Chapter 6: Chemical Bonding<br />6.2 – Covalent Bonding and Molecular Compounds<br />
Molecule – neutral group of atoms that are held together by covalent bonds<br />Molecular Compound – chemical compound whose simplest units are molecules<br />
Chemical Formula – indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical scripts<br />Molecular Formula – shows the types and numbers of atoms combined in a single molecule of a molecular compound.<br />
Diatomic Molecules – molecules containing only two atoms.<br />Br2<br />Cl2<br />F2<br />H2<br />I2<br />N2<br />O2<br />
Octet Rule<br />-> Chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its highest occupied energy level.<br />Electron-Dot Notation – notation in which only the valence electrons of an atom of a particular element are shown. Dots are placed around the elements symbol.<br />
Lewis Structure – formulas in which atomic symbols represent nuclei and inner shell electrons<br /> — covalent bonds<br /> : unshared pair of electrons<br />Lone pair (unshared pair) – pair of electrons that is not involved in bonding and that belongs exclusively to one atom.<br />
Double bond – covalent bond produced by the sharing of two pairs of electrons between atoms.<br /><ul><li> carbon, nitrogen, and oxygen can share more than one electron pair</li></ul>Triple bond – covalent bond produced by the sharing of three pairs of electron between two atoms.<br />
A particular slide catching your eye?
Clipping is a handy way to collect important slides you want to go back to later.