CHEM 101 1nd Edition Lecture 7 Outline of Last Lecture I. Periodic TableII. Elemental GroupsIII. Neils BohrIV. IonsOutline of Current Lecture I. IonsII. What is the size of an atom?III. Ionic CompoundsIV. Writing Formulas for Ionic CompoundsV. Naming Ionic CompoundsCurrent LectureI. Ionsa. Metals of Groups 1A-3A form positive ions having a charge equal to the group number of the metalb. Transition metals also form cations, but with no easily predictable patternc. Nonmetals often form ions having a negative charge equal to the group number of the element minus 8II. What is the size of an atom?a. The bonding atoms radius is defined as one-half of the distance between covalently bonded nucleiIII. Ionic Compoundsa. Formed between cations (metal or polycation) and anions (nonmetal or polyanion)b. Ionic compounds or salts cons is of a three dimensional array of ions. The cation donate electrons to the anion.c. The cation and anon are attracted to each other by electrostatic forces.i. These forces are governed by Coulomb's Lawii. As ion charge increases, the attractive force increases.iii. As the distance between the ions increases, the attractive force decreases.d. Memorize Common Cationsi. Leave copper, iron, mercury of These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.e. Memorize Common Anionsi. ClO- = chloriteii. ClO2- = hypochloriteiii. Leave of acetateIV. Writing Formulas for Ionic Compoundsa. Ionic compounds are electronically neutral therefore the sum of the charges of the anion and the cation must be zero. Formulas are always written with the cation first and the anion second.i. Mg32+ + N23- = Mg3N2b. Subscripts must always be reduced to the smallest ratioc. If a subscript is added to a polyatomic ion the entire polyatomic unit must be enclosed in parentheses.i. Al3+ + Co32- = Al2(CO3)3d. Subscripts of one are not shownV. Naming Ionic Compoundsa. Write the name of the cationb. If the anion is an element, change its ending to -ide; if the anion is a polyatomic ion simply write the name of the polyatomic ion.c. If the cation can have more than one possible charge, write the charge as a roman numeral in parentheses.i. CaCO3 = Calcium Carbonateii. CuSO3 = Copper(II) Sulfite (Sulfite is SO3-2)iii. (NH4)3PO4 = Ammonium Phosphateiv. Na2SO4 = Sodium Sulfatev. Na3N = Sodium Nitridevi. NiCl2 = Nickel Chloridevii. KBr = Potassium
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