Ionic Bonds and Charge Determination
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Questions and Answers

What type of ion is formed when metals lose electrons?

  • Anion
  • Radical
  • Molecule
  • Cation (correct)
  • Which of the following represents a common charge for Group 16 elements?

  • -2 (correct)
  • -1
  • +2
  • +3
  • What is the relationship between ionic radii and lattice energy?

  • Ionic radii have no effect on lattice energy.
  • Smaller ionic radii result in a stronger attraction between ions. (correct)
  • Larger ionic radii increase lattice energy due to expanded distance.
  • Larger ionic radii lead to more negative lattice energy.
  • What does lattice energy depend on?

    <p>The charges of the ions and the distance between them</p> Signup and view all the answers

    What is a characteristic of Group 14 elements regarding electron loss or gain?

    <p>They can lose or gain 4 electrons but often form covalent bonds.</p> Signup and view all the answers

    Which ion has a greater positive charge than sodium (Na)?

    <p>Magnesium (Mg)</p> Signup and view all the answers

    Which of the following represents the correct formula for calculating lattice energy?

    <p>U ∝ Q1 × Q2 / R</p> Signup and view all the answers

    What is the typical charge for chlorine ions?

    <p>-1</p> Signup and view all the answers

    What happens to the size of cations compared to their parent neutral atoms?

    <p>Cations are smaller than their parent atoms.</p> Signup and view all the answers

    Which ion has the largest ionic radius among the following?

    <p>Cl−</p> Signup and view all the answers

    If an ion has a charge of -2, how does its ionic radius compare to a -1 charged ion?

    <p>The -2 ion is larger than the -1 ion.</p> Signup and view all the answers

    What is the total distance $R$ between Na+ and Cl− ions in NaCl?

    <p>283 pm</p> Signup and view all the answers

    How does the ionic radius of Mg2+ compare to that of Na+?

    <p>Mg2+ is smaller than Na+.</p> Signup and view all the answers

    Which pair of ions would have the smallest total distance $R$?

    <p>Mg2+ and O2−</p> Signup and view all the answers

    In lattice energy calculations, what factor causes energy to increase?

    <p>The decrease in ionic radius.</p> Signup and view all the answers

    Which statement about ionic radii is correct?

    <p>The more positive the charge of cations, the smaller the ionic radius.</p> Signup and view all the answers

    Study Notes

    Ionic Bonds and Charge Determination

    • Ions are atoms or groups of atoms with a net positive or negative charge.
    • Cations are positively charged ions formed when metals lose electrons. The charge equals the number of electrons lost.
      • Example: Sodium (Na, Group 1) forms Na+ with a +1 charge.
      • Example: Magnesium (Mg, Group 2) forms Mg2+ with a +2 charge.
    • Anions are negatively charged ions formed when nonmetals gain electrons. The charge equals the number of electrons gained.
      • Example: Chlorine (Cl, Group 17) forms Cl with a −1 charge.
      • Example: Oxygen (O, Group 16) forms O2− with a −2 charge.
    • Common ionic charges by group:
      • Group 1: +1
      • Group 2: +2
      • Group 13: +3
      • Group 16: −2
      • Group 17: −1
    • Group 14 (Carbon Group) is a special case: can lose 4 electrons forming +4 ion or gain 4 forming −4 ions, but typically forms covalent bonds instead.

    Lattice Energy

    • Lattice energy is the energy needed to separate one mole of an ionic solid into its gaseous ions.
    • Lattice energy is proportional to (charge of ion 1 * charge of ion 2) / (distance between ions).
    • Higher charges result in stronger attractions and higher (more negative) lattice energy.
    • Smaller ion radii lead to shorter distances and higher lattice energy.
    • Factors Affecting Lattice Energy:
      • Higher ion charges = Higher lattice energy.
      • Smaller ion sizes = Higher lattice energy.

    Determining Ionic Radii

    • Ionic radius is the size of an ion in a crystal lattice, often different from the atomic radius.
    • Cations are smaller than their corresponding neutral atoms, losing electrons.
    • Anions are larger than their corresponding neutral atoms, gaining electrons.
    • Ionic radius trends:
      • Higher positive charge = Smaller ionic radius.
      • Higher negative charge = Larger ionic radius.
    • Example values:
      • Na+: 102 pm
      • Mg2+: 72 pm
      • Cl: 181 pm
      • F: 133 pm

    Calculating Lattice Energy

    • Find charges on ions
    • Utilize ionic radii to determine the distance between the ions
    • Use the formula to calculate the lattice energy.

    Example Problems

    • The examples demonstrate calculating proportional lattice energy using ion charges and ionic radii.
      • Example Problems demonstrate the relationships between the quantities listed.

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    Quiz Team

    Description

    This quiz covers the defining characteristics of ionic bonds, including the formation of cations and anions, and the concept of lattice energy. It will also explore common ionic charges across different groups in the periodic table. Test your understanding of how ions are formed and their associated charges.

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