Nomenclature. Naming Compounds

Transcription

1 Nomenclature Naming Compounds

2 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. CaCl 2 Calcium chloride

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4 There is no real bond between the ions. There is just strong attraction between the opposite charges.

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6 Try these Metal & Non-metal K 2 Se MgO Cs 3 P SrF 2 Rb 3 N FrI BeS

7 Try these Metal & Non-metal K 2 Se MgO Cs 3 P SrF 2 Rb 3 N FrI BeS Potassium Selenide Magnesium Oxide Cesium Phosphide Strontium Fluoride Rubidium Nitride Francium Iodide Beryllium Sulfide

8 Try these Metal & Non-metal K 2 Se MgO Cs 3 P SrF 2 Rb 3 N FrI BeS Potassium Selenide Magnesium Oxide Cesium Phosphide Strontium Fluoride Rubidium Nitride Francium Iodide Beryllium Sulfide

9 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) CaCl 2

10 Try these Metal & Non-metal Sodium phosphide Magnesium telluride Lithium chloride Barium carbide Strontium arsenide

11 Try these Metal & Non-metal Sodium Phosphide Na + P -3 x Na 3 P

12 Try these Metal & Non-metal Magnesium Telluride Mg +2 Te MgTe

13 Try these Metal & Non-metal Lithium Chloride Li + Cl LiCl

14 Try these Metal & Non-metal Barium Carbide Ba +2 C -4 X Ba 2 C

15 Try these Metal & Non-metal Strontium Arsenide Sr +2 As -3 X3 x Sr 3 As 2

16 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 it s name.

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20 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

21 Try these: Transition Metal & Non-metal Fe 3 N 2 NiBr 3 CoCl 2 HgI MnO 2

22 Try these: Transition Metal & Non-metal Fe 3 N 2 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

23 Try these: Transition Metal & Non-metal NiBr 3 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

24 Try these: Transition Metal & Non-metal CoCl 2 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

25 HgI Try these: Transition Metal & Non-metal 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

26 MnO 2 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 Try these: Transition Metal & Non-metal

27 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: NiI 2

28 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. Li 3 PO 4 Lithium phosphate

29 Polyatomic Ions that we use in science 10: OH -1 SO -2 4 NO -1 3 CO -2 3 PO -3 4 NH +1 4 ClO -1 3 hydroxide sulfate nitrate carbonate phosphate ammonium chlorate

30 Try these: Polyatomic Ion NaOH K 2 SO 4 Ba(NO 3 ) 2 CuCO 3 Li 3 PO 4 NH 4 Cl

31 Try these: NaOH K 2 SO 4 Ba(NO 3 ) 2 CuCO 3 Li 3 PO 4 NH 4 ClO 3 Sodium Hydroxide Potassium Sulfate Barium Nitrate Copper(II) Carbonate Lithium Phosphate Ammonium Chlorate

32 Writing Formulas Calcium sulfate Potassium carbonate Ammonium hydroxide Iron (III) chlorate Copper (I) phosphate Zinc sulfate

33 Ionic Bonding vs Molecular Bonding Makes "Compounds vs Makes "Molecules" Transfers electrons vs Shares electrons Metals & Nonmetals vs Made of Nonmetals Positive & Negative vs Neutral Weak Bond vs Strong bond NaCl KOH CaCl 2 vs H 2 O CO 2 NH 3 CH 4

34 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. Prefixes Mono Di Tri Tetra Penta Hexa Hepta Octa Nona Deca

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36 ex. N 2 O NO N 2 O 3 dinitrogen monoxide nitrogen monoxide dinitrogen trioxide NO 2 nitrogen dioxide * N 2 O 4 N 2 O 5 dinitrogen tetroxide dinitrogen pentoxide

37 ex. N 2 O NO N 2 O 3 dinitrogen monoxide nitrogen monoxide dinitrogen trioxide NO 2 nitrogen dioxide * N 2 O 4 N 2 O 5 dinitrogen tetroxide dinitrogen pentoxide * When the first atom is singular, the prefix mono is not used.

38 Try These: Non-metal & Non-metal SO 3 XeF 6 KrF 2 BrCl 5 SCl 4 PF 3 As 4 O 10 N 2 O 3 sulfur trioxide xenon hexafluoride krypton difluoride bromine pentachloride sulfur tetrachloride phosphorus trifluoride tetrarsenic decoxide dinitrogen trioxide

39 Writing Formulas Write each atom s symbol with a subscript equal to the prefix. Ex. Hexaphosphorus tribromide P 6 Br 3 Pentatellurium mononitride Te 5 N

40 Try these dinitrogen pentasulfide carbon monoxide heptasulfur trioxide xenon hexafluoride trisulfur hexafluoride phosphorus pentachloride nitrogen monoxide dibismuth trichloride

41 Try these dinitrogen pentasulfide N 2 S 5 carbon monoxide C0 heptasulfur trioxide S 7 O 3 xenon hexafluoride XeF 6 trisulfur hexafluoride S 3 F 6 phosphorus pentachloride PCl 5 nitrogen monoxide NO dibismuth trichloride Bi 2 Cl 3