Bromine water + potassium iodide

Chemical Bonding: An Introduction1. chemical bond:-ionic bond:-covalent bond:-Electronegativity:-Polar Covalent:2. octet rule:EXCEPTIONS3. Lewis dot structure4.Formal Charge:5.Resonance:Isomers:4. Types of Bonds:-Single vs. double vs.triple bonds:-Bond Strength:-Bond Length:5. VSEPR Model6. Polarity of Molecules

Rules for writing Lewis dot structures for molecules:1. Write the skeletal structure of the compound showing which atoms are bonded to what other atoms. Consider the following useful tips:A. The least electronegative atom usually occupies the central position in a molecule.B. Molecules are often symmetrical.2. Determine the sum of the valence electrons for all atoms in the molecule. For polyatomic ions,A. add an electron for every negative charge; orB. subtract an electron for every positive charge.3. A pair of bonding electrons between atoms is designated with a solid line, which represents TWO electrons. Remember that atoms can be bonded in multiple manners (i.e. double and triple bonds).4. Arrange the rest of the electrons (dots) around the atoms so that every atom has eight electrons (an octet). Remember that if the centralatom is from row 3 or higher of the periodic table, it may constitute an exceptionto the octet rule (i.e. it can possess more than 8 surrounding electrons). Also recall that elements in.Groups I, II, and III do not obey the octet rule either. The general rule for these atoms is that the number of valence electrons = number of bonds.5. Calculate the formal charge for each atom in your molecule; recall that the bestLewis dot structure is the one that minimizes formal charge amongst all the atoms (note: this may not necessarily mean “0”, but perhaps as close to “0” as possible).