You are to research the following questions and choose an appropriate format to present your answers in. Include diagrams where possible.
1. Describe metallic, ionic and covalent bonds.
Metallic - A chemical bond in which electrons are shared over many nuclei and electronic conduction occurs. Ionic – A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains an electron to form a negative ion. Covalent - A chemical bond that involves sharing a pair of electrons between atoms in a molecule.
2. Explain the structure of metals, ionic compounds, covalent molecules and covalent networks and give examples of compounds and elements that have these structures.
Metals – In a piece of metal, the outer shell of electrons are not closely to their own atoms. They leave their atoms, forming positively charged ions, and tend to wander from one atom to another, being shared by all the ions. We say that the atoms are delocalised meaning not held in their own locality or place. They form a sea of electrons within the metals. The outer shell of electrons move freely so metals are good conductors of electricity, metal ions can slide over each other without breaking which makes metals malleable and ductile. The sea of electrons reflect light with gives metals a shiny lustre. (All Metals)
Ionic Compounds – Ionic compounds is a compound that contains ions held together by ionic bonds. Most ionic compounds are crystalline solids at room temperature. An ionic compound consists of a three-dimensional lattice (network) of ions held together by ionic bonds, which extend throughout the whole crystal structure. Ionic Compounds have high melting and boiling points because of the electrostatic bonds throughout their crystal lattice. Electrons are held firmly in ions so they are bad conductors of electricity when solid. When molten, the ion vibration and causes breaks in the electrostatic bonds, which make molten...