chemistry paper 1

• Ionic bonds result in the formation of ions, one positively charged (cation) and one negatively charged (anion).
• Ionic bonds form between atoms when one atom transfers electrons to another atom.
• Ionic compounds typically have high melting and boiling points due to the strong electrostatic forces between ions.
• Non-metals do not conduct electricity as their valence electrons are tightly held by the nucleus.
• Metals are good conductors of electricity because they have delocalized electrons that can move freely through the metal lattice.
• Metals are good conductors of electricity because they contain delocalized electrons that can move freely through the lattice structure.
• The covalent bond is formed when two atoms share electrons.
• Covalent bonding occurs when two non-metal atoms share electrons to achieve a full outer shell.
• Non-metals do not conduct electricity as their outer shell is full or nearly full, making it difficult for electrons to be transferred from one atom to another.
• Covalent bonds involve sharing pairs of electrons between two non-metal atoms.
• Metallic bonding is the attraction between positive metal ions and delocalized sea of electrons.
• The ability of metals to conduct heat is related to their atomic structure and the movement of free electrons within them.
• In ionic solids, the positive and negative ions are arranged in regular patterns called lattices.
• Ionic bonds occur between oppositely charged ions.
• Why do ionic compounds only conduct electricity when molten ?

  IONS are able to carry the electrical charge because the electrostatic forces which held the ions have broken down