October 3, 2013 When the bell rings voices are at zero, working on the DO NOW Pick up daily handouts Pick up turned back docs PICK UP A WHITE BOARD, A BLACK SOCK, AND ONE MARKER Turn in your late test corrections, progress reports, any make up work DO NOT TURN ANYTHING IN UNLESS STATED ABOVE HAVE OUT YOUR REFERENCE TABLE Start on the Do Now in your Do Now form DO NOW 9/30/ 13 (5) Write the Ionic Formulas for the following compounds, be sure to balance: 1. Silver Nitride 2. Zinc Oxide

Homework 10/3 Naming Practice Handout

Notebook Check Friday 10/4/13 Electron Configuration/Lewis Structure Notes (periodic table colored in) Ionic Formula Writing Handout

Upcoming Dates 10/4/2013 Mid-Quarter Test 10/4/2013 Take home test Periodic Trends 10/9/2013 Bonding/Geometry Test Turn and talk

Tutoring Saturday 12pm-1pm University City Regional Library 301 East W.T. Harris Boulevard Charlotte, NC 28262

Objectives   SWBAT Explain how covalent bonding in compounds determines its characteristics Determine that a bond is predominately covalent by the location of the atoms on the Periodic Table Apply the concept of electrons form covalent compound that is stable Write names of ionic and covalent compounds Pop call

The Octet Rule and Covalent Compounds Covalent compounds tend to form so that each atom, by sharing electrons, has an octet of electrons in its highest occupied energy level. Covalent compounds involve atoms of nonmetals only. The term “molecule” is used exclusively for covalent bonding

The Octet Rule: The Diatomic Fluorine Molecule 1s 2s 2p Each has seven valence electrons F 1s 2s 2p F F

The Octet Rule: The Diatomic Oxygen Molecule 1s 2s 2p Each has six valence electrons O 1s 2s 2p O O

The Octet Rule: The Diatomic Nitrogen Molecule 1s 2s 2p Each has five valence electrons N 1s 2s 2p N N

Lewis Structures Lewis structures show how valence electrons are arranged among atoms in a molecule. Lewis structures Reflect the central idea that stability of a compound relates to noble gas electron configuration. Shared electrons pairs are covalent bonds and can be represented by two dots (:) or by a single line ( - )

The HONC Rule Hydrogen (and Halogens) form one covalent bond Oxygen (and sulfur) form two covalent bonds One double bond, or two single bonds Nitrogen (and phosphorus) form three covalent bonds One triple bond, or three single bonds, or one double bond and a single bond Carbon (and silicon) form four covalent bonds. Two double bonds, or four single bonds, or a triple and a single, or a double and two singles

Electron Configuration / Lewis Dot Structure Review Na O Ne S

Completing a Lewis Structure -CH3Cl Make carbon the central atom (it wants the most bonds, 4) Add up available valence electrons: C = 4, H = (3)(1), Cl = 7 Total = 14 Join peripheral atoms to the central atom with electron pairs. H .. .. .. .. .. H C Cl .. .. Complete octets on atoms other than hydrogen with remaining electrons H

NEW Lewis Dot Structure Practice SO2 CO2 PCl3 H2O

Bond Length and Bond Energy Length (pm) Energy (kJ/mol) C - C 154 346 C=C 134 612 CC 120 835 C - N 147 305 C=N 132 615 CN 116 887 C - O 143 358 C=O 799 CO 113 1072 N - N 145 180 N=N 125 418 NN 110 942

Resonance Occurs when more than one valid Lewis structure can be written for a particular molecule. These are resonance structures. The actual structure is an average of the resonance structures.

Resonance in Benzene, C6H6

Turn and Talk WHEN I SAY GO, First person shares everything they remember about metallic bonding for 30 seconds, then switch, NEXT the first person shares again 30 seconds everything they remember about ionic bonding, then switch.

Naming Binary Molecular Compounds

Binary Molecular Compounds Compounds between two nonmetals First element in the formula is named first. Keeps its element name Gets a prefix if there is a subscript on it Second element is named second Use the root of the element name plus the -ide suffix Always use a prefix on the second element

List of Prefixes 1 = mon(o) 2 = di 3 = tri 4 = tetra 5 = penta 6 = hexa 7 = hepta 8 = octa 9 = nona 10 = deka List of Prefixes

Naming Binary Compounds diphosphorus pentoxide CO2 = carbon dioxide CO = carbon monoxide N2O = dinitrogen monoxide

Practice – Write the Formula Compound Name Compound Formula Carbon dioxide Carbon monoxide Diphosphorus pentoxide Dinitrogen monoxide Silicon dioxide Carbon tetrabromide Sulfur dioxide Phosphorus pentabromide Iodine trichloride Nitrogen triiodide Dinitrogen trioxide Check next slide for answers

Answers – Write the Formula Compound Name Compound Formula Carbon dioxide CO2 Carbon monoxide CO Diphosphorus pentoxide P2O5 Dinitrogen monoxide N2O Silicon dioxide SiO2 Carbon tetrabromide CBr4 Sulfur dioxide SO2 Phosphorus pentabromide PBr5 Iodine trichloride ICl3 Nitrogen triiodide NI3 Dinitrogen trioxide N2O3

Practice – Name the Compounds Compound Formula Compound Name N2O4 SO3 NO NO2 As2O5 PCl3 CCl4 H2O SeF6 Check next slide for answers

Answers – Name the Compounds Compound Formula Compound Name N2O4 dinitrogen tetroxide SO3 sulfur trioxide NO nitrogen monoxide NO2 nitrogen dioxide As2O5 diarsenic pentoxide PCl3 phosphorus trichloride CCl4 carbon tetrachloride H2O dinitrogen monoxide SeF6 selenium hexafluoride

Naming Ionic Compounds Cation first, then anion Monatomic cation = name of the element Ca2+ = calcium ion Monatomic anion = root + -ide Cl- = chloride CaCl2 = calcium chloride Ended block 1

Naming Ionic Compounds (continued) Metals with multiple oxidation states some metal forms more than one cation use Roman numeral in name PbCl2 Pb2+ is cation PbCl2 = lead(II) chloride

Head Start on Hw! Work at a volume of 1 with your elbow partner ONLY to start hw

Objectives   SWBAT Explain how covalent bonding in compounds determines its characteristics Determine that a bond is predominately covalent by the location of the atoms on the Periodic Table Apply the concept of electrons form covalent compound that is stable Write names of ionic and covalent compounds

Exit Ticket Write the Formula Determine if ionic or covalent then name 1. NO2 2.NaCl 3. PCl3 Write the Formula 6. Carbon monoxide 5. Calcium Chloride