Atomic Radii and Periodic Trends
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Questions and Answers

What happens to the ionic radius of sodium when it forms a cation?

  • It decreases due to loss of an energy level. (correct)
  • It increases significantly.
  • It becomes equal to the atomic radius.
  • It remains unchanged.

    • How does the ionic radius of fluoride compare to its atomic radius?

  • It is smaller due to a greater nuclear charge.
  • It becomes one-third larger than the atomic radius.
  • It is larger because it gains an electron. (correct)
  • It does not change.

    • Why does the fluoride ion have a larger radius than the fluorine atom?

  • It has gained additional protons.
  • The loss of electrons reduces its size.
  • Electron repulsion increases the cloud size. (correct)
  • It has fewer energy levels than the atom.

    • What is the atomic radii a measure of?

    <p>The distance from the nucleus to the outermost electron</p> Signup and view all the answers

    What signifies the change in atomic radius for a sodium atom when it becomes a cation?

    <p>Decrease in size due to loss of an electron.</p> Signup and view all the answers

    How does the atomic radii change when moving down a group in the periodic table?

    <p>The atomic radii increase due to additional energy levels</p> Signup and view all the answers

    Which statement correctly describes the ionic transformation of sodium and fluorine?

    <p>Sodium loses an electron, reducing its ionic radius.</p> Signup and view all the answers

    What happens to atomic radii as you move from left to right across a period?

    <p>Atomic radii decrease because electrons are pulled closer to the nucleus</p> Signup and view all the answers

    Which element has the smallest atomic radii?

    <p>He</p> Signup and view all the answers

    Which of the following elements has the largest atomic radii?

    <p>Fr</p> Signup and view all the answers

    Study Notes

    Atomic Radii

    • Defined as the distance from the nucleus center to the outermost electron.
    • Increases down a group/family due to the addition of extra energy levels (electron shells).
    • Decreases from left to right across a period as increased proton count leads to stronger coulombic attraction, pulling electrons closer to the nucleus.

    Element Characteristics

    • Largest atomic radii: Francium (Fr) - Colored RED on the Periodic Table
    • Smallest atomic radii: Helium (He) - Colored ORANGE on the Periodic Table

    Order of Atomic Radii

    • Increasing Order:

      • Calcium (Ca), Strontium (Sr), Barium (Ba)
      • Nickel (Ni), Cobalt (Co), Iron (Fe)

    • Decreasing Order:

      • Lithium (Li), Sodium (Na)
      • Neon (Ne), Fluorine (F), Oxygen (O)

    Ionic Radii

    • Sodium (Na) Atomic Structure:

      • Sodium atom: Central "Na" with one ring of electrons.
      • Sodium ion (Na+): Central "Na+" with one ring of electrons; the cation has a smaller radius due to the loss of an electron.

    • Fluorine (F) Atomic Structure:

      • Fluorine atom: Central "F" with two rings of electrons.
      • Fluoride ion (F-): Central "F-" with two rings of electrons; the anion has a larger radius because it gains an electron, leading to lower nuclear charge and increased electron repulsion.

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    Description

    Explore the concept of atomic radii and how it varies across periods and groups in the periodic table. This quiz focuses on understanding the factors influencing atomic size and the trends observed in the arrangement of elements.

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