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The Nomenclature of Binary Compounds Formula of Binary Compounds (Compounds composed of two elements) (1). Shows the number of atoms of each type that.

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Presentation on theme: "The Nomenclature of Binary Compounds Formula of Binary Compounds (Compounds composed of two elements) (1). Shows the number of atoms of each type that."— Presentation transcript:

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2 The Nomenclature of Binary Compounds

3 Formula of Binary Compounds (Compounds composed of two elements) (1). Shows the number of atoms of each type that are found in the compound. These numbers are indicated by subscripts Al 2 O 3 NaClS 4 Cl 2 SF 6 Subscripts (2). In the formulas the less electronegative atom is written first

4 Compounds Covalent ( Molecular ) Ionic I-Cl NaCl Cl - Na + Cl - Na + Cl - Na + Cl - Na + Cl 1- Na +

5 Na 2 ON 2 O NO NO 2 N 2 O 3 N 2 O 5

6 NaCl CO CO 2 Be able to summerize the nomenclature of binary ionic and binary covalent ( i.e. molecular) compounds contrasting differences in the way that the two classes of compounds are named.

7 Nomenclature of Binary Compounds ionic compounds (typically compounds of metallic and non-metallic elements ) Name the Name the less electronegative element more electronegative element Prefixes like di, or tri (indicating the number of atoms) are never used when naming ionic compounds Name of the Element Root + ide

8 Nomenclature of Binary Compounds Covalent (molecular) compounds (typically compounds of non-metallic elements ) Name the Name the less electronegative element more electronegative element prefix: used to indicate the number of less electronegative atoms ( if more than one) and is always used to indicate the number of more electronegative atoms Name of the Element Root + ide Prefix+

9 Root O oxygen oxBr Bromine Cl chlorine chlorAs Arsenic N nitrogennitr Te Tellurium H hydrogenhydr I iodine Se selenium P phosphorus F fluorine S sulfur C carbon Selen Iod Phosph fluor sulf carb Brom Arsen tellur

10 Numerical Prefixes 1 mono8octa 2 di9 nona 3 tri10 deca 4 tetra11 undeca 5 penta12 dodeca 6 hexa13 trideca 7 hepta14 tetradeca

11 Name the following binary compounds As 2 S 3 Na 2 S Mo 2 Cl 8 ( name as a covalent compound ) Al 4 C 3 Cl 2 O 7 B 3 N 3 ICl RbCl MgI 2 SF 6 KF diarsenic trisulfide Sodium sulfide dimolydenum octachloride Aluminum carbide dichlorine heptoxide Triboron trinitride Iodine monochloride rubidium chloride magnesium iodide Sulfur hexafluoride potassium fluoride

12 Name the following binary compounds 1. NaCl13. SO 3 2. ICl14. P 2 S 5 3. Al 2 O 3 4. C 2 O SF 6 5. Al 4 C XeF 4 6. CS 2 7. CO 8. AlP 17. S 4 Cl 2 9. SO NI Ba 3 N OF 2 Sodium chloride Iodine monochloride Aluminum oxide Dicarbon trioxide Aluminum carbide Carbon disulfide Aluminum phosphide Sulfur trioxide Nitrogen triiodide Carbon monoxide Barium nitride Oxygen difluoride Sulfur trioxide diphosphorus pentasulfide Sulfur hexafluoride Xenon tetrafluoride tetrasulfur dichloride

13 Name the following binary compounds (name the following metal - containing compounds as covalent compounds) 18. CrO TiCl W 2 Cl PbO 2 Chromium trioxide Titanium tetrachloride ditungsten octachloride lead dioxide

14 The Formation and Nomenclature of Monatomic Ions

15 Representative Elements that may form only 1 cation H LiBe Al NaMg KCa RbSr CsBa (2). form a cation, M n+ ; where n is the number of electrons lost( designated by the Group Nb.) (1). lose all electrons from the valence shell 1A2A 3A Named as: Element name+ ion

16 Non metals and metalloids Forming Monatomic Anions 1A4A 5A6A 7A H C N O F Si P S Cl AsSe Br TeI ¶These elements gain one or more electrons into the outer shell forming an anion, A n- ËThe charge, n-, of the anion is the number of electrons gained ÌThe nb of electrons gained is that nb. needed to achieve an octet of electrons in the valance electron shell, i.e. 8-Group Nb.

17 Non metals and metalloids Forming Monatomic Anions 1A4A 5A6A 7A H 1- C 4- N 3- O 2- F 1- Si 4- P 3- S 2- Cl 1- As 3- Se 2- Br 1- Te 2- I 1- ¶These elements gain one or more electrons into the outer shell forming an anion, A n- ËThe charge, n-, of the anion is the number of electrons gained ÌThe nb of electrons gained is that nb. needed to achieve an octet of electrons in the valance electron shell, i.e. 8-Group Nb.

18 Nomenclature of Monatomic Anions Root+ ide identifies the element identifies the ion as a monatomic anion

19 Representative Elements that may form only 1 cation H LiBe Al NaMg KCa RbSr CsBa (2). form a cation, M n+ ; where n is the number of electrons lost( designated by the Group Nb.) (1). lose all electrons from the valence shell 1A2A 3A Named as: Element name+ ion

20 Non metals and metalloids Forming Monatomic Anions 1A4A 5A6A 7A ÌThe nb of electrons gained is that nb. needed to achieve an octet of electrons in the valance electron shell, i.e. 8-Group Nb. ËThe charge, n-, of the anion is the number of electrons gained ¶These elements gain one or more electrons into the outer shell forming an anion, A n- H 1- C 4- N 3- O 2- F 1- Si 4- P 3- S 2- Cl 1- As 3- Se 2- Br 1- Te 2- I 1- Names: Root + ide H C N O F Si P S Cl As Se Br Te I

21 The reaction of the elements Li and F Li F Li 1+ F 1-

22 Predicting the Formula of Binary Ionic Compounds (Formed Through the Reaction of the Elements) ¬Determine the identity of the cation and the anion that the metal and non-metal would form. ­Determine the stoichiometry of the formula unit for the compound.

23 Following the outline given on the previous slide determine the formula of the following combinations of elements Al and O Ba and Se

24 Predicting the Formula of Binary Ionic Compounds (Formed Through the Reaction of the Elements) 2 3 Al and O Al 3+ O 2- Al 2 O 3 Al 3+ O 2- ­Determine the stoichiometry of the formula unit for the compound. ¬Determine the identity of the cation and the anion that the metal and non-metal would form.

25 Predicting the Formula of Binary Ionic Compounds (Formed Through the Reaction of the Elements) 2 2 Ba and Se Ba 2+ Se 2- Ba 2+ O 2- ­Determine the stoichiometry of the formula unit for the compound. ¬Determine the identity of the cation and the anion that the metal and non-metal would form. Ba 2 Se 2 BaSe

26 Ca 2+ Cl 1- CaCl 2 Al 4 C 3 C 4- Al 3+ Na 1+ F 1- Ba 2- O 2- NaF BaO Ions Formed Formula Give formula for, and name, the binary ionic compounds that would be formed through the reaction of the following pairs of elements: 1. Ca and Cl 4. Ba and O 3. Na and F 2. C and Al Al 3+ C 4- Calcium chloride Aluminum carbide Sodium fluoride Barium oxide

27 Give formula for, and name, the binary ionic compounds that would be formed through the reaction of the following pairs of elements: 5. N and Mg 6. Li and Se 7. Ga and As N 3- Mg 2- Mg 3 N 2 Li 1+ Se 2- Li 2 Se Ga 3+ As 3- GaAs Ions Formed Formula Magnesium nitride Lithium selenide Gallium arsenide Mg 2+ N 3-

28 Metals that form more than 1 cation: Transition and Post-Transition Metals Transition Metals Post Transition Metals 3B 4B 5B 6B 7B 8B 1B 2B 3A 4B 5A Sc TiiVCrMnFeCoNiCuZnGa AgCdInSn AuHgTlPbBi

29 Metals that form more than 1 cation: Transiton Metals 3B4B5B6B7B8B 1B 2B Sc 2+ Ti 2+ V 2+ Cr 2+ Mn 2+ Fe 2+ Co 2+ Ni 2+ Cu 1+ Zn 2+ Cation of Lower Charge: Formed by losing Ag 1+ Cd 2+ all electrons from the outermost electron shell ( 2 e - for all, except for Group 1B Au 1+ Hg 1+ where 1 e - is lost)

30 Metals that form more than 1 cation: Transiton Metals 3B4B5B6B7B8B 1B 2B Sc 3+ Ti 3+ V 3+ Cr 3+ Mn 3+ Fe 3+ Co 3+ Ni 3+ Cu 2+ Zn 3+ Ag 2+ Cd 3+ Cation of Higher Charge: Possesses a charge Au 2+ Hg 2+ 1 higher than the cation of lower charge (ions in red are uncommon)

31 Nomenclature of Transition and Post-Transition Metal Ions I. Stock System Name of Metal (Ionic Charge:Roman Numerals) Fe 2+ iron(II) ion Sn 4+ tin(IV) ion Cu 1+ copper(I) ion Cr 3+ chromium(III) ion

32 II. Older Nomenclature -ic (ion of higher charge) Root + endings identifies the metal -ous (ion of lower charge) Fe 2+ ferrous ion Sn 4+ stannic ion Cu 1+ cuprous ion Cr 3+ chromic ion

33 Fe ironferrum Cucoppercuprum Sntinstannum Pbleadplumbum Agsilverargentenum Augoldaurum

34 Name the following compounds: Fe 2 O 3 Iron(III) or ferric oxide CuCl Copper (1) or cuprous chloride PbCl 4 Lead (IV) or plumbic chloride SnO Tin (II) or stannous oxide FeS Iron (II) or ferrous sulfide AgO Silver (II) or argentenic oxide


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