2.29 Apply Coulomb’s law to explain periodic trends in atomic radii and ionization energies.

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1

How does Coulomb's law explain periodic trends in atomic radii and ionization energies?

  • Coulomb’s Law describes the force between two charged particles

  • Where F is the force, q1 and q2 are the charges of the particles, and r is the distance between them.

  • Attractive force between the positively charged nucleus and negatively charged electrons is explained by Coulomb’s law.

<ul><li><p>Coulomb’s Law describes the force between two charged particles</p></li><li><p>Where F is the force, q1 and q2 are the charges of the particles, and r is the distance between them. </p></li></ul><ul><li><p><strong>Attractive force</strong> between the positively charged nucleus and negatively charged electrons is explained by Coulomb’s law.</p></li></ul><p></p>
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2

How does Coulomb’s law explain trends in atomic radii across and down the periodic table?

  • Across a Period (→):

    • As protons are added to the nucleus, the nuclear charge (positive charge) increases, strengthening the attractive force between the nucleus and electrons.

    • Electrons stay in the same energy level, and as a result, the atomic radius decreases due to stronger attraction.

  • Down a Group (↓):

    • Electrons are added to higher energy levels, farther from the nucleus, increasing the distance (rrr) in Coulomb’s law.

    • Even though nuclear charge increases, the effect of shielding from inner electrons reduces the overall attractive force, leading to an increase in atomic radius.

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3

How does Coulomb’s law explain trends in ionization energy across and down the periodic table?

  • Across a Period (→):

    • As nuclear charge increases, electrons are more tightly bound to the nucleus due to the stronger attractive force, making it harder to remove an electron.

    • This leads to an increase in ionization energy.

  • Down a Group (↓):

    • Electrons are farther from the nucleus (larger rrr), and shielding by inner electrons reduces the nuclear attraction on the outermost electron.

    • As a result, it is easier to remove the outer electron, leading to a decrease in ionization energy.

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