Covalent and Ionic Bonds

Flashcards covering key concepts about covalent and ionic bonds, including their definitions, features, and characteristics.

Covalent Bond

The electrostatic force of attraction between a shared pair of electrons and the adjacent nuclei.

Elements forming covalent bonds

Non-metals to non-metals.

Low boiling points of simple molecular substances

They have weak intermolecular forces of attraction which require little energy to overcome.

Examples of giant covalent bonding

Diamond, graphite, and silica.

High melting point of graphite

Contains many strong covalent bonds which require a lot of energy to overcome.

Soft and slippery nature of graphite

Contains layers of carbon atoms that are able to slide over one another.

Graphite's ability to conduct electricity

Each carbon atom has one spare electron, which is delocalized and free to move and carry charge.

High melting point of diamond

Contains many strong covalent bonds which require a lot of energy to overcome.

Hardness of diamond

Contains a rigid lattice of strong covalent bonds that require a lot of energy to break.

Ionic Bond

The electrostatic force of attraction between oppositely charged ions.

Elements forming ionic bonds

Metals to non-metals.

Ionic compounds in solid state

Do not conduct because ions are held in fixed positions and cannot move to carry charge.

Ionic compounds when molten or in solution

Conduct because ions are free to move and carry charge.

High melting points of ionic compounds

Due to strong electrostatic attractions between oppositely charged ions which require a lot of energy to overcome.