Chapter 4.3<br />Trends in the Periodic Table<br />
Objective 1:<br />Describe periodic trends in ionization energy, atomic radius, electronegativity, and ionic size; and rel...
Atomic Radii<br />Defined as one-half the distance between the nuclei of identical atoms that are bonded together<br />Per...
Increase down a group</li></li></ul><li>Atomic Radii<br />
Ionization Energy<br />Defined as energy required to remove one electron from a neutral atom of an element (IE)<br />A + e...
Generally decrease down a group</li></li></ul><li>Ionic radii<br />Cation – positive ion<br />Formed by loss of one or mor...
Formed by gain of one or more electrons</li></ul>Ionic Radii<br />
Valence Electrons<br />Defined as the electrons available to be lost, gained, or shared in the formation of chemical compo...
Electronegativity<br />Defined as the measure of the ability of an atom in a chemical compound to attract electrons<br />W...
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Applied Chapter 4.3 :Trends in the Periodic Table

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Applied Chapter 4.3 :Trends in the Periodic Table

  1. 1. Chapter 4.3<br />Trends in the Periodic Table<br />
  2. 2. Objective 1:<br />Describe periodic trends in ionization energy, atomic radius, electronegativity, and ionic size; and relate and relate them to atomic structures of the elements.<br />Trend : predictable change in a particular direction<br />Trends in reactivitydown a group of Alkali Metals<br />
  3. 3. Atomic Radii<br />Defined as one-half the distance between the nuclei of identical atoms that are bonded together<br />Period trends<br />Decrease from left to right<br /><ul><li>Group trends
  4. 4. Increase down a group</li></li></ul><li>Atomic Radii<br />
  5. 5. Ionization Energy<br />Defined as energy required to remove one electron from a neutral atom of an element (IE)<br />A + energy A+ + e-<br /><ul><li>Ion – atom or group of bonded atoms that has a positive or negative charge.</li></li></ul><li>Ionization Energy<br />Period trends<br />Generally increase across a period<br /><ul><li>Group trends
  6. 6. Generally decrease down a group</li></li></ul><li>Ionic radii<br />Cation – positive ion<br />Formed by loss of one or more electrons<br /><ul><li>Anion– negative ion
  7. 7. Formed by gain of one or more electrons</li></ul>Ionic Radii<br />
  8. 8. Valence Electrons<br />Defined as the electrons available to be lost, gained, or shared in the formation of chemical compounds<br />Valence electron<br />Sodium atom<br />Chlorine atom<br />
  9. 9. Electronegativity<br />Defined as the measure of the ability of an atom in a chemical compound to attract electrons<br />Want to gain electrons!!<br />Noble gases have very low electronegativity<br />Alkali metals are low as well<br />Halogens have the highest<br />Electronegativity<br /><ul><li>Period trends
  10. 10. Tend to increase across a period
  11. 11. Group trends
  12. 12. Tend to decrease down a group</li>

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