Free Science Lessons: Ionic Bonding

Overview

• Focus on how electrons are transferred during ionic bonding.
• Emphasis on reactions between Group 2 metals and Group 6 non-metals.
• Goal: Be able to draw Dot and Cross diagrams for ionic bonding.

Key Concepts

• Ionic Bonding: Occurs when a metal reacts with a non-metal.
• Group 1 metals such as Lithium and Group 7 non-metals like Fluorine were discussed in previous lessons.
• Outcome of Ionic Bonding: Formation of ions with a stable electronic structure similar to noble gases.

Ionic Bonding between Group 2 Metals and Group 6 Non-Metals

• Example Reaction: Magnesium (Group 2) and Oxygen (Group 6).
  • Magnesium Atom: 12 protons, 12 electrons; no overall charge initially.
  • Oxygen Atom: 8 protons, 8 electrons; no overall charge initially.
  • Electron Configuration:
    • Magnesium: 2 electrons in the outer energy level.
    • Oxygen: 6 electrons in the outer energy level.
  • Ionic Reaction:
    • Magnesium loses 2 electrons → Becomes a magnesium ion (Mg²⁺) with a 2+ charge.
    • Oxygen gains 2 electrons → Becomes an oxide ion (O²⁻) with a 2- charge.
  • Both ions achieve a stable electronic structure of a noble gas.

Dot and Cross Diagrams

• Purpose: Show only outer energy levels involved in reactions.
• Process: Illustrate electron transfer between atoms.
  • Magnesium’s electrons move to Oxygen, forming Mg²⁺ and O²⁻.

Recap of Ionic Bonding

• Group 2 metals lose two electrons, forming 2+ ions.
• Group 6 non-metals gain two electrons, forming 2- ions.
• Both ions reach a stable electronic structure.

Other Examples

• Lithium (Group 1) and Oxygen (Group 6):
  • Lithium has 1 electron in the outer shell; Oxygen has 6.
  • Two lithium atoms each lose one electron, transferring to one oxygen atom.
• Calcium (Group 2) and Fluorine (Group 7):
  • Calcium loses its two outer electrons.
  • Two Fluorine atoms each gain one electron.
  • Both achieve a full outer energy level.

Additional Resources

• Vision workbook available for more questions and practice on ionic bonding.

[Link to the vision workbook provided in the lecture]