Ionic Bonding Overview
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Questions and Answers

What is the primary reason that metals form cations during ionic bonding?

  • They have a tendency to share electrons with non-metals.
  • They lose electrons to achieve a stable electron configuration. (correct)
  • They combine with non-metals without changing their electron count.
  • They gain electrons to achieve stability.

    • Which of the following ions is isoelectronic with the noble gas Neon?

  • Cl⁻
  • F⁻ (correct)
  • Na⁺ (correct)
  • O²⁻

    • Which property is characteristic of ionic compounds?

  • High melting and boiling points. (correct)
  • Soluble in organic solvents.
  • Non-conductive in aqueous solution.
  • Low boiling points.

    • What happens to the electron configuration of an atom when it becomes an ion?

    <p>It loses or gains electrons to mimic that of a noble gas.</p> Signup and view all the answers

    Which of the following correctly identifies a common compound ion?

    <p>Hydroxide (OH⁻)</p> Signup and view all the answers

    What occurs during the formation of positive ions (cations)?

    <p>Metal atoms lose electrons.</p> Signup and view all the answers

    What is the charge of a sodium ion (Na⁺) after it loses one electron?

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

    Which of the following is true about ionic compounds' melting and boiling points?

    <p>They have high melting points due to strong forces.</p> Signup and view all the answers

    What happens when ionic compounds are dissolved in water?

    <p>Ions become free to move.</p> Signup and view all the answers

    Which step is NOT part of writing ionic formulas?

    <p>Indicate subscript 1’s.</p> Signup and view all the answers

    In an ionic lattice structure like sodium chloride (NaCl), how many Cl⁻ ions surround each Na⁺ ion?

    <p>6</p> Signup and view all the answers

    What is the primary reason that solid ionic compounds do not conduct electricity?

    <p>Ions are fixed in place.</p> Signup and view all the answers

    What type of ions are formed when non-metal atoms gain electrons?

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

    Study Notes

    Ionic Bonding Overview

    • Ionic bonding is an electrostatic attraction between oppositely charged ions.
    • This attraction forms when electrons are transferred from one atom to another.
    • The strong electrostatic force holds the ionic lattice structure.

    Ion Formation

    • Cations (Positive Ions): Metal atoms lose electrons, becoming positively charged.
    • Anions (Negative Ions): Non-metal atoms gain electrons, becoming negatively charged.
    • Losing an electron increases the number of positively charged protons, creating a positive ion.
    • Gaining an electron increases the number of negatively charged electrons, creating a negative ion.
      • Examples: Sodium (Na) loses one electron to form Na⁺; Chlorine (Cl) gains one electron to form Cl⁻.

    Writing Ionic Formulas

    • Write the symbols for the elements.
    • Note the valency (electrons gained/lost) above each element.
    • Cross-over the valencies as subscripts (ignore any '1's).
    • If valencies are the same, they cancel each other out (like in NaCl).
    • Roman numerals indicate the charge on an ion when needed (e.g., Fe²⁺).
    • Use brackets for multiple compound ions (e.g., CuSO₄).

    Ionic Lattice Structure

    • Ionic compounds form a giant 3-dimensional repeating structure.
    • Ions are arranged in a continuous 3D lattice.
    • Example: In sodium chloride (NaCl), each Na⁺ ion is surrounded by 6 Cl⁻ ions, and vice versa.

    Ionic Compound Properties

    • High Melting/Boiling Points: Strong electrostatic forces between ions require a lot of energy to overcome.
    • Conductivity: Solid ionic compounds don't conduct electricity (fixed ions). Molten or dissolved ionic compounds conduct electricity (free ions moving).
    • Solubility: Ionic compounds are often soluble in water.

    Ions and Isoelectronic Noble Gases

    • Ions achieve stable electron configurations (full outer shells) by gaining or losing electrons.
    • Isoelectronic ions have the same electron configuration as noble gases.
    • Examples: Na⁺ is isoelectronic with Ne; F⁻ is isoelectronic with Ne.

    Common Polyatomic Ions

    • Chloride (Cl⁻)
    • Oxide (O²⁻)
    • Sulphate (SO₄²⁻)
    • Nitrate (NO₃⁻)
    • Iodide (I⁻)

    Metal-Nonmetal Bonding

    • Ionic bonds form between metals and non-metals due to electron transfer.
    • Metals lose electrons to become cations.
    • Non-metals gain electrons to become anions.
    • The resulting ions achieve a stable electron configuration (isoelectronic with noble gases).

    Summary

    • Ionic bonding involves electron transfer creating oppositely charged ions.
    • The ions form a repeating 3-dimensional lattice.
    • Ionic compounds generally have high melting/boiling points and are soluble in water. They conduct when molten or dissolved.
    • Ionic formulas represent the ratio of ions in a compound.

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    Description

    Explore the fundamentals of ionic bonding in this quiz. Learn how cations and anions form through electron transfer and how to write ionic formulas correctly. Test your understanding of this essential chemistry topic.

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