Chem 1320 1st Edition Lecture 27Outline of Last Lecture I. Ion SizesII. Role of Atomic Radii in Ion ChannelsIII. Sodium ChannelsIV. Potassium ChannelsOutline of Current LectureI. Chemical BondingII. Ionic BondingIII. Lattice EnergyCurrent Lecture I. Chemical BondingValence electrons are the outer shell of electrons, with higher values of n, they are the least tightly held electrons. GN Lewis came up with something called Lewis Structures. The periodic table is arranged so that elements with the same number of valence electrons are in the same columns. II. Ionic BondingThis is where a metal and nonmetal exchange electrons. Charges on respective ions have an electrostatic attraction. There is a compound formation which is combining positive and negative charges to obtain a neutral molecule. D= r+ + r- . We want to be able to predict the strength of the ionic bond. Crystalline arrangements maximize the packing of the atoms. Close packing of ions maximizes interactions and measured as a quantity known as lattice energy. III. Lattice EnergyThere are multiple cations and anions that come together to form crystal that reflects energy. We use lattice energy as a measure of the strength of the ionic bond since we can easily isolate a single molecule of an ionic compound. The larger the charge is on the top, they have a larger Ewhich means they will have a stronger ionic bond. The smaller the ion, the shorter the distance between centers, and the larger the E, the stronger the ionic bond. The number of valence electrons determines how the element will bond elements because they all want the noble gas 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.configuration. Ionic bonding will get to a neutral charged specie. The strength of the ionic bond is due to the size of the charge and the size of the
View Full Document
Unlocking...