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Explain polyatomic ions and covalent bonds, using the provided notes and examples.

Chemistry

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Let's break down the notes you have there, with reasons and examples.

1. Polyatomic Ions

  • Notes: A polyatomic ion is a group of two or more atoms covalently bonded together that carries an overall positive or negative charge. These groups act as a single unit in chemical reactions.
  • Reasons: Atoms within the ion share electrons, but the overall group has an imbalance of protons and electrons, giving it a net charge. Their names often follow patterns:
    • Ions with more oxygen atoms typically end in -ate (e.g., NO3−\text{NO}_3^- nitrate).
    • Ions with fewer oxygen atoms typically end in -ite (e.g., NO2−\text{NO}_2^- nitrite).
    • Ions containing hydrogen often include "hydrogen" in their name (e.g., HCO3−\text{HCO}_3^- hydrogen carbonate).
  • Examples (from your image):
    • OH−\text{OH}^-: Hydroxide
    • NO3−\text{NO}_3^-: Nitrate
    • NO2−\text{NO}_2^-: Nitrite
    • SO42−\text{SO}_4^{2-}: Sulphate
    • SO32−\text{SO}_3^{2-}: Sulphite
    • HCO3−\text{HCO}_3^-: Hydrogen carbonate
    • MnO4−\text{MnO}_4^-: Permanganate

2. Covalent Bonds

  • Notes: A covalent bond is formed when two atoms share one or more pairs of electrons. This sharing allows both atoms to achieve a stable electron configuration, typically an octet (8 valence electrons) or a duet (2 valence electrons for hydrogen).
  • Reasons: Atoms share electrons to fill their outermost electron shells, which leads to a more stable, lower-energy state. This type of bonding usually occurs between two non-metal atoms.
  • Examples (from your image):
    • Hydrogen molecule (H2\text{H}_2):

  1. Each hydrogen atom has 1 valence electron.

  2. They share their electrons to form a single bond.

        *   Result: Each hydrogen atom effectively has 2 electrons, achieving a stable duet like Helium.
    $$
    \text{H} \cdot + \cdot \text{H} \longrightarrow \text{H} : \text{H}
    $$
*   **Oxygen molecule ($\text{O}_2$):**

  3. Each oxygen atom has 6 valence electrons.

  4. They share two pairs of electrons (a total of 4 electrons) to form a double bond.

        *   Result: Each oxygen atom effectively has 8 electrons (4 non-bonding and 4 shared), achieving a stable octet.
    $$
    : \ddot{\text{O}} \cdot + \cdot \ddot{\text{O}} : \longrightarrow : \ddot{\text{O}} :: \ddot{\text{O}} :
    $$
*   **Nitrogen molecule ($\text{N}_2$):**

  5. Each nitrogen atom has 5 valence electrons.

  6. They share three pairs of electrons (a total of 6 electrons) to form a triple bond.

        *   Result: Each nitrogen atom effectively has 8 electrons (2 non-bonding and 6 shared), achieving a stable octet.
    $$
    \cdot \ddot{\text{N}} \cdot + \cdot \ddot{\text{N}} \cdot \longrightarrow : \text{N} ::: \text{N} :
    $$

    3. Ionic Bonds

    • Notes: An ionic bond is formed when there is a complete transfer of one or more electrons from one atom to another. This creates oppositely charged ions (a positive cation and a negative anion) that are attracted to each other.
    • Reasons: This transfer typically occurs between a metal atom (which tends to lose electrons) and a non-metal atom (which tends to gain electrons). Both atoms achieve a stable electron configuration (usually an octet). The strong electrostatic attraction between the oppositely charged ions forms the bond.
    • Example (from your image - Sodium Chloride, NaCl\text{NaCl}):

  7. Sodium (Na\text{Na}) is a metal with 1 valence electron.

    Chlorine (Cl\text{Cl}) is a non-metal with 7 valence electrons.

  8. Sodium transfers its 1 valence electron to chlorine.

  9. Sodium becomes a positive ion (Na+\text{Na}^+) with a stable electron configuration.

    Chlorine becomes a negative ion (Cl−\text{Cl}^-) with a stable octet. * Result: The electrostatic attraction between Na+\text{Na}^+ and Cl−\text{Cl}^- forms the ionic bond. Na⋅+:Cl¨:⟶Na++[:Cl¨:]− \text{Na} \cdot + : \ddot{\text{Cl}} : \longrightarrow \text{Na}^+ + [: \ddot{\text{Cl}} :]^-

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