340 likes | 650 Vues
Nomenclature. Naming Compounds. Ionic Compounds. Metal bonding with non-metal One atom gains electrons, one atom loses electrons Exist as ions with full highest energy levels. Are held together in a giant crystal by the electrostatic attraction of the opposite charges.
E N D
Nomenclature Naming Compounds
Ionic Compounds • Metal bonding with non-metal • One atom gains electrons, one atom loses electrons • Exist as ions with full highest energy levels. • Are held together in a giant crystal by the electrostatic attraction of the opposite charges. • The metal is named first; the nonmetal gets “ide” at the end of it’s name. • Ex. CaCl2 Calcium chloride
There is no real bond between the ions. There is just strong attraction between the opposite charges. - - + + - + + - - + - - + + -
Metals Non-Metals Rule #1
Writing Ionic Formulas • Determine the charge on each ion. • Find the lowest common multiple that will balance the charge. ex. Calcium Chloride Ca+2 Cl- +2 x2=-2 (to balance the charge) CaCl2
Try theseMetal & Non-metal Sodium phosphide Magnesium telluride Lithium chloride Barium carbide Strontium arsenide
Ionic Compounds part II • The transition metal is named first with a Roman numeral to indicate the charge on the ion; the nonmetal gets “ide” at the end of its name.
Non- metals Rule #2 Transition Metals
Non- metals Rule #2 Transition Metals
What is the name of CuO ? We know that oxygen has a charge of –2. Therefore, copper must have a charge of +2. We must indicate the charge of the transition metal. Copper (II) oxide
Try these:Transition Metal & Non-metal Fe3N2 NiBr3 CoCl2 HgI SnS2
Try these:Transition Metal & Non-metal Fe3N2 Iron was multiplied by 3 and nitrogen (-3) was multiplied by 2 (-6) so that the charges would balance. The charge on Iron must have been +2. Iron (II) nitride
Try these:Transition Metal & Non-metal NiBr3 The charge (from the periodic table) on Br is –1. Br was multiplied by 3 (hence the subscript), so the charge on Nickel MUST be +3. Nickel (III) Bromide
Try these:Transition Metal & Non-metal CoCl2 The charge (from the periodic table) on Cl is –1. Chlorine was multiplied by 2 (hence the subscript), so the charge on Cobalt MUST be +2. Cobalt (II) Chloride
Try these:Transition Metal & Non-metal HgI The charge (from the periodic table) on I is –1. Iodine was not multiplied by anything (no subscript), so the charge on Mercury MUST be +1. Mercury (I) Iodide
Try these:Transition Metal & Non-metal MnO2 The charge (from the periodic table) on O is –2. Oxygen was multiplied by 2 (hence the subscript), so the charge on Manganese MUST be +4. Manganese (IV) Oxide
Formula writing with transition metals Simple! ex. Nickel (II) Iodide The charge on the nickel ion is obviously +2. The charge on iodide is always -1. Therefore, the formula is: NiI2
Ionic Compounds part III • Bonding with a Polyatomic ion • The metal is named first; the polyatomic anion is named second (a polyatomic cation is named first). Ex. Li3PO4 Lithium phosphate
Polyatomic Ions thatwe use in science 10: hydroxide sulfate nitrate carbonate phosphate ammonium chlorate OH-1 SO4-2 NO3-1 CO3-2 PO4-3 NH4+1 ClO3-1
Try these:Polyatomic Ion NaOH K2SO4 Ba(NO3)2 CuCO3 Li3PO4 NH4Cl
Try these: Sodium Hydroxide Potassium Sulfate Barium Nitrate Copper(II) Carbonate Lithium Phosphate Ammonium Chlorate NaOH K2SO4 Ba(NO3)2 CuCO3 Li3PO4 NH4ClO3
Writing Formulas Calcium sulfate Potassium carbonate Ammonium hydroxide Iron (III) chlorate Copper (I) phosphate Zinc sulfate
Ionic BondingvsMolecular Bonding Makes "Compounds”vsMakes "Molecules" Transfers electronsvsShares electrons Metals & NonmetalsvsMade of Nonmetals Positive & NegativevsNeutral Weak BondvsStrong bond NaCl KOH CaCl2vs H2O CO2 NH3CH4
Prefixes • Mono • Di • Tri • Tetra • Penta • Hexa • Hepta • Octa • Nona • Deca Molecular Compounds • Non-metals bond with non-metals. • Atoms share electrons. • The number of each atom present is indicated by a prefix. • Add “ide” to the end of the second atom’s name.
Non- metals Rule #3
ex. N2Odinitrogen monoxide NO nitrogen monoxide N2O3dinitrogen trioxide NO2nitrogen dioxide * N2O4dinitrogentetroxide N2O5dinitrogenpentoxide
ex. N2Odinitrogenmonoxide NO nitrogenmonoxide N2O3dinitrogentrioxide NO2nitrogen dioxide* N2O4dinitrogentetroxide N2O5dinitrogenpentoxide * When the first atom is singular, the prefix “mono” is not used.
Try These:Non-metal & Non-metal sulfur trioxide xenon hexafluoride krypton difluoride bromine pentachloride sulfur tetrachloride phosphorus trifluoride tetrarsenicdecoxide dinitrogen trioxide SO3 XeF6 KrF2 BrCl5 SCl4 PF3 As4O10 N2O3
Writing Formulas • Write each atom’s symbol with a subscript equal to the prefix. Ex. Hexaphosphorus tribromide P6Br3 Pentatellurium mononitride Te5N
Try these dinitrogen pentasulfide carbon monoxide heptasulfur trioxide xenon hexafluoride trisulfur hexafluoride phosphorus pentachloride nitrogen monoxide dibismuth trichloride
Try these dinitrogen pentasulfideN2S5 carbon monoxideC0 heptasulfur trioxideS7O3 xenon hexafluorideXeF6 trisulfur hexafluorideS3F6 phosphorus pentachloridePCl5 nitrogen monoxide NO dibismuth trichlorideBi2Cl3