Bell Ringer: 3/4/15 Classify the following elements as either a Metal, Non-Metal or Metalloid. As Na Br Ni Kr C F Fr

Ionic Compounds and Metallic Bonds Chapters 6 and 7

Chemical Formulas Chemical Formula NaCl CO2 MgCl2 Na3P 1 Na and 1 Cl Subscripts show numbers No Subscript = 1 atom NaCl CO2 MgCl2 Na3P 1 Na and 1 Cl 1 C and 2 O 1 Mg and 2 Cl 3 Na and 1 P end

Chemical Formulas # of total atoms (counting atoms): H2SO4 KNO3 Fe2O3 Hg2Cl2 end

Ba(OH)2 Chemical Formulas Cu (NO3)2 If you see ( )… Ba OH Cu NO3 O N H Subscript applies to all atoms inside ( ) Ba(OH)2 Ba OH O H Cu (NO3)2 Cu NO3 N O end

Chemical Formulas # of total atoms: Cu(NO3)2 KMnO4 Al2(SO4)3 (NH4)3PO4 end

Chemical Bonds Valence Electrons e- in highest energy level Determine chemical properties How many in: Li S Ba P F Al end

Chemical Bonds Octet Rule To get 8 valence, atoms either: Atoms want 8 val. e- Stable Configuration Nobel Gas: ns2 np6 Transition metals also want: Half-Filled d-orbital: ns2 np6 nd5 Filled d-orbital: ns2 np6 nd10 To get 8 valence, atoms either: Transfer Electrons Share Electrons end

Formation of a Chemical Bond Force holding 2 atoms together 3 types: Ionic (Metal and Nonmetal) Covalent (Nonmetal and Nonmetal) Metallic (Metal and Metal)

Chemical Bonding Ionic or Covalent? CaCl2 LiBr CO2 SO3 H2O BaSO4 NaF NO2 CH4 AlPO4 end

Chemical Bonding Complete #1-10 on “Types of Chemical Bonds”

Ionic Bonds Ionic Bonds Metal and Nonmetal (or Polyatomic Ion) ΔEN > 1.7 Electrons are TRANSFERRED Ions (atom with a charge) Charges = Oxidation States Combine to make neutral compounds Ionic Compounds = Salts end

Ionic Bonds Ions Atoms with a charge Formed by losing/gaining electrons Positively charged = Lost e- = Cation Negatively charged = Gain e- = Anion end

Ionic Bonds The Periodic Table can predict the charges Metals will lose electrons Cations Nonmetals will gain electrons Anions The charge is known as the Oxidation Number Arranged by Group Cannot predict a Transition Metal’s charge Ions will combine so the overall charge = 0 end

Ionic Bonds Group: 1 2 13 14 15 16 17 18 # of 1 2 3 4 5 6 7 8 Valence: Oxidation States follow the Valence Electrons Group: 1 2 13 14 15 16 17 18 # of 1 2 3 4 5 6 7 8 Valence: Oxidation State: +1 +2 +3 ±4 -3 -2 -1 0 end

Ionic Compounds Lattice Energy Physical Properties of Ionic Compounds: High M.P. & B.P. Brittle Conduct Electricity as liquids (molten) or when dissolved Crystal Lattice structure Anions and Cations alternate Lattice Energy Energy needed to break apart the crystal lattice end

Naming Ionic Compounds 3 steps Name the Cation Name the Anion Change the Ending to –ide NaBr Sodium Bromine Sodium Bromide end

Naming Ionic Compounds Name the following: BaS MgF2 Ca3N2 end

Naming Ionic Compounds Complete the following on “Naming Binary Compounds (Ionic)”

Naming Ionic Compounds More than 2 elements = POLYATOMIC ION!!! Get name from the REFERENCE TABLE!!! DON’T change the ending!!! NaNO3 Sodium Nitrate end

Naming Ionic Compounds Name the following: KOH NaC2H3O2 (NH4)2O Sr3(PO4)2 end

Naming Ionic Compounds Complete 1-8, 10, 11 on “Naming of Non-Binary Compounds”

Writing Ionic Compounds Binary & Ternary

Writing Ionic Formulas Writing formulas: 3 steps: Write the cation, with charge Write the anion, with charge Cross the charges to get subscripts Do NOT put the “+” or “-” end

Writing Ionic Formulas Write the formulas for the following: Beryllium Phosphide Calcium Fluoride Strontium Sulfide end

Writing Ionic Compounds

Writing Ionic Formulas Polyatomic Ions ARE A GROUP Write ( ), then cross charges Write the formula for the following: Calcium Phosphate Barium Nitrate Sodium Chromate Ammonium Acetate end

Writing Ionic Formulas Homework: p.207 #2 a-f p.211 #2 b-d, & f p. 235 #7

Bell Ringer Name the following compounds: BaCl2 K2CrO4 Na2CO3 Pb(NO3) 2 Identify the cations and anions:

Transition Metals 2 valence electrons But Many Oxidation States Names show the charge Exceptions: Silver: Ag+ Zinc: Zn2+ Lead (Pb) and Tin (Sn) can either be 2+ or 4+ end

Transition Metals The metal's charge is the Roman Numeral Vanadium (III) Sulfide V3+ S2- V2S3 Metal's Charge end

Transition Metals Write formulas for the following: Osmium (V) Fluoride Silver Nitride Technetium (VII) Phosphate end

Transition Metals Complete “Writing Binary Formulas Worksheet”

Transition Metals Names MUST have a Roman Numeral! To get charge, uncross subscripts! Fe2O3 Fe3+ O2- iron (III) oxide end

Transition Metals Name the following: HgF2 Hf2S5 YP end

Naming Ionic Compounds Complete the following on “Naming Binary Compounds (Ionic)” 3 12 4 13 5 16 6 19 7 20

HW Silver oxide Copper (I) bromide Copper (II) bromide Iron (II) oxide Iron (III) oxide Chromium (II) chloride Chromium (III) chloride Mercury (I) Iodide Manganese (II) oxide Manganese (III) oxide

DRY LAB -IONIC BONDING

Bell Ringer: Chemical Bonding Review: 1. What are the three types of Chemical Bonds? 2. What is the Octet Rule? 3. What kind of ion has a positive charge? 4. During Ionic Bonding, what type of atom loses their electrons, and which type of atom gains electrons? 5. What is an atom's oxidation state? 6. Why does a transition metal have a roman numeral in its chemical name? Get your Worksheet out from Friday (Acids on Back)

Mixed Ionic Review With Transition Metals

Acids Acids Hydrochloric Acid HCl Nitric Acid HNO3 Sulfuric Acid H2SO4 Start with hydrogen (H) Ionize when mixed with water Produce H+ and anions Common acids: Hydrochloric Acid HCl Nitric Acid HNO3 Sulfuric Acid H2SO4 Acetic Acid HC2H3O2 or CH3COOH end

NAMING ACIDS Binary Acids Hydrogen + 1 element Name as: hydro- ___ -ic acid HF H3P H2S H2O end

NAMING ACIDS Oxyacids ___ -ate  ___ -ic acid ___ -ite  ___ -ous acid Hydrogen + Polyatomic Ion Follow polyatomic names ___ -ate  ___ -ic acid ___ -ite  ___ -ous acid end

NAMING ACIDS H3PO4 HClO2 HNO2 HClO3 end

Formulas of Acids *Honors* Cross charges like Ionic Formulas Hydrogen = H+ Watch out for elements/polyatomic ions Write formulas for: Hydrosulfic acid Hydrochloric acid Nitric acid Carbonous acid end

NAMING ACIDS Complete #1-20 on “Naming Acids”

Metallic Bonds Metallic Bond Metal and Metals Valence e- shared between ALL atoms Metal Cation + a “sea of electrons” end

Metallic Bonds More Shared Electrons = Stronger Bond Properties of Metals: High M.P. & B.P. Conductive Malleable/Ductile end

Homework Complete Back Side of Worksheet on Acids