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 (D)</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. (A)</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 (B)</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. (B)</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 (C)</p> Signup and view all the answers

Which element has the smallest atomic radii?

<p>He (B)</p> Signup and view all the answers

Which of the following elements has the largest atomic radii?

<p>Fr (B)</p> Signup and view all the answers

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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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