Modern Periodic Table<br />Designed by Demitri Mendeleev based on atomic mass (1869)<br />Modified by Henry Moseley based on atomic number (1926)<br />
  3. 3. Classifying Elements<br />
  4. 4. Properties of Metals & <br />Nonmetals<br />Nonmetals<br /><ul><li>Poor conductors
  5. 5. Brittle
  6. 6. Most are gases at room temp
  7. 7. Solids (sulfur & phosphorus) are dull</li></ul>Metals<br /><ul><li>Conduct heat & electricity
  8. 8. Malleable
  9. 9. Solid at room temp (except Hg)
  10. 10. High luster/sheen</li></ul>Gold<br />Bromine Gas<br />
  11. 11. sToP & tHinK – metal or nonmetal<br />1. A gaseous substance that partially conducts electricity.<br />2. Solid that is malleable and shiny.<br />3. Solid that is brittle and dull color.<br />4. Solid that conducts electrical current and has high luster.<br />5. Has 7 valence electrons<br />6. Found on the right of the ‘staircase’<br />7. Has 1 valence electron<br />8. d and f block elements<br />
  12. 12. Elements in the same group have similar properties! (Periodic Law)<br />Group 1 - Alkali Metals<br />Group 2 - Alkaline Earth Metals<br />d block - Transition Metals<br />f block - Inner Transition Metals<br />Group 7 - Halogens<br />Group 8 - Noble Gases<br /> Reactivity increases from top to bottom <br /> for 1A, 2A<br /> Reactivity decreases from top to bottom<br />for 7A<br />Classifying Elements – Let’s Look at the Periodic Chart<br />
  13. 13. State the name of the group / family for each:<br />Magnesium<br />Bromine<br />Argon<br />Has 8 valence electrons<br />Group 1A<br />Copper<br />Tend to lose one electron to be more stable (remember octet rule).<br />sToP & tHinK<br />
  14. 14. A groups - representative elements (s and p blocks, except noble gases)<br />Display varied properties by column<br />B groups - transition elements & inner transition elements (d and f blocks)<br />Fairly similar properties<br />A Groups & B Groups<br />
  15. 15. Atomic Radius<br />
  16. 16. Let’s Look @ Atomic Radius<br />Decreases across the period (row/horizontal)<br />Increases down the group (column/vertical)<br />WHY?!? – 2 Reasons<br />1. Each added proton increases the positive nuclear charge… as electrons are added to principal energy levels the level gets smaller.<br />2. Electrons added to a new principal energy level are ‘shielded’ from the positive nucleus by the electrons in lower levels.<br />
  17. 17. SToP & THinK<br />1. Why does atomic radius decrease as you move from left to right on the PT?<br />2. Why does atomic radius increase as you move down each group on the PT?<br />
  18. 18. Anions (- charged) larger than <br />neutral atom of the same element<br />Anions Ionic Radius<br />
  19. 19. CationsIonic Radius<br />Cation(+ charged) smaller than <br /> neutral atom of the same element<br />
  20. 20. SToP & THiNk<br />1. Which has a larger radius for each: <br />K or K+? <br />S or S2-?<br />2. Explain why.<br />
  21. 21. Ionization Energy(IE)Trends<br />The amount of energy required to remove an electron from an atom.<br />Increases up the periodic chart and from left to right.<br />
  22. 22. Ionization Energy(IE)Trends<br />(IE) Increases Up the Periodic Chart.<br />(IE) Increases from Left to Right<br />
  23. 23. ElectronegativityTrends<br />The ability of an atom to pull electrons in a chemical bond.<br />Due to pull from protons and how close electrons are to nucleus.<br />More electronegative = stronger pull on electrons<br /> Same pattern as ionization energy (IE)<br />
  24. 24.
  25. 25. SToP & THiNk<br />Which is more electronegative?<br />Ca or Cl<br />P or O<br />In your own words, explain why ionization energy and electronegativity follow the same trend pattern on the periodic table.<br />
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