CHEM 120 Week 2 Ionic Compounds

Week 2 Ionic Compounds IONIC COMPOUNDS In this lesson, you will be exploring ionic bonding. You have encountered many examples of molecules containing Ionic bonds including table salt and sodium fluoride which is found in toothpaste. We will see in this lesson how ionic compounds are formed and how the formation of these compounds leads to the properties we observe. Which of the following would be considered an Ionic Compound? A. CH4 B. LiCl C. N2O4 D. SO In general, an ionic bond forms between atoms classified as: A. Metals and non-metals B. Transition metals C. More than one metal D. More than one nonmetal In an ionic bond electrons are: A. Shared B. Created C. Transferred D. Destroyed Which of the following would you classify as a polyatomic cation? A. NH4 + B. F - C. OHD. O 2- Ionic compounds are a class of molecules that form through the attraction of negative and positive charges. If you have had a pair of magnets, you have likely noticed that opposites attract. Positive and negative charges are attracted to one another. This is true not only with magnets, but also all the way down to the subatomic level. In an ionic compound, positively charged cations are attracted to negatively charged anions, holding tight to one another like a magnet and a metal surface. An example of this is sodium chloride, otherwise known as table salt. This compound is made of Na+ cations and Clanions held together due to a difference in charge. The term we use for this attraction is electrostatic attraction. FORMATION OF IONIC COMPOUNDS The outermost electrons of an atom, known as valence electrons, are transferred or shared in chemical reactions so that each atom has a full valence shell. This is typically 8 valence electrons, and this rule is known as the octet rule. In ionic compounds, the electrons are transferred, while in a molecular compound electrons are shared. In this lesson, we are focusing on Ionic compounds, so let us look into why these valence electrons are transferred