<p>Chapter 12 12.1-12.2 *The manner in which atoms are bound together have profound effect on the chemical and physical properties of a substance -graphite and diamond only differ in the way the carbon atoms are bound to each other -chemical reactions in our body, the way drugs work and many other reactions around us depends on molecular structure</p><p>Types of bonds Bond-force that holds groups of two or more atoms together and makes them function as a unit ?Give an example of a bond? Bond energy-energy required to break a bond and tells us about the strength of a bond p70-allotropes of diamond/graphite Ionic bonding-attractions among closely packed oppositely charged ions forming an ionic compound from metals and nonmetals bonding AND the atoms are very different ?Give an example of an ionic bond? NaCl</p><p>True Covalent bond-electrons are shared by very identical atoms(identical or similar electronegativity values)-two same nonmetals ?Give an example of a covalent bond? H2</p><p>Polar covalent bond-unequal sharing of electrons formed from a bond polarity- two different nonmetals ?Give an example of a polar covalent bond? H2O</p><p>Bond polarity-partial charges on atoms results from a stronger attraction to electrons by one of the atoms in the molecule</p><p>Electronegativity(p362)-ability of an atom in a molecule to attract electrons to itself -chemist determine electronegativity values for elements by measuring the polarities of the bonds between various atoms ?What are two examples of periodic trends from this chart? -increases from left to right on the periodic table -decreases going down on the periodic table -higher electronegativity the closer a shared electron will be to an atom -polarity of a bond depends on the differences in electronegativities between an atom ?What is the difference between sodium and chloride? 2.1 What is the difference between H and H? 0 -zero electronegativity difference indicates true covalent and diatomic -similar electronegativites(two nonmetals that are NOT identical indicate sharing among atoms electronegativity differences bond type covalent ionic</p><p>0 covalent intermediate polar covalent large ionic</p>