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05 CTR ch06 7/9/04 3:27 PM Page 151 Name Date Class QUICK LAB: Periodic Trends in Ionic Radii Laboratory Recordsheet Use with Section 6.3 PURPOSE Make a graph of ionic radius versus atomic number.

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  3. Fill in the date of completion in the appropriate date field to document when the lab is performed.
  4. Input your class information in the class field, allowing for organized record-keeping.
  5. Refer to Figure 6.19 to plot ionic radius versus atomic number on the provided graph paper. Ensure to label your axes clearly, with ionic radius on the y-axis and atomic number on the x-axis.
  6. Complete the analyses and conclusions section by addressing each question thoroughly and providing clear explanations.
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The size of an element's ionic radius follows a predictable trend on the periodic table. As you move down a column or group, the ionic radius increases. This is because each row adds a new electron shell. Ionic radius decreases moving from left to right across a row or period.

Major trends are electronegativity, ionization energy, electron affinity, atomic radius, and metallic character. The existence of these trends is due to the similarity in atomic structure of the elements in their group families or periods and because of the periodic nature of elements.

Ionic radii increases down a group. In a group, all the ions have the same charge as they have the same valency (that is, the same number of valence electrons on the highest energy level sub-orbital). Therefore, ionic radii increase down a group as more shells are added (per period).

Major periodic trends include: electronegativity, ionization energy, electron affinity, atomic radius, melting point, and metallic character. Periodic trends, arising from the arrangement of the periodic table, provide chemists with an invaluable tool to quickly predict an element's properties.

Purpose: To explore the reactivity trends of metals in groups and periods of the periodic table.

Ionic radii follow the same vertical trend as atomic radii; that is, for ions with the same charge, the ionic radius increases going down a column. The reason is the same as for atomic radii: shielding by filled inner shells produces little change in the effective nuclear charge felt by the outermost electrons.

From top to bottom down a group, electronegativity decreases. This is because atomic number increases down a group, and thus there is an increased distance between the valence electrons and nucleus, or a greater atomic radius. Important exceptions of the above rules include the noble gases, lanthanides, and actinides.

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