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Homework: Re-write in paragraph form – notes pages 1 and 3. Add additional information learned in practice. Agenda: 3/17 – 3 rd block. Objective: To interpret (correctly write) formulas and names for compounds – using IUPAC convention Warm-up: review names & formulas
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Homework: Re-write in paragraph form – notes pages 1 and 3. Add additional information learned in practice. Agenda: 3/17 – 3rd block Objective: To interpret (correctly write) formulas and names for compounds – using IUPAC convention Warm-up: review names & formulas Review: Binary Ionic Compounds More Complex Ionic Compounds With Polyatomic Ions With Transition Metals Covalent Compounds
Language of chemistry: Standardize system to represent compounds
Ionic Compounds Metals lose valence electrons Non-metals gain valence electrons
Ionic Bonding: Transfer of valence electrons • Ionic bonding occurs when a metal loses 1 or more electrons to a non-metal in an effort to attain a stable octet of valence electrons. • Use Electron Dot Diagrams (Lewis diagrams) to show the ionic bonds for one formula unit. • Na Cl = Na⁺¹Cl⁻¹
Electron Dot Diagram (Lewis) ClCaCl = CaCl
Some Ionic Compounds are more complex Include polyatomic ions
Ionic compounds: Found in minerals and rocks Barite = BaSO₄ Used to make paper & glass Source of barium used For x-rays of the digestive system
Ionic compounds: Found in minerals and rocks Gypsum = CaSO₄· 2H₂O Used for plaster for walls, ceilings, sculptures
Ionic compounds: Found in minerals and rocks Calcite = CaCO₃ Used in paint, Antacids, calcium Supplement for food
Ionic compound with polyatomic ions Calcium sulfate in casts Barium sulfate to absorb x-rays Acetate uses Sodium acetate In Heat packs
Sodium hydrogen carbonate (old name: sodium bicarbonate) Medical: used in emergency situations to correct pH of blood Baking soda: to make cakes rise
Bleach Dentistry: Clean and disinfect Root canals Rocket fuels: Source of oxygen
POLYATOMIC IONS Examine the names & formulas: What is the pattern? Do they end in “–ide?” Ions with -1 charge perbromate BrO4-1 bromate BrO3-1 bromite BrO2-1 hypobromite BrO-1 perchlorate ClO4-1 chlorate ClO3-1 chlorite ClO2-1 hypochlorite ClO-1 periodate IO4-1 iodate IO3-1 iodite IO2-1 hypoiodite IO-1 nitrate NO3-1 nitrite NO2-1 hydroxide OH-1 cyanide CN-1 thiocyanate SCN-1 acetate C2H3O2-1 Permanganate MnO4-1 bicarbonate HCO3-1 Ions with a -2 Charge carbonate CO3-2 phthalate C8H4O4-2 sulfate SO4-2 sulfite SO3-2 chromate CrO4-2 dichromate Cr2O7-2 oxalate C2O4-2 peroxide O2-2 Ions with a -3 Charge phosphate PO4-3 phosphite PO3-3 arsenate AsO4-3 Ions with +1 charge ammonium ion NH4+1
Using polyatomic ions: • Sodium + nitrate Calcium + nitrate Formula Name:
Ionic Compounds with Transition Metals • The transition metals are elements in Groups _____ to _______. • + post transition metals: under the staircase. • Transition metals can have more than one charge. • Use Roman numerals after the name. • Roman numbers: • I = II = III = IV = V=
Transition metals • Examples Iron II oxide Iron III oxide Write the formulas for: Copper I oxide Cobalt III chloride Nickel II sulfide
Practice: Writing Binary Formulas • Many transition and post transition metals have multiple oxidation numbers (charges) • Ni: oxidation numbers of _____ & _____ • Fe: • Find other examples: • Write formulas • Write names
Language of chemistry: Standardize system to represent compounds
Covalent Compounds Molecules Names & Formulas for Inorganic Covalent Compounds
Compounds Stable Most atoms are bonded in compounds Separated with chemical reactions Usually need high heat or electricity
Names of Binary Molecules • First-element name • 2nd – end in “ide” • Use prefixes -Always with 2nd element -With 1st element except mono- Element with lowest EN goes first On the Periodic Table – across /down
Practice: • Complete the table in your notes. • Write the names • Write the formula
Acids • Acids are molecules that are in aqueous solution (_________ in __________) and produce hydrogen ions (H¹⁺) • Typically start with H • Almost act as an ionic compound Electronegativity Difference:
Acids: H + Halogen • Hydro + Halogen (ic) + Acid • HBr • Hydrobromic acid
Oxyacids: common acids • Contains oxygen (in a polyatomic ion) • Note the endings of the anion & the acid name • H + nitrate = Nitric Acid • H + sulfate = • H + phosphate = • H + acetate =
7 Diatomic Molecules • Heck No Halogens • Named with the element name
Common Names for 3 Molecules Molecular name and formula: common name • Dihydrogen monoxide = • Carbon tetrahydride = • Nitrogen trihydride =