Here's a breakdown:
* Covalently Bonded: The atoms within the compound ion are held together by shared electrons (covalent bonds), similar to how atoms are bonded in molecules.
* Net Electrical Charge: The entire group of atoms has a positive or negative charge due to an imbalance in the number of protons and electrons.
Examples of Compound Ions:
* Nitrate (NO₃⁻): A nitrogen atom covalently bonded to three oxygen atoms, with a net charge of -1.
* Ammonium (NH₄⁺): A nitrogen atom covalently bonded to four hydrogen atoms, with a net charge of +1.
* Carbonate (CO₃²⁻): A carbon atom covalently bonded to three oxygen atoms, with a net charge of -2.
* Phosphate (PO₄³⁻): A phosphorus atom covalently bonded to four oxygen atoms, with a net charge of -3.
Key Points:
* Compound ions are important building blocks in many chemical compounds.
* They are named according to their specific atoms and charge.
* The charge on a compound ion is determined by the number of electrons gained or lost.
* Compound ions often form ionic bonds with other ions to create ionic compounds.
Note: Compound ions are different from simple ions, which consist of a single atom with a charge (like Na⁺ or Cl⁻).
