Overview of Metal and Non-Metal Ions
Key Learning Points:
- Understand the charges of metal and non-metal ions:
- Metal ions are generally positive.
- Most non-metal ions are negative.
- Relate ion charges to groups in the periodic table.
Introduction to Ionic Compounds
- Metals are located on the left side of the periodic table.
- Non-metals are found on the right side.
- Ionic compounds form when metals react with non-metals.
Metal Ions
- Positive Charge:
- Examples include Na⁺, Mg²⁺, Al³⁺.
- Charge and Group Relationship:
- Sodium (Na) is in group 1, forms 1+ ions.
- Magnesium (Mg) is in group 2, forms 2+ ions.
- Aluminium (Al) is in group 3, forms 3+ ions.
- Additional Examples:
- Lithium (Li) and Potassium (K) are in group 1, form 1+ ions.
- Beryllium (Be) and Calcium (Ca) are in group 2, form 2+ ions.
- Gallium (Ga) and Indium (In) are in group 3, form 3+ ions.
- Exceptions:
- Transition metals can form various ions:
- Iron (Fe) forms 2+ (Iron II) and 3+ (Iron III) ions.
- Copper (Cu) forms 1+ (Copper I) and 2+ (Copper II) ions.
Non-Metal Ions
- Negative Charge:
- Examples include oxide ion O²⁻ and fluoride ion F⁻.
- Charge and Group Relationship:
- Oxygen (O) is in group 6, forms 2⁻ ions.
- Sulfur (S) also in group 6, forms sulfide ion S²⁻.
- Fluorine (F) in group 7, forms 1⁻ ions.
- Chlorine (Cl) and Bromine (Br) in group 7, form 1⁻ ions.
- Compound Non-Metal Ions:
- Some consist of multiple non-metal atoms combined.
- Positive Non-Metal Ions:
- Hydrogen ion H⁺ and Ammonium ion NH₄⁺.
Practice with Ionic Compounds
- Example compounds:
- Sodium sulfate Na₂SO₄.
- Calcium hydroxide Ca(OH)₂.
- Next Steps:
- Learn how to work out formulas of such compounds.
Summary
- You should now understand:
- Metal ions are typically positive.
- Non-metal ions are typically negative.
- How to associate ion charges with their group in the periodic table.
This foundational knowledge is crucial for developing skills in determining the formulas of ionic compounds, to be explored in the next lesson.