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Exploring Periodic Trends in Atomic Properties: Setup & Analysis

Understand the setup of the periodic table, trends in atomic radius, ionization energy, electron affinity, and electronegativity. Learn how these factors change across periods and groups in elements.

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Exploring Periodic Trends in Atomic Properties: Setup & Analysis

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  1. Periodic Table Set-up

  2. Periodic Trends Atomic Radius: 1/2 distance between 2 nuclei of the same element. Group Trend: Increases Why: e-are being added to new energy levels further away, electron shielding occurs, so the nucleus can not pull electrons in a close. Period Trend: Decreases → Why: e-are being added to the same energy level. As the nucleus becomes stronger, the electrons are drawn in closer.

  3. Ionization Energy: The energy required to remove an e-. Group Trend: Decrease → Why: e-are further away (shielded) and easier to take away. Period Trend: Increase → Why: e-are closer to nucleus + harder to remove. Atoms are closer to having a complete valence shell and want to gain not lose e-.

  4. Electron Affinity : ability to attract e- Group Trend: Decreases Why : Electrons are harder to bring in further away with the nucleus pulling less. Period Trend: Increases → due to a stronger nucleus Why: e- are easier to bring in Atoms want to complete their valence shell. Electronegativity: ability to attract e-in a bond → scale of O-4 F=4.0

  5. Ion Size cations (+) : lose valence e' Effect on Radius: decrease due to loss of energy level. anions (+): gain electrons increases due to addition Effect on Radius : l , of e- to the same energy level and not changing the strength of the nucleus.

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