Unit 6: Chapters 8 and 9

StudyBlue printing of Unit 6: Chapters 8 and 9 html, body, div, span, applet, object, iframe, h1, h2, h3, h4, h5, h6, p, blockquote, pre, a, abbr, acronym, address, big, cite, code, del, dfn, em, font, img, ins, kbd, q, s, samp, small, strike, strong, sub, sup, tt, var, b, u, i, center, fieldset, form, label, legend, table, caption, tbody, tfoot, thead, tr, th, td { margin: 0; padding: 0; border: 0; outline: 0; font-size: 100%; background: transparent; } body { line-height: 1; } blockquote, q { quotes: none; } blockquote:before, blockquote:after, q:before, q:after { content: ''; content: none; } /* remember to define focus styles! */ :focus { outline: 0; } /* remember to highlight inserts somehow! */ ins { text-decoration: none; } del { text-decoration: line-through; } /* tables still need 'cellspacing="0"' in the markup */ table { border-collapse: collapse; border-spacing: 0; } /* end RESET */ .header { min-width:800px; } .logo { padding:6px 20px 2px 20px; margin:0; font-size:25px; font-weight:bold; color:#808285; position:relative; border-bottom: 1px solid #c5c5c5; } .logo-blue { color:#70adc4; } .logo-desc { font-weight:normal; font-size:19px; color:#cccccc; margin-top:50px; position:absolute; display: none; } .back-button { position:absolute; top:20px; right:20px; font-size:13px; line-height:25px; color:rgb(0,175,225); font-weight:normal; } .back-button a { color:rgb(0,175,225); } .instructions { padding:0; margin:0; width:100%; position:relative; color:rgb(100,100,100); } .step-holder { border-left:1px solid #ededed; margin-left:20px; } .steps { padding:15px 0; float:left; width:24%; border-right:1px solid #ededed; text-align:center; } .steps-01 { } .steps-02 { } .steps-03 { } .steps-04 { } .label { padding:5px 10px; } .print-button { } .print-button a { background-color:rgb(0,175,225); color:white; line-height: 19px; padding:9px 8px 5px 30px; font-size:14px; text-decoration:none; background-image: url(images/printer.png); background-repeat: no-repeat; background-position: 7px 50%; -moz-border-radius: 5px; -webkit-border-radius: 5px; } .print-button a:hover { background-color:black; } .theNote .content { width: 8.0in !important; margin: 5px auto; padding:20px; background-color:white; } .theNote .header { border-bottom: 1px dashed #C8C8C8; font-size: 17px; padding: 0 0 10px; line-height: 19px; color: #00ADE1; min-width:500px; } .theNote .body { font-size: 14px; line-height: 19px; padding: 10px 0; } .theNote{ padding:6px 0; clear:both; background-color: rgb(200,200,200); } .theNote h3{ color: rgb(100,100,100); } .theNote h1, .theNote h3{ background-color:white; padding:2px 20px; width:8.0in !important; margin: 0 auto; font-size: 15px; } .theNote h1{ padding-top: 10px; font-size: 15px; } .theNote h1:first-child{ font-size: 20px; } .theNote h3 { font-size: 14px; font-weight: normal; } #options { border: 3px double #ccc; padding: 5px 12px; margin: 10px 50px 10px 20px; float: left; } #info { border-top: 1px solid #ccc; padding-top: 5px; font-style: italic; } li { margin: 5px 10px 5px 25px; } ul li { list-style: disc; } ol li { list-style: decimal; } img { border: 0; } table { clear: both; width: 100%; border: 1px solid #c5c5c5; border-width: 1px 0; margin: 0; page-break-after: always; } table#page { page-break-after: auto; } td { text-align: center; font-size: 12px; border-bottom: 1px dashed #c5c5c5; height: 1.75in; width: 50%; padding-left: 15px; } .leftside { border-right: 1px solid #cccccc; padding: 0 15px 0 0; } .bottom td { border-bottom: none; } .clearfix { clear:both; line-height:1px; height:1px; } img { max-width:80%; max-height:150px; margin:20px; } @media print {.header { display: none; } .content .header{ display:inherit; } table { border: 1px dashed #bbb; border-width: 1px 0; } .theNote{ background-color:white; } } Questions 1 and 2 Chemical Bond-a force that holds groups of atoms together and makes them function as a unit. Types of Chemical Bonds Ionic Covalent Polar Covalent Metallic Ionic Compounds (NaCl, KCl, KBr) and Bonds made up of a metal and a nonmetal Physical Properties: solid at room temperature poor conductors of heat and electricity in solid state soluable in water conduct heat and electricity in solution have high melting points usually crystals Ionic Bond-a bond where one or more electrons transfer between atoms. formed from electrostatic attractions of closely packed, oppositely charged ions formed when an atom that easily loses electrons reacts withone that has a high electron affinity Isoelectronic Ions-ions of different elements that contain the same number of electrons O2-, F-, Na+, Mg2+ and Al3+ Sizes of Ions anions are bigger than cations ("Antelope are bigger than cats") cations are usually smaller than the parent atom anions are usually larger than the parent atom ion size increases down the family Lattice Energy-the change in energy when separated gaseous ions are packed together to form an ionic solid. LE=KQ1Q2/r r=the shortest distance between centers of cations and anions Formation of an Ionic Solid Sublimation of the solid metal Ionization of the metal atom Dissociation of the nonmetal Covalent Bonds-bonds in which electrons are shared by the nuclei Physical Properties of Covalent Compounds good conductors in aqueous solution insoluable Polar Covalent Bonds-covalent bonds with an unequal sharing of electrons. use greek lowercase delta to indicate the charge on the pole vectors indicate the direction of charge from positive to negative Bond Energy-the energy required to break a bond Calculating Bond Energy BE=sum of products-sum of reactants Coulomb's Law-the force acting between two electric charges is radial, the distance between them is inverse-sqared, and proportional to the product of the charges. like charges repel each other, while opposite charges attract radial means emanating froma a common center F=KQ1Q2/distance^2 K=2.31x10^-9 Bond Length-the optimum distance for the two nuclei bonded the larger the atom the longer the bond the more bonds the shorter the bond as bond length increases, bond energy decreases as bond strength increases bond length decreases Electronegativity-the ability of an atom in a molecule to attract shared electrons to itself increases across the period and decreases down the family Δ e=absolute value of the electronegativity of 1st-electronegativity of 2nd Polarity(or having a dipole moment)-a molecule that has a center of positive charge and a center of negative charge polar bonds do not always mean polar molecules if a molecule with polar bonds has symmetry the dipole moments cancel each other out and the molecule is nonpolar