what is ionic bonding?
Electrostatic attraction between oppositely charged ions giant ionic lattice. it has a high melting point, brittle, conducts only when molten/aqueous.
what is covalent bonding?
Shared electron pairs, directional, discrete molecules or giant covalent lattices.
what is metallic bonding?
Delocalised electrons in a sea of positive ions. Strength depends on charge density of cations. Explains conductivity and malleability.
what did van der Waals discover?
induced dipoles, increase with electron cloud size.
What is an ionic bond?
A strong electrostatic attraction between oppositely charged ions.
How do ions form?
By electron loss (cation) or gain (anion).
How do ionic radius and charge affect bond strength?
Smaller ions and higher charges = stronger bonds.
Example of ionic bonding?
Na⁺ and Cl⁻ form NaCl.
What do electronic configuration diagrams of ions show?
How electrons are arranged after gaining or losing electrons.
What is a covalent bond?
Attraction between two nuclei and shared pairs of electrons
What do dot and cross diagrams show?
Shared electrons in covalent molecules
What is a dative covalent bond?
Both electrons in the shared pair come from one atom.
How does bond length relate to bond strength?
Shorter bonds are stronger.
What is metallic bonding?
Attraction between positive metal ions and delocalised electrons.
Why can metals conduct electricity?
Delocalised electrons move freely through the structure.
Why are metals malleable?
Layers of positive ions can slide over each other.
What are van der Waals forces?
Weak attractions from temporary dipoles.
What are dipole–dipole forces?
Attractions between permanent dipoles in polar molecules.
What is hydrogen bonding?
A strong attraction between H and N, O, or F atoms.
Example of a molecule with hydrogen bonding?
Water (H₂O).
